Question

At 100 ∘C the equilibrium constant for the reaction COCl2(g)←−→CO(g)+Cl2(g) has the value Kc=2.19×10−10. Are the following mixtures of COCl2, CO, and Cl2 at 100 ∘C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. Part A [COCl2]=2.00×10−3M, [CO]=3.3×10−6M, [Cl2]=6.62×10−6M , , The reaction is at equilibrium. The reaction will proceed right to attain equilibrium. The reaction will proceed left to attain equilibrium.

Answer 1

Answer:

The reaction will proceed left to attain equilibrium.

Explanation:

Let´s consider the following reaction.

COCl₂(g)⇄CO(g)+Cl₂(g)     Kc = 2.19 × 10⁻¹⁰

To determine whether it is at equilibrium or not, we have to calculate the reaction quotient (Q).

$Q=\frac{[CO].[Cl_{2}]}{[COCl_{2}]} =\frac{3.3 \times 10^{-6} \times 6.62 \times 10^{-6} }{2.00 \times 10^{-3}} =1.09 \times 10^{-8}$

Since Q > Kc, Q has to decrease its value to achieve equilibrium. To do so, it must decrease its numerator (products) and increase its denominator (reactants). All in all, the reaction will proceed left to attain equilibrium.