What is the activation energy for a reaction if k = 1.89 × 10^-8 s^-1 at 540.K and k = 2.45 × 10^-7s^-1 at 601 K?

Question

Quizplus · Accepted Answer

We can use the Arrhenius equation, k = A*exp(-Ea/RT) where, k = rate constant A = pre-exponential factor Ea = activation energy R = gas constant T = temperature Taking the natural logarithm of both sides, ln(k) = ln(A) - Ea/RT We can rearrange this equation as follows to solve for Ea, ln(k1/k2) = (Ea/R)(1/T2 - 1/T1) Substituting the given values, ln(1.89 × 10^-8/2.45 × 10^-7) = (Ea/8.314)(1/601 - 1/540) Simplifying this gives, Ea = -8.314*(1/601 - 1/540)*ln(1.89 × 10^-8/2.45 × 10^-7) Evaluating this equation gives Ea = 113 kJ/mol. Therefore, the answer is choice A.

What Is the Activation Energy for a Reaction If K