Question

(a) How does a reaction quotient differ from an equilibrium constant? (b) If \(Q_{c}

Short answer

(a) The reaction quotient (Qc) represents the ratio of product concentrations to reactant concentrations at any particular moment during a reaction, while the equilibrium constant (Kc) represents this ratio when the reaction has reached equilibrium, with no further changes in concentration. (b) If \(Q_c < K_c\), the reaction will proceed in the forward direction to reach equilibrium, converting more reactants into products. (c) For \(Q_c\) to be equal to \(K_c\), the reaction must be at equilibrium, with no further changes in concentrations of reactants and products.

Step-by-step solution

(a) Differences Between Reaction Quotient and Equilibrium Constant

The reaction quotient (Qc) and equilibrium constant (Kc) both represent the ratio of product concentrations to reactant concentrations for a chemical reaction. However, Qc represents this ratio at any particular moment during the reaction's progress, while Kc represents this ratio when the reaction has reached equilibrium, and the concentrations of products and reactants no longer change with time.

(b) Determining Reaction Direction based on Qc and Kc values

To determine the direction of a reaction, we need to compare the values of Qc and Kc: - If \(Q_c < K_c\), it means that the concentration of the products is lower than what would be expected at equilibrium. To reach equilibrium, the reaction needs to proceed in the forward direction, converting more reactants into products. - If \(Q_c > K_c\), it means that the concentration of products is higher than what would be expected at equilibrium. To reach equilibrium, the reaction needs to proceed in the reverse direction, converting more products back into reactants. In this case, as \(Q_c < K_c\), the reaction will proceed in the forward direction to reach equilibrium.

(c) Condition for Qc to be equal to Kc

For the reaction quotient (Qc) to be equal to the equilibrium constant (Kc), the reaction must be at equilibrium. It means that the concentrations of the reactants and products have stopped changing with time and are in a balanced state.