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 a 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 occur, irrespective of their energy

Answer

B, C, D

Explanation

`k=Ae^(-(Ea)/(RT))`
High activation energy means lower value of k and slow reaction. On increasing temperature energy of particles increases hence greater number of collisions occur whose energy exceeds the activation energy. Rate of increase of k with temperature is higher when Ea has a large value Pre-exponential factor is a measure of frequency of collisions.