Determine the activation energy in kJ/mol for a first order reaction if its specific rate constant 3.00e-05 s-1 at 350. K and 2.04e+02 s-1 at 510. K Ea= An Arrhenius plot (ln k vs. 1/T) for a second order reaction (2A -> C) produced a straight line with a slope of -7.20e+03 K. What is the value of the Arrhenius pre-exponential if k = 4860 M-1 s-1 at 640 K A= The first order rate constant for a reaction at 530 oC is 2.43e-03 s-1. If the activation energy for the reaction is 220 kJ/mol, what is the rate constant at 630 oC? K=