If the change in free energy (ΔG) is , the reaction is spontaneous under the conditions specified. If ΔG is , the reaction is not spontaneous.

The change in free energy (ΔG) is a crucial concept in thermodynamics, particularly in predicting whether a chemical reaction will occur spontaneously under a given set of conditions.

1. Definitions:

   • Spontaneous Reaction: A reaction that will proceed without any external influence. This typically occurs when ΔG < 0.
   • Non-Spontaneous Reaction: A reaction that will not occur without external influence. This occurs when ΔG > 0.

2. Interpreting ΔG:

   • If ΔG < 0: This indicates that the products of the reaction have lower free energy than the reactants, leading to a release of energy, thus making the reaction spontaneous.
   • If ΔG > 0: This suggests that the products possess higher free energy than the reactants, implying that energy must be supplied for the reaction to occur, making it non-spontaneous.

In summary, a negative ΔG indicates spontaneity of a reaction, while a positive ΔG indicates non-spontaneity. If ΔG is equal to zero, the system is in equilibrium, meaning no net change is occurring.