Concept of activation energy

The excess of the energy (Over and above average energy of the reactants) which must be supplied to the reactants to undergo chemical reactions is called activation energy (E_a),

         The Activation energy = The threshold energy - Average kinetic energy of molecules which are reacting.

(a) Zero activation energy = Fraction of the effective collision (f) will be large = Very fast reaction (that is Instantaneous reaction).

(b)  Low activation energies = Fraction of the effective collision (f) will be quite large = Fast reactions.

(c)  High activation energies = Fraction of the effective collision (f) will be small = Slow reaction.

         The activation energy which is denoted by E_a depends upon the nature of chemical bonds undergoing rupture and is independent of enthalpies of reactants and products.

In accordance to the concept of activation energy, the reactants do not change straight in the products. The reactant absorbs energy the first equal to the activation energy and form activated complex. At this particular state, molecules should have energy at least equal to the threshold energy. This signifies that the reaction includes some energy barrier which should be overcome before products are formed. The energy barrier can be termed as activation energy barrier.

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