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The equilibrium constant, Kp, for the reaction: PCl3 (g) + Cl2 (g) ⇌ PCl5 (g)  is 0.0870 at 300°C. A flask is charged with 0.50 atm PCl3, 0.50 atm Cl2 and 0.20 atm PCl5, at 300°C. The equilibrium partial pressures are PCl3 = Cl2 = 0.66 atm and PCl5 = 0.38 atm. Explain which effect increasing the volume of the system, will have on the mole fraction of Cl2 in the equilibrium mixture.

The equilibrium constant, Kp, for the reaction: PCl3 (g) + Cl2 (g) ⇌ PCl5 (g)  is 0.0870 at 300°C. A flask is charged with 0.50 atm PCl3, 0.50 atm Cl2 and 0.20 atm PCl5, at 300°C. The equilibrium partial pressures are PCl3 = Cl2 = 0.66 atm and PCl5 = 0.38 atm. Explain which effect increasing the volume of the system, will have on the mole fraction of Cl2 in the equilibrium mixture.

Principles of Modern Chemistry
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 33P
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The equilibrium constant, Kp, for the reaction:

PCl3 (g) + Cl2 (g) ⇌ PCl5 (g)  is 0.0870 at 300°C.

A flask is charged with 0.50 atm PCl3, 0.50 atm Cl2 and 0.20 atm PCl5, at 300°C.

The equilibrium partial pressures are PCl3 = Cl2 = 0.66 atm and PCl5 = 0.38 atm.

Explain which effect increasing the volume of the system, will have on the mole fraction of Cl2 in the equilibrium mixture.

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