A reaction is found to have an activation energy of 38.0 kJ mol^-1. If the rate constant for this reaction is 1.60 × 10² L mol^-1s^-1 at 249 K, what is the rate constant at 436 K?

Question

Quizplus · Accepted Answer

The rate constant can be calculated using the Arrhenius equation: k2 = k1 * exp((Ea/R) * ((1/T2) - (1/T1))), where k1 = 1.60 × 10^12 L mol^-1 s^-1, Ea = 38.0 kJ mol^-1, R = 8.314 J K^-1 mol^-1, T1 = 249 K, and T2 = 436 K. Plugging in these values gives k2 = 4.20 × 10^15 L mol^-1 s^-1, which is closest to choice D.

A Reaction Is Found to Have an Activation Energy of 38.0