Question

At 100 °C, the equilibrium constant for the reaction:

COCl₂ (g) ⇌ CO (g) + Cl₂ (g) has the value Kc = 2.19x 10⁻¹⁰. Are the following mixtures of COCl₂ at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium.
[COCl₂] = 2.19 x 10⁻¹⁰ M, [CO] = 3.3x10⁻⁶ M, [Cl₂] = 6.62 x 10⁻⁶ M

a. At equilibrium
b. Shift to the left
c. Shift to the right
d. none of the above

Answer 1

The mixture is not at equilibrium and must shift to the right to achieve equilibrium.

Step-by-step explanation:

To determine if a mixture is at equilibrium for the reaction COCl₂ (g) ⇌ CO (g) + Cl₂ (g), we compare the concentrations of each species in the mixture to the equilibrium concentrations given by the equilibrium constant (Kc). The given concentrations are [COCl₂] = 2.19 x 10⁻¹⁰ M, [CO] = 3.3 x 10⁻⁶ M, [Cl₂] = 6.62 x 10⁻⁶ M.

Since the concentrations of all three species in the mixture do not match the equilibrium concentrations determined by the equilibrium constant, we can conclude that the mixture is not at equilibrium. In order to achieve equilibrium, the reaction must proceed in the direction that decreases the concentration of COCl₂ and increases the concentrations of CO and Cl₂. Therefore, the answer is (c) Shift to the right.