What does a negative value of ∆G°' indicate about a reaction?

A negative value of ∆G°' indicates that the reaction is spontaneous under standard conditions. In thermodynamics, the change in free energy (∆G) reflects the spontaneity of a reaction: a negative ∆G signifies that the products of the reaction have a lower free energy than the reactants. This means that the reaction can proceed without the input of energy.

In practical terms, spontaneous reactions are thermodynamically favored and can occur under specific conditions without requiring an external energy supply. This does not necessarily mean that the reaction will happen quickly; it simply indicates that it is thermodynamically favorable to occur.

The context of this reaction is important because it helps understand the driving forces of biochemical processes, including metabolic pathways in cells. Knowing that a reaction is spontaneous can also have implications for understanding cellular processes, natural biological events, and the direction of biochemical reactions in living organisms.