Page 115 - Modern physical chemistry

References 105

5.15 Calculate the entropy of vaporization of acetic acid at its boiling point, 118.2° C, where its
heat of vaporization is 24,390 J mo!"l.
5.16 An insulated 15.0 ohm resistor initially at 0° C carries a current of 10.0 amp for 1.00 s. If the
mass of the resistor is 5.00 g and its specific heat 0.200, what is its entropy change?
5.17 After 10.0 g ice at 0° C is added to 65.0 g water at 45° C, the ice melts and equilibrium is set
up without interchange of heat with the surroundings. If the heat of fusion of ice is 333.5 J
g-I and the specific heat of water is 1.000, what is the total entropy change in the process?
5.18 An insulated flask containing 1000 g liquid water at -3.8° C is disturbed so that freezing
occurs until equilibrium is established. What is the total entropy change?
5.19 If 25.0 g water evaporates at 100° C, where its heat of vaporization is 2254 J g-I, and mixes
with 25.0 g nitrogen at 100° C and 1.00 atm, what is the entropy change?
5.20 For water at 25° C the coefficient of cubical expansion a is 2.1 x lO-4KI and the compress-
ibility coefficient f3 4.9 x 10"6 atm· l . What is dS when the pressure on 1.00 mol H 20 is increased
from 1.00 to 20.0 atm at 25° C?
5.21 Calculate Cp - Cv for water at 25° C .
5.22 For a condensed phase, determine (a) (iJHliJP)." (b) (iJHliJV)." and (c) (iJV/iJT)s
5.23 With a result from problem 5.22, calculate dB when 1.000 mol water is compressed at 25°
C from 1.00 to 20.0 atm.
5.24 Show that
1
T
What property must a system have for S to decrease as its energy E increases above a certain
value? How would the temperature T vary with E in such a system?
5.25 Show that
( OH) =0
oP T
for an ideal gas.
5.26 A gas follows the equation
PV=RT+aP
where a is a function of T alone. Determine (iJEliJV)l" What does this imply about the
functionE?

References

Books
De Heer, J.: 1986, Phenomenological Thernwdynamics, Prentice- Hall, Englewood Cliffs, NJ, pp.
50-77, 101-189.
In his presentation, De Heer incorporates the best features of various historical papers
and textbooks. Both traditional and axiomatic approaches to the second law are sur-
veyed. Key chemical applications are covered. The third law is introduced and its relation
to the unattainability of absolute zero developed.
Haase, R.: 1971, "Survey of Fundamental Laws," in Jost, W. (editor), Physical Chemistry An
Advanced Treatise, vol. I, Academic Press, New York, pp. 38-74, 86-97.
Haase omits any discussion of cyclic processes. The second law is stated mathematically
and the connection to irreversibility pointed out. The conventional thermodynamic func-
tions are introduced and the third law covered.
Lewis, G. N., Randall, M., Pitzer, K. S., and Brewer, L.: 1961, Thermodynamics, 2nd ed., McGraw-
Hill Book Co., New York, pp. 53-157
Here we have conventional presentations of the second and third laws. But the choice of
symbols and names for some of the thermodynamic functions are outdated.