1. a) The equilbrium constant for the water-gas shift reaction is 5.0 at 400 oC:

Question

1. a) The equilbrium constant for the water-gas shift reaction is 5.0 at 400 oC: CO(g) + H2O(g) ? CO2(g) + H2(g) Determine Qc if the following amounts (in moles) of each component is placed in a 1.0 L container. CO 0.46 H2O 0.64 CO2 0.66 H2 0.63 b) Determine Qc if the following amounts (in moles) of each component is placed in a 1.0 L container. CO 0.32 H2O 0.10 CO2 0.95 H2 0.85 2. Consider 1.20 mol of carbon monoxide and 4.00 mol of chlorine sealed in a 3.00 L container at 476 oC. The equilibrium constant, Kc, is 2.50 (in M-1) for CO(g) + Cl2(g) ? COCl2(g) Calculate the equilibrium molar concentration of CO.

Explanation / Answer

FOLLOW THIS With given equilibrium pressures you can calculate the value of Kp: Kc = [H?O]?[CO] / ([CO?]?[H?]) = 0.48 ? 0.48 / (0.24 ?0.24) = 4 The setup ICE table ---------- [CO?]--------- [H?]--------- [H?O]--------- [CO] I---------- 0.86---------- 0.86--------- 0.48----------- 0.48 C--------- (-x)----------- (-x)----------- (+x)----------- (+x) E------- (0.86-x)---- (0.86-x)------ (0.48+x)---- (0.48+x) Substitute to equilibrium equation adn solve for x Kc = [H?O]?[CO] / ([CO?]?[H?]) 4 = (0.48 + x)

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