The direction or spontaneity of a chemical reaction is determined by the change in Gibbs free energy, which is the difference between the enthalpy and entropy changes of the system. Temperature affects the direction of reactions by changing the relative contributions of enthalpy and entropy. For endothermic reactions, which absorb heat, increasing temperature makes the reaction more favorable, as the enthalpy term becomes more negative. For exothermic reactions, which release heat, increasing temperature makes the reaction less favorable, as the entropy term becomes more positive. The relationship between temperature and reaction direction is often expressed by the Van't Hoff equation, which shows how the equilibrium constant varies with temperature.