The rate constant for a certain reaction is measured at two different temperatures: Temperature K
376.0°C 4.8 x 10^8
280°C 2.3 x 10^8

Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy for this reaction. Round your answer to significant digits.

22.78KJ/ mol

Explanation:

The computation of activation energy follows by formula:

Given:

Hence, the activation energy for this reaction =22.78KJ/ mol

a non redox reaction occurs when there is not a transfer of electrons. for redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. elements that are reduced gain electrons, and elements that are oxidized lose electrons.

explanation:

i have no clue hope you find the answer