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15 Nov 2019
A student ran the following reaction in the laboratory at 331 K: When he introduced CH4(B) and CCl4(g) into a 1.00 L evacuated container, so that the initial partial pressure of CH, was 0.796 atm and the initial partial pressure of CCl4 was 0.239 atm, he found that the equilibrium partial pressure of CCl, was 0.191 atm Calculate the equilibrium constant, Kp she obtained for this reaction.
A student ran the following reaction in the laboratory at 331 K: When he introduced CH4(B) and CCl4(g) into a 1.00 L evacuated container, so that the initial partial pressure of CH, was 0.796 atm and the initial partial pressure of CCl4 was 0.239 atm, he found that the equilibrium partial pressure of CCl, was 0.191 atm Calculate the equilibrium constant, Kp she obtained for this reaction.