Question

Which of the following statements is/are CORRECT?1. For a chemical system, if the reaction quotient (Q) is greater than K, reactant must be converted to products to reach equilibrium.2. For a chemical system at equilibrium, the forward and reverse rates of reaction are equal.3. For a chemical system at equilibrium, the concentrations of products divided by the concentrations of reactants equals one.1 only2 only3 only1 and 21, 2, and 3

Answer 1

Explanation:

A chemical equilibrium is defined as the state of reaction in which the rate of forward reaction is equal to the rate of backward reaction.

When Q > $K_{eq}$, then it means that the reaction is proceeding in the backward reaction. Whereas if Q < $K_{eq}$, then it means that the reaction is proceeding in the forward direction. Hence, formation of products will be favored.

On the other hand, if Q = $K_{eq}$, then it means reaction is at equilibrium.

At equilibrium, it is not necessary that the concentrations of products divided by the concentrations of reactants equals one.

Thus, we can conclude that the statement for a chemical system at equilibrium, the forward and reverse rates of reaction are equal, is correct.