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 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 70QAP: For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of...

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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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