Question

The equilibrium constant in terms of pressures for the reaction COCl2(g) = CO(g) + Cl2(g)

is Kp = 5.00 at 873 K.

(a) A pure sample of gaseous phosgene, COCl2(g), is introduced into a rigid flask at a temperature of 873 K so that its original pressure is 0.141 atm. Calculate the fraction of this starting material that is converted to products at equilibrium.

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(b) A second sample of phosgene is introduced into a rigid flask at a temperature of 873 K, this time at an original pressure of 4.21 atm. Again, calculate the fraction of the starting material that is converted to products at equilibrium.

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Answer 1