# Problem: At 100 °C the equilibrium constant for the reaction COCl2(g) → CO(g) + Cl2(g) has a value of Kc = 2.19 X 10-10. Are the following mixtures of COCl2, CO, and Cl2 at 100 C at equilibrium? If not, indicate the direction that the reaction must proceed in order to reach equilibrium.a) [COCl2] = 2.00 x 10-3 M, [CO] = 3.3 X 10-6 M, [Cl2] = 6.62 X10-6 M

###### FREE Expert Solution

The formula for, reaction quotient, Q, is:

$\overline{){\mathbf{Q}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

Depending on if Q is greater than or less than K, our reaction will shift to attain equilibrium by reaching the equilibrium constant K:

88% (159 ratings) ###### Problem Details

At 100 °C the equilibrium constant for the reaction COCl2(g) → CO(g) + Cl2(g) has a value of Kc = 2.19 X 10-10. Are the following mixtures of COCl2, CO, and Cl2 at 100 C at equilibrium? If not, indicate the direction that the reaction must proceed in order to reach equilibrium.

a) [COCl2] = 2.00 x 10-3 M, [CO] = 3.3 X 10-6 M, [Cl2] = 6.62 X10-6 M