Question

The activation energy for a certain is 334.4 KJmol.How many times larger is the rate constant at 610 K than the rate constant at 600 K?

Answer 1

the equation used is
$k=Ae^{ \frac{-E_{a}}{RT} }$

Ea=334.4 KJ mol-1

and R=8.314 *10^(-3) KJ/mol K

T1=600 K  and T2=610 K

therefore

$\frac{k_1}{k_2}= \frac{e^{ \frac{Ea}{RT_1}}}{e^{ \frac{Ea}{RT_2}}}=e^{ \frac{Ea}{RT_1}-{ \frac{Ea}{RT_2}}$

$\frac{k_1}{k_2}=e^{1.0956}$