At 30^$\circ$C, by how much is a reaction's activation energy decreased by the addition of a catalyst if the catalyst triples the reaction rate

Question

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The activation energy is decreased by 2.77 kJ/mol when a catalyst triples the reaction rate, according to the Arrhenius equation. This can be calculated using the equation that relates the rate constant to the activation energy and temperature, showing that a catalyst lowers the activation energy needed for a reaction to proceed, thus increasing the reaction rate.

At 30 ∘\circ∘ C, by How Much Is a Reaction's Activation Energy Decreased

At 30^$\circ$C, by How Much Is a Reaction's Activation Energy Decreased