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

💡 Solution & Explanation

A thermodynamically spontaneous process strictly dictates that the total change in Gibbs free energy is negative ($\Delta G < 0$). Through the relation $\Delta G^\circ = -RT \ln K_{eq}$, a spontaneous forward reaction corresponds to an equilibrium constant greater than 1 ($K_{eq} > 1$). Additionally, $\Delta G = -nFE_{cell}$, so a negative $\Delta G$ mathematically requires a positive cell electromotive force ($E^\circ_{cell} > 0$).