SOLVED

91) 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 10 atm at equilibrium and that initially only N2O4 was present inside the container, compute PN2O4 at equilibrium. A) 7.98 atm B) 8.88 atm C) 1.12 atm D) 1.01 atm E) 8.99 atm 92) Consider the equilibrium system: N2O4(g) ? 2NO2(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 10 atm at equilibrium and that initially only N2O4 was present inside the container, compute PNO2 at equilibrium. A) 7.98 atm B) 8.88 atm C) 1.12 atm D) 1.01 atm E) 8.99 atm 93) A mixture, containing 0.0750 M HCl(g) and 0.0330 M O2(g) is allowed to come to equilibrium at 480°C. 4HCl(g) + O2(g) ? 2Cl2(g) + 2H2O(g) At equilibrium [Cl2] = 0.030 M. What is the value of Kc? A) 1.1 × 10-3 B) 890 C) 0.13 D) 1.3 E) 480 94) 4.000 mol chlorine and 2.000 mol bromine were placed in a 50.0 L container and kept at 293 K until equilibrium was achieved for the reaction: Br2(l) + Cl2(g) ? BrCl(g) At the point of equilibrium there were 82.63 g of Br2(l). Compute the value of Kc for this reaction. A) 0.0699 B) 1.18 C) 0.849 D) 3.50 E) 0.849 95) 4.000 mol chlorine and 2.000 mol bromine were placed in a 50.0 L container and kept at 293 K until equilibrium was achieved for the reaction: Br2(l) + Cl2(g) ? 2 BrCl(g) At the point of equilibrium there were 82.63 g of Br2(?). Determine the total pressure in the 50.0 L container at equilibrium. A) 0.110 atm B) 2.64 atm C) 0.180 atm D) 1.43 atm E) 1.21 atm 96) For the reaction: PCl3(g) + Cl2(g) ? PCl5(g) at 85°C, Kp = 1.19 If one starts with 2.00 atm pressure of PCl3, 1.00 atm pressure of Cl2 and no PCl5, what is the partial pressure of PCl5(g) at equilibrium? A) 0.167 atm B) 0.739 atm C) 0.621 atm D) 0.465 atm E) 0.553 atm 97) Consider the following reaction: POCl3(g) ? POCl(g) + Cl2(g) Kc = 0.450 A sample of pure POCl3(g) was placed in a reaction vessel and allowed to decompose according to the above reaction. At equilibrium, the concentrations of POCl(g) and Cl2(g) were each 0.150 M. What was the initial concentration of POCl3(g)? A) 0.225 M B) 0.200 M C) 0.633 M D) 0.483 M E) 0.350 M 98) Consider the following reaction occurring at 960 K: CO2(g) + H2(g) ? CO(g) + H2O(g) At equilibrium, the concentrations of reactants and products are: [CO2] = 0.0400 M, [H2] = 0.0220 M, [CO] = 0.0240 M, and [H2O] = 0.0190 M. This equilibrium is perturbed by adding CO2(g) to the system such that when a new equilibrium is reached, the concentration of CO2 is 0.050 M. What is the concentration of H2(g) at this equilibrium? A) 0.050 M B) 0.482 M C) 0.462 M D) 0.300 M E) 0.0504 M 99) One of the reactions in the gasification of coal is CO(g) + 3H2(g) ? CH4(g) + H2O(g)ΔH° = -237 kJ For each of the following changes, explain the effect (increase, decrease, no effect) on the number of moles of CH4(g) produced. (a) increase the concentration of H2O(g) (b) decrease the volume of the container (c) add a catalyst