A sample of gaseous PCl5 was introduced into an evacuated flask so the pressure of pure PCl5 would be 0.50 atm at 523 K. However, PCl5 decomposes to gaseous PCl3 and Cl2, and the equilibrium partial pressure of PCL5 in the flask was found to be 0.16 atm. Calculate the Kp for the decomposition reaction PCl5(g) ⇌ PCl3(g) + Cl2(g)
A sample of gaseous PCl5 was introduced into an evacuated flask so the pressure of pure PCl5 would be 0.50 atm at 523 K. However, PCl5 decomposes to gaseous PCl3 and Cl2, and the equilibrium partial pressure of PCL5 in the flask was found to be 0.16 atm. Calculate the Kp for the decomposition reaction PCl5(g) ⇌ PCl3(g) + Cl2(g)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 34QAP: At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105....
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A sample of gaseous PCl5 was introduced into an evacuated flask so the pressure of pure PCl5 would be 0.50 atm at 523 K. However, PCl5 decomposes to gaseous PCl3 and Cl2, and the equilibrium partial pressure of PCL5 in the flask was found to be 0.16 atm. Calculate the Kp for the decomposition reaction
PCl5(g) ⇌ PCl3(g) + Cl2(g)
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