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

`"log" (k_2)/(k_1) = (E_a)/(19.17) [(T_2 - T_1)/(T_1 T_2)]`
`"log" (0.07)/(0.02) = (E_a)/(19.17)[(700 - 500)/(350000)]`
`"log" 3.5 = (E_a)/(19.17) [200/350000]`
`0.5441 = (E_a)/(19.17) [2/3500]`
`E_a = (0.5441 xx 19.17 xx 3500)/2`
`E_a = 18.25 "kJ mol"^(-1)`