Question

At temperatures above 500 K, phosphorous pentachloride dissociates according to the reaction:
PCl5 -> PCl3 + Cl2
into phosphorous tricloride and molecular chlorine. A PCl5 sample of 1.9 grams is in chemical equilibrium with a temperature of 593 K and a pressure of 0.314 x 105 Pascals. The system is found to have a volume of 2.4 liters.

(a) Determine the equilibrium reaction constant K(T) at 593 K using the law of mass action and assuming ideal gas behavior.

(b) What is the fraction of phosphorous trichloride in the equilibrium gas mixture at 593 K?

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