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Arrhenius studies the effect of temperat...

Arrhenius studies the effect of temperature on the rate of a reaction and postulted that rate constant varies with temperature exponentially as `k=Ae^(-E_(a)//RT)` . Thuis 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.
If the rate of reaction doubles for `10^(@)C` rise of temperature form 290K to 300K, the activation energy of the reaction will be approximately :

A

40 Kcal `mol^(-1)`

B

12 Kcal `mol^(-1)`

C

60 Kcal `mol^(-1)`

D

70 Kcal `mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
B
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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 activationenergy barrier and increases the rate of reaction. The pre-exponential factor in the Arrhenius equation of a second order reaction has the units

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