1. The equilibrium constant for the reaction



at a given temperature is = 2.5 X 10. The quantities and are the forward and reverse rate constants. If the reverse rate constant has a numerical value of 151 atm sec, what is the value of ?

2. The equilibrium constant for the reaction
+ 2NO at 2130C is 2.5 x 10. What are the units for this equilibrium constant? What is the numerical value for the equilibrium constant for the reaction NO 1/2 + 1/2 ?

3. Does the synthesis of NO as described in Problem 2 occur with the absorption, or emission, of heat? For the following conditions, decide whether the gas mixture described is at equilibrium, or whether a net forward or reverse reaction will take place spontaneously:
(a) A 1-liter box contains 0.020 mole of NO, 0.010 mole of , and 0.020 mole of at 2130C.
(b) A 20-liter box contains 1 x 10 mole of , 1 x10 mole of , and 2 x 10 mole of NO at 2130C.

(c) A 1-liter box contains 1.00 mole of , 16 moles of , and 0.2 mole of NO at 2500C.

4. At 25C and 20 atm pressure, the reaction
(g) + (g) (g) has a standard enthalpy change of -22.1 kcal per mole of .
(a) If the temperature is raised to 300C while the pressure is held at 20 atm, will more ammonia be present at equilibrium, or less?
(b) If the pressure is increased to 30 atm while the temperature remains at 25C, will more, or less, ammonia be present, compared with initial conditions?
(c) If half the ammonia is removed and the system is allowed to come to equilibrium again, will the amount of nitrogen gas present increase, or decrease?
(d) What will be the effect on the original equilibrium mixture if a catalyst for ammonia synthesis is added?