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).

the dependant variable is spilled water

the independent is the heat