Arrhenius equation

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

Arrhenius relation

Definition of Arrhenius equation

chemistry

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

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Origin and Etymology of arrhenius equation

after Svante August Arrhenius †1927 Swedish chemist


First Known Use: 1902


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