What does a negative ΔG indicate about the direction of a chemical reaction?

A negative ΔG, or Gibbs free energy change, indicates that a reaction is spontaneous in the forward direction under the given conditions. This means that the reactants have sufficient energy to convert into products, and the process will tend to occur without needing additional energy input.

In thermodynamic terms, a negative ΔG signifies that the products of the reaction have lower free energy compared to the reactants. As a result, the system will favor the formation of products, and the reaction generally proceeds to the right, leading to an increase in product concentration over time. This characteristic is essential in understanding how reactions can be driven toward product formation, and it is a fundamental concept in predicting reaction feasibility.

In contrast, a positive ΔG would indicate that the reaction is non-spontaneous in the forward direction, which may lead to a reverse reaction or equilibrium taking over without significant product formation under the same conditions.