What is the activation energy for a reaction which proceeds 50 times as fast at 400 K as it does at 300 K? Answer in units of J/mol rxn."

Activation energy for the reaction is 39029J/mol

Explanation:

Arrhenius equation is an useful equation that relates rate of reaction at two different temperatures as follows:

Where K₁ and K₂ are rate of reaction, Ea is activation energy and R is gas constant (8.314J/molK

If the reaction at 400K is 50 times more faster than at 300K:

K₂/K₁ = 50 where T₂ = 400K and T₁ = 300K:

Ea = 39029 J/mol

answer seismograph;