The rate constant for a reaction is 1.5 $\times$ 10^-² s^-¹ at 734 K and 3.9 $\times$ 10^-²s^-¹ at 878 K.What is the activation energy?

Question

Quizplus · Accepted Answer

The activation energy can be calculated using the Arrhenius equation in its logarithmic form: ln(k2/k1) = (Ea/R) * (1/T1 - 1/T2), where k1 and k2 are the rate constants at temperatures T1 and T2, respectively, Ea is the activation energy, and R is the gas constant (8.314 J/mol·K). Given the rate constants and temperatures, the activation energy can be calculated without needing the frequency factor.

The Rate Constant for a Reaction Is 1 ×\times× 10-2 S-1 at 734 K and 3

The Rate Constant for a Reaction Is 1 $\times$ 10^-² S^-¹ at 734 K and 3