Gibbs free energy (ΔG) must be negative for a reaction to be:

A) Endothermic

B) Spontaneous (thermodynamically favorable)

C) At equilibrium

D) Endergonic

Explanation

ΔG < 0: spontaneous (exergonic). ΔG = 0: equilibrium. ΔG > 0: non-spontaneous. ΔG = ΔH − TΔS.