In general it is observed that the rate of a chemical reaction doubles with every 10 degree rise in temperature. If the generalization holds good for the reaction in the temperature range 295 K to 305 K, what would be the value of activation energy for this reaction ? `[R = 8.314 mol^(-1)JK^(-1)]`

Explanation

`log.(K_(1))/(K_(2)) = (E)/(2.303 R)[(T_(2)-T_(1))/(T_(1) xx T_(2))]`
`log.(2)/(1) = (E_(a))/(2.303 xx 8.314)[(305-295)/(295 xx 305)]`
`0.3010 = (E_(a))/(19.14714)[(10)/(89975)]`
`E_(a) = (0.3010 xx 19.147 xx 89975)/(10)`
`E_(a) = 51906 J mol^(-1)`
`= 51.906 KJ//mol`