A colliison between reactant molecules must occur with a certain minimum energy before it is effective in yielding Product molecules. This minimum energy is called activation energy `E_(a)` Large the value of activation energy, smaller the value of rate constant `k`. Larger is the value of activation energy, greater is the effect of temperature rise on rate constant `k`.

`E_(f) =` Activation energy of forward reaction
`E_(b) =` Activation energy of backward reaction
`Delta H = E_(f) - E_(b)`
`E_(f) =` threshold energy
The rate constant of a certain reaction is given by `k = Ae^(-E_(a)//RT)`
(where `A =` Arrhenius constant). Which factor should be lowered so that the rate of reaction may increase?

Options

A. T
B. Z
C. A
D. `E_(a)`

Answer

D