# Scientific Papers of Josiah Willard Gibbs, Volume 1/Chapter IIIa

Scientific Papers of Josiah Willard Gibbs, Volume 1
On the Equilibrium of Heterogeneous Substances, Part 1
1874418Scientific Papers of Josiah Willard Gibbs, Volume 1 — On the Equilibrium of Heterogeneous Substances, Part 1Josiah Willard Gibbs

III.

ON THE EQUILIBRIUM OF HETEROGENEOUS SUBSTANCES.

[Transactions of the Connecticut Academy, III., pp. 108–248, Oct. 1875–May, 1876, and pp. 343–524, May, 1877–July, 1878.]

"Die Energie der Welt ist constant.
Die Entropie der Welt strebt einem Maximum zu."

Clausius[1]

The comprehension of the laws which govern any material system is greatly facilitated by considering the energy and entropy of the system in the various states of which it is capable. As the differences of the values of the energy for any two states represents the combined amount of work and heat received or yielded by the system when it is brought from one state to the other, and the difference of entropy is the limit of all the possible values of the integral ${\displaystyle \int {\frac {dQ}{t}}}$, (${\displaystyle dQ}$ denoting the element of heat received from external sources, and ${\displaystyle t}$ the temperature of the part of the system receiving it,) the varying values of the energy and entropy characterize in all that is essential the effects producible by the system in passing from one state to another. For by mechanical and thermodynamic contrivances, supposed theoretically perfect, any supply of work and heat may be transformed into any other which does not differ from it either in the amount of work and heat taken together or in the value of the integral ${\displaystyle \int {\frac {dQ}{t}}}$. But it is not only in respect to the external relations of a system that its energy and entropy are of predominant importance. As in the case of simply mechanical systems, (such as are discussed in theoretical mechanics,) which are capable of only one kind of action upon external systems, viz., the performance of mechanical work, the function which expresses the capability of the system for this kind of action also plays the leading part in the theory of equilibrium, the condition of equilibrium being that the variation of this function shall vanish, so in a thermodynamic system, (such as all material systems actually are,) which is capable of two different kinds of action upon external systems, the two functions which express the twofold capabilities of the system afford an almost equally simple criterion of equilibrium.

Criteria of Equilibrium and Stability.

The criterion of equilibrium for a material system which is isolated from all external influences may be expressed in either of the following entirely equivalent forms:—

I. For the equilibrium of any isolated system it is necessary and sufficient that in all possible variations of the state of the system which do not alter its energy, the variation of its entropy shall either vanish or be negative. If ${\displaystyle \epsilon }$ denote the energy, and ${\displaystyle \eta }$ the entropy of the system, and we use a subscript letter after a variation to indicate a quantity of which the value is not to be varied, the condition of equilibrium may be written

 ${\displaystyle (\delta \eta )_{\epsilon }\leqq 0.}$ (1)
II. For the equilibrium of any isolated system it is necessary and sufficient that in all possible variations in the state of the system which do not alter its entropy, the variation of its energy shall either vanish or be positive. This condition may be written
 ${\displaystyle (\delta \epsilon )_{\eta }\geqq 0.}$ (2)
That these two theorems are equivalent will appear from the consideration that it is always possible to increase both the energy and the entropy of the system, or to decrease both together, viz., by imparting heat to any part of the system or by taking it away. For, if condition (1) is not satisfied, there must be some variation in the state of the system for which
 ${\displaystyle \delta \eta >0}$ and ${\displaystyle \delta \epsilon =0}$;
therefore, by diminishing both the energy and the entropy of the system in its varied state, we shall obtain a state for which (considered as a variation from the original state)
 ${\displaystyle \delta \eta =0}$ and ${\displaystyle \delta \epsilon <0}$;
therefore condition (2) is not satisfied. Conversely, if condition (2) is not satisfied, there must be a variation in the state of the system for which
 ${\displaystyle \delta \epsilon <0}$ and ${\displaystyle \delta \eta =0}$;
hence there must also be one for which
 ${\displaystyle \delta \epsilon =0}$ and ${\displaystyle \delta \eta >0}$;
therefore condition (1) is not satisfied.

The equations which express the condition of equilibrium, as also its statement in words, are to be interpreted in accordance with the general usage in respect to differential equations, that is, infinitesimals of higher orders than the first relatively to those which express the amount of change of the system are to be neglected. But to distinguish the different kinds of equilibrium in respect to stability, we must have regard to the absolute values of the variations. We will use the ${\displaystyle \Delta }$ as the sign of variation in those equtions which are to be construed strictly, i.e., in which infinitesimals of the higher orders are not to be neglected. With this understanding, we may express the necessary and sufficient conditions of the different kinds of equilibrium as follows;—for stable equilibrium

 ${\displaystyle (\Delta \eta )_{\epsilon }<0,}$ i.e., ${\displaystyle (\Delta \epsilon )_{\eta }>0;}$ (3)
for neutral equilibrium there must be some variations in the state of the system for which
 ${\displaystyle (\Delta \eta )_{\epsilon }=0,}$ i.e., ${\displaystyle (\Delta \epsilon )_{\eta }=0;}$ (4)
while in general
 ${\displaystyle (\Delta \eta )_{\epsilon }\leqq 0,}$ i.e., ${\displaystyle (\Delta \epsilon )_{\eta }\geqq 0;}$ (5)
and for unstable equilibrium there must be some variations for which
 ${\displaystyle (\Delta \eta )_{\epsilon }>0,}$ (6)
i.e., there must be some for which
 ${\displaystyle (\Delta \epsilon )_{\eta }<0,}$ (7)
while in general
 ${\displaystyle (\Delta \eta )_{\epsilon }\leqq 0,}$ i.e., ${\displaystyle (\Delta \epsilon )_{\eta }\geqq 0.}$ (4)
In these criteria of equilibrium and stability, account is taken only of possible variations. It is necessary to explain in what sense this is to be understood. In the first place, all variations in the state of the system which involve the transportation of any matter through any finite distance are of course to be excluded from consideration, although they may be capable of expression by infinitesimal variations of quantities which perfectly determine the state of the system. For example, if the system contains two masses of the same substance, not in contact, nor connected by other masses consisting of or containing the same substance or its components, an infinitesimal increase of the one mass with an equal decrease of the other is not to be considered as a possible variation in the state of the system. In addition to such cases of essential impossibility, if heat can pass by conduction or radiation from every part of the system to every other, only those variations are to be rejected as impossible, which involve changes which are prevented by passive forces or analogous resistances to change. But, if the system consist of parts between which there is supposed to be no thermal communication, it will be necessary to regard as impossible any diminution of the entropy of any of these parts, as such a change can not take place without the passage of heat. This limitation may most conveniently be applied to the second of the above terms of the condition of equilibrium, which will then become
 ${\displaystyle (\delta \epsilon )_{\eta ',\eta ^{\prime \prime },etc.}\geqq 0,}$ (9)
${\displaystyle \eta ',\eta ^{\prime \prime }}$, etc., denoting the entropies of the various parts between which there is no communication of heat. When the condition of equilibrium is thus expressed, the limitation in respect to the conduction of heat will need no farther consideration.

In order to apply to any system the criteria of equilibrium which have been been given, a knowledge is requisite of its passive forces or resistances to change, in so far, at least, as they are capable of preventing change. (Those passive forces which only retard change, like viscosity, need not be considered.) Such properties of a system are in general easily recognized upon the most superficial knowledge of its nature. As examples, we may instance the passive force of friction which prevents sliding when two surfaces of solids are pressed together,—that which prevents the different components of a solid, and sometimes of a fluid, from having different motions one from another,—that resistance to change which sometimes prevents either of two forms of the same substance (simple or compound), which are capable of existing, from passing in to the other,—that which prevents the changes in solids which imply plasticity, (in other words, changes of the form to which the solid tends to return,) when the deformation does not exceed certain limits.

It is a characteristic of all these passive resistances that they prevent a certain kind of motion or change, however the initial state of the system may be modified, and to whatever external agencies of force and heat it may be subjected, whitin limits, it may be, but yet within limits which allow finite variations in the values of all the quantities which express the initial state of the system or the mechanical or thermal influences acting on it, without producing the change in question. The equilibrium which is due to such passive properties is thus widely distinguished from that caused by the balance of the active tendencies of the system, where an external influence, or a change in the initial state, infinitesimal in amount, is sufficient to produce change either in the positive or negative direction. Hence the ease with which these passive resistances are recognized. Only in the case that the state of the system lies so near the limit at which the resistances cease to be operative to prevent change, as to create a doubt whether the case falls within or without the limit, will a more accurate knowledge of these resistances be necessary.

To establish the validity of the criterion of equilibrium we will consider first the sufficiency, and afterwards the necessity, of the condition as expressed in either of the two equivalent forms.

In the first place, if the system is in a state in which the entropy is greater than in any other state of the ame energy, it is evidently in equilibrium, as any change of state must involve either a decrease of entropy or an increase of energy, which are alike impossible for an isolated system. We may add that this is a case of stable equilibrium, as no infinitely small cause (whether relating to a variation of the initial state or to the action of any external bodies) can produce a finite change of state, as this would involve a finite decrease of entropy or increase of energy.

We will next suppose that the system has the greatest entropy consistent with its energy, and therefore the least energy consistent with its entropy, but that there are other states of the same energy and entropy as its actual state. In this case, it is impossible that any motion of masses should take place; for if any of the energy of the system should come to consist of vis viva (of sensible motions), a state of the system identical in other respects but without the motion would have less energy and not less entropy, which would be contrary to the supposition. (But we cannot apply this reasoning to the motion within any mass of its different components in different directions, as in diffusion, when the momenta of the components balance one another.) Nor, in the case supposed, can any conduction of heat take place, for this involves an increase of entropy, as heat is only conducted from bodies of higher to those of lower temperature. It is equally impossible that any changes should be produced by the transfer of heat by radiation. The condition which we have supposed is therefore sufficient for equilibrium, so far as the motion of masses and the transfer of heat are concerned, but to show that the same is true in regard to the motions of diffusion and chemical or molecular changes, when these can occur without being accompanied or followed by the motions of masses or the transfer of heat, we must have recourse to considerations of a more general nature. The following considerations seem to justify the belief that the condition is sufficient for equilibrium in every respect.

Let us suppose, in order to test the tenability of such a hypothesis, that a system may have the greatest entropy consistent with its energy without being in equilibrium. In such a case, changes in the state of the system must take place, but these will necessarily be such that the energy and the entropy will remain unchanged and the system will continue to satisfy the same condition, as initially, of having the greatest entropy consistent with its energy. Let us consider the change which takes place in any time so short that the change may be regarded as uniform in nature throughout that time. This time must be so chosen that the change does not take place in it infinitely slowly, which is always easy, as the change which we suppose to take place cannot be infinitely slow except at particular moments. Now no change whatever in the state of the system, which does not alter the value of the energy, and which commences with the same state in which the system was supposed at the commencement of the short time considered, will cause an increase of entropy. Hence, it will generally be possible by some slight variation in the circumstances of the case to make all changes in the state of the system like or nearly like that which is supposed actually to occur, and not involving a change of energy, to involve a necessary decrease of entropy, which would render any such change impossible. This variation may be in the values of the variables which determine the nature of the system, or in the form of the functions which express its laws,—only there must be nothing in the system as modified which is thermodynamically impossible. For example, we might suppose temperature or pressure to be varied, or the composition of the different bodies in the system, or, if no small variations which could be actually realized would produce the required result, we might suppose the properties themselves of the substances to undergo variation, subject to the general laws of matter. If, then, there is any tendency toward change in the system as first supposed, it is a tendency which can be entirely checked by an infinitesimal variation in the circumstances of the case. As this supposition cannot be allowed, we must believe that a system is always in equilibrium when it has the greatest entropy consisten with its energy, or, in other words, when it has the least energy consistent with its entropy.

The same considerations will evidently apply to any case in which a system is in such a state that ${\displaystyle \Delta \eta \leqq 0}$ for any possible infinitesimal variation of the state for which ${\displaystyle \Delta \epsilon =0}$, even if the entropy is not the greatest which the system is capable with the same energy. (The term possible has here the meaning previously defined, and the character ${\displaystyle \Delta }$ is used, as before, to denote that the equations are to be construed strictly, i.e., without neglect of the infinitesimals of the higher orders.)

The only case in which the sufficiency of the condition of equilibrium which has been given remains to be proved is that in which in our notation ${\displaystyle \delta \eta \leqq 0}$ for all possible variations not affecting the energy, but for some of these variations ${\displaystyle \Delta \eta >0}$, that is, when the entropy has in some respects the characteristics of a minimum. In this case the considerations adduced in the last paragraph will not apply without modification, as the change of state may be infinitely slow at first, and it is only in the initial state that the condition ${\displaystyle \delta \eta _{\epsilon }\leqq 0}$ holds true. But the differential coefficients of all orders of the quantities which determine the state of the system, taken with respect of the time, must be functions of these same quantities. None of these differential coefficients can have any value other than 0, for the state of the system for which ${\displaystyle \delta \eta _{\epsilon }\leqq 0}$. For otherwise, as it would generally be possible, as before, by some infinitely small modification of the case, to render impossible any change like or nearly like that which might be supposed to occur, this infinitely small modification of the case would make a finite difference in the value of the differential coefficients which had before the finite values, or in some of lower orders, which is contrary to that continuity which we have reason to expect. Such considerations seem to justify us in regarding such a state as we are discussing as one of theoretical equilibrium; although as the equilibrium is evidently unstable, it cannot be realized.

We have still to prove that the condition enunciated is in every case necessary for equilibrium. It is evidently so in all cases in which the active tendencies of the system are so balanced that changes of every kind, except those excluded in the statement of the condition of equilibrium, can take place reversibly (i.e., both in the positive and the negative direction,) in states of the system differing infinitely little from the state in question. In this case, we may omit the sign of inequality and write as the condition of such a state of equilibrium

 ${\displaystyle (\delta \eta )_{\epsilon }=0}$, i.e., ${\displaystyle (\delta \epsilon )_{\eta }=0.}$ (10)
But to prove that the condition previously enunciated is in every case necessary, it must be shown that whenever an isolated system remains without change, if there is any infinitesimal variation in its state, not involving a finite change of position of any (even an infinitesimal part) of its matter, which would diminish its energy by a quantity which is not infinitely small relatively to the variations of the quantities which determine the state of the system, without altering its entropy,—or, if the system has thermally isolated parts, without altering the entropy of any such part,—this variation involves changes in the system which are prevented by its passive forces or analogous resistances to change. Now, as the described variation in the state of the system diminishes its energy without altering its entropy, it must be regarded as theoretically possible to produce that variation by some process, perhaps a very indirect one, so as to gain a certain amount of work (above all expended on the system). Hence we may conclude that the active forces or tendencies of the system favor the variation in question, and that equilibrium cannot subsist unless the variation is prevented by passive forces.

The preceding considerations will suffice, it is believed, to establish the validity of the criterion of equilibrium which has been given. The criteria of stability may readily be deduced from that of equilibrium. We will now proceed to apply these principles to systems consisting of heterogeneous substances and deduce the special laws which apply to different classes of phenomena. For this purpose we shall use the second form of the criterion of equilibrium, both because it admits more readily the introduction of the condition that there shall be no thermal communication between the different parts of the system, and because it is more convenient, as respects the form of the general equations relating to equilibrium, to make the entropy one of the independent variables which determine the state of the system, than to make the energy one of these variables.

The Conditions of Equilibrium for Heterogeneous Masses in Contact when Uninfluenced by Gravity, Electricity, Distortion of the Solid Masses, or Capillary Tensions.

In order to arrive as directly as possible at the most characteristic and essential laws of chemical equilibrium, we will first give our attention to a case of the simplest kind. We will examine the conditions of equilibrium of a mass of matter of various kinds enclosed in a rigid and fixed envelop, which is impermeable to and unalterable by any of the substances enclosed, and perfectly non-conducting to heat. We will suppose that the case is not complicated by the action of gravity, or by any electrical influences, and that in the solid portions of the mass the pressure is the same in every direction. We will farther simplify the problem by supposing that the variations of the parts of the energy and entropy which depend upon the surfaces separating heterogeneous masses are so small in comparison with the variations of the parts of the energy and entropy which depend upon the quantities of these masses, that the former may be neglected by the side of the latter; in other words, we will exclude the considerations which belong to the theory of capillarity.

It will be observed that the supposition of a rigid and non-conducting envelop enclosing the mass under discussion involves no real loss of generality, for if any mass of matter is in equilibrium, it would also be so, if the whole or any part of it were enclosed in an envelop as supposed; therefore the conditions of equilibrium for a mass thus enclosed are the general conditions which must always be satisfied in case of equilibrium. As for the other suppositions which have been made, all the circumstances and considerations which are here excluded will afterward be made the subject of special discussion.

Conditions relating to the Equilibrium between the initially existing Homogeneous Parts of the given Mass.

Let us first consider the energy of any homogeneous part of the given mass, and its variation for any possible variation in the composition and state of this part. (By homogeneous is meant that the part in question is uniform throughout, not only in chemical composition, but also in physical state.) If we consider the amount and kind of matter in this homogeneous mass as fixed, its energy ${\displaystyle \epsilon }$ is a function of its entropy ${\displaystyle \eta }$, and its volume ${\displaystyle v}$, and the differentials of these quantities are subject to the relation

 ${\displaystyle d\epsilon =td\eta -pdv,}$ (11)
${\displaystyle t}$ denoting the (absolute) temperature of the mass, and ${\displaystyle p}$ its pressure. For ${\displaystyle td\eta }$ is the heat received, and ${\displaystyle pdv}$ the work done, by the mass during its change of state. But if we consider the matter in the mass as variable, and write ${\displaystyle m_{1},m_{2},...,m_{n}}$ for the quantities of the various substances ${\displaystyle S_{1},S_{2},...,S_{n}}$ of which the mass is composed, ${\displaystyle \epsilon }$ will evidently be a function of ${\displaystyle \eta ,v,m_{1},m_{2},...,m_{n}}$, and we shall have for the complete value of the differential of ${\displaystyle \epsilon }$
 ${\displaystyle d\epsilon =td\eta -pdv+\mu _{1}dm_{1}+\mu _{2}dm_{2}+...+\mu _{n}dm_{n},}$ (12)
${\displaystyle \mu _{1},\mu _{2},...,\mu _{n}}$ denoting the differential coefficients of ${\displaystyle \epsilon }$ taken with respect to ${\displaystyle m_{1},m_{2},...,m_{n}}$.

The substances ${\displaystyle S_{1},S_{2},...,S_{n}}$, of which we consider the mass composed, must of course be such that the values of the differentials ${\displaystyle dm_{1},dm_{2},...,dm_{n}}$ shall be independent, and shall express every possible variation in the composition of the homogeneous mass considered, including those produced by the absorption of substances different from any initially present. It may therefore be necessary to have terms in the equation relating to component substances which do not initially occur in the homogeneous mass considered, provided, of course, that these substances, or their components, are to be found in some part of the whole given mass.

If the conditions mentioned are satisfied, the choice of the substances which we are to regard as the components of the mass considered, may be determined entirely by convenience, and independently of any theory in regard to the internal constitution of the mass. The number of components will sometimes be greater, and sometimes less, than the number of chemical elements present. For example, in considering the equilibrium in a vessel containing water and free hydrogen and oxygen, we should be obliged to recognize three components in the gaseous part. But in considering the equilibrium of dilute sulphuric acid with the vapor which it yields, we should have only two components to consider in the liquid mass, sulphuric acid (anhydrous, or of any particular degree of concentration) and (additional) water. If, however, we are considering sulphuric acid in a state of maximum concentration in connection with substances which might possibly afford water to the acid, it must be noticed that the condition of the independence of the differentials will require that we consider the acid in the state of maximum concentration as one of the components. The quantity of this component will then be capable of variation both in the positive and in the negative sense, while the quantity of the other component can increase but cannot decrease below the value 0.

For brevity's sake, we may call a substance S a an actual component of any homogeneous mass, to denote that the quantity ${\displaystyle S_{a}}$ of that substance in the given mass may be either increased or diminished (although we may have so chosen the other component substances that ${\displaystyle m_{a}=0}$); and we may call a substance ${\displaystyle S_{b}}$ a possible component to denote that it may be combined with, but cannot be subtracted from the homogeneous mass in question. In this case, as we have seen in the above example, we must so choose the component substances that ${\displaystyle m_{b}=0}$.

The units by which we measure the substances of which we regard the given mass as composed may each be chosen independently. To fix our ideas for the purpose of a general discussion, we may suppose all substances measured by weight or mass. Yet in special cases, it may be more convenient to adopt chemical equivalents as the units of the component substances.

It may be observed that it is not necessary for the validity of equation (12) that the variations of nature and state of the mass to which the equation refers should be such as do not disturb its homogeneity, provided that in all parts of the mass the variations of nature and state are infinitely small. For, if this last condition be not violated, an equation like (12) is certainly valid for all the infinitesimal parts of the (initially) homogeneous mass ; i.e., if we write ${\displaystyle D\epsilon ,D\eta ,}$ etc., for the energy, entropy, etc., of any infinitesimal part,

 ${\displaystyle dD\epsilon =tdD\eta -pdDv+\mu _{1}dDm_{1}++\mu _{2}dDm_{2}+...+\mu _{n}dDm_{n}}$ (13)
whence we may derive equation (12) by integrating for the whole initially homogeneous mass.

�We will now suppose that the whole mass is divided into parts so that each part is homogeneous, and consider such variations in the energy of the system as are due to variations in the composition and state of the several parts remaining (at least approximately) homogeneous, and together occupying the whole space within the envelop. We will at first suppose the case to be such that the component substances are the same for each of the parts, each of the substances ${\displaystyle S_{1},S_{2},...,S_{n}}$ being an actual component of each part. If we distinguish the letters referring to the different parts by accents, the variation in the energy of the system may be expressed by ${\displaystyle \delta \epsilon '+\delta \epsilon ''+etc.}$, and the general condition of equilibrium requires that

 ${\displaystyle \delta \epsilon '+\delta \epsilon ''+etc.\geqq 0}$ (14)

for all variations which do not conflict with the equations of condition. These equations must express that the entropy of the whole given mass does not vary, nor its volume, nor the total quantities of any of the substances ${\displaystyle S_{1},S_{2},...,S_{n}}$. We will suppose that there are no other equations of condition. It will then be necessary for equilibrium that

 ${\displaystyle t'\delta \eta '-p'\delta v'+\mu _{1}\delta m'_{1}+\mu _{2}\delta m'_{2}...+\mu _{n}\delta m'_{n}+t''\delta \eta ''-p''\delta v''+\mu _{1}\delta m''_{1}+\mu _{2}\delta m''_{2}...+\mu _{n}\delta m''_{n}+etc.\geqq 0}$ (15)
for any values of the variations for which
 ${\displaystyle \delta \eta '+\delta \eta ''+\delta \eta '''+{\text{etc.}}=0,}$ (16)
 ${\displaystyle \delta v'+\delta v''+\delta v'''+{\text{etc.}}=0,}$ (17)
 ${\displaystyle \delta m'_{1}+\delta m''_{1}+\delta m'''_{1}+{\text{etc.}}=0,}$ ${\displaystyle \scriptstyle {\left.{\begin{matrix}\ \\\\\ \\\ \ \end{matrix}}\right\}\,}}$ (18) ${\displaystyle \delta m'_{2}+\delta m''_{2}+\delta m'''_{2}+{\text{etc.}}=0,}$ ${\displaystyle .............................................}$ ${\displaystyle \delta m'_{n}+\delta m''_{n}+\delta m'''_{n}+{\text{etc.}}=0.}$

For this it is evidently necessary and sufficient that

 ${\displaystyle t'=t''=t'''={\text{etc.}}}$ (19)
 ${\displaystyle p'=p''=p'''={\text{etc.}}}$ (20)
 ${\displaystyle \mu _{1}'=\mu _{1}''=\mu _{1}'''={\text{etc.}}}$ ${\displaystyle \scriptstyle {\left.{\begin{matrix}\ \\\\\ \\\ \ \end{matrix}}\right\}\,}}$ (21) ${\displaystyle \mu _{2}'=\mu _{2}''=\mu _{2}'''={\text{etc.}}}$ ${\displaystyle ................................}$ ${\displaystyle \mu _{n}'=\mu _{n}''=\mu _{n}'''={\text{etc.}}}$

Equations (19) and (20) express the conditions of thermal and mechanical equilibrium, viz., that the temperature and the pressure must be constant throughout the whole mass. In equations (21) we have the conditions characteristic of chemical equilibrium. If we call a quantity ${\displaystyle \mu _{x}}$ as defined by such an equation as (12), the potential for the substance ${\displaystyle S_{x}}$ in the homogeneous mass considered, these conditions may be expressed as follows:—

The potential for each component substance must be constant throughout the whole mass.

It will be remembered that we have supposed that there is no restriction upon the freedom of motion or combination of the component substances, and that each is an actual component of all parts of the given mass.

The state of the whole mass will be completely determined (if we regard as immaterial the position and form of the various homogeneous parts of which it is composed), when the values are determined of the quantities of which the variations occur in (15). The number of these quantities, which we may call the independent variables, is evidently ${\displaystyle (n+2)_{\nu }}$, ${\displaystyle \nu }$ denoting the number of homogeneous parts into which the whole mass is divided. All the quantities which occur in (19), (20), (21), are functions of these variables, and may be regarded as known functions, if the energy of each part is known as a function of its entropy, volume, and the quantities of its components. (See eq. (12).) Therefore, equations (19), (20), (21), may be regarded as ${\displaystyle (\nu -1)(n+2)}$ independent equations between the independent variables. The volume of the whole mass and the total quantities of the various substances being known afford ${\displaystyle n+1}$ additional equations. If we also know the total energy of the given mass, or its total entropy, we will have as many equations as there are independent variables.

But if any of the substances ${\displaystyle S_{1},S_{2},...S_{n}}$ are only possible components of some parts of the given mass, the variation ${\displaystyle \delta m}$ of the quantity of such a substance in such a part cannot have a negative value, so that the general condition of equilibrium (15) does not require that the potential for that substance in that part should be equal to the potential for the same substance in the parts of which it is an actual component, but only that it shall not be less. In this case instead of (21) we may write

 ${\displaystyle \mu _{1}=M_{1}}$ ${\displaystyle \scriptstyle {\left.{\begin{matrix}\ \\\\\ \\\ \\\ \\\ \\\ \\\ \\\ \ \end{matrix}}\right\}\,}}$ (21) for all parts of which ${\displaystyle S_{1}}$ it is an actual component, and ${\displaystyle \mu _{1}\geqq M_{1}}$ for all parts of which ${\displaystyle S_{1}}$ is a possible (but not actual) component, ${\displaystyle \mu _{2}=M_{2}}$ for all parts of which ${\displaystyle S_{2}}$ it is an actual component, and ${\displaystyle \mu _{2}\geqq M_{2}}$ for all parts of which ${\displaystyle S_{2}}$ is a possible (but not actual) component, etc.,

${\displaystyle M_{1},M_{2}}$, etc., denoting constants of which the value is only determined by these equations.

If we now suppose that the components (actual or possible) of the various homogeneous parts of the given mass are not the same, the result will be of the same character as before, provided that all the different components are independent (i.e., that no one can be made out of the others), so that the total quantity of each component is fixed. The general condition of equilibrium (15) and the equations of condition (16), (17), (18) will require no change, except that, if any of the substances ${\displaystyle S_{1},S_{2},...S_{n}}$ is not a component (actual or possible) of any part, the term ${\displaystyle \mu \delta m}$ for that substance and part will be wanting in the former, and the ${\displaystyle \delta m}$ in the latter. This will require no change in the form of the particular conditions of equilibrium as expressed by (19), (20), (22); but the number of single conditions contained in (22) is of course less than if all the component substances were components of all the parts. Whenever, therefore, each of the different homogeneous parts of the given mass may be regarded as composed of some or of all of the same set of substances, no one of which can be formed out of the others, the condition which (with equality of temperature and pressure) is necessary and sufficient for equilibrium between the different parts of the given mass may be expressed as follows:—

The potential for each of the component substances must have a constant value in all parts of the given mass of which that substance is an actual component, and have a value not less than this in all parts of which it is a possible component.

The number of equations afforded by these conditions, after elimination of ${\displaystyle M_{1},M_{2},...M_{n}}$, will be less than ${\displaystyle (n+2)(\nu -1)}$ by the number of terms in (15) in which the variation of the form ${\displaystyle \delta m}$ is either necessarily nothing or incapable of a negative value. The number of variables to be determined is diminished by the same number, or, if we choose, we may write an equation of the form ${\displaystyle m=0}$ for each of these terms. But when the substance is a possible component of the part concerned, there will also be a condition (expressed by ${\displaystyle \geqq }$) to show whether the supposition that the substance is not an actual component is consistent with equilibrium.

We will now suppose that the substances ${\displaystyle S_{1},S_{2},...S_{n}}$ are not all independent of each other, i.e., that some of them can be formed out of others. We will first consider a very simple case. Let ${\displaystyle S_{3}}$ be composed of ${\displaystyle S_{1}}$ and ${\displaystyle S_{2}}$ combined in the ratio of ${\displaystyle a}$ to ${\displaystyle b}$, ${\displaystyle S_{1}}$ and ${\displaystyle S_{2}}$ occurring as actual components in some parts of the given mass, and ${\displaystyle S_{3}}$ in other parts, which do not contain ${\displaystyle S_{1}}$ and ${\displaystyle S_{2}}$ as separately variable components. The general condition of equilibrium will still have the form of (15) with certain of the terms of the form ${\displaystyle \mu \delta m}$ omitted. It may be written more briefly

 ${\displaystyle \sum (t\delta \eta )-\sum (p\delta v)+\sum (\mu _{1}\delta m_{1})+\sum (\mu _{2}\delta m_{2})...+\sum (\mu _{n}\delta m_{n})\geqq 0}$ (23)
the sign ${\displaystyle \sum }$ denoting summation in regard to the different parts of the given mass. But instead of the three equations of condition,
 ${\displaystyle \sum (\mu _{1}\delta m_{1})=0,\,\,\,\sum (\mu _{2}\delta m_{2})=0,\,\,\,\sum (\mu _{3}\delta m_{3})=0}$ (24)
we shall have the two,
 ${\displaystyle \sum \delta m{1}+{\frac {a}{a+b}}\sum \delta m_{3}=0,}$ ${\displaystyle \scriptstyle {\left.{\begin{matrix}\ \\\\\ \\\ \ \end{matrix}}\right\}\,}}$ (25) ${\displaystyle \sum \delta m{2}+{\frac {b}{a+b}}\sum \delta m_{3}=0.}$

The other equations of condition,

 ${\displaystyle \sum \delta \eta =0,\,\,\,\sum \delta v=0,\,\,\,\sum \delta m_{4}=0}$, etc., (26)

will remain unchanged. Now as all values of the variations which satisfy equations (24) will also satisfy equations (25), it is evident that all the particular conditions of equilibrium which we have already deduced, (19), (20), (22), are necessary in this case also. When these are satisfied, the general condition (23) reduces to

 ${\displaystyle M_{1}\sum \delta m_{1}+M_{2}\sum \delta m_{2}+M_{3}\sum \delta m_{3}\geqq 0.}$ (27)
For, although it may be that ${\displaystyle \mu _{1}'}$, for example, is greater than ${\displaystyle M_{1}}$ yet it can only be so when the following ${\displaystyle \delta m'_{1}}$ is incapable of a negative value. Hence, if (27) is satisfied, (23) must also be. Again, if (23) is satisfied, (27) must also be satisfied, so long as the variation of the quantity of every substance has the value in all the parts of which it is not an actual component. But as this limitation does not affect the range of the possible values of ${\displaystyle \sum \delta m_{1}}$, ${\displaystyle \sum \delta m_{2}}$, and ${\displaystyle \sum \delta m_{3}}$, it may be disregarded. Therefore the conditions (23) and (27) are entirely equivalent, when (19), (20), (22) are satisfied. Now, by means of the equations of condition (25), we may eliminate ${\displaystyle \sum \delta m_{2}}$ and ${\displaystyle \sum \delta m_{3}}$ from (27), which becomes
 ${\displaystyle -aM_{1}\sum \delta m_{3}+(a+b)M_{3}\delta m_{3}\geqq 0,}$ (28)
i.e., as the value of ${\displaystyle \sum \delta m_{3}}$ may be either positive or negative,
 ${\displaystyle aM_{1}+bM_{2}=(a+b)M_{3},}$ (29)
which is the additional condition of equilibrium which is necessary in this case.

The relations between the component substances may be less simple than in this case, but in any case they will only affect the equations of condition, and these may always be found without difficulty, and will enable us to eliminate from the general condition of equilibrium as many variations as there are equations of condition, after which the coefficients of the remaining variations may be set equal to zero, except the coefficients of variations which are incapable of negative values, which coefficients must be equal to or greater than zero. It will be easy to perform these operations in each particular case, but it may be interesting to see the form of the resultant equations in general.

We will suppose that the various homogeneous parts are considered as having in all n components, ${\displaystyle S_{1},S_{2},...S_{n}}$, and that there is no restriction upon their freedom of motion and combination. But we will so far limit the generality of the problem as to suppose that each of these components is an actual component of some part of the given mass.[2] If some of these components can be formed out of others, all such relations can be expressed by equations such as

 ${\displaystyle \alpha {\mathfrak {S}}_{a}+\beta {\mathfrak {S}}_{b}+{\text{etc.}}=\kappa {\mathfrak {S}}_{k}+\gamma {\mathfrak {S}}_{l}+{\text{etc.}}}$ (30)
where ${\displaystyle {\mathfrak {S}}_{a},{\mathfrak {S}}_{b},{\mathfrak {S}}_{k}}$ etc. denote the units of the substances ${\displaystyle S_{a},S_{b},S_{k}}$, etc., (that is, of certain of the substances ${\displaystyle S_{1},S_{2},S_{3}}$,) and ${\displaystyle \alpha ,\beta ,\kappa }$, etc. denote numbers. These are not, it will be observed, equations between abstract quantities, but the sign ${\displaystyle =}$ denotes qualitative as well as quantitative equivalence. We will suppose that there are ${\displaystyle r}$ independent equations of this character. The equations of condition relating to the component substances may easily be derived from these equations, but it will not be necessary to consider them particularly. It is evident that they will be satisfied by any values of the variations which satisfy equations (18); hence, the particular conditions of equilibrium (19), (20), (22) must be necessary in this case, and, if these are satisfied, the general equation of equilibrium (15) or (23) will reduce to
 ${\displaystyle M_{1}\sum \delta m_{1}+M_{2}\sum \delta m_{2}...+M_{n}\sum \delta m_{n}\geqq 0.}$ (31)
This will appear from the same considerations which were used in regard to equations (23) and (27). Now it is evidently possible to give to ${\displaystyle \sum \delta m_{a}}$, ${\displaystyle \sum \delta m_{b}}$, ${\displaystyle \sum \delta m_{k}}$, etc. values proportional to ${\displaystyle \alpha }$, ${\displaystyle \beta }$, ${\displaystyle \kappa }$, etc. in equation (30), and also the same values taken negatively, making ${\displaystyle \sum \delta m=0}$ in each of the other terms; therefore
 ${\displaystyle \alpha M_{a}+\beta M_{b}+etc...-\kappa M_{k}-\lambda M_{l}-etc.=0,}$ (32)
 ${\displaystyle {\text{or}}\,\,\alpha M_{a}+\beta M_{b}+etc=\kappa M_{k}+\lambda M_{l}+etc.=0.}$ (33)
It will be observed that this equation has the same form and coefficients as equation (30), ${\displaystyle M}$ taking the place of ${\displaystyle {\mathfrak {S}}}$. It is evident that there must be a similar condition of equilibrium for every one of the ${\displaystyle r}$ equations of which (30) is an example, which may be obtained simply by changing in these equations into ${\displaystyle M}$. When these conditions are satisfied, (31) will be satisfied with any possible values of ${\displaystyle \sum \delta m_{1},\sum \delta m_{2},...\sum \delta m_{n}}$. For no values of these quantities are possible, except such that the equation
 ${\displaystyle \left(\sum \delta m_{1}\right){\mathfrak {S}}_{1}+\left(\sum \delta m_{2}\right){\mathfrak {S}}_{2}...+\left(\sum \delta m_{n}\right){\mathfrak {S}}_{n}=0}$ (34)
after the substitution of these values, can be derived from the ${\displaystyle r}$ equations like (30), by the ordinary processes of the reduction of linear equations. Therefore, on account of the correspondence between (31) and (34), and between the r equations like (33) and the ${\displaystyle r}$ equations like (30), the conditions obtained by giving any possible values to the variations in (31) may also be derived from the r equations like (33); that is, the condition (31) is satisfied if the r equations like (33) are satisfied. Therefore the ${\displaystyle r}$ equations like (33) are with (19), (20), and (22) the equivalent of the general condition (15) or (23).

For determining the state of a given mass when in equilibrium and having a given volume and given energy or entropy, the condition of equilibrium affords an additional equation corresponding to each of the ${\displaystyle r}$ independent relations between the n component substances. But the equations which express our knowledge of the matter in the given mass will be correspondingly diminished, being ${\displaystyle n-r}$ in number, like the equations of condition relating to the quantities of the component substances, which may be derived from the former by differentiation.

Conditions relating to the possible Formation of Masses Unlike any Previously Existing.

The variations which we have hitherto considered do not embrace every possible infinitesimal variation in the state of the given mass, so that the particular conditions already formed, although always necessary for equilibrium (when there are no other equations of condition than such as we have supposed), are not always sufficient. For, besides the infinitesimal variations in the state and composition of different parts of the given mass, infinitesimal masses may be formed entirely different in state and composition from any initially existing. Such parts of the whole mass in its varied state as cannot be regarded as parts of the initially existing mass which have been infinitesimally varied in state and composition, we will call new parts. These will necessarily be infinitely small. As it is more convenient to regard a vacuum as a limiting case of extreme rarefaction than to give a special consideration to the possible formation of empty spaces within the given mass, the term new parts will be used to include any empty spaces which may be formed, when such have not existed initially. We will use ${\displaystyle Dm_{1},Dm_{2},...Dm_{n}}$ to denote the infinitesimal energy, entropy, and volume of any one of these new parts, and the infinitesimal quantities of its components. The component substances ${\displaystyle S_{1},S_{2},...S_{n}}$ must now be taken to include not only the independently variable components (actual or possible) of all parts of the given mass as initially existing, but also the components of all the new parts, the possible formation of which we have to consider. The character ${\displaystyle \delta }$ will be used as before to express the infinitesimal variations of the quantities relating to those parts which are only infinitesimally varied in state and composition, and which for distinction we will call original parts, including under this term the empty spaces, if such exist initially, within the envelop bounding the system. As we may divide the given mass into as many parts as we choose, and as not only the initial boundaries, but also the movements of these boundaries during any variation in the state of the system are arbitrary, we may so define the parts which we have called original, that we may consider them as initially homogeneous and remaining so, and as initially constituting the whole system.

The most general value of the variation of the energy of the whole system is evidently

 ${\displaystyle \sum \delta \epsilon +\sum D\epsilon ,}$ (35)
the first summation relating to all the original parts, and the second to all the new parts. (Throughout the discussion of this problem, the letter ${\displaystyle \delta }$ or ${\displaystyle D}$ following ${\displaystyle \sum }$ will sufficiently indicate whether the summation relates to the original or to the new parts.) Therefore the general condition of equilibrium is
 ${\displaystyle \sum \delta \epsilon +\sum D\epsilon \geqq 0,}$ (36)
or, if we substitute the value of ${\displaystyle \delta \epsilon }$ taken from equation (12),
 ${\displaystyle \sum D\epsilon +\sum (t\delta \eta )-\sum (p\delta v)+\sum (\mu _{1}\delta m_{1})+\sum (\mu _{2}\delta m_{2})...+\sum (\mu _{n}\delta m_{n})\geqq 0.}$ (37)
If any of the substances ${\displaystyle S_{1},S_{2},...S_{n}}$ can be formed out of others, we will suppose, as before (see page 69), that such relations are expressed by equations between the units of the different substances.

Let these be

 ${\displaystyle a_{1}{\mathfrak {S}}_{1}+a_{1}{\mathfrak {S}}_{2}...+a_{n}{\mathfrak {S}}_{n}=0}$ ${\displaystyle \scriptstyle {\left.{\begin{matrix}\ \\\\\ \ \end{matrix}}\right\}\,}}$ ${\displaystyle r}$ equations.⁠(38) ${\displaystyle b_{1}{\mathfrak {S}}_{1}+b_{2}{\mathfrak {S}}_{2}...+b_{n}{\mathfrak {S}}_{n}=0}$ etc.

The equations of condition will be (if there is no restriction upon the freedom of motion and composition of the components)

 ${\displaystyle \sum \delta \eta +\sum D\eta =0,}$ (39)
 ${\displaystyle \sum \delta v+\sum Dv=0,}$ (40)
and ${\displaystyle n-r}$ equations of the form
 ${\displaystyle h_{1}(\sum \delta m_{1}+\sum Dm_{1})+h_{2}(\sum \delta m_{2}+\sum Dm_{2})...+h_{n}(\sum \delta m_{n}+\sum Dm_{n})=0}$ ${\displaystyle \scriptstyle {\left.{\begin{matrix}\ \\\\\ \ \end{matrix}}\right\}\,}}$ (41)[3] ${\displaystyle i_{1}(\sum \delta m_{1}+\sum Dm_{1})+i_{2}(\sum \delta m_{2}+\sum Dm_{2})...+i_{n}(\sum \delta m_{n}+\sum Dm_{n})=0}$ etc.

Now, using Lagrange's "method of multipliers,"[4] we will subtract ${\displaystyle T(\sum \delta \eta +\sum D\eta )-P(\sum \delta v+\sum Dv)}$ from the first member of the general condition of equilibrium (37), ${\displaystyle T}$ and ${\displaystyle P}$ being constants of which the value is as yet arbitrary. We might proceed in the same way with the remaining equations of condition, but we may obtain the same result more simply in another way. We will first observe that

 ${\displaystyle (\sum \delta m_{1}+\sum Dm_{2}){\mathfrak {S}}_{1}+(\sum \delta m_{2}+\sum Dm_{2}){\mathfrak {S}}_{2}...+(\sum \delta m_{n}+\sum Dm_{n}){\mathfrak {S}}_{n}}$ (42)
which equation would hold identically for any possible values of the quantities in the parentheses, if for ${\displaystyle r}$ of the letters ${\displaystyle {\mathfrak {S}}_{1},{\mathfrak {S}}_{2},...{\mathfrak {S}}_{n}}$ were substituted their values in terms of the others as derived from equations (38). (Although ${\displaystyle {\mathfrak {S}}_{1},{\mathfrak {S}}_{2},...{\mathfrak {S}}_{n}}$ do not represent abstract quantities, yet the operations necessary for the reduction of linear equations are evidently applicable to equations (38).) Therefore, equation (42) will hold true if for ${\displaystyle {\mathfrak {S}}_{1},{\mathfrak {S}}_{2},...{\mathfrak {S}}_{n}}$ we substitute ${\displaystyle n}$ numbers which satisfy equations (38). Let ${\displaystyle M_{1},M_{2},...M_{n}}$ be such numbers, i.e., let
 ${\displaystyle a_{1}M_{1}+a_{2}M_{2}+...+a_{n}M_{n}=0,}$ ${\displaystyle \scriptstyle {\left.{\begin{matrix}\ \\\\\ \ \end{matrix}}\right\}\,}}$ ${\displaystyle r}$ equations. (43) ${\displaystyle b_{1}M_{1}+b_{2}M_{2}+...+b_{n}M_{n}=0,}$ etc.

then

 ${\displaystyle M_{1}(\sum \delta m{1}+\sum Dm_{1})+M_{2}(\sum \delta m{2}+\sum Dm_{2})...+M_{n}(\sum \delta m{n}+\sum Dm_{n})=0.}$ (44)
This expression, in which the values of ${\displaystyle n-r}$ of the constants ${\displaystyle M_{1},M_{2},...M_{n}}$ are still arbitrary, we will also subtract from the first member of the general condition of equilibrium (37), which will then become
 ${\displaystyle \sum D\epsilon +\sum (t\delta \eta )-\sum (p\delta v)+\sum (\mu _{1}\delta m_{1})..+\sum (\mu _{n}\delta m_{n})-T\sum \delta \eta +P\sum \delta v-M_{1}\sum \mu _{1}\delta m_{1}...-M_{n}\sum \mu _{n}\delta m_{n}-T\sum D\eta +PDv-M_{1}\sum Dm_{1}...-M_{n}\sum Dm_{n}\geqq 0.}$ (45)
That is, having assigned to ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$ any values consistent with (43), we may assert that it is necessary and sufficient for equilibrium that (45) shall hold true for any variations in the state of the system consistent with the equations of condition (39), (40), (41). But it will always be possible, in case of equilibrium, to assign such values to ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$, without violating equations (43), that (45) shall hold true for all variations in the state of the system and in the quantities of the various substances composing it, even though these variations are not consistent with the equations of condition (39), (40), (41). For, when it is not possible to do this, it must be possible by applying (45) to variations in the system not necessarily restricted by the equations of condition (39), (40), (41) to obtain conditions in regard to ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$, some of which will be inconsistent with others or with equations (43). These conditions we will represent by
 ${\displaystyle A\geqq 0,\,\,B\geqq 0,\,\,etc.}$ (46)
${\displaystyle A,B}$, etc. being linear functions of ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$. Then it will be possible to deduce from these conditions a single condition of the form
 ${\displaystyle \alpha A+\beta B\geqq 0,}$ (47)
${\displaystyle \alpha ,\beta }$, etc. being positive constants, which cannot hold true consistently with equations (43). But it is evident from the form of (47) that, like any of the conditions (46), it could have been obtained directly from (45) by applying this formula to a certain change in the system (perhaps not restricted by the equations of condition (39), (40), (41)). Now as (47) cannot hold true consistently with eqs. (43), it is evident, in the first place, that it cannot contain ${\displaystyle T}$ or ${\displaystyle P}$, therefore in the change in the system just mentioned (for which (45) reduces to (47))
 ${\displaystyle \sum \delta \eta +\sum D\eta =0,}$ and ${\displaystyle \sum \delta v+\sum Dv=0,}$
so that the equations of condition (39) and (40) are satisfied. Again, for the same reason, the homogeneous function of the first degree of ${\displaystyle M_{1},M_{2},...M_{n}}$ in (47) must be one of which the value is fixed by eqs. (43). But the value thus fixed can only be zero, as is evident from the form of these equations. Therefore
 ${\displaystyle (\sum \delta m_{1}+\sum Dm_{1})M_{1}+(\sum \delta m_{2}+\sum Dm_{2})M_{2}...+(\sum \delta m_{n}+\sum Dm_{n})M_{n}=0}$ (48)
for any values of ${\displaystyle M_{1},M_{2},...M_{n}}$ which satisfy eqs. (43), and therefore
 ${\displaystyle (\sum \delta m_{1}+\sum Dm_{1}){\mathfrak {S}}_{1}+(\sum \delta m_{2}+\sum Dm_{2}){\mathfrak {S}}_{2}...+(\sum \delta m_{n}+\sum Dm_{n}){\mathfrak {S}}_{n}=0}$ (49)
for any numerical values of ${\displaystyle {\mathfrak {S}}_{1},{\mathfrak {S}}_{2},...{\mathfrak {S}}_{n}}$ which satisfy eqs. (38). This equation (49) will therefore hold true, if for ${\displaystyle r}$ of the letters ${\displaystyle {\mathfrak {S}}_{1},{\mathfrak {S}}_{2},...{\mathfrak {S}}_{n}}$ we substitute their values in terms of the others taken from eqs. (38), and therefore it will hold true when we use ${\displaystyle {\mathfrak {S}}_{1},{\mathfrak {S}}_{2},...{\mathfrak {S}}_{n}}$, as before, to denote the units of the various components. Thus understood, the equation expresses that the values of the quantities in the parentheses are such as are consistent with the equations of condition (41). The change in the system, therefore, which we are considering, is not one which violates any of the equations of condition, and as (45) does not hold true for this change, and for all values of ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$ which are consistent with eqs. (43), the state of the system cannot be one of equilibrium. Therefore it is necessary, and it is evidently sufficient for equilibrium, that it shall be possible to assign to ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$ such values, consistent with eqs. (43), that the condition (45) shall hold true for any change in the system irrespective of the equations of condition (39), (40), (41).

For this it is necessary and sufficient that

 ${\displaystyle t=T,\,\,\,p=P,}$ (50)
 ${\displaystyle \mu _{1}\delta m_{1}\geqq M_{1}\delta m_{1},\,\,\,\mu _{2}\delta m_{2}\geqq M_{2}\delta m_{2},\,...\,\,\mu _{n}\delta m_{n}\geqq M_{n}\delta m_{n}}$ (51)
for each of the original parts as previously defined, and that
 ${\displaystyle D\epsilon -TD\eta +PDv-M_{1}Dm_{1}-M_{2}Dm_{2}...-M_{n}Dm_{n}\geqq 0,}$ (52)
for each of the new parts as previously defined. If to these conditions we add equations (43), we may treat ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$ simply as unknown quantities to be eliminated.

In regard to conditions (51), it will be observed that if a substance ${\displaystyle S_{1}}$, is an actual component of the part of the given mass distinguished by a single accent, ${\displaystyle \delta m'_{1}}$ may be either positive or negative, and we shall have ${\displaystyle \mu _{1}'=M_{1}}$; but if ${\displaystyle S_{1}}$ is only a possible component of that part, ${\displaystyle \delta m'_{1}}$ will be incapable of a negative value, and we will have ${\displaystyle \mu _{1}'\geqq M_{1}}$.

The formulæ (50), (51), and (43) express the same particular conditions of equilibrium which we have before obtained by a less general process. It remains to discuss (52). This formula must hold true of any infinitesimal mass in the system in its varied state which is not approximately homogeneous with any of the surrounding masses, the expressions ${\displaystyle D\epsilon ,D\eta ,Dv,Dm_{1},Dm_{2},...Dm_{n}}$ denoting the energy, entropy, and volume of this infinitesimal mass, and the quantities of the substances ${\displaystyle S_{1},S_{2},...S_{n}}$ which we regard as comppsing it (not necessarily as independently variable components). If there is more than one way in which this mass may be considered as composed of these substances, we may choose whichever is most convenient. Indeed it follows directly from the relations existing between ${\displaystyle M_{1},M_{2},...}$ and ${\displaystyle M_{n}}$ that the result would be the same in any case. Now, if we assume that the values of ${\displaystyle D\epsilon ,D\eta ,Dv,Dm_{1},Dm_{2},...Dm_{n}}$ are proportional to the values of ${\displaystyle \epsilon ,\eta ,v,m_{1},m_{2},...m_{n}}$ for any large homogeneous mass of similar composition, and of the same temperature and pressure, the condition is equivalent to this, that

 ${\displaystyle \epsilon -T\eta +Pv-M_{1}m_{1}-M_{2}m_{2}...-M_{n}m_{n}\geqq 0,}$ (53)
for any large homogeneous body which can be formed out of the substances ${\displaystyle S_{1},S_{2},...S_{n}}$.

But the validity of this last transformation cannot be admitted without considerable limitation. It is assumed that the relation between the energy, entropy, volume, and the quantities of the different components of a very small mass surrounded by substances of different composition and state is the same as if the mass in question formed a part of a large homogeneous body. We started, indeed, with the assumption that we might neglect the part of the energy, etc., depending upon the surfaces separating heterogeneous masses. Now, in many cases, and for many purposes, as, in general, when the masses are large, such an assumption is quite legitimate, but in the case of these masses which are formed within or among substances of different nature or state, and which at their first formation must be infinitely small, the same assumption is evidently entirely inadmissible, as the surfaces must be regarded as infinitely large in proportion to the masses. We shall see hereafter what modifications are necessary in our formulæ in order to include the parts of the energy, etc., which are due to the surfaces, but this will be on the assumption, which is usual in the theory of capillarity, that the radius of curvature of the surfaces is large in proportion to the radius of sensible molecular action, and also to the thickness of the lamina of matter at the surface which is not (sensibly) homogeneous in all respects with either of the masses which it separates. But although the formulæ thus modified will apply with sensible accuracy to masses (occurring within masses of a different nature) much smaller than if the terms relating to the surfaces were omitted, yet their failure when applied to masses infinitely small in all their dimensions is not less absolute.

Considerations like the foregoing might render doubtful the validity even of (52) as the necessary and sufficient condition of equilibrium in regard to the formation of masses not approximately homogeneous with those previously existing, when the conditions of equilibrium between the latter are satisfied, unless it is shown that in establishing this formula there have been no quantities neglected relating to the mutual action of the new and the original parts, which can affect the result. It will be easy to give such a meaning to the expressions ${\displaystyle D\epsilon ,D\eta ,Dv,Dm_{1},Dm_{2},...Dm_{n}}$ that this shall be evidently the case. It will be observed that the quantities represented by these expressions have not been perfectly defined. In the first place, we have no right to assume the existence of any surface of absolute discontinuity to divide the new parts from the original, so that the position given to the dividing surface is to a certain extent arbitrary. Even if the surface separating the masses were determined, the energy to be attributed to the masses separated would be partly arbitrary, since a part of the total energy depends upon the mutual action of the two masses. We ought perhaps to consider the case the same in regard to the entropy, although the entropy of a system never depends upon the mutual relations of parts at sensible distances from one another. Now the condition (52) will be valid if the quantities ${\displaystyle D\epsilon ,D\eta ,Dv,Dm_{1},Dm_{2},...Dm_{n}}$ are so defined that none of the assumptions which have been made, tacitly or otherwise, relating to the formation of these new parts, shall be violated. These assumptions are the following: that the relation between the variations of the energy, entropy, volume, etc., of any of the original parts is not affected by the vicinity of the new parts; and that the energy, entropy, volume, etc., of the system in its varied state are correctly represented by the sums of the energies, entropies, volumes, etc., of the various parts (original and new), so far at least as any of these quantities are determined or affected by the formation of the new parts. We will suppose ${\displaystyle D\epsilon ,D\eta ,Dv,Dm_{1},Dm_{2},...Dm_{n}}$ to be so defined that these conditions shall not be violated. This may be done in various ways. We may suppose that the position of the surfaces separating the new and the original parts has been fixed in any suitable way. This will determine the space and the matter belonging to the parts separated. If this does not determine the division of the entropy, we may suppose this determined in any suitable arbitrary way. Thus we may suppose the total energy in and about any new part to be so distributed that equation (12) as applied to the original parts shall not be violated by the formation of the new parts. Or, it may seem more simple to suppose that the imaginary surface which divides any new part from the original is so placed as to include all the matter which is affected by the vicinity of the new formation, so that the part or parts which we regard as original may be left homogeneous in the strictest sense, including uniform densities of energy and entropy, up to the very bounding surface. The homogeneity of the new parts is of no consequence, as we have made no assumption in that respect. It may be doubtful whether we can consider the new parts, as thus bounded, to be infinitely small even in their earliest stages of development. But if they are not infinitely small, the only way in which this can affect the validity of our formulse will be that in virtue of the equations of condition, i.e., in virtue of the evident necessities of the case, finite variations of the energy, entropy, volume, etc., of the original parts will be caused, to which it might seem that equation (12) would not apply. But if the nature and state of the mass be not varied, equation (12) will hold true of finite differences. (This appears at once, if we integrate the equation under the above limitation.) Hence, the equation will hold true for finite differences, provided that the nature and state of the mass be infinitely little varied. For the differences may be considered as made up of two parts, of which the first are for a constant nature and state of the mass, and the second are infinitely small. We may therefore regard the new parts to be bounded as supposed without prejudice to the validity of any of our results.

The condition (52) understood in either of these ways (or in others which will suggest themselves to the reader) will have a perfectly definite meaning, and will be valid as the necessary and sufficient condition of equilibrium in regard to the formation of new parts, when the conditions of equilibrium in regard to the original parts, (50), (51), and (43), are satisfied.

In regard to the condition (53), it may be shown that with (50), (51), and (43) it is always sufficient for equilibrium. To prove this, it is only necessary to show that when (50), (51), and (43) are satisfied, and (52) is not, (53) will also not be satisfied. We will first observe that an expression of the form

 ${\displaystyle -\epsilon +T\eta -Pv+M_{1}m_{1}+M_{2}m_{2}...+M_{n}m_{n}}$ (54)
denotes the work obtainable by the formation (by a reversible process) of a body of which ${\displaystyle \epsilon ,\eta ,v,m_{1},m_{2},...m_{n}}$ are the energy, entropy, volume, and the quantities of the components, within a medium having the pressure ${\displaystyle P}$, the temperature ${\displaystyle T}$, and the potentials ${\displaystyle M_{1},M_{2},...M_{n}}$. (The medium is supposed so large that its properties are not sensibly altered in any part by the formation of the body.) For ${\displaystyle \epsilon }$ is the energy of the body formed, and the remaining terms represent (as may be seen by applying equation (12) to the medium) the decrease of the energy of the medium, if, after the formation of the body, the joint entropy of the medium and the body, their joint volumes and joint quantities of matter, were the same as the entropy, etc., of the medium before the formation of the body. This consideration may convince us that for any given finite values of ${\displaystyle v}$ and of ${\displaystyle T,P,M_{1}}$ , etc., this expression cannot be infinite when ${\displaystyle \epsilon ,\eta ,m_{1}}$, etc., are determined by any real body, whether homogeneous or not (but of the given volume), even when ${\displaystyle T,P,M_{1}}$, etc., do not represent the values of the temperature, pressure, and potentials of any real substance. (If the substances ${\displaystyle S_{1},S_{2},...S_{n}}$ are all actual components of any homogeneous part of the system of which the equilibrium is discussed, that part will afford an example of a body having the temperature, pressure, and potentials of the medium supposed.)

Now by integrating equation (12) on the supposition that the nature and state of the mass considered remain unchanged, we obtain the equation

 ${\displaystyle \epsilon =t\eta -pv+\mu _{1}m_{1}+\mu _{2}m_{2}...+\mu _{n}m_{n},}$ (55)
which will hold true of any homogeneous mass whatever. Therefore for any one of the original parts, by (50) and (51),
 ${\displaystyle \epsilon -T\eta +Pv-M_{1}m_{1}-M_{1}m_{2}...+M_{n}m_{n}=0.}$ (56)
If the condition (52) is not satisfied in regard to all possible new parts, let ${\displaystyle N}$ be a new part occurring in an original part ${\displaystyle O}$, for which the condition is not satisfied. It is evident that the value of the expression
 ${\displaystyle \epsilon -T\eta +Pv-M_{1}m_{1}-M_{2}m_{2}...-M_{n}m_{n}}$ (57)
applied to a mass like ${\displaystyle O}$ including some very small masses like ${\displaystyle N}$, will be negative, and will decrease if the number of these masses like ${\displaystyle N}$ is increased, until there remains within the whole mass no portion of any sensible size without these masses like ${\displaystyle N}$, which, it will be remembered, have no sensible size. But it cannot decrease without limit, as the value of (54) cannot become infinite. Now we need not inquire whether the least value of (57) (for constant values of ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$) would be obtained by excluding entirely the mass like ${\displaystyle O}$, and filling the whole space considered with masses like ${\displaystyle N}$, or whether a certain mixture would give a smaller value,—it is certain that the least possible value of (57) per unit of volume, and that a negative value, will be realized by a mass having a certain homogeneity. If the new part ${\displaystyle N}$ for which the condition (52) is not satisfied occurs between two different original parts ${\displaystyle O'}$ and ${\displaystyle O''}$, the argument need not be essentially varied. We may consider the value of (57) for a body consisting of masses like ${\displaystyle O'}$ and ${\displaystyle O''}$ separated by a lamina ${\displaystyle N}$. This value may be decreased by increasing the extent of this lamina, which may be done within a given volume by giving it a convoluted form; and it will be evident, as before, that the least possible value of (57) will be for a homogeneous mass, and that the value will be negative. And such a mass will be not merely an ideal combination, but a body capable of existing, for as the expression (57) has for this mass in the state considered its least possible value per unit of volume, the energy of the mass included in a unit of volume is the least possible for the same matter with the same entropy and volume, hence, if confined in a non-conducting vessel, it will be in a state of not unstable equilibrium. Therefore when (50), (51), and (43) are satisfied, if the condition (52) is not satisfied in regard to all possible new parts, there will be some homogeneous body which can be formed out of the substances ${\displaystyle S_{1},S_{2},...S_{n}}$ which will not satisfy condition (53).

Therefore, if the initially existing masses satisfy the conditions (50), (51), and (43), and condition (53) is satisfied by every homogeneous body which can be formed out of the given matter, there will be equilibrium.

On the other hand, (53) is not a necessary condition of equilibrium. For we may easily conceive that the condition (52) shall hold true (for any very small formations within or between any of the given masses), while the condition (53) is not satisfied (for all large masses formed of the given matter), and experience shows that this is very often the case. Supersaturated solutions, superheated water, etc. are familiar examples. Such an equilibrium will, however, be practically unstable. By this is meant that, although, strictly speaking, an infinitely small disturbance or change may not be sufficient to destroy the equilibrium, yet a very small change in the initial state, perhaps a circumstance which entirely escapes our powers of perception, will be sufficient to do so. The presence of a small portion of the substance for which the condition (53) does not hold true, is sufficient to produce this result, when this substance forms a variable component of the original homogeneous masses. In other cases, when, if the new substances are formed at all, different kinds must be formed simultaneously, the initial presence of the different kinds, and that in immediate proximity, may be necessary.

It will be observed, that from (56) and (53) we can at once obtain (50) and (51), viz., by applying (53) to bodies differing infinitely little from the various homogeneous parts of the given mass. Therefore, the condition (56) (relating to the various homogeneous parts of the given mass) and (53) (relating to any bodies which can be formed of the given matter) with (43) are always sufficient for equilibrium, and always necessary for an equilibrium which shall be practically stable. And, if we choose, we may get rid of limitation in regard to equations (43). For, if we compare these equations with (38), it is easy to see that it is always immaterial, in applying the tests (56) and (53) to any body, how we consider it to be composed. Hence, in applying these tests, we may consider all bodies to be composed of the ultimate components of the given mass. Then the terms in (56) and (53) which relate to other components than these will vanish, and we need not regard the equations (43). Such of the constants ${\displaystyle M_{1},M_{2},...M_{n}}$ as relate to the ultimate components, may be regarded, like T and P, as unknown quantities subject only to the conditions (56) and (53).

These two conditions, which are sufficient for equilibrium and necessary for a practically stable equilibrium, may be united in one, viz. (if we choose the ultimate components of the given mass for the component substances to which ${\displaystyle m_{1},m_{2},...m_{n}}$ relate), that it shall be possible to give such values to the constants ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$ in the expression (57) that the value of the expression for each of the homogeneous parts of the mass in question shall be as small as for any body whatever made of the same components.

Effect of Solidity of any Part of the given Mass.

If any of the homogeneous masses of which the equilibrium is in question are solid, it will evidently be proper to treat the proportion of their components as invariable in the application of the criterion of equilibrium, even in the case of compounds of variable proportions, i.e., even when bodies can exist which are compounded in proportions infinitesimally varied from those of the solids considered. (Those solids which are capable of absorbing fluids form of course an exception, so far as their fluid components are concerned.) It is true that a solid may be increased by the formation of new solid matter on the surface where it meets a fluid, which is not homogeneous with the previously existing solid, but such a deposit will properly be treated as a distinct part of the system (viz., as one of the parts which we have called new). Yet it is worthy of notice that if a homogeneous solid which is a compound of variable proportions is in contact and equilibrium with a fluid, and the actual components of the solid (considered as of variable composition) are also actual components of the fluid, and the condition (53) is satisfied in regard to all bodies which can be formed out of the actual components of the fluid (which will always be the case unless the fluid is practically unstable), all the conditions will hold true of the solid, which would be necessary for equilibrium if it were fluid.

This follows directly from the principles stated on the preceding pages. For in this case the value of (57) will be zero as determined either for the solid or for the fluid considered with reference to their ultimate components, and will not be negative for any body whatever which can be formed of these components; and these conditions are sufficient for equilibrium independently of the solidity of one of the masses. Yet the point is perhaps of sufficient importance to demand a more detailed consideration.

Let ${\displaystyle S_{a},...S_{g}}$ be the actual components of the solid, and ${\displaystyle S_{h},...S_{k}}$ its possible components (which occur as actual components in the fluid); then, considering the proportion of the components of the solid as variable, we shall have for this body by equation (12)

 ${\displaystyle d\epsilon '=t'd\eta '-p'dv'+\mu _{a}'dm'_{a}...+\mu _{g}'dm'_{g}+\mu _{h}'dm'_{h}...+\mu _{k}'dm'_{k}.}$ (58)
By this equation the potentials ${\displaystyle \mu _{a}',...\mu _{k}'}$ are perfectly defined. But the differentials dm ${\displaystyle dm'_{a},...dm'_{k}}$, considered as independent, evidently express variations which are not possible in the sense required in the criterion of equilibrium. We might, however, introduce them into the general condition of equilibrium, if we should express the dependence between them by the proper equations of condition. But it will be more in accordance with our method hitherto, if we consider the solid to have only a single independently variable component ${\displaystyle S_{x}}$ of which the nature is represented by the solid itself. We may then write
 ${\displaystyle \delta \epsilon '=t'\delta \eta '-p'\delta v'+\mu '\delta m'_{x}.}$ (59)

In regard to the relation of the potential ${\displaystyle \mu _{x}'}$ to the potentials occurring in equation (58) it will be observed, that as we have by integration of (58) and (59)

 ${\displaystyle \epsilon '=t'\eta '-p'v'+\mu _{a}'m'_{a}...+\mu _{g}'m'_{g},}$ (60)
 ${\displaystyle \epsilon '=t'\eta '-p'v'+\mu _{x}'m'_{x},}$ (61)
 therefore ${\displaystyle \mu _{x}'m'_{x}=\mu _{a}'m'_{a}...+\mu _{g}'m'_{g}.}$ (62)
Now, if the fluid has besides ${\displaystyle S_{a},...S_{g}}$ and ${\displaystyle S_{h},...S_{k}}$ the actual components ${\displaystyle S_{l},...S_{n}}$, we may write for the fluid
 ${\displaystyle \delta \epsilon ''=t''\delta \eta ''-p''\delta v''+\mu _{a}''m''_{a}...+\mu _{g}''m''_{g}+\mu _{h}''m''_{h}...\mu _{k}''m''_{k}+\mu _{l}''m''_{l}...+\mu _{n}''m''_{n}}$ (63)
and as by supposition
 ${\displaystyle m'_{x}{\mathfrak {S}}_{x}=m'_{a}{\mathfrak {S}}_{a}...+m'_{g}{\mathfrak {S}}_{g}}$ (64)
equations (43), (50), and (51) will give in this case on elimination of the constants ${\displaystyle T,P}$, etc.,
 ${\displaystyle t'=t'',\,\,p'=p'',}$ (65)
 ${\displaystyle m'_{x}\mu _{x}'=m'_{a}\mu _{a}''...+m'_{g}\mu _{g}''.}$ (66)
Equations (65) and (66) may be regarded as expressing the conditions of equilibrium between the solid and the fluid. The last condition may also, in virtue of (62), be expressed by the equation
 ${\displaystyle m'_{a}\mu _{a}'...+m'_{g}\mu _{g}'=m'_{a}\mu _{a}''...+m'_{g}\mu _{g}''.}$ (67)
But if condition (53) holds true of all bodies which can be formed of ${\displaystyle S_{a},...S_{g},S_{h},...S_{k},S_{h}...S_{n}}$ , we may write for all such bodies
 ${\displaystyle \epsilon -t''\eta +p''v-\mu _{a}''m_{a}...-\mu _{g}''m_{g}-\mu _{h}''m_{h}...-\mu _{k}''m_{k}-\mu _{l}''m_{l}...-\mu _{l}''m_{l}\geqq 0.}$ (68)
(In applying this formula to various bodies, it is to be observed that only the values of the unaccented letters are to be determined by the different bodies to which it is applied, the values of the accented letters being already determined by the given fluid.) Now, by (60), (65), and (67), the value of the first member of this condition is zero when applied to the solid in its given state. As the condition must hold true of a body differing infinitesimally from the solid, we shall have
 ${\displaystyle d\epsilon '-t''d\eta '+p''dv'-\mu _{a}''dm'_{a}...-\mu _{g}''dm'_{g}-\mu _{h}''dm'_{h}...-\mu _{k}''dm'_{k}\geqq 0,}$ (69)
or, by equations (58) and (65),
 ${\displaystyle (\mu _{a}'-\mu _{a}'')dm'_{a}...+(\mu _{g}'\mu _{g}'')dm'_{g}+(\mu _{h}'-\mu _{h}'')dm'_{h}...+(\mu _{k}'-\mu _{k}'')dm'_{k}\geqq 0.}$ (70)
Therefore, as these differentials are all independent,
 ${\displaystyle \mu _{a}'=\mu _{a}'',...\mu _{g}'=\mu _{g}'',\mu _{h}'\geqq \mu _{h}'',...\mu _{k}'\geqq \mu _{k}'';}$ (71)

which with (65) are evidently the same conditions which we would have obtained if we had neglected the fact of the solidity of one of the masses.

We have supposed the solid to be homogeneous. But it is evident that in any case the above conditions must hold for every separate point where the solid meets the fluid. Hence, the temperature and pressure and the potentials for all the actual components of the solid must have a constant value in the solid at the surface where it meets the fluid. Now, these quantities are determined by the nature and state of the solid, and exceed in number the independent variations of which its nature and state are capable. Hence, if we reject as improbable the supposition that the nature or state of a body can vary without affecting the value of any of these quantities, we may conclude that a solid which varies (continuously) in nature or state at its surface cannot be in equilibrium with a stable fluid which contains, as independently variable components, the variable components of the solid. (There may be, however, in equilibrium with the same stable fluid, a finite number of different solid bodies, composed of the variable components of the fluid, and having their nature and state completely determined by the fluid.)[5]

Effect of Additional Equations of Condition.

As the equations of condition, of which we have made use, are such as always apply to matter enclosed in a rigid, impermeable, and non-conducting envelop, the particular conditions of equilibrium which we have found will always be sufficient for equilibrium. But the number of conditions necessary for equilibrium, will be diminished, in a case otherwise the same, as the number of equations of condition is increased. Yet the problem of equilibrium which has been treated will sufficiently indicate the method to be pursued in all cases and the general nature of the results.

It will be observed that the position of the various homogeneous parts of the given mass, which is otherwise immaterial, may determine the existence of certain equations of condition. Thus, when different parts of the system in which a certain substance is a variable component are entirely separated from one another by parts of which this substance is not a component, the quantity of this substance will be invariable for each of the parts of the system which are thus separated, which will be easily expressed by equations of condition. Other equations of condition may arise from the passive forces (or resistances to change) inherent in the given masses. In the problem which we are next to consider there are equations of condition due to a cause of a different nature.

Effect of a Diaphragm (Equilibrium of Osmotic Forces).

If the given mass, enclosed as before, is divided into two parts, each of which is homogeneous and fluid, by a diaphragm which is capable of supporting an excess of pressure on either side, and is permeable to some of the components and impermeable to others, we shall have the equations of condition

 ${\displaystyle \delta \eta '+\delta \eta ''=0,}$ (72)
 ${\displaystyle \delta v'=0,\,\,\,\delta v''=0,}$ (73)
and for the components which cannot pass the diaphragm
 ${\displaystyle \delta m'_{a}=0,\,\,\,\delta m''_{a}=0,\,\,\,\delta m'_{b}=0,\,\,\,\delta m''_{b}=0,\,\,etc.,}$ (74)
and for those which can
 ${\displaystyle \delta m'_{k}+\delta m''_{k}=0,\,\,\,\delta m'_{l}+\delta m''_{l}=0,\,\,etc.}$ (75)
With these equations of condition, the general condition of equilibrium (see (15)) will give the following particular conditions:—
 ${\displaystyle t'=t'',}$ (76)
and for the components which can pass the diaphragm, if actual components of both masses,
 ${\displaystyle \mu _{k}'=\mu _{k}'',\,\,\,\mu _{l}'=\mu _{l}''\,\,\,etc.,}$ (77)
 but not ${\displaystyle p'=p''}$
 nor ${\displaystyle \mu _{a}'=\mu _{a}'',\,\,\,\mu _{b}'=\mu _{b}'',\,\,etc.}$
Again, if the diaphragm is permeable to the components in certain proportions only, or in proportions not entirely determined yet subject to certain conditions, these conditions may be expressed by equations of condition, which will be linear equations between ${\displaystyle \delta m'_{1},\delta m'_{2}}$, etc., and if these be known the deduction of the particular conditions of equilibrium will present no difficulties. We will however observe that if the components ${\displaystyle S_{1},S_{2}}$, etc. (being actual components on each side) can pass the diaphragm simultaneously in the proportions ${\displaystyle a_{1},a_{2}}$, etc. (without other resistances than such as vanish with the velocity of the current), values proportional to ${\displaystyle a_{1},a_{2}}$, etc. are possible for ${\displaystyle \delta m'_{1},\delta m'_{2}}$, etc. in the general condition of equilibrium, ${\displaystyle \delta m''_{1},\delta m''_{2}}$, etc.,

having the same values taken negatively, so that we shall have for one particular condition of equilibrium

 ${\displaystyle a_{1}\mu _{1}'+a_{2}\mu _{2}'+etc.=a_{1}\mu _{1}''+a_{2}\mu _{2}''+etc.}$ (78)
There will evidently be as many independent equations of this form as there are independent combinations of the elements which can pass the diaphragm.

These conditions of equilibrium do not of course depend in any way upon the supposition that the volume of each fluid mass is kept constant, if the diaphragm is in any case supposed immovable. In fact, we may easily obtain the same conditions of equilibrium, if we suppose the volumes variable. In this case, as the equilibrium must be preserved by forces acting upon the external surfaces of the fluids, the variation of the energy of the sources of these forces must appear in the general condition of equilibrium, which will be

 ${\displaystyle \delta \epsilon '+\delta \epsilon ''+P'\delta v'+P''\delta v''\geqq 0,}$ (79)
${\displaystyle P}$ and ${\displaystyle P''}$ denoting the external forces per unit of area. (Compare (14).) From this condition we may evidently derive the same internal conditions of equilibrium as before, and in addition the external conditions
 ${\displaystyle p'=P',\,\,\,p''=P''.}$ (80)
In the preceding paragraphs it is assumed that the permeability of the diaphragm is perfect, and its impermeability absolute, i.e., that it offers no resistance to the passage of the components of the fluids in certain proportions, except such as vanishes with the velocity, and that in other proportions the components cannot pass at all. How far these conditions are satisfied in any particular case is of course to be determined by experiment.

If the diaphragm is permeable to all the ${\displaystyle n}$ components without restriction, the temperature and the potentials for all the components must be the same on both sides. Now, as one may easily convince himself, a mass having ${\displaystyle n}$ components is capable of only ${\displaystyle n+1}$ independent variations in nature and state. Hence, if the fluid on one side of the diaphragm remains without change, that on the other side cannot (in general) vary in nature or state. Yet the pressure will not necessarily be the same on both sides. For, although the pressure is a function of the temperature and the n potentials, it may be a many-valued function (or any one of several functions) of these variables. But when the pressures are different on the two sides, the fluid which has the less pressure will be practically unstable, in the sense in which the term has been used on page 79. For

 ${\displaystyle \epsilon ''-t''\eta ''+p''v''-\mu _{1}''m''_{1}-\mu _{2}''m''_{2}...-\mu _{n}''m''_{n}=0,}$ (81)
as appears from equation (12) if integrated on the supposition that the nature and state of the mass remain unchanged. Therefore, if ${\displaystyle p' while ${\displaystyle t'=t'',\,\mu _{1}'=\mu _{1}''}$, etc.,
 ${\displaystyle \epsilon ''-t''\eta ''+p''v''-\mu _{1}''m''_{1}-\mu _{2}''m''_{2}...-\mu _{n}''m''_{n}<0.}$ (82)
This relation indicates the instability of the fluid to which the single accents refer. (See page 79.)

But independently of any assumption in regard to the permeability of the diaphragm, the following relation will hold true in any case in which each of the two fluid masses may be regarded as uniform throughout in nature and state. Let the character ${\displaystyle {\scriptstyle {\text{D}}}}$ be used with the variables which express the nature, state, and quantity of the fluids to denote the increments of the values of these quantities actually occurring in a time either finite or infinitesimal. Then, as the heat received by the two masses cannot exceed ${\displaystyle t'{\scriptstyle {\text{D}}}\eta '+t''{\scriptstyle {\text{D}}}\eta ''}$, and as the increase of their energy is equal to the difference of the heat they receive and the work they do,

 ${\displaystyle {\scriptstyle {\text{D}}}\epsilon '+{\scriptstyle {\text{D}}}\epsilon ''\leqq t'{\scriptstyle {\text{D}}}\eta '+t''{\scriptstyle {\text{D}}}\eta ''-p'{\scriptstyle {\text{D}}}v'-p''{\scriptstyle {\text{D}}}v''}$ (83)
i.e., by (12),
 ${\displaystyle \mu _{1}'{\scriptstyle {\text{D}}}m'_{1}+\mu _{1}''{\scriptstyle {\text{D}}}m''_{1}+\mu _{2}'{\scriptstyle {\text{D}}}m'_{2}+\mu _{2}''{\scriptstyle {\text{D}}}m''_{2}+\,{\text{etc.}}\,\leqq 0,}$ (84)
or
 ${\displaystyle (\mu _{1}''-\mu _{1}'){\scriptstyle {\text{D}}}m''_{1}+(\mu _{2}''-\mu _{2}'){\scriptstyle {\text{D}}}m''_{2}+\,{\text{etc.}}\,\leqq 0.}$ (85)
It is evident that the sign ${\displaystyle =}$ holds true only in the limiting case in which no motion takes place.

Definition and Properties of Fundamental Equations.

The solution of the problems of equilibrium which we have been considering has been made to depend upon the equations which express the relations between the energy, entropy, volume, and the quantities of the various components, for homogeneous combinations of the substances which are found in the given mass. The nature of such equations must be determined by experiment. As, however, it is only differences of energy and of entropy that can be measured, or indeed, that have a physical meaning, the values of these quantities are so far arbitrary, that we may choose independently for each simple substance the state in which its energy and its entropy are both zero. The values of the energy and the entropy of any compound body in any particular state will then be fixed. Its energy will be the sum of the work and heat expended in bringing its components from the states in which their energies and their entropies are zero into combination and to the state in question; and its entropy is the value of the integral ${\displaystyle \int {\frac {dQ}{T}}}$ for any reversible process by which that change is effected (${\displaystyle dQ}$ denoting an element of the heat communicated to the matter thus treated, and ${\displaystyle t}$ the temperature of the matter receiving it). In the determination both of the energy and of the entropy, it ia understood that at the close of the process, all bodies which have been used, other than those to which the determinations relate, have been restored to their original state, with the exception of the sources of the work and heat expended, which must be used only as such sources.

We know, however, a priori, that if the quantity of any homogeneous mass containing ${\displaystyle n}$ independently variable components varies and not its nature or state, the quantities ${\displaystyle \epsilon ,\eta ,v,m_{1},m_{2},...m_{n}}$ will all vary in the same proportion; therefore it is sufficient if we learn from experiment the relation between all but any one of these quantities for a given constant value of that one. Or, we may consider that we have to learn from experiment the relation subsisting between the ${\displaystyle n+2}$ ratios of the ${\displaystyle n+3}$ quantities ${\displaystyle \epsilon ,\eta ,v,m_{1},m_{2},...m_{n}}$. To fix our ideas we may take for these ratios ${\displaystyle {\frac {\epsilon }{v}},{\frac {\eta }{v}},{\frac {m_{1}}{v}},{\frac {m_{2}}{v}},...{\frac {m_{n}}{v}}}$, etc., that is, the separate densities of the components, and the ratios ${\displaystyle {\frac {\epsilon }{v}}}$ and ${\displaystyle {\frac {\eta }{v}}}$, which may be called the densities of energy and entropy. But when there is but one component, it may be more convenient to choose ${\displaystyle {\frac {\epsilon }{m}},{\frac {\eta }{m}},{\frac {v}{m}}}$, as the three variables. In any case, it is only a function of ${\displaystyle n+1}$ independent variables, of which the form is to be determined by experiment.

Now if ${\displaystyle \epsilon }$ is a known function of ${\displaystyle \eta ,v,m_{1},m_{2},...m_{n}}$, as by equation (12)

 ${\displaystyle d\epsilon =td\eta -pdv+\mu _{1}m_{1}+\mu _{2}m_{2},...+\mu _{n}m_{n},}$ (86)
${\displaystyle \epsilon ,\eta ,v,m_{1},m_{2},...m_{n}}$ ${\displaystyle t,p,\mu _{1},\mu _{2},...\mu _{n}}$ are functions of the same variables, which may be derived from the original function by differentiation, and may therefore be considered as known functions. This will make ${\displaystyle n+3}$ independent known relations between the ${\displaystyle 2n+5}$ variables, ${\displaystyle \epsilon ,\eta ,v,m_{1},m_{2},...m_{n},t,p,\mu _{1},\mu _{2},...\mu _{n}}$. These are all that exist, for of these variables, ${\displaystyle n+2}$ are evidently independent. Now upon these relations depend a very large class of the properties of the compound considered,—we may say in general, all its thermal, mechanical, and chemical properties, so far as active tendencies are concerned, in cases in which the form of the mass does not require consideration. A single equation from which all these relations may be deduced we will call a fundamental equation for the substance in question. We shall hereafter consider a more general form of the fundamental equation for solids, in which the pressure at any point is not supposed to be the same in all directions. But for masses subject only to isotropic stresses an equation between ${\displaystyle \epsilon ,\eta ,v,m_{1},m_{2},...m_{n}}$ is a fundamental equation. There are other equations which possess this same property.[6]

Let
${\displaystyle \psi =\epsilon -t\eta }$
(87)
then by differentiation and comparision with (86) we obtain
 ${\displaystyle d\psi =-\eta dt-pdv+\mu _{1}dm_{1}+\mu _{2}dm_{2}...+\mu _{n}dm_{n}.}$ (88)
If, then, ${\displaystyle \psi }$ is known as a function of ${\displaystyle t,v,m_{1},m_{2},...m_{n}}$ we can find ${\displaystyle \eta ,p,\mu _{1},\mu _{2},...\mu _{n}}$ in terms of the same variables. If we then substitute for ${\displaystyle \psi }$ in our original equation its value taken from eq. (87), we shall have again ${\displaystyle n+3}$ independent relations between the same ${\displaystyle 2n+5}$ variables as before.
Let
${\displaystyle \chi =\epsilon +pv,}$
(89)
then by (86),
 ${\displaystyle d\chi =td\eta +vdp+\mu _{1}dm_{1}+\mu _{2}dm_{2}...+\mu _{n}dm_{n}.}$ (90)
If, then, ${\displaystyle \chi }$ be known as a function of ${\displaystyle \eta ,p,m_{1},m_{2},...m_{n}}$, we can find ${\displaystyle t,v,\mu _{1},\mu _{2},...\mu _{n}}$ in terms of the same variables. By eliminating ${\displaystyle \chi }$, we may obtain again ${\displaystyle n+3}$ independent relations between the same ${\displaystyle 2n+5}$ variables as at first.
Let
${\displaystyle \zeta =\epsilon -t\eta +pv,}$
(91)
then, by (86),
 ${\displaystyle d\zeta =-\eta dt+vdp+\mu _{1}dm_{1}+\mu _{2}dm_{2}...+\mu _{n}dm_{n}.}$ (92)
If, then, ${\displaystyle \zeta }$ is known as a function of ${\displaystyle t,p,m_{1},m_{2},...m_{n}}$, we can find ${\displaystyle \eta ,v,\mu _{1},\mu _{2},...\mu _{n}}$ in terms of the same variables. By eliminating ${\displaystyle \zeta }$, we may obtain again ${\displaystyle n+3}$ independent relations between the same ${\displaystyle 2n+5}$ variables as at first.

If we integrate (86), supposing the quantity of the compound substance considered to vary from zero to any finite value, its nature and state remaining unchanged, we obtain

 ${\displaystyle \epsilon =t\eta -pv+\mu _{1}m_{1}+\mu _{2}m_{2}...+\mu _{n}m_{n},}$ (93)
and by (87), (89), (91)
 ${\displaystyle \psi =-pv+\mu _{1}m_{1}+\mu _{2}m_{2}...+\mu _{n}m_{n},}$ (94)
 ${\displaystyle \chi =t\eta +\mu _{1}m_{1}+\mu _{2}m_{2}...+\mu _{n}m_{n},}$ (95)
 ${\displaystyle \zeta =\mu _{1}m_{1}+\mu _{2}m_{2}...+\mu _{n}m_{n},}$ (96)
The last three equations may also be obtained directly by integrating (88), (90), and (92).

If we differentiate (93) in the most general manner, and compare the result with (86), we obtain

 ${\displaystyle -vdp+\eta dt+m_{1}d\mu _{1}+m_{2}d\mu _{2}...+m_{n}d\mu _{n}=0,}$ (97)
 or⁠${\displaystyle dp={\frac {\eta }{v}}dt+{\frac {m_{1}}{v}}d\mu _{1}+{\frac {m_{2}}{v}}d\mu _{2}...+{\frac {m_{n}}{v}}d\mu _{n}\cdot }$ (98)
Hence, there is a relation between the ${\displaystyle n+2}$ quantities ${\displaystyle t,p,\mu _{1},\mu _{2},...\mu _{n}}$, which, if known, will enable us to find in terms of these quantities all the ratios of the ${\displaystyle n+2}$ quantities ${\displaystyle \eta ,v,m_{1},m_{2},...m_{n}}$. With (93), this will make ${\displaystyle n+3}$ independent relations between the same ${\displaystyle 2n+5}$ variables as at first.

Any equation, therefore, between the quantities

 ⁠${\displaystyle \epsilon ,}$⁠${\displaystyle \eta ,}$⁠${\displaystyle v,}$⁠${\displaystyle m_{1},}$⁠${\displaystyle m_{2},...m_{n},}$ (99)
 or⁠${\displaystyle \psi ,}$⁠${\displaystyle t,}$⁠${\displaystyle v,}$⁠${\displaystyle m_{1},}$⁠${\displaystyle m_{2},...m_{n},}$ (100)
 or⁠${\displaystyle \chi ,}$⁠${\displaystyle \eta ,}$⁠${\displaystyle p,}$⁠${\displaystyle m_{1},}$⁠${\displaystyle m_{2},...m_{n},}$ (101)
 or⁠${\displaystyle \zeta ,}$⁠${\displaystyle t,}$⁠${\displaystyle p,}$⁠${\displaystyle m_{1},}$⁠${\displaystyle m_{2},...m_{n},}$ (102)
 or⁠${\displaystyle t,}$⁠${\displaystyle p,}$⁠${\displaystyle \mu _{1},}$⁠${\displaystyle \mu _{2},...\mu _{n},}$ (103)
is a fundamental equation, and any such is entirely equivalent to any other.[7] For any homogeneous mass whatever, considered (in general) as variable in composition, in quantity, and in thermodynamic state, and having ${\displaystyle n}$ independently variable components, to which the subscript numerals refer (but not excluding the case in which ${\displaystyle n=1}$ and the composition of the body is invariable), there is a relation between the quantities enumerated in any one of the above sets, from which, if known, with the aid only of general principles and relations, we may deduce all the relations subsisting for such a mass between the quantities ${\displaystyle \epsilon ,\psi ,\chi ,\zeta ,\eta ,m_{1},m_{2},...m_{n},t,p,\mu _{1},\mu _{2},\mu _{n}}$. It will be observed that, besides the equations which define ${\displaystyle \psi ,\chi }$, and ${\displaystyle \zeta }$, there is one finite equation, (93), which subsists between these quantities independently of the form of the fundamental equation.

Other sets of quantities might of course be added which possess the same property. The sets (100), (101), (102) are mentioned on account of the important properties of the quanties ${\displaystyle \psi ,\chi ,\zeta }$, and because the equations (88), (90), (92), like (86), afford convenient definitions of the potentials, viz.,

 ${\displaystyle \mu _{1}=\left({\frac {d\epsilon }{dm_{1}}}\right)_{\eta ,v,m}=\left({\frac {d\psi }{dm_{1}}}\right)_{t,v,m}=\left({\frac {d\chi }{dm_{1}}}\right)_{\eta ,p,m}=\left({\frac {d\zeta }{dm_{1}}}\right)_{t,p,m}}$ (104)
etc., where the subscript letters denote the quantities which remain constant in the differentiation, m being written for brevity for all the letters ${\displaystyle m_{1},m_{2},...m_{n}}$ except the one occurring in the denominator. It will be observed that the quantities in (103) are all independent of the quantity of the mass considered, and are those which must, in general, have the same value in contiguous masses in equilibrium.

On the quantities ${\displaystyle \psi ,\chi ,\zeta }$.

The quantity ${\displaystyle \psi }$ has been defined for any homogeneous mass by the equation

 ${\displaystyle \psi =\epsilon -t\eta .}$ (105)
We may extend this definition to any material system whatever which has a uniform temperature throughout.

If we compare two states of the system of the same temperature, we have

 ${\displaystyle \psi '-\psi ''=\epsilon '-\epsilon ''-t(\eta '-\eta '').}$ (106)
If we suppose the system brought from the first to the second of these states without change of temperature and by a reversible process in which ${\displaystyle W}$ is the work done and ${\displaystyle Q}$ the heat received by the system, then
 ${\displaystyle \epsilon '-\epsilon ''=W-Q,}$ (107)
 and⁠${\displaystyle t(\eta '-\eta '')=0.}$ (108)
 Hence⁠ (109)
and for an infinitely small reversible change in the state of the system, in which the temperature remains constant, we may write
 ${\displaystyle -d\psi =dW.}$ (110)
Therefore, ${\displaystyle -\psi }$ is the force function of the system for constant temperature, just as ${\displaystyle -\epsilon }$ is the force function for constant entropy. That is, if we consider ${\displaystyle \psi }$ as a function of the temperature and the variables which express the distribution of the matter in space, for every different value of the temperature ${\displaystyle -\psi }$ is the different force function required by the system if maintained at that special temperature.

From this we may conclude that when a system has a uniform temperature throughout, the additional conditions which are necessary and sufficient for equilibrium may be expressed by

 ${\displaystyle (\delta \psi )_{t}\geqq 0.}$[8] (111)

When it is not possible to bring the system from one to the other of the states to which ${\displaystyle \psi '}$ and ${\displaystyle \psi ''}$ relate by a reversible process without altering the temperature, it will be observed that it is not necessary for the validity of (107)-(109) that the temperature of the system should remain constant during the reversible process to which ${\displaystyle W}$ and ${\displaystyle Q}$ relate, provided that the only source of heat or cold used has the same temperature as the system in its initial or final state. Any external bodies may be used in the process in any way not affecting the condition of reversibility, if restored to their original condition at the close of the process; nor does the limitation in regard to the use of heat apply to such heat as may be restored to the source from which it has been taken.

It may be interesting to show directly the equivalence of the conditions (111) and (2) when applied to a system of which the temperature in the given state is uniform throughout.

If there are any variations in the state of such a system which do not satisfy (2), then for these variations

 ${\displaystyle \delta \epsilon <0\,\,{\text{and}}\,\,\delta \eta =0.}$
If the temperature of the system in its varied state is not uniform, we may evidently increase its entropy without altering its energy by supposing heat to pass from the warmer to the cooler parts. And the state having the greatest entropy for the energy ${\displaystyle \epsilon +\delta \epsilon }$ will necessarily be a state of uniform temperature. For this state (regarded as a variation from the original state)
 ${\displaystyle \delta \epsilon <0\,\,{\text{and}}\,\,\delta \eta >0.}$
Hence, as we may diminish both the energy and the entropy by cooling the system, there must be a state of uniform temperature for which (regarded as a variation of the original state)
 ${\displaystyle \delta \epsilon <0\,\,{\text{and}}\,\,\delta \eta =0.}$
From this we may conclude that for systems of initially uniform temperature condition (2) will not be altered if we limit the variations to such as do not disturb the uniformity of temperature.

Confining our attention, then, to states of uniform temperature, we have by differentiation of (105)

 ${\displaystyle \delta \epsilon -t\delta \eta =\delta \psi +\eta \delta t.}$ (112)
Now there are evidently changes in the system (produced by heating or cooling) for which
 ${\displaystyle \delta \epsilon -t\delta \eta =0\,\,{\text{and therefore}}\,\,\delta \psi +\eta \delta t=0,}$ (113)
neither ${\displaystyle \delta \eta }$ nor ${\displaystyle \delta t}$ having the value zero. This consideration is sufficient to show that the condition (2) is equivalent to
 ${\displaystyle \delta \epsilon -t\delta \eta \geqq 0,}$ (114)
and that the condition (111) is equivalent to
 ${\displaystyle \delta \psi +\eta \delta t\geqq 0,}$ (115)
and by (112) the two last conditions are equivalent.

In such cases as we have considered on pages 62-82, in which the form and position of the masses of which the system is composed are immaterial, uniformity of temperature and pressure are always necessary for equilibrium, and the remaining conditions, when these are satisfied, may be conveniently expressed by means of the function ${\displaystyle \zeta }$, which has been defined for a homogeneous mass on page 87, and which we will here define for any mass of uniform temperature and pressure by the same equation

 ${\displaystyle \zeta =\epsilon -t\eta +pv.}$ (116)
For such a mass, the condition of (internal) equilibrium is
 ${\displaystyle (\delta \zeta )_{t,p}\geqq 0.}$ (117)
That this condition is equivalent to (2) will easily appear from considerations like those used in respect to (111).

Hence, it is necessary for the equilibrium of two contiguous masses identical in composition that the values of ${\displaystyle \zeta }$ as determined for equal quantities of the two masses should be equal. Or, when one of three contiguous masses can be formed out of the other two, it is necessary for equilibrium that the value of ${\displaystyle \zeta }$ for any quantity of the first mass should be equal to the sum of the values of ${\displaystyle \zeta }$ for such quantities of the second and third masses as together contain the same matter. Thus, for the equilibrium of a solution composed of ${\displaystyle a}$ parts of water and ${\displaystyle b}$ parts of a salt which is in contact with vapor of water and crystals of the salt, it is necessary that the value of ${\displaystyle \zeta }$ for the quantity ${\displaystyle a+b}$ of the solution should be equal to the sum of the values of ${\displaystyle \zeta }$ for the quantities a of the vapor and 6 of the salt. Similar propositions will hold true in more complicated cases. The reader will easily deduce these conditions from the particular conditions of equilibrium given on page 74.

In like manner we may extend the definition of ${\displaystyle \chi }$ to any mass or combination of masses in which the pressure is everywhere the same, using ${\displaystyle \epsilon }$ for the energy and ${\displaystyle v}$ for the volume of the whole and setting as before

 ${\displaystyle \chi =\epsilon +pv.}$ (118)
If we denote by ${\displaystyle Q}$ the heat received by the combined masses from external sources in any process in which the pressure is not varied, and distinguish the initial and final states of the system by accents we have
 ${\displaystyle \chi ''-\chi '=\epsilon ''-\epsilon '+p(v''-v')=Q.}$ (119)
This function may therefore be called the heat function for constant pressure (just as the energy might be called the heat function for constant volume), the diminution of the function representing in all cases in which the pressure is not varied the heat given out by the system. In all cases of chemical action in which no heat is allowed to escape the value of ${\displaystyle \chi }$ remains unchanged.

Potentials.

In the definition of the potentials ${\displaystyle \mu _{1},\mu _{2},}$ etc., the energy of a homogeneous mass was considered as a function of its entropy, its volume, and the quantities of the various substances composing it. Then the potential for one of these substances was defined as the differential coefficient of the energy taken with respect to the variable expressing the quantity of that substance. Now, as the manner in which we consider the given mass as composed of various substances is in some degree arbitrary, so that the energy may be considered as a function of various different sets of variables expressing quantities of component substances, it might seem that the above definition does not fix the value of the potential of any substance in the given mass, until we have fixed the manner in which the mass is to be considered as composed. For example, if we have a solution obtained by dissolving in water a certain salt containing water of crystallization, we may consider the liquid as composed of ${\displaystyle m_{S}}$ weight-units of the hydrate and ${\displaystyle m_{W}}$ of water, or as composed of ${\displaystyle m_{s}}$ of the anhydrous salt and ${\displaystyle m_{w}}$ of water. It will be observed that the values of ${\displaystyle m_{S}}$ and ${\displaystyle m_{s}}$, are not the same, nor those of ${\displaystyle m_{W}}$ and ${\displaystyle m_{w}}$, and hence it might seem that the potential for water in the given liquid considered as composed of the hydrate and water, viz.,

 ${\displaystyle \left({\frac {d\epsilon }{dm_{W}}}\right)_{\eta ,v,m_{S}},}$
would be different from the potential for water in the same liquid considered as composed of anhydrous salt and water, viz.,
 ${\displaystyle \left({\frac {d\epsilon }{dm_{w}}}\right)_{\eta ,v,m_{s}}\cdot }$
The value of the two expressions is, however, the same, for, although ${\displaystyle m_{W}}$ is not equal to ${\displaystyle m_{w}}$, we may of course suppose ${\displaystyle dm_{W}}$ to be equal to ${\displaystyle dm_{w}}$, and then the numerators in the two fractions will also be equal, as they each denote the increase of energy of the liquid, when the quantity ${\displaystyle dm_{W}}$ or ${\displaystyle dm_{w}}$ of water is added without altering the entropy and volume of the liquid. Precisely the same considerations will apply to any other case.

In fact, we may give a definition of a potential which shall not presuppose any choice of a particular set of substances as the components of the homogeneous mass considered.

Definition.—If to any homogeneous mass we suppose an infinitesimal quantity of any substance to be added, the mass remaining homogeneous and its entropy and volume remaining unchanged, the increase of the energy of the mass divided by the quantity of the substance added is the potential for that substance in the mass considered. (For the purposes of this definition, any chemical element or combination of elements in given proportions may be considered a substance, whether capable or not of existing by itself as a homogeneous body.)

In the above definition we may evidently substitute for entropy, volume, and energy, respectively, either temperature, volume, and the function ${\displaystyle \psi }$; or entropy, pressure, and the function ${\displaystyle \chi }$; or temperature, pressure, and the function ${\displaystyle \zeta }$. (Compare equation (104).)

In the same homogeneous mass, therefore, we may distinguish the potentials for an indefinite number of substances, each of which has a perfectly determined value.

Between the potentials for different substances in the same homogeneous mass the same equations will subsist as between the units of these substances. That is, if the substances, ${\displaystyle S{a},S_{b}}$, etc., ${\displaystyle S_{k},S_{l}}$, etc., are components of any given homogeneous mass, and are such that

 ${\displaystyle \alpha {\mathfrak {S}}_{a}+\beta {\mathfrak {S}}_{b}+{\text{etc.}}=\kappa {\mathfrak {S}}_{k}+\lambda {\mathfrak {S}}_{l}+{\text{etc.,}}}$ (120)
${\displaystyle {\mathfrak {S}}_{a},{\mathfrak {S}}_{b}}$, etc., ${\displaystyle {\mathfrak {S}}_{k},{\mathfrak {S}}_{l}}$, etc., denoting the units of the several substances, and ${\displaystyle \alpha ,\beta }$, etc., ${\displaystyle \kappa ,\lambda }$, etc., denoting numbers, then if ${\displaystyle \mu _{a},\mu _{b}}$, etc., ${\displaystyle \mu _{k},\mu _{l}}$, etc., denote the potentials for these substances in the homogeneous mass,
 ${\displaystyle \alpha \mu _{a}+\beta \mu _{b}+{\text{etc.}}=\kappa \mu _{k}+\lambda \mu _{l}+{\text{etc.}}}$ (121)
To show this, we will suppose the mass considered to be very large. Then, the first member of (121) denotes the increase of the energy of the mass produced by the addition of the matter represented by the first member of (120), and the second member of (121) denotes the increase of energy of the same mass produced by the addition of the matter represented by the second member of (120), the entropy and volume of the mass remaining in each case unchanged. Therefore, as the two members of (120) represent the same matter in kind and quantity, the two members of (121) must be equal.

But it must be understood that equation (120) is intended to denote equivalence of the substances represented in the mass considered, and not merely chemical identity; in other words, it is supposed that there are no passive resistances to change in the mass considered which prevent the substances represented by one member of (120) from passing into those represented by the other. For example, in respect to a mixture of vapor of water and free hydrogen and oxygen (at ordinary temperatures), we may not write

 ${\displaystyle 9{\mathfrak {S}}_{Aq}=1{\mathfrak {S}}_{H}+8{\mathfrak {S}}_{O},}$
but water is to be treated as an independent substance, and no necessary relation will subsist between the potential for water and the potentials for hydrogen and oxygen.

The reader will observe that the relations expressed by equations (43) and (51) (which are essentially relations between the potentials for actual components in different parts of a mass in a state of equilibrium) are simply those which by (121) would necessarily subsist between the same potentials in any homogeneous mass containing as variable components all the substances to which the potentials relate.

In the case of a body of invariable composition, the potential for the single component is equal to the value of ${\displaystyle \zeta }$ for one unit of the body, as appears from the equation

 ${\displaystyle \zeta =\mu m,}$ (122)
to which (96) reduces in this case. Therefore, when ${\displaystyle n=1}$, the fundamental equation between the quantities in the set (102) (see page 88) and that between the quantities in (103) may be derived either from the other by simple substitution. But, with this single exception, an equation between the quantities in one of the sets (99)–(103) cannot be derived from the equation between the quantities in another of these sets without differentiation.

Also in the case of a body of variable composition, when all the quantities of the components except one vanish, the potential for that one will be equal to the value of ${\displaystyle \zeta }$ for one unit of the body. We may make this occur for any given composition of the body by choosing as one of the components the matter constituting the body itself, so that the value of ${\displaystyle \zeta }$ for one unit of a body may always be considered as a potential. Hence the relations between the values of ${\displaystyle \zeta }$ for contiguous masses given on page 91 may be regarded as relations between potentials.

The two following propositions afford definitions of a potential which may sometimes be convenient.

The potential for any substance in any homogeneous mass is equal to the amount of mechanical work required to bring a unit of the substance by a reversible process from the state in which its energy and entropy are both zero into combination with the homogeneous mass, which at the close of the process must have its original volume, and which is supposed so large as not to be sensibly altered in any part. All other bodies used in the process must by its close be restored to their original state, except those used to supply the work, which must be used only as the source of the work. For, in a reversible process, when the entropies of other bodies are not altered, the entropy of the substance and mass taken together will not be altered. But the original entropy of the substance is zero; therefore the entropy of the mass is not altered by the addition of the substance. Again, the work expended will be equal to the increment of the energy of the mass and substance taken together, and therefore equal, as the original energy of the substance is zero, to the increment of energy of the mass due to the addition of the substance, which by the definition on page 93 is equal to the potential in question.

The potential for any substance in any homogeneous mass is equal to the work required to bring a unit of the substance by a reversible process from a state in which ${\displaystyle \psi =0}$ and the temperature is the same as that of the given mass into combination with this mass, which at the close of the process must have the same volume and temperature as at first, and which is supposed so large as not to be sensibly altered in any part. A source of heat or cold of the temperature of the given mass is allowed, with this exception other bodies are to be used only on the same conditions as before. This may be shown by applying equation (109) to the mass and substance taken together.

The last proposition enables us to see very easily how the value of the potential is affected by the arbitrary constants involved in the definition of the energy and the entropy of each elementary substance. For we may imagine the substance brought from the state in which ${\displaystyle \psi =0}$ and the temperature is the same as that of the given mass, first to any specified state of the same temperature, and then into combination with the given mass. In the first part of the process the work expended is evidently represented by the value of ${\displaystyle \psi }$ for the unit of the substance in the state specified. Let this be denoted by ${\displaystyle \psi '}$, and let ${\displaystyle \mu }$ denote the potential in question, and ${\displaystyle W}$ the work expended in bringing a unit of the substance from the specified state into combination with the given mass as aforesaid; then

 ${\displaystyle \mu =\psi '+W.}$ (123)
Now as the state of the substance for which ${\displaystyle \epsilon =0}$ and ${\displaystyle \eta =0}$ is arbitrary, we may simultaneously increase the energies of the unit of the substance in all possible states by any constant ${\displaystyle C}$, and the entropies of the substance in all possible states by any constant ${\displaystyle K}$. The value of ${\displaystyle \psi }$, or ${\displaystyle \epsilon -t\eta }$, for any state would then be increased by ${\displaystyle C-tK}$, ${\displaystyle t}$ denoting the temperature of the state. Applying this to ${\displaystyle \psi '}$ in (123) and observing that the last term in this equation is independent of the values of these constants, we see that the potential would be increased by the same quantity ${\displaystyle C-tK}$, ${\displaystyle t}$ being the temperature of the mass in which the potential is to be determined.

On Coexistent Phases of Matter.

In considering the different homogeneous bodies which can be formed out of any set of component substances, it will be convenient to have a term which shall refer solely to the composition and thermodynamic state of any such body without regard to its quantity or form. We may call such bodies as differ in composition or state different phases of the matter considered, regarding all bodies which differ only in quantity and form as different examples of the same phase. Phases which can exist together, the dividing surfaces being plane, in an equilibrium which does not depend upon passive resistances to change, we shall call coexistent.

If a homogeneous body has ${\displaystyle n}$ independently variable components, the phase of the body is evidently capable of ${\displaystyle n+1}$ independent variations. A system of ${\displaystyle r}$ coexistent phases, each of which has the same ${\displaystyle n}$ independently variable components is capable of ${\displaystyle n+2-r}$ variations of phase. For the temperature, the pressure, and the potentials for the actual components have the same values in the different phases, and the variations of these quantities are by (97) subject to as many conditions as there are different phases. Therefore, the number of independent variations in the values of these quantities, i.e., the number of independent variations of phase of the system, will be ${\displaystyle n+2-r.}$

Or, when the ${\displaystyle r}$ bodies considered have not the same independently variable components, if we still denote by ${\displaystyle n}$ the number of independently variable components of the ${\displaystyle r}$ bodies taken as a whole, the number of independent variations of phase of which the system is capable will still be ${\displaystyle n+2-r}$. In this case, it will be necessary to consider the potentials for more than ${\displaystyle n}$ component substances. Let the number of these potentials be ${\displaystyle n+h}$. We shall have by (97), as before, ${\displaystyle r}$ relations between the variations of the temperature, of the pressure, and of these ${\displaystyle n+h}$ potentials, and we shall also have by (43) and (51) ${\displaystyle h}$ relations between these potentials, of the same form as the relations which subsist between the units of the different component substances.

Hence, if ${\displaystyle r=n+2}$, no variation in the phases (remaining coexistent) is possible. It does not seem probable that ${\displaystyle r}$ can ever exceed ${\displaystyle n+2}$. An example of ${\displaystyle n=1}$ and ${\displaystyle r=3}$ is seen in the coexistent solid, liquid, and gaseous forms of any substance of invariable composition. It seems not improbable that in the case of sulphur and some other simple substances there is more than one triad of coexistent phases; but it is entirely improbable that there are four coexistent phases of any simple substance. An example of ${\displaystyle n=2}$ and ${\displaystyle r=4}$ is seen in a solution of a salt in water in contact with vapor of water and two different kinds of crystals of the salt.

Concerning ${\displaystyle n+1}$ Coexistent Phases.

We will now seek the differential equation which expresses the relation between the variations of the temperature and the pressure in a system of ${\displaystyle n+1}$ coexistent phases (${\displaystyle n}$ denoting, as before, the number of independently variable components in the system taken as a whole). In this case we have ${\displaystyle n+1}$ equations of the general form of (97) (one for each of the coexistent phases), in which we may distinguish the quantities ${\displaystyle \eta ,v,m_{1},m_{2},}$ etc., relating to the different phases by accents. But ${\displaystyle t}$ and ${\displaystyle p}$ will each have the same value throughout, and the same is true of ${\displaystyle \mu _{1},\mu _{2},}$, etc., so far as each of these occurs in the different equations. If the total number of these potentials is ${\displaystyle n+h}$, there will be ${\displaystyle h}$ independent relations between them, corresponding to the ${\displaystyle h}$ independent relations between the units of the component substances to which the potentials relate, by means of which we may eliminate the variations of ${\displaystyle h}$ of the potentials from the equations of the form of (97) in which they occur.

Let one of these equations be

 ${\displaystyle v'dp=\eta 'dt+m'_{a}d\mu _{a}+m'_{b}d\mu _{b}+{\text{ etc.,}}}$ (124)
and by the proposed elimination let it become
 ${\displaystyle v'dp=\eta 'dt+A'_{1}d\mu _{a}+A'_{2}d\mu _{b}...+A'_{n}d\mu _{n}.}$ (125)

It will be observed that ${\displaystyle \mu _{a}}$, for example, in (124) denotes the potential in the mass considered for a substance ${\displaystyle S_{a}}$ which may or may not be identical with any of the substances ${\displaystyle S_{1},S_{2}}$, etc., to which the potentials in (125) relate. Now as the equations between the potentials by means of which the elimination is performed are similar to those which subsist between the units of the corresponding substances (compare equations (38), (43), and (51)), if we denote these units by ${\displaystyle {\mathfrak {S}}_{a},{\mathfrak {S}}_{b}}$, etc., ${\displaystyle {\mathfrak {S}}_{1},{\mathfrak {S}}_{2}}$, etc., we must also have

 ${\displaystyle m'_{a}{\mathfrak {S}}_{a}+m'_{b}{\mathfrak {S}}_{a}+{\text{ etc.}}=A'_{1}{\mathfrak {S}}_{1}+A'_{2}{\mathfrak {S}}_{2}...+A'_{n}{\mathfrak {S}}_{n}.}$ (126)
But the first member of this equation denotes (in kind and quantity) the matter in the body to which equations (124) and (125) relate. As the same must be true of the second member, we may regard this same body as composed of the quantity ${\displaystyle A'_{1}}$ of the substance ${\displaystyle S_{1}}$ with the quantity ${\displaystyle A'_{2}}$ of the substance ${\displaystyle S_{2}}$, etc. We will therefore, in accordance with our general usage, write ${\displaystyle m_{1},m_{2}}$, etc., for ${\displaystyle A'_{1},A'_{2}}$, etc., in (125), which will then become
 ${\displaystyle v'dp=\eta 'dt+m'_{1}d\mu _{1}+m'_{2}d\mu _{2}...+m'_{n}d\mu _{n}.}$ (127)
But we must remember that the components to which the ${\displaystyle m'_{1},m'_{2}}$, etc., of this equation relate are not necessarily independently variable, as are the components to which the similar expressions in (97) and (124) relate. The rest of the ${\displaystyle n+1}$ equations may be reduced to a similar form, viz.,
 ${\displaystyle v''dp=\eta ''dt+m''_{1}d\mu _{1}+m''_{2}d\mu _{2}...+m''_{n}d\mu _{n},\,\,{\text{etc.}}}$ (128)
By elimination of ${\displaystyle d\mu _{1},d\mu _{2},...d\mu _{n}}$ from these equations we obtain
 ${\displaystyle {\begin{vmatrix}v'&m'_{1}&m'_{2}&...&m'_{n}\\v''&m''_{1}&m''_{2}&...&m''_{n}\\v'''&m'''_{1}&m'''_{2}&...&m'''_{n}\\.&.&.&...&.\\.&.&.&...&.\end{vmatrix}}dp={\begin{vmatrix}\eta '&m'_{1}&m'_{2}&...&m'_{n}\\\eta ''&m''_{1}&m''_{2}&...&m''_{n}\\\eta '''&m'''_{1}&m'''_{2}&...&m'''_{n}\\.&.&.&...&.\\.&.&.&...&.\end{vmatrix}}dt.}$ (129)
In this equation we may make ${\displaystyle v',v''}$, etc., equal to unity. Then ${\displaystyle m'_{1},m'_{2},m''_{1},}$, etc., will denote the separate densities of the components

in the different phases, and rf, rf f , etc., the densities of entropy.

When ${\displaystyle n=1}$,

 ${\displaystyle (m''v'-m'v'')dp=(m''\eta '-m'\eta '')}$ (130)
or, if we make ${\displaystyle m'=1}$ and ${\displaystyle m''=1}$, we have the usual formula
 ${\displaystyle {\frac {dp}{dt}}={\frac {\eta '-\eta ''}{v'-v''}}={\frac {Q}{t(v''-v')}},}$ (131)
in which ${\displaystyle Q}$ denotes the heat absorbed by a unit of the substance in passing from one state to the other without change of temperature or pressure.

Concerning Cases in which the Number of Coexistent Phases is less than n + 1.

When ${\displaystyle n>1}$, if the quantities of all the components ${\displaystyle S_{1},S_{2},...S_{n}}$ are proportional in two coexistent phases, the two equations of the form of (127) and (128) relating to these phases will be sufficient for the elimination of the variations of all the potentials. In fact, the condition of the coexistence of the two phases together with the condition of the equality of the ${\displaystyle n-1}$ ratios of ${\displaystyle m'_{1},m'_{2},...m'_{n}}$ with the ${\displaystyle n-1}$ ratios of ${\displaystyle m''_{1},m''_{2},...m''_{n}}$ is sufficient to determine ${\displaystyle p}$ as a function of ${\displaystyle t}$ if the fundamental equation is known for each of the phases. The differential equation in this case may be expressed in the form of (130), ${\displaystyle m'}$ and ${\displaystyle m''}$ denoting either the quantities of any one of the components or the total quantities of matter in the bodies to which they relate. Equation (131) will also hold true in this case if the total quantity of matter in each of the bodies is unity. But this case differs from the preceding in that the matter which absorbs the heat ${\displaystyle Q}$ in passing from one state to another, and to which the other letters in the formula relate, although the same in quantity, is not in general the same in kind at different temperatures and pressures. Yet the case will often occur that one of the phases is essentially invariable in composition, especially when it is a crystalline body, and in this case the matter to which the letters in (131) relate will not vary with the temperature and pressure.

When ${\displaystyle n=2}$, two coexistent phases are capable, when the temperature is constant, of a single variation in phase. But as (130) will hold true in this case when ${\displaystyle m'_{1}:m'_{2}::m''_{1}::m''_{2}}$, it follows that for constant temperature the pressure is in general a maximum or a minimum when the composition of the two phases is identical. In like manner, the temperature of the two coexistent phases is in general a maximum or a minimum, for constant pressure, when the composition of the two phases is identical. Hence, the series of simultaneous values of ${\displaystyle t}$ and ${\displaystyle p}$ for which the composition of two coexistent phases is identical separates those simultaneous values of ${\displaystyle t}$ and ${\displaystyle p}$ for which no coexistent phases are possible from those for which there are two pair of coexistent phases. This may be applied to a liquid having two independently variable components in connection with the vapor which it yields, or in connection with any solid which may be formed in it.

When ${\displaystyle n=3}$, we have for three coexistent phases three equations of the form of (127), from which we may obtain the following,

 ${\displaystyle {\begin{vmatrix}v'&m'_{1}&m'_{2}\\v''&m''_{1}&m''_{2}\\v'''&m'''_{1}&m'''_{2}\end{vmatrix}}dp={\begin{vmatrix}\eta '&m'_{1}&m'_{2}\\\eta ''&m''_{1}&m''_{2}\\\eta '''&m'''_{1}&m'''_{2}\end{vmatrix}}dt+{\begin{vmatrix}m'_{1}&m'_{2}&m'_{3}\\m''_{1}&m''_{2}&m''_{3}\\m'''_{1}&m'''_{2}&m'''_{3}\end{vmatrix}}d\mu _{3}}$ (132)

Now the value of the last of these determinants will be zero, when the composition of one of the three phases is such as can be produced by combining the other two. Hence, the pressure of three coexistent phases will in general be a maximum or minimum for constant temperature, and the temperature a maximum or minimum for constant pressure, when the above condition in regard to the composition of the coexistent phases is satisfied. The series of simultaneous values of ${\displaystyle t}$ and ${\displaystyle p}$ for which the condition is satisfied separates those simultaneous values of ${\displaystyle t}$ and ${\displaystyle p}$ for which three coexistent phases are not possible, from those for which there are two triads of coexistent phases. These propositions may be extended to higher values of ${\displaystyle n}$ and illustrated by the boiling temperatures and pressures of saturated solutions of ${\displaystyle n-2}$ different solids in solvents having two independently variable components.

Internal Stability of Homogeneous Fluids as indicated by Fundamental Equations.

We will now consider the stability of a fluid enclosed in a rigid envelop which is non-conducting to heat and impermeable to all the components of the fluid. The fluid is supposed initially homogeneous in the sense in which we have before used the word, i.e., uniform in every respect throughout its whole extent. Let ${\displaystyle S_{1},~S_{2},~\ldots ~S_{n}}$ be the ultimate components of the fluid; we may then consider every body which can be formed out of the fluid to be composed of ${\displaystyle S_{1},~S_{2},~\ldots ~S_{n}}$, and that in only one way. Let ${\displaystyle m_{1},~m_{2},~\ldots ~m_{n}}$ denote the quantities of these substances in any such body, and let ${\displaystyle \epsilon ,~\eta ,~v}$, denote its energy, entropy, and volume. The fundamental equation for compounds of ${\displaystyle S_{1},~S_{2},~\ldots ~S_{n}}$, if completely determined, will give us all possible sets of simultaneous values of these variables for homogeneous bodies.

Now, if it is possible to assign such values to the constants ${\displaystyle T,~P,~M_{1},~M_{2},~\ldots ~M_{n}}$ that the value of the expression

 ${\displaystyle \epsilon -T\eta +Pv-M_{1}m_{1}-M_{2}m_{2}\ldots -M_{n}m_{n}}$ (133)
shall be zero for the given fluid, and shall be positive for every other phase of the same components, i.e., for every homogeneous body[9] not identical in nature and state with the given fluid (but composed entirely of ${\displaystyle S_{1},~S_{2},~\ldots ~S_{n}}$), the condition of the given fluid will be stable.

For, in any condition whatever of the given mass, whether or not homogeneous, or fluid, if the value of the expression (133) is not negative for any homogeneous part of the mass, its value for the whole mass cannot be negative; and if its value cannot be zero for any homogeneous part which is not identical in phase with the mass in its given condition, its value cannot be zero for the whole except when the whole is in the given condition. Therefore, in the case supposed, the value of this expression for any other than the given condition of the mass is positive. (That this conclusion cannot be invalidated by the fact that it is not entirely correct to regard a composite mass as made up of homogeneous parts having the same properties in respect to energy, entropy, etc., as if they were parts of larger homogeneous masses, will easily appear from considerations similar to those adduced on pages 77–78.) If, then, the value of the expression (133) for the mass considered is less when it is in the given condition than when it is in any other, the energy of the mass in its given condition must be less than in any other condition in which it has the same entropy and volume. The given condition is therefore stable. (See page 57.)

Again, if it is possible to assign such values to the constants in (133) that the value of the expression shall be zero for the given fluid mass, and shall not be negative for any phase of the same components, the given condition will be evidently not unstable. (See page 57.) It will be stable unless it is possible for the given matter in the given volume and with the given entropy to consist of homogeneous parts for all of which the value of the expression (133) is zero, but which are not all identical in phase with the mass in its given condition. (A mass consisting of such parts would be in equilibrium, as we have already seen on pages 78, 79.) In this case, if we disregard the quantities connected with the surfaces which divide the homogeneous parts, we must regard the given condition as one of neutral equilibrium. But in regard to these homogeneous parts, which we may evidently consider to be all different phases, the following conditions must be satisfied. (The accents distinguish the letters referring to the different parts, and the unaccented letters refer to the whole mass.)

 ${\displaystyle \eta '+\eta ''+{\text{etc.}}=\eta ,}$ ${\displaystyle \scriptstyle {\left.{\begin{matrix}\ \\\\\ \\\ \\\ \ \end{matrix}}\right\}\,}}$ (134) ${\displaystyle v'+v''+{\text{etc.}}=v;}$ ${\displaystyle m'_{1}+m''_{1}+{\text{etc.}}=m_{1},}$ ${\displaystyle m'_{2}+m''_{2}+{\text{etc.}}=m_{2},}$ ${\displaystyle {\text{etc.}}}$

Now the values of ${\displaystyle \eta ,v,m_{1},m_{2},}$ etc., are determined by the whole fluid mass in its given state, and the values of ${\displaystyle {\frac {\eta '}{v'}},{\frac {\eta ''}{v''}},}$ etc., ${\displaystyle {\frac {m'_{1}}{v'}},{\frac {m''_{1}}{v''}},}$ etc., ${\displaystyle {\frac {m'_{2}}{v'}},{\frac {m''_{2}}{v''}},}$ etc., etc., are determined by the phases of the various parts. But the phases of these parts are evidently determined by the phase of the fluid as given. They form, in fact, the whole set of coexistent phases of which the latter is one. Hence, we may regard (134) as ${\displaystyle n+2}$ linear equations between ${\displaystyle v',v'',}$, etc. (The values of ${\displaystyle v',v'',}$ etc., are also subject to the condition that none of them can be negative.) Now one solution of these equations must give us the given condition of the fluid; and it is not to be expected that they will be capable of any other solution, unless the number of different homogeneous parts, that is, the number of different coexistent phases, is greater than ${\displaystyle n+2}$. We have already seen (page 97) that it is not probable that this is ever the case.

We may, however, remark that in a certain sense an infinitely large fluid mass will be in neutral equilibrium in regard to the formation of the substances, if such there are, other than the given fluid, for which the value of (133) is zero (when the constants are so determined that the value of the expression is zero for the given fluid, and not negative for any substance); for the tendency of such a formation to be reabsorbed will diminish indefinitely as the mass out of which it is formed increases.

When the substances ${\displaystyle S_{1},S_{2},...S_{n}}$ are all independently variable components of the given mass, it is evident from (86) that the conditions that the value of (133) shall be zero for the mass as given, and shall not be negative for any phase of the same components, can only be fulfilled when the constants ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$ are equal to the temperature, the pressure, and the several potentials in the given mass. If we give these values to the constants, the expression (133) will necessarily have the value zero for the given mass, and we shall only have to inquire whether its value is positive for all other phases. But when ${\displaystyle S_{1},S_{2},...S_{n}}$ are not all independently variable components of the given mass, the values which it will be necessary to give to the constants in (133) cannot be determined entirely from the properties of the given mass; but ${\displaystyle T}$ and ${\displaystyle P}$ must be equal to its temperature and pressure, and it will be easy to obtain as many equations connecting ${\displaystyle M_{1},M_{2},...M_{n}}$ with the potentials in the given mass as it contains independently variable components.

When it is not possible to assign such values to the constants in (133) that the value of the expression shall be zero for the given fluid, and either zero or positive for any phase of the same components, we have already seen (pages 75–79) that if equilibrium subsists without passive resistances to change, it must be in virtue of properties which are peculiar to small masses surrounded by masses of different nature, and which are not indicated by fundamental equations. In this case, the fluid will necessarily be unstable, if we extend this term to embrace all cases in which an initial disturbance confined to a small part of an indefinitely large fluid mass will cause an ultimate change of state not indefinitely small in degree throughout the whole mass. In the discussion of stability as indicated by fundamental equations it will be convenient to use the term in this sense.[10]

In determining for any given positive values of ${\displaystyle T}$ and ${\displaystyle P}$ and any given values whatever of ${\displaystyle M_{1},M_{2},...M_{n}}$ whether the expression (133) is capable of a negative value for any phase of the components ${\displaystyle S_{1},S_{2},...S_{n}}$, and if not, whether it is capable of the value zero for any other phase than that of which the stability is in question, it is only necessary to consider phases having the temperature ${\displaystyle T}$ and pressure ${\displaystyle P}$. For we may assume that a mass of matter represented by any values of ${\displaystyle m_{1},m_{2},...m_{n}}$ is capable of at least one state of not unstable equilibrium (which may or may not be a homogeneous state) at this temperature and pressure. It may easily be shown that for such a state the value of ${\displaystyle \epsilon =T\eta -Pv}$ must be as small as for any other state of the same matter. The same will therefore be true of the value of (133). Therefore if this expression is capable of a negative value for any mass whatever, it will have a negative value for that mass at the temperature ${\displaystyle T}$ and pressure ${\displaystyle P}$. And if this mass is not homogeneous, the value of (133) must be negative for at least one of its homogeneous parts. So also, if the expression (133) is not capable of a negative value for any phase of the components, any phase for which it has the value zero must have the temperature ${\displaystyle T}$ and the pressure ${\displaystyle P}$.

It may easily be shown that the same must be true in the limiting cases in which ${\displaystyle T=0}$ and ${\displaystyle P=0}$. For negative values of ${\displaystyle P}$, (133) is always capable of negative values, as its value for a vacuum is ${\displaystyle Pv}$.

For any body of the temperature ${\displaystyle T}$ and pressure ${\displaystyle P}$, the expression (133) may by (91) be reduced to the form

 ${\displaystyle \zeta -M_{1}m_{1}-M_{2}m_{2}...-M_{n}m_{n}.}$ (135)
We have already seen (page 77) that an expression like (133), when ${\displaystyle T,P,M_{1},M_{2},...M_{n}}$ and ${\displaystyle v}$ have any given finite values, cannot have an infinite negative value as applied to any real body. Hence, in determining whether (133) is capable of a negative value for any phase of the components ${\displaystyle S_{1},S_{2},...S_{n}}$, and if not, whether it is capable of the value zero for any other phase than that of which the stability is in question, we have only to consider the least value of which it is capable for a constant value of ${\displaystyle v}$. Any body giving this value must satisfy the condition that for constant volume
 ${\displaystyle d\epsilon -Td\eta -M_{1}dm_{1}-M_{2}dm_{2}...-M_{n}\geqq 0,}$ (136)
or, if we substitute the value of de taken from equation (86), using subscript ${\displaystyle a,...g}$ for the quantities relating to the actual components of the body, and subscript ${\displaystyle h,...k}$ for those relating to the possible,
 ${\displaystyle td\eta +\mu _{a}dm_{a}...+\mu _{g}dm_{g}+\mu _{h}dm_{h}...+\mu _{k}dm_{k}-Td\eta -M_{1}dm_{1}-M_{2}dm_{2}...-M_{n}dm_{n}\geqq 0.}$ (137)
That is, the temperature of the body must be equal to ${\displaystyle T}$, and the potentials of its components must satisfy the same conditions as if it were in contact and in equilibrium with a body having potentials ${\displaystyle M_{1},M_{2},...M_{n}}$. Therefore the same relations must subsist between ${\displaystyle \mu _{1},\mu _{2},...\mu _{n}}$ and ${\displaystyle M_{1},M_{2},...M_{n}}$ as between the units of the corresponding substances, so that
 ${\displaystyle \mu _{a}m_{a}..+\mu _{g}m_{g}=m_{1}M_{1}..+m_{n}M_{n},}$ (138)
and as we have by (93)
 ${\displaystyle \epsilon =t\eta -pv+\mu _{a}m_{a}..+\mu _{g}m_{g},}$ (139)
the expression (133) will reduce (for the body or bodies for which it has the least value per unit of volume) to
 ${\displaystyle (P-p)v,}$ (140)
the value of which will be positive, null, or negative, according as the value of
 ${\displaystyle P-p}$ (141)
is positive, null, or negative.

Hence, the conditions in regard to the stability of a fluid of which all the ultimate components are independently variable admit a very simple expression. If the pressure of the fluid is greater than that of any other phase of the same components which has the same temperature and the same values of the potentials for its actual components, the fluid is stable without coexistent phases; if its pressure is not as great as that of some other such phase, it will be unstable; if its pressure is as great as that of any other such phase, but not greater than that of every other, the fluid will certainly not be unstable, and in all probability it will be stable (when enclosed in a rigid envelop which is impermeable to heat and to all kinds of matter), but it will be one of a set of coexistent phases of which the others are the phases which have the same pressure.

The considerations of the last two pages, by which the tests relating to the stability of a fluid are simplified, apply to such bodies as actually exist. But if we should form arbitrarily any equation as a fundamental equation, and ask whether a fluid of which the properties were given by that equation would be stable, the tests of stability last given would be insufficient, as some of our assumptions might not be fulfilled by the equation. The test, however, as first given (pages 100–102) would in all cases be sufficient.

Stability in respect to Continuous Changes of Phase.

In considering the changes which may take place in any mass, we have already had occasion to distinguish between infinitesimal changes in existing phases, and the formation of entirely new phases. A phase of a fluid may be stable in regard to the former kind of change, and unstable in regard to the latter. In this case it may be capable of continued existence in virtue of properties which prevent the commencement of discontinuous changes. But a phase which is unstable in regard to continuous changes is evidently incapable of permanent existence on a large scale except in consequence of passive resistances to change. We will now consider the conditions of stability in respect to continuous changes of phase, or, as it may also be called, stability in respect to adjacent phases. We may use the same general test as before, except that the expression (133) is to be applied only to phases which differ infinitely little from the phase of which the stability is in question. In this case the component substances to be considered will be limited to the independently variable components of the fluid, and the constants ${\displaystyle M_{1},M_{2},}$ etc., must have the values of the potentials for these components in the given fluid. The constants in (133) are thus entirely determined and the value of the expression for the given phase is necessarily zero. If for any infinitely small variation of the phase the value of (133) can become negative, the fluid will be unstable; but if for every infinitely small variation of the phase the value of (133) becomes positive, the fluid will be stable. The only remaining case, in which the phase can be varied without altering the value of (133) can hardly be expected to occur. The phase concerned would in such a case have coexistent adjacent phases. It will be sufficient to discuss the condition of stability (in respect to continuous changes) without coexistent adjacent phases.

This condition, which for brevity's sake we will call the condition of stability, may be written in the form

 ${\displaystyle \epsilon ''-t'\eta ''+p'v''-\mu _{1}'m''_{1}...-\mu _{n}'m''_{n}>0,}$ (142)
in which the quantities relating to the phase of which the stability is in question are distinguished by single accents, and those relating to the other phase by double accents. This condition is by (93) equivalent to
 ${\displaystyle \epsilon ''-t'\eta ''+p'v''-\mu _{1}'m''_{1}...-\mu _{n}'m''_{n}-\epsilon '-t'\eta '+p'v'-\mu _{1}'m'_{1}...-\mu _{n}'m'_{n}>0,}$ (143)
and to
 ${\displaystyle -t'\eta ''+p'v''-\mu _{1}'m''_{1}...-\mu _{n}'m''_{n}+t''\eta ''+p''v''-\mu _{1}''m''_{1}...-\mu _{n}''m''_{n}>0.}$ (144)
The condition (143) may be expressed more briefly in the form
 ${\displaystyle \Delta \epsilon >t\Delta \eta -p\Delta v+\mu _{1}\Delta m_{1}...+\mu _{n}\Delta m_{n},}$ (145)
if we use the character ${\displaystyle \Delta }$ to signify that the condition, although relating to infinitesimal differences, is not to be interpreted in accordance with the usual convention in respect to differential equations with neglect of infinitesimals of higher orders than the first, but is to be interpreted strictly, like an equation between finite differences. In fact, when a condition like (145) (interpreted strictly) is satisfied for infinitesimal differences, it must be possible to assign limits within which it shall hold true of finite differences. But it is to be remembered that the condition is not to be applied to any arbitrary values of ${\displaystyle \Delta \eta ,\Delta v,\Delta m_{1},...\Delta m_{n}}$, but only to such as are determined by a change of phase. (If only the quantity of the body which determines the value of the variables should vary and not its phase, the value of the first member of (145) would evidently be zero.) We may free ourselves from this limitation by making v constant, which will cause the term ${\displaystyle -p\Delta v}$ to disappear. If we then divide by the constant ${\displaystyle v}$, the condition will become
 ${\displaystyle \Delta {\frac {\epsilon }{v}}>t\Delta {\frac {\eta }{v}}+\mu _{1}\Delta {\frac {m_{1}}{v}}...+\mu _{n}\Delta {\frac {m_{n}}{v}},}$ (146)
in which form it will not be necessary to regard ${\displaystyle v}$ as constant. As we may obtain from (86)
 ${\displaystyle d{\frac {\epsilon }{v}}>=td{\frac {\eta }{v}}+\mu _{1}d{\frac {m_{1}}{v}}...+\mu _{n}d{\frac {m_{n}}{v}},}$ (147)

we see that the stability of any phase in regard to continuous changes depends upon the same conditions in regard to the second and higher differential coefficients of the density of energy regarded as a function of the density of entropy and the densities of the several components which would make the density of energy a minimum, if the necessary conditions in regard to the first differential coefficients were fulfilled. When ${\displaystyle n=1}$, it may be more convenient to regard ${\displaystyle m}$ as constant in (145) than ${\displaystyle v}$. Regarding ${\displaystyle m}$ a constant, it appears that the stability of a phase depends upon the same conditions in regard to the second and higher differential coefficients of the energy of a unit of mass regarded as a function of its entropy and volume, which would make the energy a minimum, if the necessary conditions in regard to the first differential coefficients were fulfilled.

The formula (144) expresses the condition of stability for the phase to which ${\displaystyle t',p',}$ etc., relate. But it is evidently the necessary and sufficient condition of the stability of all phases of certain kinds of matter, or of all phases within given limits, that (144) shall hold true of any two infinitesimally differing phases within the same limits, or, as the case may be, in general. For the purpose, therefore, of such collective determinations of stability, we may neglect the distinction between the two states compared, and write the condition in the form

 ${\displaystyle -\eta \Delta t+v\Delta p-m_{1}\Delta \mu _{1}...-m_{n}\Delta \mu _{n}>0,}$ (148)
 or ${\displaystyle \Delta p>{\f$