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

(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

(i) =

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

(ii)

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!

3 1/4 %

explanation:

acid rain does not usually kill trees directly. instead, it is more likely to weaken the trees by damaging their leaves, limiting the nutrients available to them, or poisoning them with toxic substances slowly released from the soil. the main atmospheric pollutants that affect trees are nitrates and sulphates.