Question

For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a CO concentration of 0.1470 M and a Cl2 concentration of 0.170 M at 1000 K. What is the equilibrium of (1)CO, (2) CL2, (3) COCL2; at 1000K?

Answer 1

For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g)

A reaction mixture initially contains a CO concentration of 0.1470 M and a Cl2 concentration of 0.170 M at 1000 K. What is the equilibrium of (1)CO, (2) CL2, (3) COCL2; at 1000K?

Kc = 225, fr K = [COCl2]/([CO][Cl2])

initially

[COCl2] = 0

[CO] = 0.1470

[Cl2] = 0.170

in equilbirium

[COCl2] = 0 +x

[CO] = 0.1470 - x

[Cl2] = 0.170 - x

substitute in Kc

Kc = 225, for K = [COCl2]/([CO][Cl2])

K = [COCl2]/([CO][Cl2])

225 = x / ((0.1470 - x)(0.170 - x))

225 * ( 0.1470 *0.170 - (0.170 +0.1470 )x + x^2) = x

( 0.1470 *0.170 - (0.170 +0.1470 )x + x^2) = 0.004444x

0.02499-0.317x + x^2 =  0.004444x

x^2 - (0.317 + 0.004444)x + 0.02499 = 0

x^2 - 0.321444x + 0.02499 = 0

x = 0.13171

[COCl2] = 0 +x = 0.13171

[CO] = 0.1470 - x = 0.147-0.13171 = 0.01529 M

[Cl2] = 0.170 - x = 0.17-0.13171 = 0.03829 M