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Kinetic Study of Esterification of Acetic Acid with n- butanol and isobutanol Catalyzed by Ion Exchange Resin
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Kinetic Study of Esterification of Acetic Acid with n- butanol and isobutanol Catalyzed by Ion Exchange Resin


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  • 1. Kinetic Study of Esterification of Acetic Acid with n- butanol and isobutanol Catalyzed by Ion Exchange Resin Amrit Pal Toor *, Mamta Sharma, Ghansyam Kumar, and R. K. Wanchoo University Institute of Chemical Engineering & Technology Panjab University, Chandigarh-160014, INDIA Received: 16th December 2010; Revised: 19th March 2011; Accepted: 7th April 2011Presented by:Víctor Hugo Balderrama JustoEugenio de Jesús Bautista SagreroJosé Manuel Cebrero OrtizOmar Alberto Cervantes CárdenasHeriberto Cruz HernándezAna Bertha de la Cruz TapiaCirce Nereyda García LópezSet Ángel Legaspi SánchezLaura Itzel Pérez EstradaMichel Romero Flores
  • 2. AbstractEsters are an important pharmaceutical intermediates andvery useful perfumery agents. In this study the esterificationof acetic acid with n-butanol and iso-butanol over an acidiccation exchange resin, Amberlyst 15 were carried out. Theeffects of certain parameters such as temperature, catalystloading, initial molar ratio between reactants on the rate ofreaction were studied. The experiments were conducted in astirred batch reactor in the temperature range of 351.15 K to366.15K.Variation of parameters on rate of reactiondemonstrated that the reaction was intrinsicallycontrolled.The activation energy for the esterification ofacetic acid with n-butanol and iso butanol is found to be28.45 k J/mol and 23.29 kJ/mol respectively.
  • 3. 1. IntroductionIn the simplest terms, esters can be defined as the reactionproducts of acids and alcohols. Thousands of different kindsof esters are commercially produced for a broad range ofapplications. Within the realm of synthetic lubrication, arelatively small substantial family of esters has been found tobe very useful in severe environment applications. The esterof acetic acid and isobutanol, namely, isobutyl acetate, findswide industrial applications. Butyl acetates are usedprimarily as solvents in the lacquer and enamel industries. Itis used in coatings, where its solvent capacity and its lowrelative volatility make it useful for adjustment ofevaporation rate and viscosity. It is particularly useful as asolvent or thinner for acrylic polymers, vinyl resins, asreaction medium for adhesives, as solvent for leatherdressings, and a process solvent in various applications and incosmetic formulations
  • 4. 2. Materials and Method2.1 Material usedAcetic acid, n-butanol and iso-butanol all werepurchased from Merck with a claimed purity of 99.8 %.Sodium Hydroxide (s.d. fine chemicals ltd., Boisar),Phenolphthalein indicator, (Qualigens fine chemicals,Mumbai). All of them were used without furtherpurification. Amberlyst -15 supplied by Rohm andHaas was used as catalyst and its relevantcharacteristics are summarized in Table 1
  • 5. 2.2 Experimental setup andprocedure
  • 6. Acetic acid 1.93 MIon exchange resin ΔT1 ±0.5K
  • 7. B ΔT2 = ΔT1 t=0 Acetic acid 1.93 M AIon exchange resin
  • 8. ΔT2 = ΔT1 t=0 Acetic acid 1.93 M A C D BIon exchange resin
  • 9. NaOH 1N Sample Phenolphtalein
  • 10. 3. Results and Discussion3.1 Kinetic modelingThe general reaction rate expression for this reactioncan be written as:A+B C +DWhere A=acetic acid, B=butanol, C=butyl acetate andD=water
  • 11. At steady state the rate of mass transfer per unit volume of the liquidphase can be expressed as rA = kLSA αP [CA-CAS]which is the rate of diffusion of A from bulk liquid phase to the catalystsurface and : rA =kLSB αP [CB-CBS]which is the rate of diffusion of B from bulk liquid phase to the catalystsurface . The rate of surface reaction per unit volume, (-rA) in presenceof intraparticle diffusion can be expressed as: (4)This equation is a Langmuir-Hinshelwood-Hougen- Watson type model(LHHW). Adsorption or desorption steps are unimportant in this casebecause catalyst used is a macro porous ion exchange resin and thereactants are able to diffuse into pores and the products diffuse outwithout any resistance .Hence Equation 4 can be replaced by power law model and η is unity forcatalyst particle size less than 700µm [Table 1]. rA= k1 w [C A] [C B]
  • 12. • When external and internal resistances to mass transfer are absent, the following holdsThen the surface reaction is the controlling mechanism and the overallrate of the reaction will be the same as given by the surface reaction, i.e.After integrating Equation this becomes:Putting CAw (M-1) k1=k in the equation we getPlotting the left hand side of this Equation versus time, a straight line witha slope k is obtained
  • 13. 3.1 Elimination of masstransfer resistancePrevious studies pointed that external diffusion doesnot usually control the overall rate in the reactionscatalyzed by ion exchanges resin unless the agitationspeed is very low or the reaction mixture is very viscousand intraparticle diffusion resistances of the reactant inthe ion exchange resins are not so important [6-8, 18].Hence all the experiments were conducted with the ionexchange resin that was supplied by manufacture (Rohmand Hass Co.) and at a fixed 500 rpm for all theexperiments.
  • 14. 3.2 Effect of catalyst loadingThe catalyst loading was varied from 4 to 11 % (22.43 kg/m3to 139.6 kg/m3) while keeping the other parametersconstant(molar ratio 1:5 and temperature 366.15 K). It wasfound that with an increase in catalyst loading the conversionof acid increases with the increase in the active sites. Athigher catalysts loading the rate of mass transfer is high andtherefore there is no significant increase in the rate .Gangadwala et al have achieved 60% conversion using 20 g/gmol of acetic acid in 50 minutes with 1:1 molar ratio of aceticacid to n-butanol whereas by increasing the molar ratio up to1:5 the conversion up to 80 % in same time
  • 15. with catalyst 5.3 g/g mol of acetic acid was achieved. The rateconstants for both the reactions were obtained by plottingLHS of Equation (9) vs. t as shown in Figures 3 and 4, Thevalues of k are given in table 2 for both n-butanol andisobutanol. It is also observed from Figure 5 and Table 2 thatthe rate constant k for isobutanol is higher than n-butanol.The k values were plotted against weight of the catalystand it was observed that with increase in w there was linearincrease in k (Fig 5).
  • 16. 3.3 Effect of Molar RatioTo investigate the effect of the initial molar ratio of alcohols toacetic acid on conversion of acetic acid, the initial molar ratiowas 1:3, 1:5 and 1:10 for n butanol and isobutanol both. Itseems that the conversion of acetic acid increases withincreasing the initial molar ratio of alcohols to acetic acid.Gangadwala et al have also reported that conversionincreases from 50 % to 80 % in 90 minutes from 1:1 to 1:3molar ratio of acetic acid to n-butanol. By increasing themolar ratio up to 1:10 the conversion was achieved up to 92% in 75 minutes and using 79.4% of catalyst used byGangadwala . The results observed for the effect of initialmolar ratio of alcohols to acetic acid indicated that theconversion of acid can be enhanced by using a large excessof alcohols, which is consistent with the results of Sanz et alwho studied the esterification of acetic acid with isopropanol.
  • 17. 3.4 Effect of Temperature• The results from the esterification of acetic acid with n butanol and isobutanol over Amberlyst 15 at different temperatures and with a fixed initial molar ratio 1:5 of the reactant are displayed in Figures 8 and 9. It was seen that the conversion increases with temperature, indicating absence of mass transfer effects. Same trend was observed by Roy and Bhatia for the esterification of acetic acid with benzyl alcohol over Amberlyst 15. Both esterification reactions were carried out in the temperature range from 351.15 to 366.15 K. The study of the effect of temperature is very important since it is useful to calculate activation energy of the reaction. The observed reaction rate constants (k) data at different temperatures were fitted to the Arrhenius-type equation and the model parameters, ko (frequency factor) and Eo (activation energy), were determined using linear regression technique. k = k0 exp(- E0 )RT
  • 18. 4. ConclusionIn this study the kinetics of the esterification of acetic acidwith n-butanol and isobutanol catalyzed by Amberlyst 15 wasexperimentally investigated. The reaction rate was foundto increase with increasing catalyst loading, temperature andmolar ratio. The LHHW (Langmuir-Hinshelwood) model wasused to simulate the experimental data. Reactivity of n-butanol and isobutanol towards the synthesis of butyl acetatevia the esterification of acetic acid with these alcohols waschecked. Comparison of these alcohols shows that activationenergy reduces from 28.45 kJ/mol in case of n- butanol to23.29 kJ/mol in case of isobutanol.