Question

CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 464 ∘C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm) CO 0.780 Cl2 1.22 COCl2 0.120 What is the equilibrium constant, Kp, of this reaction? Part B The following reaction was performed in a sealed vessel at 767 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.75M and [I2]=2.05M. The equilibrium concentration of I2 is 0.0700 M . What is the equilibrium constant, Kc, for the reaction at this temperature? Express your answer numerically.

Answer 1

P-CO = 0.780

P-Cl2 = 1.22

P-COCl2 = 0.120

If in equilibrium

Kp = PCOCl2 /(P-CO)(P-Cl2)

then

Kp = 0.12/(0.78*1.22) = 0.1261

Kp = 0.1261

B)

K = [HI]^2 / ([H2][I2])

in equilibrium

[H2] = 3.75 - x

[I2] = 2.05 - x

[HI] = 0 +2x

and w eknow that

[I2] = 2.05 - x = 0.007

x = (0.07 - 2.05)/(-1) = 1.98

x = 1.98

then

[H2] = 3.75 - 1.98= 1.77

[I2] = 2.05 - 1.98= 0.07

[HI] = 0 +2x = 2*1.98= 3.96

since

K = [HI]^2 / ([H2][I2])

K = [3.96]^2 / ([1.77][0.07) = 126.56

K = 126.56