Temperature significantly influences \(k_{eq}\). According to the van't Hoff equation: \[\frac{d \ln k_{eq}}{dT} = \frac{\Delta H}{RT^2}\] where \(\Delta H\) is the enthalpy change of the reaction, \(R\) is the gas constant, and \(T\) is the temperature in Kelvin. For exothermic reactions, increasing the temperature decreases \(k_{eq}\), while for endothermic reactions, increasing the temperature increases \(k_{eq}\).
