The equlibrium constant Kc, for the decomposition of phosgene, COCl2 is 4.63 x 1

Question

The equlibrium constant Kc, for the decomposition of phosgene, COCl2 is 4.63 x 10^-3 at 527 C. COCL2(g) --><-- CO(g) + Cl2 (g) If the reaction mixture at 527 C, the concentration of COCl2, CO, and Cl2 are .25M, .050M and .050M, respectively then which one one of the statements is true? A)The system is at a equilibrium; no change will occur B) The concentrations of CO and Cl2 will increase as the system approaches equilibrium C) The concentration of COCl2 will fall as the system approaches equilibrium D) The concentrations of CO and Cl2 will fall as the system approaches equilibrium Please show how. Thanks

Explanation / Answer

D) The concentrations of CO and Cl2 will fall as the system approaches equilibrium assume 1 L volume, n = PV/RT = 0.760 atm x 1 / 0.08206 x 800 K, n = 0.01158 mole/L, Kc = [CO][Cl2][ / [COCl2], let [CO] = [Cl2] = X, [COCl2] = 0.01158 - X, 4.63x10^-3 = X^2 / (0.01158 - X), X = 0.00536 mol, [CO] = 0.00536 mol, [Cl2] = 0.00536 mol, [COCl2] = 0.00622 mol, total moles = 0.01694, P total = 0.760 atm x (0.01694 / 0.01158) = 1.112 atm, partial pressure CO = 0.352 atm, partial pressure Cl2 = 0.352 atm, partial pressure COCl2 = 0.408 atm, Kp = (0.352)^2 / 0.408 = 0.304 , Kc x RT = 4.63x10^-3 x 0.08206 x 800 = 0.304,

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