Experimental Assessment of Artificial Flavour Production

Abstract

The esterification kinetics of acetic acid with isopropanol in the presence of sulfuric acid as a homogenous catalyst was studied with isothermal batch experiments at 60, 70 and 80°C and at a different molar ratio of isopropanol to acetic acid. Investigation of kinetics of the reaction indicated that the low of molar ratio is favored for esterification reaction, this is due to the reaction is catalyzed by acid. The maximum conversion, approximately 60.6% was obtained at 80°C for molar ratio of 1:3 acid: alcohol. It was found that increasing temperature of the reaction, increases the rate constant and conversion at a certain mole ratio that is due to the esterification is exothermic. The homogenous reaction has been described with simple power-law model. Arrhenius equation has been applied to found kinetic constants dependency temperature. The activation energy is found to be 740.5 kJ /mol.