Definition of Arrhenius equation
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 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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