## Definition of Arrhenius equation

**:**an equation describing the mathematical relationship between temperature and the rate of a chemical reaction

^{-E/RT}where

*k*is the rate of chemical reaction,

*A*is a constant depending on the chemicals involved,

*E*is the activation energy,

*R*is the universal gas constant, and

*T*is the temperature.

- What we’re really looking at here is what’s known as the Arrhenius equation. Svante August Arrhenius was a Nobel Prize winning Swedish chemist around the turn of the century. He observed that an increase of 18° F will about double the rate of the average chemical reaction. And the same holds true in reverse: the colder the temperature, the less the rate of reaction.
- —Matt Kramer,
*Wine Spectator*, 15 May 1998

- Ideas from elementary statistical mechanics allowed determination of the energies displayed in the figure: The activation barriers were obtained using the Arrhenius relation, whereas the Boltzmann relation was used to determine the bound-state energy difference.
- —Harold J. W. Zandvliet et al.,
*Physics Today*, July 2001