A student ran the following reaction in the laboratory at 332 K: 2CH2Cl2(g) ---->CH4(g) + CCl4(g) When she introduced

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answerhappygod
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A student ran the following reaction in the laboratory at 332 K: 2CH2Cl2(g) ---->CH4(g) + CCl4(g) When she introduced

Post by answerhappygod »

A student ran the following reaction in the laboratory
at 332 K:

2CH2Cl2(g)
---->CH4(g)
+ CCl4(g)

When she
introduced CH2Cl2(g) at
a pressure of 0.455 atm into a 1.00 L
evacuated container, she found the equilibrium partial
pressure of CCl4(g) to
be 0.201 atm.

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

Kp =
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