Which values of the equilibrium constant K indicate that there is more product B than reactant A at equilibrium for the reaction A ⇌ B?

• A. K = 1
• B. K < 1
• C. K > 1

Answer: (C)

Verified step by step guidance

1. Recall that the equilibrium constant \(K\) for the reaction \(A \rightleftharpoons B\) is defined as \(K = \frac{[B]_{eq}}{[A]_{eq}}\), where \([B]_{eq}\) and \([A]_{eq}\) are the equilibrium concentrations of products and reactants, respectively.
2. Understand that if \(K = 1\), it means the concentrations of product \(B\) and reactant \(A\) are equal at equilibrium, so \([B]_{eq} = [A]_{eq}\).
3. If \(K < 1\), then \(\frac{[B]_{eq}}{[A]_{eq}} < 1\), which implies that \([B]_{eq} < [A]_{eq}\), meaning there is more reactant \(A\) than product \(B\) at equilibrium.
4. If \(K > 1\), then \(\frac{[B]_{eq}}{[A]_{eq}} > 1\), which means \([B]_{eq} > [A]_{eq}\), so there is more product \(B\) than reactant \(A\) at equilibrium.
5. Therefore, the condition \(K > 1\) indicates that the equilibrium favors the formation of product \(B\) over reactant \(A\).