state 2 advantages of transitional theory over collision theory
Rate of a reaction can be expressed by the two theories namely collision theory and transition state theory (not translational theory).
As per collision theory, for reaction to occur, the reactants must have optimum energy and must be oriented in such a way that products can be formed. So, rate constant of reaction is the product of rate of reaction is proportional to frequency of effective collisions.
As per transition state theory, a transition state which is formed when reactants combine but products are not formed. In this state, the species termed as activated complex is formed which contains partial bonds. This activated complex may form products or revert back to reactants. The rate constant can be used to calculate the standard enthalpy, standard entropy and standard Gibbs free energy of formation of activated complex.
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