# Internal energy and entropy of a Van der Waals gas

7.4

Consider n moles of a Van der Waals gas. Show that (dU/dV)_T = n^2a/V^2. Hence show that the internal energy is

U = the integral from zero to T of C_vdT - an^2/V + U0

where U0 is a constant. {Hint: Express U = U(T,V)}.

7.5

As in the previous question, consider n moles of Van der Waals gas. Show that

(a) S = the integral from zero to T of C_v/TdT + nRln(V - nb) + S0

where S0 is a constant. {Hint: Use dS = 1/T(dU + PdV)

(b) The equation for a reversible adiabatic process is

T(V -nb)^(nR/C_v) = a constant

if C_v is assumed to be independent of T.

https://brainmass.com/physics/energy/internal-energy-and-entropy-of-a-van-der-waals-gas-531309

#### Solution Preview

The fundamental thermodynamic relation expresses dU in terms of dS and dV

dU = T dS - P dV (1)

If we want to consider U as a function of T and V, then all we need to do is rewrite this in terms of dT and dV. We substitute:

dS = (dS/dT)_V dT + (dS/dV)_T dV (2)

Here (dX/dY)_Z denotes the partial derivative of X w.r.t. Y at constant Z. Substituting (2) in (1) gives:

dU = T (dS/dT)_V dT + (T (dS/dV)_T - P) dV

The term T (dS/dT)_V is the heat capacity at constant volume. The term T dS is always the heat supplied to the system in case of a quasistatic change, so the T times the derivative of S w.r.t. temperature is the heat capacity. Because we keep V constant in the derivative, it is the heat capacity at constant volume. So, we can write:

dU = Cv dT + (T (dS/dV)_T - P) dV (3)

We can simplify the term (dS/dV)_T ...

#### Solution Summary

I explain in detail how the desired expressions for the internal energy and entropy can be obtained.

Find the entropy change of an ideal gas and of a van der Waals gas in case of isothermal expansion in which the volume increases by a factor alpha. Also, find the entropy change in case of a free expansion in which the volume increases by a factor alpha.

In case of the free expansion of the van der Waals gas, find the temperature change.

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