**Q1: **

Which of the following statements is false?

- AAccording to the third law of thermodynamics, the entropies of all perfectly crystalline substances must be the same at the absolute zero of temperature (i.e., at ).
- BCalorimetry involves the measurement of heat transfer during a physical or chemical process.
- CThe Joule-Thompson effect relates to the temperature change occurring in a gas during an isenthalpic expansion of the gas.
- DFor any given change of state, the work done by a system in an irreversible process is always greater than that in a reversible process.

**Q2: **

Suppose a 1-mol sample of an ideal gas is expanded isothermally and reversibly from a volume of 10 L to a volume of 20 L at a temperature of 298 K. How much work is done in this process, and what are the changes in the internal energy and entropy of the gas?

- A ; ;
- B ; ;
- C ; ;
- D ; ;

**Q3: **

Consider a process in which a gas is expanded adiabatically and reversibly under constant-pressure conditions, and the amount of work done by the gas in this process is 10 kJ. What changes in the internal energy and entropy of the gas will accompany this process?

- A and
- B and
- CThere is not enough information to determine the values of and .
- D and

**Q4: **

Consider a process in which a 2-mol sample of a certain gas is heated reversibly from 275 K to 375 K under a constant pressure of 1 bar, and the entropy change for the gas is . What will be the value of for a process in which the same gas sample is heated irreversibly from 275 K to 375 K under a fixed pressure of 1 bar?

- A
- B
- CThere is not enough information provided to answer this question.
- D

**Q5: **

Consider a container with rigid, adiabatic walls that is fitted with a partition that separates the container into two chambers (one having twice the volume of the other). The larger chamber contains a 2 mol sample of at 298 K and 1 bar pressure, and the smaller chamber contains a 1 mol sample of at 298 K and 1 bar pressure. The partition between the chambers is removed and the and gases are allowed to mix. This mixing process is isothermal and also adiabatic. Assuming that the gases behave ideally, what would be the (change in internal energy), (enthalpy change), and (entropy change) that accompany this mixing process?

- A ; ; there is not enough information to determine
- B
- C ; ;
- D ; ;

**Q6: **

Suppose you want to cool a sample of from to by a one-step process involving a Joule-Thomson expansion in which the final pressure is 1 bar. The Joule-Thomson coefficient for over the specified temperature range may be taken to be . Determine if the enthalpy change for this cooling process is less than, greater than or equal to zero and calculate to the nearest bar what the initial pressure of the gas must be in order to produce the desired temperature change.

- A and
- B and
- C and
- D and
- E and

**Q7: **

Which of the following processes carried out on a 1-mole sample of a monatomic gas (assumed to exhibit ideal-gas behavior) will result in the greatest increase in the entropy of the gas?

- AIsothermal expansion from a volume of 10 L to a volume of 15 L
- BHeating the gas from 300 K to 600 K under constant-volume conditions
- CReversible adiabatic expansion from a volume of 5 L to a volume of 10 L
- DIsothermal expansion from a volume of 5 L to a volume of 10 L

**Q8: **

Consider 0.1 mol of an ideal gas
contained in a cylinder of volume
2.5 dm^{3} at a
pressure of 1 bar and a temperature
of 301 K. Next, suppose you
consider three different processes for changing the state of the gas sample to one
in which the volume is reduced to
0.25 dm^{3}, the
pressure is increased to 10 bar, and
the temperature is 301 K (the
same as the temperature in the initial state). The paths of the three alternative processes are specified as follows:

Process #1 is a two-step process in which the gas sample is first heated at constant
volume until the pressure reaches a value of
10 bar, and then the gas is
cooled under constant pressure
(10 bar) until its equilibrium
volume is reduced to
0.25 dm^{3} and its
temperature is 301 K.

Process #2 is a two-step process in which the gas sample is first cooled under
constant pressure (1 bar) until its
equilibrium volume is reduced to
0.25 dm^{3}, and then
the gas is heated under constant volume conditions until its pressure reaches a
value of 10 bar and its temperature
is 301 K.

Process #3 is a single-step process in which the gas is isothermally compressed from its initial state to its final state at a fixed temperature of 301 K.

Which of the three processes above would require the least amount of work in effecting the specified change of state, and what would be the (change in internal energy) for this process?

- AProcess #2;
- B Process #1;
- C Process #3;
- DProcess #2;