1. What is the difference between the spontaneity and the rate of a chemical reaction? Give an example of a spontaneous but slow chemical reaction.

2. How can a spontaneous but slow reaction be accelerated?

3. What is the form of the equilibrium-constant expression for the reaction 2NO (g) + (g) (g) ? Justify the exponents that you use on the concentration terms.

4. The reaction of Question 3 just as easily could be written
NO(g) + 1/2 (g) (g). What is the equilibrium-constant expression for the reaction written in this way? How are the numerical values of the in this question and Question 3 related?

5. Write the equilibrium-constant expression for the reaction
(g) 2NO (g) + (g). How does the numerical value for this equilibrium constant and that in Question 3 compare?

6. What are the units for the equilibrium constants in Questions 3, 4, and 5?

7. Why is it reasonable that the rate constant for the first-order process in the crabapple war should have units of square feet per second, and in what sense is this an "agility constant"? Why should it also be reasonable for the first-order rate constant in molecular processes to have units of liters per second?

8. What principle about the meaning of equilibrium is used to relate the equilibrium constant to the forward and reverse rate constants?

9. Does a state of equilibrium mean that all activity on the molecular level has stopped? If not, then what does equilibrium mean?

10. What is the definition of mole fraction for a mixture of gases? If pure water is decomposed by electrolysis, and the resulting gases are collected as a mixture, what is the mole fraction of each component?