According to the Arrhenius equation:

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

In Arrhenius equation, factor $e^{- E a / R T}$ corresponds to fraction of reactant molecules that have kinetic energy equal to activation energy.

The pre-exponential factor depends on the frequency at which collision between reactant molecules per unit volume per unit time occur, irrespective of their energy.

Higher the magnitude of activation energy of a reaction, stronger is the temperature dependence of its rate constant.

answer is B, C, D.

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Detailed Solution

B) Rate constant increases with increases in temperature. This is mainly due to a greater number of collisions whose energy exceeds the activation energy.
C) Higher the magnitude of activation energy of a reaction, stronger is the temperature dependence of its rate constant.
D) The pre-exponential factor depends on the frequency at which collision between reactant molecules per unit volume per unit time occur, irrespective of their energy.

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