The rate constants of a reaction at 500K and 700K are `0.02s^(-1)` and `0.07s^(-1)` respectively. Calculate the values of `E_a` and A.

Explanation

`k_1=0.02s^(-1)=500K`
`k_2=0.07s^(-1),T_2=700K`
R=8.314 J `K^(-1)" mol"^(-1),E_a`=?
`[(T_2-T_2)/(T_1T_2)]`
log=`(0.07)/(0.02)`
=`(E_a)/(2.303xx8.314 JK^(-1)mol^(-1))xx[(700-500)/(700xx500K)]`
`log3.5=(E_a)/(18.JK^(-1)mol^(-1))xx(200)/(700xx500K)`
`5441=(E_a)/(18.15 JK^(-1)mol^(-1))xx(1)/(350xx5K)`
`E_a=0.5441xx19.15xx350xx5" J "mol^(-1)`
=17281.97 `mol^(-1)`
=17.28 kJ `mol^(-1)`