A student ran the following reaction in the laboratory at 329 K: ? CH4(g) + CCl4(g) 2CH₂Cl₂(g) When he introduced CH4(g) and CCl4(g) into a 1.00 L evacuated container, so that the initial partial pressure of CH4 was 0.602 atm and the initial partial pressure of CCl4 was 0.262 atm, he found that the equilibrium partial pressure of CCl4 was 0.219 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. =

Principles of Modern Chemistry
8th Edition
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Chapter14: Chemical Equilibrium
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A student ran the following reaction in the laboratory at 329 K:
CH4(g) + CCl4(g) 2CH₂Cl₂(g)
When he introduced CH4(g) and CCl4(g) into a 1.00 L evacuated container, so that the initial
partial pressure of CH4 was 0.602 atm and the initial partial pressure of CCl4 was 0.262 atm,
he found that the equilibrium partial pressure of CCl4 was 0.219 atm.
Calculate the equilibrium constant, Kp, she obtained for this reaction.
Кр
=
?
Transcribed Image Text:A student ran the following reaction in the laboratory at 329 K: CH4(g) + CCl4(g) 2CH₂Cl₂(g) When he introduced CH4(g) and CCl4(g) into a 1.00 L evacuated container, so that the initial partial pressure of CH4 was 0.602 atm and the initial partial pressure of CCl4 was 0.262 atm, he found that the equilibrium partial pressure of CCl4 was 0.219 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр = ?
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