Consider the gas-phase reaction, Cl2(g) + Br2(g) <=> 2 BrCl(g), for which Kp = 32 at 500 K. If the mixture is analyzed and found to contain 0.19 bar of Cl2, 0.29 bar of Br2 and 1.4 bar of BrCl, describe the situation:a) Q > K and more reactants will be made to reach equilibrium. b) Q > K and more products will be made to reach equilibrium. c) Within 1 decimal place, Q = K and the reaction is at equilibriumd) Q < K and more products will be made to reach equilibrium. e) Q < K and more reactants will be made to reach equilibrium.

Explanation:

The reaction quotient, Q, is the actual ratio of concentrations or pressure of products to reactants.

When Q is equal to the equilibrium constant, the reaction is at equilibrium.

When Q > K, the concentrations, or pressures, of the products will have to decrease to reach the equilibrium, thus more reactants will be made.

When Q < K the concentrations, or pressures, of the reactants will have to decrease to reach the equilibrium, thus more products will be made.

Calculate Q:

Therefore, since Q > K, the pressure of the products should decrease to reach the equilibrium, meaning that more reactants will be made, i.e. option a).

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