Esterification Reaction Kinetics Using Ion Exchange Resin Catalyst by Pseudo-Homogenous and Eley-Ridel Models (original) (raw)
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Kinetics of Esterification Reaction using Ion- Exchange Resin Catalyst
Journal 4 Research - J4R Journal, 2017
The reaction kinetics of esterification between n-butanol and acetic acid on acidic solid catalyst named SERALITE SRC-120 under atmospheric pressure was investigated in this work. Reaction experiments were carried out in a stirred batch reactor at temperature range of 353 to 356 K, under various catalyst loads and various starting reactants feed ratios. The experimental data were fitted to estimate the kinetic parameters for reaction mechanisms. The chemical equilibrium composition was measured and kinetic information was obtained at the same temperature range. The results show that the activation energy of n-butanol esterification reaction was found to be 622.28 KJ/mol. Finally the results of produced reaction mechanisms were compared with Experimental results to validate the reaction mechanism. Then it was conclude that the model results with the regressed kinetic parameters are in excellent agreement with the experimental results.
Industrial & Engineering Chemistry Research, 2008
The heterogeneous catalysis of lactic acid (88 wt %) esterification with ethanol in the presence of Amberlyst 15-wet was studied for catalyst loading of 1.2-3.9 wt %, initial molar ratio of reactants of 1.1-2.8, and temperature from 50 to 90°C. In this work a methodology based on the UNIQUAC model was developed to determine the thermodynamic equilibrium constant since in the literature there is inconsistency concerning the temperature dependence of the thermodynamic equilibrium constant. A simplified Langmuir-Hinshelwood kinetic model was used to predict the experimental data. The proposed rate law is r) k c (a Eth a Laa EL a W / K)/(1 + K Eth a Eth + K W a W) 2 ; the kinetic parameters are the preexponential factor, k c,0) 2.70 × 10 7 mol‚g-1 ‚min-1 , and the activation energy, E a) 49.98 kJ/mol. The equilibrium reaction constant is K) 19.35 exp(-515.13/T (K)) with reaction enthalpy 4.28 kJ/mol. The model reasonably predicts the kinetic experimental data, and it will be very useful to apply to the design and optimization of industrial hybrid reactive separation processes.
Kinetics of Esterification of Ethylene Glycol with Acetic Acid Using Cation Exchange Resin Catalyst
2011
The esterification of ethylene glycol with acetic acid was investigated in a batch reactor in presence of a strongly acidic cation exchange resin, seralite SRC-120, as catalyst in the temperature range of 333 to 363 K. The detailed kinetic study was performed to understand the effect of various process variables such as catalyst loading, ethylene glycol to acetic acid mole ratio, and temperature on conversion of reactants and selectivity to products. Further, two different kinetic models, empirical and kinetic model based on Langmuir-Hinshelwood-Hougen-Watson (LHHW) approach, were developed to correlate the experimental concentration versus time data. The kinetic parameters of the developed models were then estimated at different temperatures using non-linear regression technique based on modified Levenberg-Marquardt algorithm. The calculated results based on the estimated kinetic and equilibrium constants at different temperatures were then compared with the experimental values and LHHW-based model was found to fit the experimental data reasonably better compared to empirical kinetic model. The estimated rate constants at different temperatures of LHHW-based model were then used to estimate the activation energy and frequency factor of the rate constants.
Esterification represents one of the most important reactions in chemical industry and the esters produced have applications in a variety of areas such as plasticizers, flavours and fragrances, pesticides, solvents, medicinal and surface active agents. The Esterification kinetics of acetic acid with ethanol in the presence of sulphuric acid as a homogenous catalyst was studied with batch experiments at four different temperatures and at a different molar ratio of ethanol to acetic acid with 5% catalyst loading. Investigation of kinetics of the reaction indicated that the increasing the [Ac/EtOH] molar ratio is favoured for esterification reaction, this is due to the reaction is catalyzed by acid. The maximum conversion, approximately 83% was obtained at 65°C for molar ratio of Ac/5EtOH. With the help of Aspen Plus we can design plants and can attempt profitability in existing plants. We can interactively change specifications, such as flow sheet Configuration, operating conditions, ...
Advances in Environmental Technology (AET), 2015
In the chemical industry, process intensification is needed to meet important goals such as sustainable and eco-friendly processes. For esterification reaction the “produce more with less pollution” objective can be achieved by coupling reaction and separation in a so called integrated process. In this work a model for describing the esterification reaction of ethyl acetate in pervaporation membrane reactor using amberlyst 15 as a heterogeneous catalyst and polydimethylsiloxane (PDMS) membrane, was developed. This earth-friendly method with low pollution and high yield is an alternative to hazardous methods because using pervaporation membrane reactor reduces both waste and energy consumption. The validity of the model was tested by comparing the calculated results with experimental data reported in the literature. It was shown rate of conversion increased by removing ethyl acetate from the reaction mixture. A parametric study was carried out to evaluate the effects of operating conditions on the performance of the pervaporation membrane reactor. Conversion increased by increasing the temperature, molar ratios of reactants and catalyst concentration.
Liquid-phase esterification of acetic acid with isobutanol catalyzed by ion-exchange resins
Reactive and Functional Polymers, 2007
Esterification of carboxylic acids with alcohols represents well-known liquid-phase reactions of considerable industrial interest due to the importance of organic ester products. These ester products include environmentally friendly solvents, flavors, pharmaceuticals, plasticizers, and cosmetics. In this study, the esterification kinetics of acetic acid with isobutanol in 1,4-dioxan as a solvent without adding a catalyst and catalyzed by ion-exchange resins are carried out using a batch reactor. The effect of catalyst type, stirrer speed, the effects of reaction temperature and catalyst loading on the initial reaction rate, the effect of speed of agitation and the conversion of acetic acid versus time were investigated. The kinetics of heterogeneous catalyzed esterification of acetic acid with isobutanol was correlated by a kinetic model based on pseudo-homogeneous catalysis. The strong acidic cation exchange resins were used as solid catalysts, Dowex 50 Wx2, Amberlite IR-120, respectively. As a result, it was found that the weight-based activity of the heterogeneous catalysts increases in the following order: Dowex 50 Wx2 > Amberlite IR-120 and these catalysts were effectively for the synthesis of isobutyl acetate under these experimental conditions.
Korean Journal of Chemical Engineering, 2016
The esterification of propionic acid with isopropyl alcohol was studied in an isothermal batch reactor. The activities of three different types of ion exchange resin catalysts (Amberlyst 15, Amberlyst 70 and Dowex 50 WX8) were investigated, and Amberlyst 15 was found to be an effective catalyst for the reaction. The effects of process parameters, namely, catalyst loading, alcohol to acid molar ratio and reaction temperature, were studied and optimized. Response surface methodology (RSM) was applied to optimize the process parameters as well as to investigate the interaction between process parameters. The internal and external diffusion limitations were found to be absent at a stirring speed of 500 rpm. The RSM model predicted response (83.26%) was verified experimentally with a good agreement of experimental value (83.62±0.39%). Moreover, the kinetics was studied and the Langmuir-Hinshelwood model was used to fit the kinetic data.
Chemical Engineering Journal, 2007
The esterification of lactic acid with ethanol and the hydrolysis of the corresponding ester, ethyl lactate, have been studied in the presence of the commercial cation-exchange resin Amberlyst 15. The influence of different operating parameters such as stirrer speed, catalyst particle size, initial reactant molar ratio, reaction temperature and catalyst loading, has been examined. Additionally, the adsorption constants for the four components on Amberlyst 15 were determined by performing adsorption experiments between two non-reacting species. The values found for the adsorption constants follow the order: water > ethanol > lactic acid > ethyl lactate. Experimental kinetic data of the esterification and the hydrolysis reactions were correlated simultaneously with the Langmuir-Hinshelwood (LH) and pseudo-homogeneous (PH) models. The activity coefficients were calculated according to the UNIQUAC model. The LH model gave the best agreement with the kinetic experimental data. The activation energy of esterification and hydrolysis reactions were found to be 52.29 and 56.05 kJ mol −1 , respectively.