The rate of a reaction increases four times when the temperature changes from 300K to 320 K. Calculate the energy of activation of the reaction. `(R=8.314JK^(-1)mol^(-1))`

The rate of a reaction increases four times when the temperature chang

1.	The rate of a reaction increases four times when the temperature changes from 300K to 320 K. Calculate the energy of activation of the reaction. `(R=8.314JK^(-1)mol^(-1))`
Answer» According to the available data: `k_(2)//k_(1) = 4, T_(1)=300K , T_(2)=320K`. `logK_(2)/k_(1) = E_(a)/(2.303 xx (8.314JK^(-1)mol^(-1)))[(320K-300K)/(320Kxx 300K)]` `0.6020 = (E_(a) xx 20)/((2.303) xx (8.314Jmol^(-1)) xx (320) xx (300))` `E_(a) = (0.6020 xx 2.303 xx 8.314 J mol^(-1) xx 320 xx 300)/(20)` `=55327.6 Jmol^(-1) = 55.328 kJ mol^(-1)`

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The rate of a reaction increases four times when the temperature changes from 300K to 320 K. Calculate the energy of activation of the reaction. `(R=8.314JK^(-1)mol^(-1))`

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