According to the Arrhenius equation,

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a high activation energy usually implies a fast reaction.

rate constant increases with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy.

higher the magnitude of activation energy, stronger is the temperature dependence of the rate constant

the pre-exponential factor is a measure of the rate at which collisions occur, irrespective of their energy.

answer is B, C, D.

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Detailed Solution

As activation energy increases. Rate of reaction decreases

Arrhenius equation:

$k = {Ae}^{- E_{a} / RT}$

Rate of reaction increases with increase the temperature. The pre-exponential factor, A is a measure of the rate at which collisions occur, irrespective of their energy. More is the magnitude of activation energy, stronger is the temperature dependence of the rate constant

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