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
For two reactions, activation energies are `E_(a1)` and `E_(a2)`, rate constant are `k_(1)` and `k_(2)` at the same temperature. If `k_(1) gt k_(2)`, then

Options

A. `E_(a_(1))gtE_(a_(2))`
B. `E_(a_(1))=E_(a_(2))`
C. `E_(a_(1))ltE_(a_(2))`
D. `E_(a_(1))geE_(a_(2))`

Answer

C