If the $E_{cell}^{\circ }$ for a given reaction has a negative value, which of the following gives the correct relationships for the values of $\Delta G^{\circ }$ and $K_{eq}$?

Solution & Explanation

\textbf{Answer:} (A) $\Delta G^{\circ }>0$; $K_{eq}<1$ \textbf{Solution:} $\Delta G^{\circ }=-nF{E}_{cell}^{\circ }$. With $E_{cell}^{\circ }$ negative, $\Delta G^{\circ }$ is positive ($\Delta G^{\circ }>0$). Since $\Delta G^{\circ }=-RT\ln K_{eq}$, a positive $\Delta G^{\circ }$ gives $\ln K_{eq}<0$, i.e. $K_{eq}<1$.