Study of the Kinetics and Thermodynamic Parameters of Schiff Bases Derived from 4-Aminoantipyrin
Abstract
The kinetic and thermodynamic properties of six well-known Schiff bases (A1, A3, A5, A6,
A8, A12) derived from 4-aminoantipyrine and six different aromatic aldehydes were studied. The
substituent on aldehydic ring of the compounds ranged from electron-withdrawing to electrondonating substituents, in addition to benzaldehyde itself. The hydrolysis kinetics of the Schiff bases
revealed minimal disparity in their rate constant values. Faster rate of hydrolysis was observed in
the case of (A5) comparing with the remaining compounds. The effect of an acidic pH on the
hydrolysis process is in line with earlier research and studies, indicating that conducting the reaction
in acidic or basic environments, as opposed to a neutral environment, speeds up the process. An
investigation into the effect of temperature on the hydrolysis of the examined compounds revealed
that the activation energy values for all compounds were quite low. This indicates that the reaction
occursreadily and rapidly. The ΔG values indicated that the hydrolysis processes of the compounds
under investigation did not proceed spontaneously, but were instead facilitated by the presence of a
catalyst, specifically hydrogen and hydroxyl ions. The investigation verified the significance of the
thermodynamic variables (∆H and ∆S) in regulating reaction rates. Additionally, the calculated
negative entropy value suggests a probable formation of the activated active complex.
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