Paper Title
Thermodynamic Equilibrium of Ethyl Acetate Synthesis: Validation of Obtained Data by Different Tackled Methodologies and Techniques

Abstract
The esterification reaction between acetic acid and ethyl alcohol was examined over a temperature range of 298.15 to 328.15 K, utilizing both homogeneous and heterogeneous catalysts. Experimental conditions included equimolar reactant ratios and catalyst loadings of 40 g/L. Equilibrium was achieved within two days across all systems, with minimal temperature-dependent variation in equilibrium conversions. Catalyst characteristics significantly impacted equilibrium conversion, alongside temperature effects. The Modified UNIFAC-Dortmund model accurately predicted the system's non-idealities, with activity coefficients following the sequence: acid < alcohol < ester < water. Equilibrium constants (Ka) demonstrated a slight decrease with rising temperature. The average Ka values for sulfuric acid and various heterogeneous catalysts (Amberlyst 15, Amberlite IR-120, Dowex 50wx8) were 13.92, 8.16, 10.60, and 9.31, respectively. The catalyst type influenced equilibrium conversion, with Ka values for sulfuric acid comparable to those reported for para-toluene sulfonic acid. Theoretical equilibrium constants, sensitive to ΔG0 values, aligned closely with experimental results, particularly for the Amberlyst 15-catalyzed system.