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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Chapter12: Chemical 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.
Transcribed Image Text: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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