In arrhenius law k = a*exp(-e/rt), probability of a collision between molecules to lead to reaction is given by
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The original Arrhenius expression above corresponds to n = 0. Fitted rate constants typically lie in the range −1<n<1. Theoretical analyses yield various predictions for n. It has been pointed out that "it is not feasible to establish, on the basis of temperature studies of the rate constant, whether the predicted T½dependence of the pre-exponential factor is observed experimentally."[4]:190 However, if additional evidence is available, from theory and/or from experiment (such as density dependence), there is no obstacle to incisive tests of the Arrhenius law.
The original Arrhenius expression above corresponds to n = 0. Fitted rate constants typically lie in the range −1<n<1. Theoretical analyses yield various predictions for n. It has been pointed out that "it is not feasible to establish, on the basis of temperature studies of the rate constant, whether the predicted T½dependence of the pre-exponential factor is observed experimentally."[4]:190 However, if additional evidence is available, from theory and/or from experiment (such as density dependence), there is no obstacle to incisive tests of the Arrhenius law.
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