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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?

this question is a little hard


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


 \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}}


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