Question
Calculate the activation energy of a reaction whose rate constant is tripled by a rise in temperature in the vicinity of
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Answer :
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We are asked to calculate the activation energy (E_a) for a reaction whose rate constant (k) is tripled by a temperature rise of (10^\circ \text{C}) near (32^\circ \text{C}). We use the Arrhenius equation in its logarithmic form: [ \ln\frac{k_2}{k_1} = \frac{E_a}{R}\left(\frac{1}{T_1} - \frac{1}{T_2}\right) ] Here: [ k_2 = 3 k_1, \quad T_1 = 32^\circ C = 305,\text{K}, \quad T_2 =
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