My watch list
my.chemeurope.com
Login

# Maxwell relations

Thermodynamic equations
Laws of thermodynamics
Conjugate variables
Thermodynamic potential
Material properties
Maxwell relations
Bridgman's equations
Exact differential
Table of thermodynamic equations
edit

Maxwell's relations are a set of equations in thermodynamics which are derivable from the definitions of the thermodynamic potentials. The Maxwell relations are statements of equality among the second derivatives of the thermodynamic potentials. They follow directly from the fact that the order of differentiation of an analytic function of two variables is irrelevant. If Φ is a thermodynamic potential and xi and xj are two different natural variables for that potential, then the Maxwell relation for that potential and those variables is:

$\frac{\partial }{\partial x_j}\left(\frac{\partial \Phi}{\partial x_i}\right)= \frac{\partial }{\partial x_i}\left(\frac{\partial \Phi}{\partial x_j}\right)$

where the partial derivatives are taken with all other natural variables held constant. It is seen that for every thermodynamic potential there are n(n-1)/2 possible Maxwell relations where n is the number of natural variables for that potential.

## The four most common Maxwell relations

The four most common Maxwell relations are the equalities of the second derivatives of each of the four thermodynamic potentials, with respect to their thermal natural variable (temperature T  or entropy S ) and their mechanical natural variable (pressure p  or volume V ):

$\left(\frac{\partial T}{\partial V}\right)_S = -\left(\frac{\partial p}{\partial S}\right)_V\qquad= \frac{\partial^2 U }{\partial S \partial V}$
$\left(\frac{\partial T}{\partial p}\right)_S = +\left(\frac{\partial V}{\partial S}\right)_p\qquad= \frac{\partial^2 H }{\partial S \partial p}$
$\left(\frac{\partial S}{\partial V}\right)_T = +\left(\frac{\partial p}{\partial T}\right)_V\qquad= - \frac{\partial^2 A }{\partial T \partial V}$
$\left(\frac{\partial S}{\partial p}\right)_T = -\left(\frac{\partial V}{\partial T}\right)_p\qquad= \frac{\partial^2 G }{\partial T \partial P}$

where the potentials as functions of their natural thermal and mechanical variables are:

$U(S,V)\,$ - The internal energy
$H(S,p)\,$ - The Enthalpy
$A(T,V)\,$ - The Helmholtz free energy
$G(T,p)\,$ - The Gibbs free energy

## Derivation of the Maxwell relations

Derivation of the Maxwell equations can be deduced from the differential forms of the thermodynamic potentials:

$dU = TdS-pdV \,$
$dH = TdS+Vdp \,$
$dA =-SdT-pdV \,$
$dG =-SdT+Vdp \,$

These equations resemble total differentials of the form

$dz = \left(\frac{\partial z}{\partial x}\right)_y\!dx + \left(\frac{\partial z}{\partial y}\right)_x\!dy$

And indeed, it can be shown that for any equation of the form

$dz = Mdx + Ndy \,$

that

$M = \left(\frac{\partial z}{\partial x}\right)_y, \quad N = \left(\frac{\partial z}{\partial y}\right)_x$

Consider, as an example, the equation $dH=TdS+Vdp\,$. We can now immediately see that

$T = \left(\frac{\partial H}{\partial S}\right)_p, \quad V = \left(\frac{\partial H}{\partial p}\right)_S$

Since we also know that for functions with continuous second derivatives, the mixed partial derivatives are identical, that is, that

$\frac{\partial}{\partial y}\left(\frac{\partial z}{\partial x}\right)_y = \frac{\partial}{\partial x}\left(\frac{\partial z}{\partial y}\right)_x = \frac{\partial^2 z}{\partial y \partial x} = \frac{\partial^2 z}{\partial x \partial y}$

we therefore can see that

$\frac{\partial}{\partial p}\left(\frac{\partial H}{\partial S}\right)_p = \frac{\partial}{\partial S}\left(\frac{\partial H}{\partial p}\right)_S$

and therefore that

$\left(\frac{\partial T}{\partial p}\right)_S = \left(\frac{\partial V}{\partial S}\right)_p$

Each of the four Maxwell relationships given above follows similarly from one of the Gibbs equations.

## General Maxwell relationships

The above are by no means the only Maxwell relationships. When other work terms involving other natural variables besides the volume work are considered or when the number of particles is included as a natural variable, other Maxwell relations become apparent. For example, if we have a single-component gas, then the number of particles N  is also a natural variable of the above four thermodynamic potentials. The Maxwell relationship for the enthalpy with respect to pressure and particle number would then be:

$\left(\frac{\partial \mu}{\partial p}\right)_{S, N} = \left(\frac{\partial V}{\partial N}\right)_{S, p}\qquad= \frac{\partial^2 H }{\partial p \partial N}$

where μ is the chemical potential. In addition, there are other thermodynamic potentials besides the four that are commonly used, and each of these potentials will yield a set of Maxwell relations.

Each equation can be re-expressed using the relationship

$\left(\frac{\partial y}{\partial x}\right)_z = 1\left/\left(\frac{\partial x}{\partial y}\right)_z\right.$

which are sometimes also known as Maxwell relations.

## See also

This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Maxwell_relations". A list of authors is available in Wikipedia.
Your browser is not current. Microsoft Internet Explorer 6.0 does not support some functions on Chemie.DE