COMEDK 2024 Shift 2 Paper

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.