The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is `:`
( Assume Activation energy and pre-exponential factor are independent of temperature, `ln(2) = 0.693, R = 8.314J - mol^(-1) K^(-1))`

Options

A. `107.2 kJ mol^(-1)`
B. `53.6 kJ mol^(-1)`
C. `26.8 kJ mol^(-1)`
D. `214.4 kJ mol^(-1)`

Answer

A

Explanation

In `(K_(2))/(K_(1))=(E_(a))/(R)((1)/(T_(1))-(1)/(T_(2)))`
In `4=(E_(a))/(8.314)((310-300)/(310 xx 300))`
`2 In 2=(E_(a))/(8.314)((310-300)/(310 xx 300))`
`E_(a)=(0.693 xx 2 xx 8.314 xx 300 xx 310)/(10)=107.2 KJ // mol`