The rate constant at 373 K for a certain reaction is 8.29 × 10−⁴ s−¹ and the activation energy is 12.0 kJ/mole.What is the value of the constant,A,in the Arrhenius equation?

Question

Quizplus · Accepted Answer

The Arrhenius equation is k=Aexp(Ea/RT), where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin. To find A, we need to rearrange the equation to isolate it: A=k/exp(Ea/RT). Substituting the given values, we get A=8.29 × 10^-14 s^-1 exp(12000 J/mol / (8.314 J/mol*K * 373 K)) = 0.0398 s^-1. Therefore, the correct answer is B.

The Rate Constant at 373 K for a Certain Reaction