The Activation energy for the reaction A⟶B+C, at a temperature TK was 0.04606‌RT‌J∕mol. What is the ratio of Arrhenius factor to the Rate constant for this reaction?
The Arrhenius equation is given by: k=Ae−Ea∕RT, where: k is the rate constant A is the Arrhenius factor or pre-exponential factor Ea is the activation energy R is the ideal gas constant ( 8.314J∕mol‌K ) T is the temperature in Kelvin. We are given that the activation energy is 0.04606‌RT‌J∕mol and we need to find the ratio of the Arrhenius factor to the rate constant. This ratio can be obtained by rearranging the Arrhenius equation: A∕k=eEa∕RT Substituting the given value of activation energy: A∕k=e0.04606‌RT‌J∕mol∕RT Simplifying the equation: A∕k=e0.04606 Evaluating the exponential term: A∕k≈1.047 Therefore, the ratio of Arrhenius factor to the rate constant is approximately 1.047. The correct answer is Option D.