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

Explanation

log `K_2//K_1=E_(a)|2.303R[(T_2-T_1)//T_(1)T_(2)]`.
log `0.07//0.02 =[E_(a) |2.303xx8.31yJK^(-1)mol^(-))[(700-500)//700xx500]`
`=0.544=E_axx5.714xx10^(-4)//19.15`
`E_(a) =0.544xx19.15//5.714xx10^(-4)=18230.8J`.
Since,
`K=A_e^(-E_a//RT)`
`0.02=Ae^(18230.8//8.314xx500)`
`A=0.02//0.12=1.61`.