5. A 1-liter tank contains 0.095 mole of ammonia, 1.13 moles of nirogen gas, and 1.5 moles of hydrogen gas at equilibrium.
(a) Calculate for the reaction
+ .
(b) Calculate for the reaction
1/2 + 3/2 .
(c) How are the 's calculated for parts (a) and (b) related?
(d) Calculate for the reaction as written in part (a).

6. for the reaction + is 0.00237 at 1000K. If a 10-liter steel tank at this temperature contains 20 moles of and 30 moles of , how many liters of ammonia will be present?

7. For the reaction of Problem 6, in a 10-liter tank at 1000K what will be the equilibrium concentration of hydrogen gas, if 6.8 moles of nitrogen and 10.5 moles of ammonia are present? How many moles of hydrogen gas will be present?

8. The equilibrium constant for the reaction
PCl (g) PCl (g) + (g) is = 0.0224 at 500K.
(a) What are the proper units for this ?
(b) What is the numerical value for , and what are its units?(c) How many moles of will be present at equilibrium in a 100-liter tank at 500K, if there are 4.3 moles of PCl and 132 moles of PCl?
(d) If the pressure on the contents of the tanks is increased, will more, or less, be present at equilibrium?
(e) If the temperature of the tank is raised, will more, or less, be present?

9. The equilibrium constant for the dissociation of gaseous iodine molecules at 1000K is = 3.76 x 10 for the reaction
I (g) 2I (g). An experiment is begun by placing 1.00 mole of pure I in a 2.00-liter box at 1000K. How much atomic iodine will be present after the contents have come to equilibrium?