A reaction with an activation energy of 84.6 kJ mol^-1 has a rate constant of 0.00681 L mol^-1 s^-1 at 325 K. What is the rate constant at 375 K?

Question

Quizplus · Accepted Answer

We can use the Arrhenius equation to solve for the rate constant at 375 K:
ln(k2/k1) = (Ea/R) ((1/T1) - (1/T2))
where k1 and T1 are the initial rate constant and temperature respectively, k2 and T2 are the new rate constant and temperature respectively, Ea is the activation energy, and R is the gas constant (8.314 J/K*mol).

Plugging in the given values, we get:
ln(k2/0.00681) = (84.6*10^3 J/mol) / (8.314 J/K*mol) * ((1/325 K) - (1/375 K))
ln(k2/0.00681) = 12.23
k2/0.00681 = e^12.23
k2 = 0.443 L/mol*s
Therefore, the best choice is C.

A Reaction with an Activation Energy of 84