The rate constant of a reaction is 1.78 x 10^-3 s^-1 at 27°C and 2.57 x 10^-2 s^-1 at 37°C. Calculate the activation energy (in kJ/mol) for the reaction. [R = 8.314 J/mol K]
Correct: B
Using the Arrhenius equation: ln(k2/k1) = (Ea/R) * (1/T1 - 1/T2). ln(2.57 x 10^-2 / 1.78 x 10^-3) = (Ea/8.314) * (1/300 - 1/310). Solving for Ea, we get approximately 63969 J/mol, which is about 64.0 kJ/mol.