What happens when K is greater than Q in a reaction?

What happens when K is greater than Q in a reaction?

• A. The reaction goes left
• B. The reaction goes right
• C. No shift occurs
• D. The reaction stops

Answer: (B)

When the equilibrium constant (K) is greater than the reaction quotient (Q), it indicates that the products of the reaction are favored over the reactants. Specifically, K reflects the ratio of concentrations of products to reactants at equilibrium, while Q represents the same ratio but at any point in time as the reaction is progressing. In this scenario, if K is greater than Q, it means there are fewer products compared to reactants than what is expected at equilibrium. To reach equilibrium, the reaction must shift to the right, favoring the formation of more products. This shift continues until the concentrations of reactants and products reach the ratio defined by K, where the forward and reverse reactions occur at equal rates. Thus, when K exceeds Q, the reaction proceeds in the direction that increases the concentration of products, confirming that the reaction moves to the right.

When the equilibrium constant (K) is greater than the reaction quotient (Q), it indicates that the products of the reaction are favored over the reactants. Specifically, K reflects the ratio of concentrations of products to reactants at equilibrium, while Q represents the same ratio but at any point in time as the reaction is progressing.

In this scenario, if K is greater than Q, it means there are fewer products compared to reactants than what is expected at equilibrium. To reach equilibrium, the reaction must shift to the right, favoring the formation of more products. This shift continues until the concentrations of reactants and products reach the ratio defined by K, where the forward and reverse reactions occur at equal rates.

Thus, when K exceeds Q, the reaction proceeds in the direction that increases the concentration of products, confirming that the reaction moves to the right.