The activation energy for a reaction at the temperature TK was found to be 2.303 RTJmol−1. The ratio of the rate constant to Arrhenius factor is
10−1
k=Ae−EaRT
Ea=2.303RT
∴kA=e−(2.303RTRT);kA=e−2.303
loge(kA)=loge e−2.303
loge(kA)=−2.303 or 2.303log10(kA)=−2.303
log(kA)=−1;log(AK)=1
∴Ak=anti log1=10 or kA=110=10−1