Physical Chemistry , 1st ed.

(Darren Dugan) #1
Example 4.7
What is ( S/ V)Tfor a gas that follows a van der Waals equation of state?

Solution
The Maxwell relationship in equation 4.36 shows that ( S/ V)Tis equal to
( p/ T)V. Using the van der Waals equation,

p
V

n


RT

nb




a
V

n
2

2


Taking the derivative ofpwith respect to Tat constant volume gives


T

p

V


V

nR
nb




Therefore, by Maxwell’s relationships,


V

S


T


V

nR
nb




We do not need to measure the entropy changes experimentally. We can get
the isothermal change in entropy versus volume from the van der Waals pa-
rameters.

Example 4.8
In Chapter 1, we showed that


T

p

V









where is the expansion coefficient and is the isothermal compressibility.
For mercury,1.82 10 ^4 /K and 3.87  10 ^5 /atm at 20°C. Determine
how entropy changes with volume under isothermal conditions at this tem-
perature.

Solution
The derivative of interest is ( S/ V)T, which by equation 4.36 is equal to
( p/ T)V. Using the expansion coefficient and the isothermal compress-
ibility:


T

p

V


3

1

.8

.8

7

2





1

1

0

0





(^5) /
4
a


/

t

K

m

4.70 


at
K

m


These do not seem to be appropriate units for entropy and volume. However,
if we note that



at
K

m
 

1

L

0

1

a

.3

tm

2J

101.32 


J/

L

K



we can convert our answer into more identifiable units and find that


V

S


T

 476 

J/

L

K



102 CHAPTER 4 Free Energy and Chemical Potential

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