For a strictly spontaneous electrochemical reaction operating under constant temperature and pressur — Thermodynamics and Thermochemistry Chemistry Question

💡 Solution & Explanation

A spontaneous process dictates $\Delta G < 0$. Through the relation $\Delta G^\circ = -RT \ln K_{eq}$, a spontaneous forward reaction corresponds to $K_{eq} > 1$. Additionally, $\Delta G = -nFE^\circ_{cell}$, so a negative $\Delta G$ requires a positive cell electromotive force ($E^\circ_{cell} > 0$).