At 500 K, the Kp of the reaction PCl5 (g) = PCl3 (g) + Cl2 (g) is 0.497. In a chamber at 500 K, we mix the gases, and their partial pressures are given by P (PCl5(g)) = 0.325 atm, P(PCl3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm. Which of the following statements is/are correct regarding how the mixture will proceed to reach equilibrium? a) The partial pressure of PCl3 will increase during the reaction course to reach equilibrium. b) The partial pressure of PCl5 will increase during the reaction course to reach equilibrium. c) The reaction Gibbs energy change ∆G is less than zero for the above condition: P (PCl5(g)) = 0.325 atm, P(PCl3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm. Note that the question is about ∆G not ∆Go. a) only b) only c) only a) and b) b) and c) a) and c) a), b) and c) None of the 3 statements is correct.
At 500 K, the Kp of the reaction PCl5 (g) = PCl3 (g) + Cl2 (g) is 0.497. In a chamber at 500 K, we mix the gases, and their partial pressures are given by P (PCl5(g)) = 0.325 atm, P(PCl3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm. Which of the following statements is/are correct regarding how the mixture will proceed to reach equilibrium? a) The partial pressure of PCl3 will increase during the reaction course to reach equilibrium. b) The partial pressure of PCl5 will increase during the reaction course to reach equilibrium. c) The reaction Gibbs energy change ∆G is less than zero for the above condition: P (PCl5(g)) = 0.325 atm, P(PCl3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm. Note that the question is about ∆G not ∆Go. a) only b) only c) only a) and b) b) and c) a) and c) a), b) and c) None of the 3 statements is correct.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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At 500 K, the Kp of the reaction PCl5 (g) = PCl3 (g) + Cl2 (g) is 0.497. In a chamber at 500 K, we mix the gases, and their partial pressures are given by P (PCl5(g)) = 0.325 atm, P(PCl3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm.
Which of the following statements is/are correct regarding how the mixture will proceed to reach equilibrium?
a) The partial pressure of PCl3 will increase during the reaction course to reach equilibrium.
b) The partial pressure of PCl5 will increase during the reaction course to reach equilibrium.
c) The reaction Gibbs energy change ∆G is less than zero for the above condition: P (PCl5(g)) = 0.325 atm, P(PCl3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm. Note that the question is about ∆G not ∆Go.
a) only
b) only
c) only
a) and b)
b) and c)
a) and c)
a), b) and c)
None of the 3 statements is correct.
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