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)
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 30P
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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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