Definition
In 1889, the Swedish chemist Svante Arrhenius showed that the rate of a chemical reaction as a function of temperature could be described by the equation
where k is the reaction rate, R is the universal gas constant, E a is the activation energy (the energy required in order for the reactants to react), T is the absolute temperature (K), and A is the so-called pre-exponential factor (associated with collision and transition state theory).
A plot of ln k versus 1/T often yields a straight line, the slope of which is equal to the activation energy of the reaction divided by the universal gas constant (E a/R) and the y-intercept of which is equal to ln A.
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© 2014 Springer-Verlag Berlin Heidelberg
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Bada, J. (2014). Arrhenius Plot. In: Amils, R., et al. Encyclopedia of Astrobiology. Springer, Berlin, Heidelberg. https://doi.org/10.1007/978-3-642-27833-4_108-2
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DOI: https://doi.org/10.1007/978-3-642-27833-4_108-2
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