According to the Arrhenius equation,

Options

A. a high activation energy usually implies a fast reaction
B. rate constant increases with increase in temperature. This is due to greater number of collisions whose energy exceeds the activation energy
C. higher the magnitude of activation energy, stronger is the temperature dependence of the rate constant
D. the pre-exponential factor is a measure of the rate at which collisions occure, irrespective of their energy

Answer

B, C, D

Explanation

is incorrect because high activation energy implies a slow reaction (b), (c ) and (d) are correct and follow from Arrhenius equation, viz.,
`k=Ae^(-E_(a)//RT)`.