Kinetic study of esterification reaction

Abstract EN

The Esterification kinetics of acetic acid with ethanol in the presence of sulfuric acid as a homogenous catalyst was studied with isothermal batch experiments at 50-60°C and at a different molar ratio of ethanol to acetic acid [EtOH / Ac].

Investigation of kinetics of the reaction indicated that the low of [EtOH / Ac] molar ratio is favored for esterification reaction, this is due to the reaction is catalyzed by acid.

The maximum conversion, approximately 80% was obtained at 60 ˚C for molar ratio of 10 EtOH / Ac.

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.

Activity coefficients were calculated using UNIFAC program.

Results showed deviation in activation energy in the non-ideal system of about 20 % this is due to the polarities of water and ethanol compared to the non-polar ethyl acetate this dissimilarity leading to strong non-ideal behavior.

The homogenous reaction has been described with simple power-law model.

The chemical equilibrium combustion calculated form the kinetic model in agreement with the measured chemical equilibrium.