The Arrhenius equation is a formula for the temperature dependence of reaction rates. The equation was proposed by Svante Arrhenius in 1889, based on the work of Dutch chemist Jacobus Henricus van 't Hoff who had noted in 1884 that Van 't Hoff's equation for the temperature dependence of equilibrium constants suggests such a formula for the rates of both forward and reverse reactions.
Arrhenius' equation gives the dependence of the rate constant k of a chemical reaction on the absolute temperature T (in Kelvin),
A is the pre-exponential factor,
Ea is the activation energy,
and R is the universal gas constant
The equation relates k, the rate constant for a given chemical reaction, with the temperature, T, the activation energy for the reaction, Ea , the pre-exponential factor A, and the universal gas constant,
High temperature and low activation energy favor larger rate constants, and therefore speed up the reaction.
The equation is a combination of the concepts of activation energy and the Maxwell-Boltzmann distribution.