The rate of a reaction quadruples when temperature charges from 293 K to 312K, Calculate the energy of activation of the reaction assuming that it does not charge with temperature.

Explanation

According to Arrhenius equation
`log ""(k_(2))/(k_(1))=(E_(a))/(2.303)[(1)/(T_(1))-(1)/(T_(2))],`
Given
`[therefore T_(i) =293 K, T_(2) -T_(1) =20K]`
`log ""(4)/(1) =(E_(a))/(2.303 xx(8.314 J mol ^(-1)k^(-1)))xx(20)/(293xx313)`
`E_(a)=(0.6021xx2.303xx8.314xx293xx313)/(20) J mol ^(-1)`
`=52863mol ^(-1)`
`E_(a)=52.863kJ mol ^(-1).`