Experimental and Computational Investigation of the Thermodynamic and Kinetic Behavior of a Model Chemical Reaction in Aqueous Solution

Understanding the thermodynamic and kinetic characteristics of chemical reactions in aqueous media is essential for elucidating reaction mechanisms and predicting their behavior under different operating conditions. In the present study, an integrated experimental and computational approach was employed to investigate the temperature-dependent thermodynamic and kinetic behavior of a model chemical reaction in aqueous solution. The reaction rate was evaluated at different temperatures, and the corresponding kinetic parameters were determined using temperature-dependent rate constants. The activation energy was estimated using the Arrhenius equation, while the thermodynamic parameters, including the standard enthalpy change (ΔH°), standard entropy change (ΔS°), and standard Gibbs free energy change (ΔG°), were determined from the temperature dependence of the equilibrium and kinetic data. Computational analysis was further used to examine the relationship between molecular-level interactions and the experimentally observed reaction behavior. The results demonstrate that temperature significantly influences both the reaction rate and the thermodynamic characteristics of the investigated system. The combined interpretation of experimental and computational results provides a comprehensive framework for relating macroscopic kinetic parameters to molecular-scale energetic changes. This approach can contribute to a better understanding of reaction mechanisms in aqueous environments and provide a useful methodology for the thermodynamic and kinetic characterization of chemically relevant processes.

کلیدواژه ها:

Chemical kinetics ، Thermodynamics ، Activation energy ، Aqueous solution ، Computational chemistry