Arrhenius studied the effect of temperature on the rate of a reaction and postulated that rate constant varies with temperature exponentially as k=Ae^(-E_(a)//RT). For most of the reactions, it was found that the temperature coefficient of the reaction lies between 2 to 3. The method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied by studying how much the rate of reaction changes in the presence of catalyst. In most of the cases, it is observed that catalyst lowers the activation energy barrier and increases the rate of reaction. If x is the fraction of molecules having energy greater than E_(a), it will be given by

Arrhenius studied the effect of temperature on the rate of a reaction

1.	Arrhenius studied the effect of temperature on the rate of a reaction and postulated that rate constant varies with temperature exponentially as k=Ae^(-E_(a)//RT). For most of the reactions, it was found that the temperature coefficient of the reaction lies between 2 to 3. The method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied by studying how much the rate of reaction changes in the presence of catalyst. In most of the cases, it is observed that catalyst lowers the activation energy barrier and increases the rate of reaction. If x is the fraction of molecules having energy greater than E_(a), it will be given by
Answer» `X=-(E_(a))/(RT)` ln `x=-(E_(a))/(RT)` `x=e^(E_(a)//RT)` Any of these. Solution :Fraction of molecules having ENERGY greater than `E_a` at temperature `T=e^(-E_(a)//RT)` (BOLTZMANN factor ), i.e., `x=e^(-E_(a)//RT)`. Hence, In `x=-E_a/(RT)`