A chemical reaction has an equilibrium constant of 2 × 10⁶. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

Question

Quizplus · Accepted Answer

An equilibrium constant represents the ratio of products to reactants at equilibrium. Therefore, if the equilibrium constant is not equal to 1, then the forward and reverse reaction rates are not equal. In this case, the equilibrium constant is quite large (greater than 1), indicating that the reaction strongly favors product formation at equilibrium. Therefore, we can conclude that the forward and reverse reaction rates must be significantly different, and that the forward and reverse reactions are still occurring at significant rates (not stopped). The limiting reactant has no relevance to the equilibrium constant or the conditions at equilibrium, so we cannot make any conclusions about it based on the given information.

A Chemical Reaction Has an Equilibrium Constant of 2 ×