# Thermodynamics Problem Set

This problem set was developed by S.E. Van Bramer for Chemistry 145 at Widener University.

1. Nitrogen Oxides are very important species in atmospheric chemistry. They are critical for a number of reactions that contribute to photochemical smog. The major anthropogenic (man made) source of NO is from the following reaction:

N2 + O2 <--> 2 NO

In this problem you will study the temperature dependence of this reaction to learn how the emission of NO may be reduced. Answer the following questions (assume that H is constant at each temperature):

1. What is [delta]Hrxn, [delta] Srxn, [delta] Grxn, and K at

1. 25 °C
2. 1000 °C
3. 2000 °C
4. 3000 °C

2. The atmospheric pressure of N2 is 0.80 atm and O2 is 0.20 atm. Determine the equilibrium pressure of NO at each temperature.

3. At high temperatures the above reaction is fast enough that the system can reach equilibrium. When exhaust gases leave a combustion chamber (an automobile, truck, boiler, or power plant) the air quickly cools. At the lower temperature the reaction is much slower so the reaction does not return to equilibrium. Would lowering the combustion temperature from 3000 °C to 2000 °C or even to 1000 °C have any effect on the NO emission?

4. Dr Madigoski and I recently purchased an instrument to determine the concentration of NO and NO2 with funds provided by a grant from the National Science Foundation. Based upon the Gibbs free energy, which of the following reactions is a feasible mechanism for converting NO into NO2?

1. 2 NO + O2 <--> 2 NO2
2. NO + O3 <--> NO2 + O2
3. NO + NO3 <--> 2 NO2
4. CH3OO + NO <--> NO2 + CH3O

2. Calculate [delta] G at 20°C for the reaction H2 + I2 <--> 2 HI. Starting with 1.0 atm H2 and 1.0 atm I2. What is [delta] G when:

1. 0.1% has reacted
2. 1% has reacted
3. 10% has reacted
4. 50% has reacted
5. 90% has reacted
6. 99% has reacted
7. 99.9% has reacted