SOLVED

81) A mixture containing 0.392 M A(g) and 0.452 M B(g) is allowed to come to equilibrium at 300 K. The reaction 3 A(g) + 2 B(g) ? C(g) + D(g) occurs. At equilibrium, [C] = 0.00128 M. What is the value of Kc? A) 7.35 × 10-3 B) 1.39 × 10-4 C) 1.36 × 102 D) 9.24 × 10-6 E) 7.19 × 106 82) A mixture containing 0.0392 M A(g) and 0.0452 M B(g) is allowed to come to equilibrium at 300 K. The reaction: 3 A(g) + 2 B(g) ? C(g) + D(g) occurs. At equilibrium, [C] = 0.00128 M. What is the value of Kc? A) 2.13 × 10-3 B) 0.849 C) 20.4 D) 4.91 × 10-2 E) 470 83) For the decomposition of ammonium carbamate NH4(NH2CO2)(s) ? 2NH3(g) + CO2(g) Kp = 0.0596 at a certain temperature. A solid sample of ammonium carbamate is introduced into an evacuated container and at equilibrium some solid remains in the container. What is the total pressure in the container? A) 0.738 atm B) 1.17 atm C) 0.930 atm D) 0.179 atm 84) Consider the following equilibrium. A(g) + 3B(g) ? 2C(g) If the initial concentrations are [A(g)] = 1.00 M, [B(g)] = 3.00 M, and [C(g)] = 0, at equilibrium it is found that [C(g)] = 0.980 M. Calculate Kc for this reaction. A) 0.526 B) 0.268 C) 1.26 D) 0.131 85) Consider the following reversible reaction: POCl3(g) ? POCl(g) + Cl2(g)Kc = 0.450 The following initial amounts of reactants and products were mixed: [POCl3] = 0.750 M, [POCl] = 0.550 M, and [Cl2] = 0.150 M. What is the equilibrium concentration of POCl? A) 0.395 M B) 0.155 M C) 0.740 M D) 0.945 M E) 0.360 M 86) Consider the equilibrium system: N2O4(g) ? 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N2O4 was present inside the container, compute PN2O4 at equilibrium. A) 0.398 atm B) 0.113 atm C) 0.602 atm D) 0.285 atm E) 0.715 atm 87) Consider the equilibrium system: N2O4(g) ? 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N2O4 was present inside the container, compute PNO2 at equilibrium. A) 0.398 atm B) 0.113 atm C) 0.602 atm D) 0.285 atm E) 0.715 atm 88) Consider the equilibrium system: N2O4(g) ? 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assume that 1 mole of N2O4 and 2 moles of NO2 are introduced into a 5.0 liter container. What will be the equilibrium value of [N2O4]? A) 0.928 M B) 0.0822 M C) 0.358 M D) 0.379 M E) 0.042 M 89) At 35°C, Kp = 0.315 for the reaction N2O4(g) ? 2 NO2(g), if the initial pressure of NO2(g) in a container is 3.00 atm, what is the equilibrium pressure of N2O4(g)? A) 1.88 atm B) 0.315 atm C) 0.471 atm D) 1.19 atm E) 0.685 atm 90) Consider the equilibrium system: N2O4(g) ? 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assume that 1 mole of N2O4 and 2 moles of NO2 are introduced into a 5.0 liter container. What will be the equilibrium value of [N2O]? A) 0.928 M B) 0.0822 M C) 0.358 M D) 0.379 M E) 0.042 M