The first order reaction `2N_(2)O(g)rarr2N_(2)(g)+O_(2)(g)` has a rate constant of `1.3 xx 10^(-11)s^(-1)` at `270^(@)C` and `4.5 xx 10^(-10)s^(-1)` at `350^(@)C`. What is the activation energy for this reaction ?

Options

A. 15 kJ
B. 30 kJ
C. 68 kJ
D. 120 kJ

Explanation

`log((k_(2))/(k_(1)))=(E_(a))/(2.303R)[(1)/(T_(1))-(1)/(T_(2))]`
`log ((4.5xx10^(-10))/(1.3xx10^(-11)))=(E_(a))/(2.303xx8.314xx10^(-3))[(1)/(543)-(1)/(623)]`
`E_(a)=120 kJ`