Direct Relationship between ΔG° and K

Definition

There's a direct relationship between ΔG° (standard Gibbs free energy change) and K (equilibrium constant). When ΔG° is negative, reactions tend to proceed forward, making products favored over reactants; hence K>1. Conversely, when ΔG° is positive, reactants are favored over products; hence K<1.

Related terms

Equilibrium Constant(K): In chemistry, this term refers to the ratio of concentrations at equilibrium for products over reactants raised to their stoichiometric coefficients.

Standard Gibbs Free Energy Change(ΔG°): This term refers to the change in Gibbs free energy that occurs when a reaction is carried out under standard conditions.

Reaction Quotient(Q): This term refers to the ratio of concentrations or partial pressures of products and reactants at any point in time. It can be used to predict the direction of a reaction.