Which of the following correctly expresses the standard Gibbs free energy change of a reaction in terms of the reaction temperature (T) and equilibrium constant (K) ?

A) ΔG° = e^-K/RT
B) ΔG° = e^K/RT
C) ΔG° = RTlnK
D) ΔG° = -RTlnK
E) none of the above

The correct expression for the standard Gibbs free energy change of a reaction in terms of the reaction temperature (T) and equilibrium constant (K) is ΔG° = -RTlnK. This equation shows that the value of ΔG° is dependent on the temperature and the natural logarithm of the equilibrium constant, with a negative sign indicating that the reaction is thermodynamically favorable if ΔG° is negative.