The rate constants of a reaction at 300 and 320 K are `0.0231 s^-1` and `0.0693 s^-1` respectively. Calculate the value of activation energy of the reaction. [R=8.314J `K^-1 mol^-1`, `log3=0.4771`]

Explanation

`"log" (0.0693)/(0.0231) . (E_a)/(19.17) [(320 - 300)/(96000)]`
`log 3 = (E_a)/(19.17)[20/96000]`
`E_a = (0.4771 xx 19.17 xx 9600)/(2)`
`E_a = 43.9 "kJ mol"^(-1)`