Accroding to the Arrhenius equation

Options

A. a high activation energy usually implies a fast reaction.
B. rate constant increases with increases temperature. This is due to a greater number of colliision 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

A reaction with high activation energy will be a slow reaction not a fast reaction.
Relation : `k=Ae^(-E_(a)//RT)` shows that the constant will increase with increases in temperature
`log.((k_(2))/(k_(1)))=(E_(a))/(2.303)((DeltaT)/(T_(1)T_(2)))`
It is logrithmic form of Arrhenius equation. It show that higher value of activation energy will result stronger dependence on temperature
In the equation :
`k=Ae^(-E_(a)//RT)`
`'A'rarr` frequecny factor. i.e., collision frequency among the reactant molecules irrespective of their energy