SOLVED

31) Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl)eq = 0.22 atm, P(NO)eq = 0.10 atm, P(Cl2)eq = 0.20 atm. 2 NOCl(g) ? 2 NO(g) + Cl2(g) A) 1.0 B) 24 C) 4.1 × 102 D) 4.1 × 10-2 E) 0.97 32) At a certain temperature, nitrogen and hydrogen react to form ammonia: N2(g) + 3 H2(g) ? 2 NH3(g). When initial amounts of N2, H2, and NH3 are mixed, the concentration of NH3 increases. Which statement below is true? A) Kc < Q B) Kc > Q C) Kc = Q D) More information is needed to make a statement about Kc. 33) Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) ? SO3(g) + NO(g)Kc = 0.33 A reaction mixture contains 0.41 M SO2, 0.14 M NO2, 0.12 M SO3 and 0.14 M NO. Which of the following statements is true concerning this system? A) The reaction will shift in the direction of reactants. B) The equilibrium constant will decrease. C) The reaction will shift in the direction of products. D) The reaction quotient will decrease. E) The system is at equilibrium. 34) Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH4(g) ? CO2(g) + 4 Cu(s) + 2 H2O(g)Kc = 1.10 A reaction mixture contains 0.22 M CH4, 0.70 M CO2 and 1.5 M H2O. Which of the following statements is true concerning this system? A) The reaction will shift in the direction of products. B) The equilibrium constant will increase. C) The reaction quotient will increase. D) The reaction will shift in the direction of reactants. E) The system is at equilibrium. 35) Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ? 2 IBr(g)Kc = 1.1 × 102 A reaction mixture contains 0.35 M I2, 0.31 M Br2 and 3.5 M IBr. Which of the following statements is true concerning this system? A) The reaction will shift in the direction of products. B) The reaction will shift in the direction of reactants. C) The reaction quotient will decrease. D) The equilibrium constant will increase. E) The system is at equilibrium. 36) Consider the following reaction and its equilibrium constant: I2(g) ? 2I(g)Kp = 0.209 A reaction mixture contains 0.89atm I2 and1.53 atm I. Which of the following statements is true concerning this system? A) The reaction will shift in the direction of reactants. B) The reaction quotient will increase. C) The reaction will shift in the direction of products. D) The equilibrium constant will decrease. E) The system is at equilibrium. 37) Cyclohexane (C6H12) undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane (MCP) according to the equation: C6H12 ? MCP If Kc = 0.143 at 25°C for this reaction, predict the direction in which the system will shift if the initial concentrations of C6H12 and MCP are 0.0400 M and 0.0200 M, respectively. The system A) will shift left. B) will shift right. C) is already at equilibrium. D) is not at equilibrium and will remain in an unequilibrated state. 38) The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g) + O2(g) ? 2 SO3(g). If initial concentrations are [SO2] = 1.20 M, [O2] = 0.45 M, and [SO3] = 1.80 M, the system is A) at equilibrium. B) not at equilibrium and will remain in an unequilibrated state. C) not at equilibrium and will shift to the left to achieve an equilibrium state. D) not at equilibrium and will shift to the right to achieve an equilibrium state. 39) The equilibrium constant, Kp, equals 3.40 at 25°C for the isomerization reaction: cis-2-butene ? trans-2-butene. If a flask initially contains 2.00 atm of each gas, in what direction will the system shift to reach equilibrium? A) It will shift left. B) It will shift right. C) The system is already at equilibrium. D) The system is not at equilibrium and will remain in an unequilibrated state. 40) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g). N2O4(g) ? 2 NO2(g) Kc = 0.21 [N2O4]eq = 0.029 M A) 1.64 M B) 7.8 × 10-2 M C) 13 × 10-2 M D) 6.1 × 10-3 M E) 164 M