The rate constant at 366 K for a first-order reaction is 7.7 × 10^-3 s^-1 and the activation energy is 15.9 kJ/mol.What is the value of the frequency factor,A,in the Arrhenius equation? (R = 8.314 J/K⋅mol)

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Quizplus · Accepted Answer

The Arrhenius equation is k = A * e^(-Ea/(RT)). Rearranging for A gives A = k / e^(-Ea/(RT)). Substituting the given values (k = 7.7 × 10^-3 s^-1, Ea = 15.9 kJ/mol = 15900 J/mol, R = 8.314 J/K⋅mol, T = 366 K) into the equation gives A ≈ 1.4 s^-1.

The Rate Constant at 366 K for a First-Order Reaction