Kinetic Study of the Hydrolysis of Ethyl Acetate in Different Solvent Media
DOI:
https://doi.org/10.59436/ijpsr.v2i2.15.3139-342XKeywords:
Ethyl acetate, Hydrolysis, Chemical Kinetics, Solvent Media, Solvent Polarity, Pseudo-first-order Kinetics, Rate Constant, Arrhenius Equation, Activation EnergyAbstract
Hydrolysis of ethyl acetate is one of the most investigated reactions in physical chemistry, since it is seen as an ideal system for studying of reaction kinetics and generation of solvent effects and catalytic mechanisms. This paper studies kinetics of acid catalyzed hydrolysis of ethyacetate in various solvents including distilled water, water-methanol, water-ethanol and water-acetone mixtures. The main goal of the research is to assess the role of solvent polarity in the reaction rate, as well as obtain pseudo-first-order rate constants and activation energy by means of Arrhenius equation. The experiments in the laboratory have been conducted in controlled conditions, where excess water was used for conducting reaction in the way of pseudo-first order kinetics. Hydrochloric acid is selected as the catalyst. Observations of the conducted experiments were made throughout the process of interval sampling and titration with standard sodium hydroxide solutions. The data obtained was analyzed with the assistance of kinetic methods, Arrhenius plots, regression and statistical analysis. The experiments showed high dependency of rate of reaction in the environment of the solvent being used. The highest constant was found for distilled water due to its high value of dielectric constant and hydrogen bond formation ability. Adding organic solvents to the system resulted in slowing down the reaction rate significantly. The order of catalysts in terms of reaction speed is like this: Water > Water-Methanol > Water-Ethanol > Water-Acetone. Thus, the influence of solvent polarity on the transition state as well as kinetics of reaction can be confirmed by the results obtained.
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