If the activation energies of the forward and backward reactions of a reversible reaction are `E_(a)(f)` and `E_(a)(b)`, respectively. The `DeltaE` of the reaction is ………..

When the activation energies of the forward and backward reactions are equal, then :

The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.4kJ/mol respectively. The reaction is:

The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.5 KJ/mol , respectively . The reaction is:

The activation energies of the forward and reverse reaction in the case of a chemical reaction are 30.5 and 45.4 kJ//mol respectively. The reaction is:

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 activation eneries for forward and backward reactions in a chemical reaction are 30.5 and 45.4 kJ mol^(-1) respectively. The reaction is

If the activation energy of both the forward and the backward reactions are equal, then change in internal energy is

For the reaction, for which the activation energies for forward and backward reactions are same, then: