Which of the following thermodynamic equations and conditions are correct for a reversible reaction — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

Option A is the fundamental isotherm equation relating non-standard free energy to the reaction quotient $Q$. Option B is false; at equilibrium, $\Delta G = 0$, but standard free energy $\Delta G^\circ$ is only zero if $K=1$. Option C is correct because $\Delta G^\circ = -RT \ln K$; if $\Delta G^\circ$ is positive, $\ln K$ must be negative, meaning $K < 1$. Option D is the thermodynamic definition of spontaneity.