A student ran the following reaction in the laboratory at 331 K: 2CH2Cl2(g) CH4

Jul 29th, 2015
Price: $5 USD

Question description

A student ran the following reaction in the laboratory at 331 K:

2CH2Cl2(g) CH4(g) + CCl4(g)

When he introduced CH2Cl2(g) at a pressure of 0.426 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CCl4(g) to be0.188 atm. 

Calculate the equilibrium constant, Kp, he obtained for this reaction. 

Kp = 

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School: Duke University

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