The Activation energy for the reaction A B+C , at a temperature TK was 0.04606 ~RT ~J / mol . What is the ratio of Arrhenius factor to the Rate constant for this reaction?

Step-by-step solution

The Arrhenius equation is given by k = A e^ -E_a / RT , where k is the rate constant, A is the Arrhenius factor, E_a is the activation energy, R is the gas constant, and T is the temperature. Given E_a = 0.04606 RT J/mol, we substitute this into the Arrhenius equation: k = A e^ -(0.04606 RT) / RT k = A e^ -0.04606 The ratio of the Arrhenius factor to the rate constant is A k . A k = 1 e^ -0.04606 = e^ 0.04606 Using the relation e^x 10^ x / 2.303 : A k = 10^ 0.04606 / 2.303 A k = 10^ 0.02 = 1.0471285... Rounding to