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 37.5 and 51.3 kJ/mole 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 E_(f) and E_(r) are the activation energies of forward and backward reactions and the reaction is known to be exothermic, then

The activation energies for forward and backward reactions are E_f and E_b respectively. If the reaction is exothermic then which is true regarding relation of activation energies?

A reaction having equal energies of activation for forward and reverse reactions has

A reaction having equal energies of activation for forward and reverse reactions has

Energy of activation of forward and backward reaction are equal in case (numerical calues) where

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 In a hypothetical reaction A rarr B , the activation energies for the forward and backward reactions are 15 and 9 kJ mol^(-1) , respectively. The potential energy of A is 10 kJ mol^(-1) . Which of the following is wrong?