# Gibbs–Duhem equation

# Gibbs–Duhem equation

In thermodynamics, the **Gibbs–Duhem equation** describes the relationship between changes in chemical potential for components in a thermodynamic system:^{[1]}

`whereis the number ofmolesof componentthe infinitesimal increase in chemical potential for this component,theentropy,theabsolute temperature,volumeandthepressure.is the number of different components in the system. This equation shows that in thermodynamicsintensive propertiesare not independent but related, making it a mathematical statement of thestate postulate. When pressure and temperature are variable, onlyofcomponents have independent values for chemical potential andGibbs' phase rulefollows. The Gibbs−Duhem equation cannot be used for small thermodynamic systems due to the influence of surface effects and other microscopic phenomena.`

^{[2]}The equation is named after Josiah Willard Gibbs and Pierre Duhem.

Derivation

`Deriving the Gibbs–Duhem equation from the fundamental thermodynamic equation is straightforward.`

^{[3]}Thetotal differentialof the extensiveGibbs free energyin terms of itsnatural variablesisSince the Gibbs free energy is the Legendre transformation of the internal energy, the derivatives can be replaced by its definitions transforming the above equation into:^{[4]}

The chemical potential is simply another name for the partial molar Gibbs free energy (or the partial Gibbs free energy, depending on whether N is in units of moles or particles). Thus the Gibbs free energy of a system can be calculated by collecting moles together carefully at a specified T, P and at a constant molar ratio composition (so that the chemical potential doesn't change as the moles are added together), i.e.

- .

The total differential of this expression is^{[4]}

Combining the two expressions for the total differential of the Gibbs free energy gives

which simplifies to the Gibbs–Duhem relation:^{[4]}

Alternative derivation

Another way of deriving the Gibbs-Duhem equation can be found be taking the extensivity of energy into account. Extensivity implies that

`wheredenotes all extensive variables of theinternal energy. The internal energy is thus afirst-order homogenous function. ApplyingEuler's homogeneous function theorem, one finds the following relation when taking only volume, number of particles, and entropy as extensive variables:`

Taking the total differential, one finds

`Finally, one can equate this expressionto the definition ofto find the Gibbs-Duhem equation`

Applications

`By normalizing the above equation by the extent of a system, such as the total number of moles, the Gibbs–Duhem equation provides a relationship between the intensive variables of the system. For a simple system withdifferent components, there will beindependent parameters or "degrees of freedom". For example, if we know a gas cylinder filled with pure nitrogen is at room temperature (298 K) and 25 MPa, we can determine the fluid density (258 kg/m3), enthalpy (272 kJ/kg), entropy (5.07 kJ/kg⋅K) or any other intensive thermodynamic variable.`

^{[5]}If instead the cylinder contains a nitrogen/oxygen mixture, we require an additional piece of information, usually the ratio of oxygen-to-nitrogen.If multiple phases of matter are present, the chemical potentials across a phase boundary are equal.^{[6]} Combining expressions for the Gibbs–Duhem equation in each phase and assuming systematic equilibrium (i.e. that the temperature and pressure is constant throughout the system), we recover the Gibbs' phase rule.

One particularly useful expression arises when considering binary solutions.^{[7]} At constant P (isobaric) and T (isothermal) it becomes:

`or, normalizing by total number of moles in the systemsubstituting in the definition ofactivity coefficientand using the identity:`

^{[8]}

This equation is instrumental in the calculation of thermodynamically consistent and thus more accurate expressions for the vapor pressure of a fluid mixture from limited experimental data.

Ternary and multicomponent solutions and mixtures

`Lawrence Stamper Darkenhas shown that the Gibbs-Duhem equation can be applied to the determination of chemical potentials of components from a multicomponent system from experimental data regarding the chemical potentialof only one component (here component 2) at all compositions. He has deduced the following relation`

^{[9]}xi, amount (mole) fractions of components.

Making some rearrangements and dividing by (1 – x2)2 gives:

or

or

- as formatting variant

The derivative with respect to one mole fraction x2 is taken at constant ratios of amounts (and therefore of mole fractions) of the other components of the solution representable in a diagram like ternary plot.

`The last equality can be integrated fromtogives:`

Applying LHopital's rule gives:

- .

This becomes further:

- .

Express the mole fractions of component 1 and 3 as functions of component 2 mole fraction and binary mole ratios:

and the sum of partial molar quantities

gives

`andare constants which can be determined from the binary systems 1_2 and 2_3. These constants can be obtained from the previous equality by putting the complementary mole fraction x3= 0 for x1and vice versa.`

Thus

and

The final expression is given by substitution of these constants into the previous equation:

See also

Margules activity model

Darken's equations

Gibbs-Helmholtz equation

## References

*A to Z of Thermodynamics*Pierre Perrot ISBN 0-19-856556-9

*American Journal of Physics*.

**42**(6): 478–481. doi:10.1119/1.1987755.

*Fundamentals of Engineering Thermodynamics, 3rd Edition*Michael J. Moran and Howard N. Shapiro, p. 538 ISBN 0-471-07681-3

*Chemical Thermodynamics*. University of Arizona. Archived from the original on 2007-07-07. Retrieved 2007-10-11.

*Fundamentals of Engineering Thermodynamics, 3rd Edition*Michael J. Moran and Howard N. Shapiro, p. 710 ISBN 0-471-07681-3

*The Properties of Gases and Liquids, 5th Edition*Poling, Prausnitz and O'Connell, p. 8.13, ISBN 0-07-011682-2

*Chemical Thermodynamics of Materials, 2004*Svein Stølen, p. 79, ISBN 0-471-49230-2

*Journal of the American Chemical Society*.

**72**(7): 2909–2914. doi:10.1021/ja01163a030.