If a reaction `A+B to C` is exothermic to the extent of 30KJ/mol, the forward reaction has an activation energy 70KJ/mol. The activation energy for the reverse reaction is

If a reaction A+BrarrC is exothermic to the extent of 30 KJ mol^(-1) , the the forward reaction has an activation energy , 70KJ mol^(-1) , the activation energy for the reverse 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 If a reaction A + B rarr C is exothermic to the extent 30 kJ mol^(-1) and the forward reaction has an activation energy of 249 kJ mol^(-1) the activation energy for reverse reaction in kJ mol^(-1) is

The energy required to form the intermediate, called activated complex (C ) is known as activation energy (E_(a)) . The diagram is obtained by plotting potential energy vs. reaction coordinate. Reaction coordinate represents the profile of energy change when reactants change into products. Some energy is released when the complex decomposes to form products. So, the heat of the reaction depends upon the nature of reactants and products. If a reaction A+Brarr C , is exothermic to the extent of 30 kJ mol^(-1) and the forward reaction has an activation energy of 249 kJ mol^(-1) , the activation energy for reverse reaction in kJ mol^(-1) is:

The reaction A+B rarr C+D+40KJ has activation energy of "18KJ" .Then the activation energy for the reaction C+D rarr A+B is

The activation energy for the forward reaction X rarr Y is 60 kJ mol^(-1) and Delta H is -20 kJ mol^(-1) . The activation energy for the reverse reaction is