Arrhenius equation

noun Ar·rhe·ni·us equation \ ə-ˈrē-nē-əs- , -ˈrā- \
variants: or less commonly Arrhenius relation

Definition of Arrhenius equation

chemistry
:an equation describing the mathematical relationship between temperature and the rate of a chemical reaction
Note: The Arrhenius equation is sometimes expressed as k = Ae-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 KramerWine Spectator15 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 TodayJuly 2001

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Origin and Etymology of arrhenius equation

after Svante August Arrhenius †1927 Swedish chemist


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