The activation energy Ea for a particular reaction is 50.0 kJ/mol. How much faster is the reaction at 322 K than at 310.0 K? (R = 8.314 J/mol
•K)

About two times faster.

Explanation:

Hello!

In this case, since we need a k2/k1 ratio to figure out the increase in the reaction rate for a chemical process, we need to use the following version of the Arrhenius equation:

Thus, we plug in Ea, R and the temperatures to obtain:

Now, we use exponential to obtain:

Thus, we infer that the reaction is about two times faster.

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