Gibbs Free Energy: Unlocked

Predicting the Direction of Reactions

The Gibbs free energy, a fundamental concept in thermodynamics, unlocks the ability to predict the spontaneity of chemical reactions. It provides a quantitative measure of the maximum non-volume expansion work that can be extracted from a closed system or the minimum work required to drive a reaction in the non-spontaneous direction.

Delta G and Reaction Direction

The change in Gibbs free energy, denoted as ΔG, is a key indicator of the direction of a reaction. If ΔG is negative (ΔG < 0), the reaction is spontaneous and will proceed in the forward direction, releasing energy to its surroundings. Conversely, if ΔG is positive (ΔG > 0), the reaction is non-spontaneous and external work is required to drive it in the forward direction. When ΔG is zero (ΔG = 0), the reaction is at equilibrium, with no net change occurring.