Entropy of activation

From Wikipedia, the free encyclopedia
Jump to navigation Jump to search

In chemical kinetics, the entropy of activation of a reaction is one of the two parameters (along with the enthalpy of activation) which are typically obtained from the temperature dependence of a reaction rate constant, when these data are analyzed using the Eyring equation. The standard entropy of activation is symbolized ΔS and equals the change in entropy when the reactants change from their initial state to the activated complex or transition state (Δ = change, S = entropy, ‡ = activation). It determines the preexponential factor A of the Arrhenius equation for temperature dependence of reaction rates. The relationship depends on the molecularity of the reaction: for reactions in solution and unimolecular gas reactions A = (ekBT/h) exp(ΔS/R), while for bimolecular gas reactions A = (e2kBT/h) (R'T/p) exp(ΔS/R). In these equations e is the base of natural logarithms, h is the Planck constant, kB is the Boltzmann constant and T the absolute temperature. R' is the ideal gas constant in units of (bar*L)/(mol*K). The factor is needed because of the pressure dependence of the reaction rate. R' = 8.3145 * 10^-2 (bar*L)/(mol*K).[1]

The value of ΔS provides clues about the molecularity of the rate determining step in a reaction, i.e. whether the reactants are bonded to each other, or not. Positive values suggest that entropy increases upon achieving the transition state, which often indicates a dissociative mechanism in which the activated complex is loosely bound and about to dissociate. Negative values for ΔS indicate that entropy decreases on forming the transition state, which often indicates an associative mechanism in which two reaction partners form a single activated complex.[2]


  1. ^ Laidler, K.J. and Meiser J.H. Physical Chemistry (Benjamin/Cummings 1982) p.381-2 ISBN 0-8053-5682-7
  2. ^ James H. Espenson Chemical Kinetics and Reaction Mechanisms (2nd ed., McGraw-Hill 2002), p.156-160 ISBN 0-07-288362-6