2. The second order decomposition of PCl5 has an initial rate of 5.00 10–4 atm/s at 1550 K when the initial partial pressure of PCl5 is 0.100 atm. It reaches equilibrium after 2.72 hours. 2PCl5(g) ⇌ 2P(s) + 5Cl2(g) a. Calculate the rate constant at 1550 K. b. Calculate the equilibrium partial pressure of PCl5. c. Calculate Kp and Kc for the reaction at 1550 K.
2. The second order decomposition of PCl5 has an initial rate of 5.00 10–4 atm/s at 1550 K when the initial partial pressure of PCl5 is 0.100 atm. It reaches equilibrium after 2.72 hours. 2PCl5(g) ⇌ 2P(s) + 5Cl2(g) a. Calculate the rate constant at 1550 K. b. Calculate the equilibrium partial pressure of PCl5. c. Calculate Kp and Kc for the reaction at 1550 K.
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 73AE: Consider the decomposition of the compound C5H6O3 as follows: C5H6O3(g)C2H6(g)+3CO(g) When a 5.63-g...
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2. The second order decomposition of PCl5 has an initial rate of 5.00 10–4 atm/s at 1550 K when the initial partial pressure of PCl5 is 0.100 atm. It reaches equilibrium after 2.72 hours. 2PCl5(g) ⇌ 2P(s) + 5Cl2(g)
a. Calculate the rate constant at 1550 K.
b. Calculate the equilibrium partial pressure of PCl5.
c. Calculate Kp and Kc for the reaction at 1550 K.
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