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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.

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As activation energy increases. Rate of reaction decreases,K =Ae -Ea /RT K α T by Increasing temperature rate constant also increases

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