Question

Several rate constants were measured for a particular reaction at several temperatures. It was found that k = 0.0173 at 923 K, and k = 0.00919 at 773 K. What is the activation energy, Ea , for this reaction?

Answer 1

You would use the Arrhenius equation for that. \[\ln({k _{2} \over k _{1}}) = {Ea \over R}({1 \over T _{1}}-{1 \over T _{2}}) \]R = 8.314joules per mol K. Plug and chug.