The Arrhenius equation is used to calculate the activation energy of a reaction from its rate constants at different temperatures. The equation is:
Ea = (2.303 RT) ln (k2/k1)
Where Ea is the activation energy, R is the gas constant (8.314 J/K/mol), T is the temperature (Kelvin), and k1 and k2 are the rate constants at different temperatures.
In this case, we can calculate the activation energy by plugging in the values given:
Ea = (2.303 x 8.314 x 541) ln (4.36 x 10²/3.76 x 10-6)
Ea = 11,721.16 J/mol
Therefore, the activation energy for the reaction is 11,721.16 J/mol.