60. Consider the reaction. CO(g) + Cl2(g) — COCl2(g) Kp = 1.49 × 108 at 373.2 K An equilibrium mixture contains a CO and Cl₂ partial pressure of 0.1702 torr. Calculate the equilibrium partial pressures of the product.

60. Consider the reaction. CO(g) + Cl2(g) — COCl2(g) Kp = 1.49 × 108 at 373.2 K An equilibrium mixture contains a CO and Cl₂ partial pressure of 0.1702 torr. Calculate the equilibrium partial pressures of the product.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.2QE: Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium...

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60. Consider the reaction.
CO(g) + Cl2(g) — COCl2(g)
Kp = 1.49 × 108 at 373.2 K
An equilibrium mixture contains a CO and Cl₂ partial pressure
of 0.1702 torr. Calculate the equilibrium partial pressures of the
product.

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