A KINETIC STUDY OF THE SOLVENT EFFECT OF AQUO-ETHANOL SOLVENT SYSTEMS ON THE MEECHANISM AND THERMODYNAMIC FUNCTIONS OF CATALYSED SOLOLYSIS OF HIGHER BUTANOATE

The values of Iso-composition activation energy of the reaction were found to decrease with increasing proportion of EtOH in the reaction media. The plausible explanation for such depletion is due to solvation and desolvation of transition and initial states of the reaction respectively. From increase observed in ∆G* values with simultaneous decrease in the values of ∆H* and ∆S* of the reaction, it is inferred that the organic cosolvent EtOH acts as entropy controller solvent. From the evaluated values of water molecules associated with the activated complex of the reaction, it is concluded that bimolecular mechanistic path is changed to unimolecular in presence of the organic components of the reaction media. The numerical value of iso-kinetic temperature of the reaction, which comes to be 286.31 indicates that there is weak but considerable solvent-solute interaction in the reaction media.