The rate of a reaction quadruples when the temperature changes from $300$ to $310 K$ . The activation energy of this reaction is:

(Assume Activation energy and pre-exponential factor are independent of temperature; $\ln (2) = 0.693; R = 8.314 J - {mol}^{- 1} K^{- 1}$ )

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TestHub · Accepted Answer

ln k 2 k 1 = E a R 1 T 1 - 1 T 2 ln 4 = E a R 1 300 - 1 310 2 × 0 . 693 = E a R 10 300 × 310 E a = 2 × 0.693 × 300 × 310 × 8.314 10 = 107.2 kJ/mol

Chemistry - Chemical Kinetics Question with Solution | TestHub

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