The rate of a reaction quadruples when the temperature changes from 27^\circC to 57^\circC. Calculate the energy of activation. (Given R = 8.314\ \mathrm{J\,K^{-1}\,mol^{-1}}, \log 4 = 0.6021.)

Question

Vishal Gupta · Accepted Answer

D. \log\frac{k2}{k1} = \frac{Ea}{2.303R}\left(\frac{1}{T1} - \frac{1}{T2}ight) with k2/k1 = 4, T1 = 300 K, T2 = 330 K: 0.6021 = \frac{Ea}{2.303 	imes 8.314} 	imes \frac{30}{300 	imes 330} \Rightarrow Ea \approx 38.04 kJ/mol.

Chemical Kinetics

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