In general it is observed that the rate of a chemical reaction becomes double for every `10^@` rise in temperature. If this generalisation holds for a reaction in the temperature range 2908 K to 398 K, what would be the value of activation energy for the reaction.
(R=8.314 J `K^(-1)mol^(-1)`)

Explanation

`lay 2 = (E_a)/(2.303 xx 8.314) ((308 - 298))/((308)(298))`
`E_a = (0.301 xx 19.17)/(0.0001089)`
`E_a = 52.922 kJ mol^(-1)`