13. A study of the system, 4NH3(g)+7O2(g)2N2O4(g)+6H2O(g), was carried out. A system was prepared with [NH3]=[O2]=3.60M as the only components initially. At equilibrium, [N2O4] is 0.60M. Calculate the equilibrium concentration of O2. a. 3.00M b. 2.40M c. 1.50M d. 2.10M e. 3.30M 14. For the reaction system, 2SO2(g)+O2(g)2SO3(g), the equilibrium concentrations are: SO3:0.120MSO2:0.860MO2:0.330M. Calculate the value of Kc for this reaction. a. 1.31 b. 2.51 c. 0.423 d. 0.872 c. 0.0590 15. At 1500C the system, 2NO(g)N2(g)+O2(g), was allowed to come to equilibrium. The equilibrium concentrations were: NO(g)=0.00035M,N2(g)=0.040 M, and O2(g)=0.040M. What is the value of K for the system at this temperature? a. 1.5106 b. 7.7105 c. 2.2101 d. 4.6 e. 1.3104 16. A chemical system is considered to have reached equilibrium when a. the rate of consumption of each of the product species by the reverse reaction is equal to the rate of production of each of the reactant species by the reverse reaction. b. the sum of the concentrations of each of the reactant species is equal to the sum of the concentrations of each of the product species. c. the rate of production of each of the product species is equal to the rate of consumption of each of the product species by the reverse reaction. d. the rate of production of each of the product species is equal to the rate of consumption of each of the reactant species by the reverse reaction. e. the rate of production of each of the product species by the forward reaction is equal to the rate of production of each of the reactant species by the reverse reaction