Thermodynamic functions involving the molecular partition function

Thermodynamic functions involving the molecular partition function describe the macroscopic thermodynamic properties of solids and ideal gases composed of non-interacting particles in the canonical ensemble.

These functions are derived using thermodynamic functions involving the canonical partition function :

Thermodynamic Property Function Derivation
Pressure eq146
Internal energy

eq148

eq157

Entropy eq159
Helmholtz energy eq159a
Enthalpy eq159b
Constant-volume heat capacity eq159c
Gibbs energy eq159d
Chemical potential eq159e

For example, substituting eq166 into eq157 yields the internal energy for a system of  non-interacting, distinguishable particles (such as those in a solid):

Here, is the total single-particle partition function (i.e. eq257), with contributions from translational, rotational, vibrational and electronic degrees of freedom. Eq320 assumes that all components of , including , are defined using absolute energy levels — for example, the vibrational molecular partition function includes the zero-point energy (i.e. eq290). However, if is instead defined relative to the zero-point energy (i.e. eq292), then we need to add back the zero-point energy term giving:

 

Question

Show how eq320 is applicable to a system in which particles can occupy two states with absolute energies 0 and .

Answer

From eq250, . Therefore,

As , , which implies that all particles are in the ground state. As , . This is also physically intuitive. At very high temperatures, thermal energy far exceeds the energy gap . The two energy states are equally populated, and the average energy per particle is . The total internal energy is therefore  times this average energy.

 

The above Q&A demonstrates that although the molecular partition function is defined for a single particle, thermodynamic functions derived from it describe the macroscopic properties of a system. In the case of an ideal gas (composed of non-interacting, indistinguishable particles), substituting eq167 into eq157 also results in eq320. Similarly, for non-interacting, indistinguishable particles, each of the expressions for pressure , enthalpy and constant-volume heat capacity in terms of the molecular partition function is the same. They are given by:

 

Question

Compare the expressions for pressure derived from the canonical partition function and the molecular partition function.

Answer

Comparing eq322 and eq146,

Aspect

Dependence

Canonical (full system) partition function

Molecular (single-particle) partition function

Assumed interactions

Valid for both interacting and non-interacting particles

Assumes non-interacting, indistinguishable particles

Application Real gases

Ideal gases

 

However, the statistical thermodynamic expressions for entropy , as well as for Helmholtz energy, Gibbs energy and chemical potential, differ between distinguishable and indistinguishable particles due to the Gibbs paradox. For an ideal gas, substituting eq167 into eq159 results in:

It follows that the Helmholtz energy expression for an ideal gas is:

For Gibbs energy, we have . Hence,

 

Question

Show that .

Answer

Substituting into eq326 yields , where . For an ideal gas, , where is the number of moles and , with  being the Avogadro constant. So,

where .

Using Stirling’s approximation and ,

where is the molar molecular partition function.

Dividing eq328 through by gives:

 

Substituting eq167 into eq159e gives the expression for the chemical potential of an ideal gas:

 

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