11 
Definitions. Levine's true/false problems encourage very careful thinking. Note that an intensive variable (like P or T) does not depend on the amount of the substance while an extensive variable (like V or n) does. The difference is important because adding or subtracting intensive variables often results in nonsense. The terms homogeneous and heterogeneous are defined beginning at the bottom of pg 5. A homogeneous system must be composed of one phase; a system containing pure liquid water and pure ice has only one substance but is not homogeneous. If there is more than one component (or, substance) present then the mixing must be at the molecular (or atomic or ionic) level for the system to be homogeneous. 
111 
Still more definitions. The
reasoning necessary for part a, which is true, is
very subtle. See pg. 14. To be really correct Levine should have
specified the normal boiling point.
Note that at the normal boiling point the pressure is 1 atm (for historical reasons) rather than 1 bar. 
112 
A basic exercise in doing conversions. It is useful to remember that there are 760 torr (or, mm Hg) in an atmosphere and 750 torr in a bar. There are 10^{5} Pa (the SI unit for pressure) in 1 bar. (The SI unit for pressure is seldom used because it is inconveniently small). 
122 
Mole relationships in an equilibrium reaction. Dalton's Law of Partial Pressures is important. (Dalton’s Law says that the total pressure, which is what would be measured with a barometer, is the sum of the pressures of the individual gases. The pressures of the individual gases would not change if all the other gases were removed from the system). Being able to do problems like this one will become important in Chpt 6. 
123 
An exercise in symbolic manipulation and in spotting a common error. 
129 
How good is a good vacuum? This problem can be solved by using the perfect gas law. 


114 
More about pressure. How does the density of the fluid in a manometer or barometer affect the height of the column? Does the crosssectional area of the column have any effect? (See pp. 1112 of the textbook). 
143 
An exercise in taking total differentials.
(Please note that the answer in the Solutions Manual appears to be the
answer to a different problem). 
145 
More practice with partial derivatives. 
152 
Yet more practice with partial derivatives. Tthis problem is not short. It is important to avoid making mistakes
while doing it. 
153 
Calculation of a
, k , and their ratio from
simple density measurements. The derivative is approximated by small
differences, eg,
(¶V/¶T)_{P} @ (DV/ DT)_{P} for small changes. 