The rate constants `k_(1)` and `k_(2)` for two different reactions are `10^(25)e^(-4000//T)` and `10^(25)e^(-1000//T)`, respectively. The temperature at which `k_(2)=k_(2)` is

Options

A. `2000/2.303K`
B. `2000K `
C. `3000/2.303K`
D. 1000K

Explanation

`k_1=10^26e^(-4000//T), k_2= 10^25e^(-1000//T)`
if `k_1=k_2" then " 10^26e^(-4000/T)= 10^25e^(-1000//T)`
or `log10-4000/T=-1000/Tor T=3000/2.303`