At 100oC the equilibrium constant for the reaction below has the value of Keq = 2.19 x 10−10. COCl2(g) ⇄ CO(g) + Cl2(g) Are the following mixtures of COCl2, CO, and Cl2 at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. (i) PCOCl2 = 5.00 × 10−2 atm; PCO = 3.31 × 10−6 atm; PCl2 = 3.31 × 10−6 atm (ii) PCOCl2 = 3.50 × 10−3 atm; PCO = 1.11 × 10−5 atm; PCl2= 3.25 × 10−6 atm

(i) not at equilibrium, left to right (ii) equilibrium

(i) equilibrium, (ii) not at equilibrium, right to left

(i) equilibrium, (ii) not at equilibrium, left to right

(i) not at equilibrium, right to left, (ii) equilibrium

(i) equilibrium, (ii) equilibrium

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jufsanabriasa jufsanabriasa · Answer 1 · 2020-02-22T02:37:35+01:00

Answer:

(i) equilibrium, (ii) not at equilibrium, right to left

Explanation:

A reaction is in equilibrium when the ki = keq. If ki>keq, the reaction proceeds from the right to the left and vice versa.

For the reaction:

COCl₂(g) ⇄ CO(g) + Cl₂(g)

keq = 2,19x10⁻¹⁰

[tex]ki = \frac{P_{CO}P_{Cl_2}}{P_{COCl_2}}[/tex]

(i) = [tex]ki = \frac{3,31x10^{-6}3,31x10^{-6}}{5,00x10^{-2}} = 2,19x10^{-10}[/tex]

As ki = keq; the mixture (i) is in equilibrium

(ii) [tex]ki = \frac{1,11x10^{-5}3,25x10^{-6}}{3,50x10^{-3}} = 1,03x10^{-8}[/tex]

As ki > keq, the reaction proceeds from the right to the left.

Thus, right answer is:

(i) equilibrium, (ii) not at equilibrium, right to left

I hope it helps!