Adsorption of catechin from aqueous solutions on polymeric resins and activated carbon

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1 Indian Journal of Chemical Technology Vol. 17, September 2010, pp Adsorption of catechin from aqueous solutions on polymeric resins and activated carbon Parikshit Gogoi, Narendra N Dutta* & Paruchuri G Rao* Chemical Engineering Division, North East Institute of Science and Technology (CSIR), Jorhat , India pgrao24@hotmail.com; nndutta@rediffmail.com Received 15 October 2009; revised 1 July 2010 Catechin, a bioflavonoid found in green tea leaves has various applications in food and pharmaceutical industries. With a view to develop adsorptive separation process for the extraction of catechin from green tea, the batch equilibrium adsorption of catechin from aqueous solutions using commercially available activated charcoal, styrene-divinylbenzene (SDVB) and acrylic resins with different hydrophobicity, surface areas and pore radii has been studied. Adsorption isotherms were interpreted from Langmuir, Freundlich and Redlich-Peterson isotherms. However, almost in all cases, Langmuir isotherm exhibited better fit of experimental data. It appears that capacity of the adsorbate/adsorbent system depends on various interactions that occur at the solid liquid interface i.e., hydrophobic, dipole-dipole and hydrogen bonding. Physical properties of the resin such as surface area, pore radius, and porosity and the chemical characteristics of the solution i.e., solvent type and ph also play a major role in determining rates and equilibrium of adsorption. The heat of adsorption ( Hº) was determined from Van t Hoff plot using equilibrium data generated at different temperatures and the observed differences in Hº for different adsorbents have been explained from mechanistic consideration. Keywords: Catechin, Activated carbon, Polymeric resin, Adsorption, Langmuir isotherm Catechin, a monomeric flavanoid (Fig. 1a), is reported to have hydroxyl, peroxyl, superoxide and DPPH (1,1-diphenyl-2-picrylhydrazyl) radical scavenging activities 1. In recent years, catechins have been increasingly used as a natural ingredient in foodstuffs and feedstuffs for various purposes due to their antioxidant properties for obtaining certain desired components initially retained in a food matrix 2. Extraction of catechins from green tea is one of the most important processing steps in technological perspectives. Though the classical method of solvent extraction is available for the extraction of tea catechins, adsorption and membrane based separation methods are the most emerging and attractive from the economic view point. The most widely used adsorbent for industrial applications is activated carbon. In recent years, polymeric adsorbents have been increasingly used as an alternative to activated carbon due to their wide variations in functionality, surface area and porosity 3-5. The resins are durable nonpolar (styrene-divinylbenzene) or slightly hydrophilic (acrylic) polymers having a high adsorption capacity with possible recovery of the adsorbed molecules, relatively low cost, and ease of regeneration. Because of their particular physical properties, adsorbent resins are employed by the pharmaceutical industries for the purification of amino acids and peptides 6, β-lactum antibiotics, vitamins, prostaglandins and to remove and recover phenolic compounds from products and byproducts of food processing plants 7-9. Earlier, study on membrane and adsorptive separation process has been persued for extraction and purification of β-lactum antibiotics For the design of adsorbent systems, the knowledge of adsorption equilibria, kinetics and adsorbent s capacity is essential. These depend on the external physicochemical parameters such as ph, competing compounds present in solution, and on the resin chemical structure 20 or other characteristics such as particle size, porosity, specific surface area, and pore volume distribution 21. The capacity of an adsorbent is Fig. 1a (+)-Catechin structure

2 338 INDIAN J. CHEM. TECHNOL., SEPTEMBER 2010 characterized by isotherm. The most common isotherms applied in solid/liquid system are those presented by Langmuir 22, Freundlich 23, and Redlich Peterson 24. The temperature effect on adsorption is also important for estimating heat of adsorption data, which will be useful from mechanistic consideration and design point of view. In view of the above, the present study on adsorption behaviour of (+)-catechin from batch solutions on different commercially available resins and activated carbon has been performed. In order to quantify and compare their adsorption capacity, the experimental equilibrium data at 25ºC were fitted to various isotherm models given by Langmuir, Freundlich and Redlich-Peterson. This is expected to provide a basis for understanding the sorption process and to predict the adsorbent performance. The heat of adsorption was estimated from the Van t Hoff plot generated from data at four different temperature levels. Experimental Procedure Materials (+)-Catechin used in this study was obtained from Sigma Chemicals Co. USA. Buffer reagents and activated carbon were supplied by CDH, Mumbai, India and were of analytical grade. The polymeric resins Amberlite XAD-4, XAD-7, XAD-16 and dianion HP 2MG were also obtained from Sigma Chemicals Co. USA and have the structure shown in Fig. 1b. The properties of these resins are shown in Table 1. Activated carbon was obtained from E. Merck, Germany and had a specific surface area of 920 m 2 /g (by BET N 2 adsorption), an average diameter of m, porosity of 55%, apparent density of 410 kg/m 3, particle density of 1100 kg/m 3 and a sphericity of nearly 1. The adsorbent was washed with distilled water and dried overnight before use. Adsorption isotherm Equilibrium isotherms were obtained by contacting 20 ml of aqueous catechin solution with different Fig. 1b Structure of activated carbon and resins Table 1 Chemical and physical properties of resins (Reported by manufacturers) Trade Name Structure Surface area (m 2 /g) Pore radius (Å) Porosity (ml/g) Particle size (mm) Density (g/ml) Amberlite XAD-7 Acrylic Amberlite XAD-4 SDVB Amberlite XAD-16 SDVB Dianion HP-2MG Acrylic

3 GOGOI et al.: ADSORPTION OF CATECHIN FROM AQUEOUS SOLUTIONS ON POLYMERIC RESINS 339 amount of polymeric resins in a thermostatted shaker maintained at 25 ± 0.5 C for 3-4 h. Preliminary runs showed that the equilibrium adsorption was achieved after 3-4 h of contact time for all tested resins. The initial concentration of the catechin was taken between 5 and 10 mm. The ph of the solution was varied between 4 and 8 by using buffer reagents of appropriate dosages. After attainment of equilibrium, the aqueous phase was analysed by a UV-Vis spectrophotometer (Shimadzu 160A) calibrated at appropriate wavelength (280 nm) using a calibration curve. The amount of catechin adsorbed per gram of adsorbent q (mol/g) was calculated as q = V(C-C e )/W, where C and C e are the initial and equilibrium solute concentrations (mmol/l), V is the solution volume (L) and W is the weight of the adsorbent (g). Adsorption rate experiments were conducted at ph 5.5 and the liquid volume was 100 ml with g of adsorbents. The initial concentration of (+)-catechin was 5 to 10 mm at 25 ± 0.5 C. The liquid phase concentration was monitored at equal interval of time till the equilibrium is attained. Measurement of enthalpies using Van t Hoff plots Van t Hoff method was used to estimate the enthalpy of adsorption by relating the temperature dependence of the adsorption equilibrium constant. The Van t Hoff method utilizes two thermodynamic relationships, the first being G = - RT ln K = - RT ln (Ψ q/c e ) (1) where, G is the standard free energy change of adsorption, R is the universal gas constant, T is the absolute temperature in degree Kelvin and K is the equilibrium constant for the adsorption process. At low solute concentration adsorption is limited to the linear region of the isotherm and therefore the equilibrium constant can be related to the adsorption affinity (q/c e ). The factor Ψ includes the terms for the activity coefficient of the solute in the two phases and activity of the unbound adsorption sites. For a narrow range of solute concentrations, Ψ may be assumed to be constant under the standard conditions. The second thermodynamic relationship used in the Van t Hoff method is Combining the two equations, the following equation is obtained ln (q/c e ) = - H /RT + [ S /R- ln Ψ] (3) Thus, a plot of ln (q/c e ) versus 1/T should give a straight line with a slope of - H /R, from which - H can be calculated under the assumption that H, S and Ψ are constant over the temperature range of study. Results and Discussion Adsorption equilibrium Adsorption isotherms measured for (+)-catechin on various polymeric adsorbents and activated carbon are shown in Fig. 2. The adsorption isotherm of (+)-catechin could not be obtained in the same equilibrium concentration range of liquid phase as with other adsorbents, due to high adsorption capacity of adsorbents. The data of Fig. 2 shows that XAD-7 has q values greater than those of the other resins at all aqueous (+)-catechin residual concentrations and may be the most appropriate one for removing (+)-catechin from aqueous solutions and the least effective resins for (+)-catechin is XAD-16 resin, with the least q values. For the adsorption of cephalexin antibiotic 9 on hydrophobic surfaces the intensity was reported to be low probably due to higher hydrophilic nature of solute implying probably that the hydrophobic interaction is the probable adsorptive mechanism. The observed effect of the nature of adsorbent on (+)-catechin adsorption is noteworthy. The reason for the difference in (+)-catechin adsorption with different resins and activated carbon are complex and not well understood. In general, activated carbon G = H - T S (2) where, H is the standard enthalpy change and S is the standard entropy change of adsorption. Fig. 2 Adsorption isotherms of (+)-catechin on different adsorbents

4 340 INDIAN J. CHEM. TECHNOL., SEPTEMBER 2010 provides high adsorption behaviour for phenols compared with any other polymeric resins owing to their predominantly acidic surface oxides such as carbonyl, carboxyl, phenolic hydroxyl, lactone and quinine groups as the surface structure which may probably interact through hydrogen bonding. Similar mechanism was hypothesized by adsorption of phenolic compounds from aqueous solutions on activated carbon 25. In case of activated carbon, the values of the adsorption intensity obtained are comparable to those reported for systems of phenol and indol as the solute 26. Adsorption could be affected by external physicochemical parameters such as ph, temperature, competing compounds present in solution, and on the chemical structure of resin or other characteristics such as particle size, porosity, adsorbent polarity, specific surface area, and pore volume distribution. Surface area and pore radius keeps a linear relation with adsorption capacity with pore radius 90 A 27. However, in the present study chemical nature of the adsorbent plays more important role than the physical structure for (+)-catechin adsorption. Amberlite XAD-7, which exihibited the best results in terms of the adsorptive capacity, is a non-ionic aliphatic acrylic polymer whereas XAD-4 and XAD-16 are composed of styrene-divinylbenzene, a hydrophobic polyaromatic polymer, making them more efficient for adsorption of compounds of higher hydrophobicity. Dianion HP- 2MG, which is also a non-ionic aliphatic acrylic polymer, shows moderate adsorption capacity for the adsorbate molecules. So the high affinity of all the adsorbate molecules for XAD-7 may be due to the hydrophilic nature of polyphenols. Therefore, polarity matching between XAD-7 among the resins is used here and polar adsorbate may partially account for the increase in adsorption capacities as is also reported for the adsorption of polyphenols on macroporous resins 28. Different values of adsorption intensity of different resins perhaps indicate that hydrophobic interaction may be the adsorption mechanism, whereas the difference in values of adsorption intensity of XAD-7 and activated carbon may be attributed to hydrogen bonding as the probable adsorption mechanism. This is inconformity with the observation for adsorption of polyphenols by resins containing amide groups, which may be driven by hydrophobic interaction and multiple hydrogen bonding 29,30. Phenol molecules adsorb effectively from aqueous solutions onto the acrylic ester polymer through Vander Waals interaction, while adsorption from their hexane solution can be achieved onto Amberlite XAD-7 primarily through the intermolecular hydrogen bond formed between the phenolic hydroxyl group and the carbonyl group on the polymeric matrix 31,32. Such specific interaction plays a positive role in phenol adsorption from aqueous solution too 33, however, adsorption driven by hydrogen bonding alone in aqueous solution is very weak because of the strong hydrogen bonding characteristics of water 13,30. The effect of ph on (+)-catechin adsorption on XAD-7 is shown in Fig. 3 from which it is evident that the variation is marginal only. The ph dependence of the adsorption is important and higher adsorption at acidic ph onto acidic resin may be attributable to polar polar interactions due to the acidic nature of (+)-catechin (Fig. 1). Catechin possesses four OH phenolic groups located in two benzene ring in which oxygen atom (C-O-C) group and one more OH group are present. Therefore, (+)-catechin molecule is not a planar one. The spatial arrangement of the (+)-catechin molecule is important for their stability against ph, because susceptibility to a chemical changes depends on OH and pi electron system. In higher ph range it polymerizes and the presence of OH - ions prevents the adsorption of (+)-catechin from the aqueous solutions. The polar resins adsorption of glycyrrhizic acid and flavanoids was maximum at ph 5 due to hydrogen bonding. At higher ph the hydrogen bonding interactions are reduced and dissociate to form H + and their corresponding anions. Such ionization process also reduces their adsorption on polar resins 34. This result is inaccordance with those of Yoon et al. 35 who Fig. 3 Adsorption isotherm for (+)-catechin on XAD-7 as a function of ph at 25ºC

5 GOGOI et al.: ADSORPTION OF CATECHIN FROM AQUEOUS SOLUTIONS ON POLYMERIC RESINS 341 found significant variations of the adsorption of flavanols from Ginkgo biloba extracts when studied in large range of ph (3 to 12). By contrast, no significant effect in anthocyanin adsorption at variable ph (1 to 4.5) and adsorption of polyphenols from Ing edulis (ph from 2.0 to 5.0) on polymeric resins was observed and may be attributabed to the different equilibrium forms of flavanoids, which is independent of neither for partially hydrophilic resins nor for hydrogen bonding 28,36. Adsorption isotherm The adsorption equilibria can be interpreted with Langmuir, Freundlich and Redlich Peterson isotherms. Table 2 shows the value of the isotherm parameters estimated by non-linear regression analysis. Comparing the coefficients of determination (R 2 ) of the models it appears that Langmuir isotherm provides the most satisfactory representation of the experimental data almost at all experimental sets. For aqueous phase adsorption of solutes on activated carbon and on polymeric resins Langmuir, Freundlich and Redlich-Peterson isotherm models have been found to be satisfactory for compounds such as β-lactum antibiotics, phenols and flavonoids, etc. 18,28. The Freundlich constant n represents the adsorption intensity and in particular the effect of residual concentration on adsorption capacity which lies between 0.1 to are compatible to present results ranging from to for resins and for activated carbon. The classification of adsorption isotherm of solutes from aqueous solutions depends on the configuration of the initial part of the isotherm and it gives the quasi-qualitative information on the nature of the solute-surface interaction 38. The adsorption isotherms obtained in this work are of type L i.e., Langmuir class, with a linear initial part showing the high diffusion of solute into the adsorbent and suggests that there is no strong competition between solvent and solute for occupation of the adsorption sites. A Langmuir analysis 39 was made to the results over a given equilibrium liquid phase concentration, C ref to characterize the type of isotherm as originally demonstrated by Vermeulan et al. 40 using the following relationship 1 r= (4) 1+ KLC ref The type of isotherm depends on the value of r as illustrated in Table 2 r >1 r =1 0<r <1 r =0 unfavourable linear favourable irreversible The values of the constant r was found to be in the range of to for the tested adsorbents. The values of the Langmuir constants were found to be marginally higher than the adsorption of cyanidin3-glycosides 36, total phenolics and total flavanoids 28 on polymeric resins. This marginal difference in the adsorption intensity may be considered reasonable since the polar nature of the sorbates studied is expected to establish identical adsorption intensity. Adsorption enthalpy The temperature effect of the adsorption equilibrium was evaluated by measuring the adsorption at three different temperatures and at a constant ph of 5.5. The adsorption isotherms of (+)- catechin on activated carbon and XAD-7 at three different temperatures are shown in Figs 4 and 5, and it appears that the adsorption intensity increases with decrease in temperature indicating exothermic nature of the adsorption process. For adsorption equilibrium studies low concentrations of (+)-catechin were used to limit the adsorption to the linear region of the isotherm where all of the isotherms could be extrapolated to the origin. The temperature dependent adsorption affinity (q/c e ) was evident from the slopes Adsorbent Table 2 Equilibrium isotherm constants of (+) catechin at different conditions n Langmuir q=kx m /(1+KC e ) Freundlich q=k F C e Redlich-Peterson q=kc e / (1+a R C b e ) K X m R 2 r K F n R 2 K a R b R 2 XAD Dianion HP XAD XAD Charcoal

6 342 INDIAN J. CHEM. TECHNOL., SEPTEMBER 2010 Fig. 4 Adsorption isotherm of (+)-catechin on activated carbon as a function of temperature, ºC Fig. 6 Typical Vant Hoff plot for adsorption of (+) catechin on XAD 7 Table 3 Reported - Hº values for different systems Molecule Adsorbent - Hº (kcal/ mol) References Caffeine XAD [41] Cephalexin Activated carbon [18] Cephalexin XAD [18] N-methyl Polycarboxylic -5.1 [42] aniline ester Phenol Polycarboxylic -8.2 [42] ester Benzyl Polycarboxylic -6.3 [42] alcohol Phenyl propanol ester Polycarboxylic ester -6.4 [42] Fig. 5 Adsorption isotherm of (+)-catechin on XAD-7 as a function of temperature, ºC of individual isotherms in the linear region and these data were interpreted in terms of Van t Hoff relation given by Eq. (3). Figure 6 shows a typical Van t Hoff plot for (+)-catechin adsorption on activated carbon and XAD-7 and the estimated value of Hº is found to be 9.79 kcal/mol (R 2 =0.9999) and kcal/mol (R 2 =0.9967) respectively. Since the adsorption enthalpy is a measure of the strength of the solutesorbent binding interaction, the strength of the solutesorbent binding interaction significantly affects the adsorption affinity. The adsorbent, which shows the highest affinity, also shows the highest adsorption enthalpy 41,42. This seems to be reasonable since the adsorption of phenolic compounds exhibited identical behaviour of high adsorption affinity corresponding to the adsorption enthalpy. High value of the adsorption enthalpy for activated carbon in comparison to resins (Table 3) corresponds to high adsorption affinity. In the present case higher value for activated carbon as compared to XAD-7 may be due to the difference in л-electron interactions. However, more data is necessary to establish the dominant adsorption mechanism for the present system. Adsorption kinetics Study of adsorption kinetics is important for understanding the uptake rates of (+)-catechin on the adsorbents particle and determining the equilibrium times of adsorption and column breakthrough for design of adsorption system. Adsorption rate curve were generated for (+)-catechin molecules on activated carbon and XAD-7 only as these two adsorbents show better adsorption capacity than the other resins. The change of rate of (+)-catechin removal from aqueous solutions with contact time is shown in Fig. 7. The rate curves exhibit a rapid initial

7 GOGOI et al.: ADSORPTION OF CATECHIN FROM AQUEOUS SOLUTIONS ON POLYMERIC RESINS 343 particles, the above workers demonstrated the applicability of the model to adsorption on porous small particles. The equation describing the model is given below. The rate of change of concentration of the solid phase is equated to the rate of mass transfer of the solute from the fluid phase through the film to obtain the Eq. dqt k ( Cs,t ) dt (1 ) f = Ct Vpρp ε p (5) Fig. 7 Adsorption rate curve for (+)-catechin on activated carbon and XAD-7 uptake followed by a relatively slow approach to equilibrium, a behaviour not likely to be consistent with a single effective parameter model and it reveals that the removal rate follows the first order kinetics. The observation is similar to that reported for the adsorption of antibiotics in polymeric resins and activated carbon 10,18,43. The adsorption kinetics was much faster for activated carbon than for XAD-7. For both the adsorbents, an asymptotic curve was reached after 3 h of contact time implying that adsorption equilibrium was reached. The kinetics of solute transport from the solution (solvent-solute) phase to the surface of the adsorbent is controlled either by the film or by external diffusion, internal diffusion in the liquid filled pores, pore surface diffusion (homogeneous particle diffusion) and adsorption on the particle surface or the combined effect of more than one of these. In general, adsorption is a rapid process, not a rate-controlling step. The internal diffusion comprises pore and surface diffusion. Whether surface diffusion or pore diffusion (intraparticle) is the rate controlling mechanism depends to a large extent on the method by which the adsorbed particles are contacted with the solution. Because of the rough external surface, activated carbon and resins external mass transfer can be significant under vigorous stirring of the liquid phase and should not be ignored in modeling adsorption kinetics of organics from an aqueous solution 18,44. A two-resistance model based on external mass transfer and particle diffusion, as reported by Mathew and Weber 45 and McKay and McConvey 39 has been used to generate a theoretical concentration versus time decay curve. Although such a model usually holds good for homogeneous permeable, non-porous The average solid phase concentration of the particles is obtained by averaging the point concentration over the volume of the particle r p 3 q = dr (6) t 3 2 rp q0r The Langmuir isotherm will be used to represent the equilibrium adsorption at the surface of the particle q e ( Kqm ) C = 1+ KC s s (7) The Langmuir isotherm for activated carbon and XAD-7 will only be considered for the analysis. For a special particle, the variation of the solid-phase concentration in the radial direction is given by 2 q q 2 q = D + 2 t r r r The material balance for the solute is given by c q V = W t t Initial conditions (8) (9) q(r, 0) = 0 C(0) = C 0 (10) Boundary conditions q q(r p,t) = q s (t) (0,t) = 0 t (11) Eq. (8) can be changed to dimensionless variables by use of the transformations τ = Dt/r p 2 and x = r / r p. Change of variable with U = x q and rearrangement gives

8 344 INDIAN J. CHEM. TECHNOL., SEPTEMBER U U = 2 τ x (12) U (0, τ) = 0 = U (x, 0) and U (k, τ) = U s (τ) (13) 1 k r (C C ) = (14) 0 U f p s dx τ 1000ρp D(1 ε p ) 1 q = 3 Ux dx (15) 0 dc V = -W dt dq dt (16) The set of Eqs (12)-(16) with Eq. (7) was solved by the finite difference techniques illustrated by Mathew and Weber 39. The values of the external mass transfer coefficient, k f, was estimated by using an expression for the initial mass transfer rate (when all the mass transfer resistance is restricted to the external boundary layer and the surface concentration is assumed negligible) 1 d( C / C0 ) k f = S s dt (17) t= 0 where 6W Ss = d ρ (1 ε ) p p p (18) where, W is the weight, d p is diameter, φ p is the density and ε p is the porosity (subscript p refers to particle). The values of the surface diffusion coefficient, which predicted the concentration time decay curves in agreement with the experimental data (Fig. 7) are cm 2 /s and cm 2 /s for XAD-7 and activated carbon respectively. The observed variation in the values of K f and surface diffusivity values may be attributed to approximate assumptions made based on the previous work 10. However, the assumption may appears reasonable in as much as the results of a computation of the concentration versus time profile (Fig. 8) using a single diffusion mode (D α) by the numerical method may be considered to exhibit certain inaccuracy. Further, the slow decay of concentrations with time that suggests an additional resistance, which affect the rate of adsorption, particularly beyond the Fig. 8 Concentration-time decay curve for activated carbon and XAD-7 for aqueous solution of catechin definite amount of time. In both the cases adsorption from the aqueous solutions film diffusion controls the solute uptake initially, and particle diffusion controls the solute uptake in the latter stages. Conclusions The adsorption of (+)-catechin from aqueous phase on activated carbon and four neutral polymeric resins was studied and the experimental data are interpreted on the basis of Langmuir, Freundlich and Redlich- Peterson isotherms. In general activated carbon provides higher adsorption intensity than all the resins. The adsorption intensity is weakly dependent on the aqueous phase ph and the nature of adsorbent was found to be important. Among the four resins studied XAD-7 provides the highest adsorption capacity because of its appropriate surface functional polarity. The adsorption equilibrium data exhibited better fit to Langmuir model for all the adsorbent studied. The rate of adsorption onto activated carbon and XAD-7 appears to be controlled by both external mass transfer and particle diffusion. Nomenclature a R parameter of Redlich-Peterson model b parameter of Redlich-Peterson model C concentration of (+)-catechin (mol -1 ) C e equilibrium concentration of (+)-catechin (mol -1 ) C 0 initial solute concentration (moll -1 ) C ref maximum equilibrium liquid phase concentration of (+)-catechin (mol -1 ) C t solute concentration at time t (moll -1 ) C s,t surface liquid phase solute concentration at time t (moll -1 )

9 GOGOI et al.: ADSORPTION OF CATECHIN FROM AQUEOUS SOLUTIONS ON POLYMERIC RESINS 345 D particle phase diffusion coefficient (cm 2 s -1 ) d p adsorbent particle diameter (cm) K adsorption equilibrium constant K F Freundlich constant (L /g) k constant in Langmuir equation defined as K L X m (Lg -1 ) K L Langmuir constant (L mmol -1 ) k f external mass transfer coefficient (cm s -1 ) n parameter in Freundlich isotherm model q amount of (+)-catechin adsorbed per gram of adsorbent (mmol g -1 ) q e amount of (+)-catechin adsorbed at equilibrium per gram of adsorbent (mmol g -1 ) q t amount of (+)-catechin adsorbed at time t per gram of adsorbent (mmol g -1 ) r separation factor in Vermeulan equation r radial distance (cm) r p particle radius (cm) R universal gas law constant (kcal g mol -1 K -1 ) S s particle surface area (cm -1 ) T absolute temperature (K) t time (s) V volume (l) W weight of adsorbent (g) x dimensionless radial distance (r / r p ) X m monolayer saturation value (mmol g -1 ) ε p porosity of adsorbent particle (-) ρ p density of adsorbent particle (g cm -1 ) Ψ term signifying solute activity coefficient (-) C change in (+)-catechin concentration (mol -1 ) Gº standard free energy of adsorption (kcal mol -1 ) Hº standard enthalpy of adsorption (kcal mol -1 ) Sº standard entropy of adsorption (kcal mol -1 ) References 1 Moini H, Guo Q O & Packer L, Adv Exp Med Biol, 505 (2002) Gramza A & Korczak J, Trends in Food Sci Technol, 16 (2005) Payne G F, Payne N N, Ninomiya Y & Shulter M L, Sep Sci Technol, 24 (1989) Gusler G M, Browne T E & Yoram C, Ind Eng Chem Res, 322 (1993) Payne G F & Shuler M L, Biotechnol Bioeng, 31 (1988) Iskandarani Z & Pietrzyk D J, Anal Chem, 53 (1981) Couture R & Rouseff R, J Food Sci, 57 (1992) Di Mauro A, Fallico B, Passerini A, Rapisarda P & Maccarone E, J Agric Food Chem, 47 (1999) Wilson C W, Wagner C J & Shaw P E, J Agric Food Chem, 37 (1989) Ghosh A C, Satyanarayan K, Srivastava R C & Dutta N N, Colloids Surf A Physichochem Eng Aspects, 96 (1995) Bora M M, Ghosh A C, Mathur R K & Dutta N N, Biosep, 6 (1996) Sahoo G C, Ghosh A C & Dutta N N, J Membrane Sci, 112 (1996) Sahoo G C, Ghosh A C & Dutta N N, Proc Biochem, 32(4) (1997) Dutta M, Baruah R, Dutta N N & Ghosh A C, Colloids Surf A Physichochem Eng Aspects, 127 (1997) Dutta M, Baruah R & Dutta N N, Sep Purif Technol, 12 (1997) Sahoo G C, Dass N N & Dutta N N, J Membrane Sci, 145 (1998) Sahoo G C, Dutta N N & Dass N N, J Membrane Sci, 157 (1999) Dutta M, Dutta N N & Bhattacharya K G, Sep Purif Technol, 16 (1999) Dutta M, Dutta N N & Bhattacharya K G, J Chem Eng Japan, 33(2) (2000) Trochimczuk A W, Streat M & Kolarz B N, React Polym, 46 (2001) Johnson R L & Chandler B V, Food Technol, 42 (1988) Langmuir I, J Am Chem Soc, 38 (1916) Freundlich H, Z Phys Chem, 57(1907) Redlich O & Peterson D L, Phys Chem, 63 (1959) Juang R S, Wu F C & Tseng R L, J Chem Eng Data, 41 (1996) Seidel A, Tzscheutschler E, Radeke K H & Gelbin D, Chem Eng Sci, 40 (1985) Scordino M, Di Mauro A, Passerine A & Maccarone E, J Agric Food Chem, 51 (2003) Silva E M, Pompeu D R, Larondelle Y & Rogez H, Sep Purif Technol, 53 (2007) Huang J, Huang K, Liu S, Luo Q & Xu M, J Colloid Interface Sci, 315 (2007) Liu G, Yu H, Yan H, Shi Z & He B, J Chromatogr A, 952 (2002) Brune B J, Koehler J A, Smith P J & Payne G F, Langmuir, 15 (1999) Brown J L, Chen T H, Embree H D & Payne G F, Ind Eng Chem Res, 41 (2002) Yang W B, Li A M, Zhang Q X & Fei Z H, Sep Purif Technol, 46 (2005) Boqiang F, Liu J, Lei L, Lee F S C & Wang X, J Chromatogr A, 1089 (2005) Yoon S Y, Choi W J, Park J M & Yang J W, Biotechnol Technol, 11 (1997) Scordino M, Di Mauro A, Passerine A & Maccarone E, J Agric Food Chem, 52 (2004) Treybal R E, Mass Transfer Operations (McGraw-Hill International, Singapore), Dabrowski A, Podkoscielny P, Hubicki Z & Barczak M, Chemsphere, 58 (2005) McConvey I F & McKay G, Chem. Eng Process, 19 (1985) Vermeulan Th, Hall K R, Eggleton L C & Acrivos A, Ind Eng Chem Fundam, 5 (1966) Maity N, Payne G F, Ernest M V & Albright R L, React Polym 17 (1992) Maity N, Payne G F & Chipchosky J L, Ind Eng Chem Res, 30 (1991) Otero M, Zabkova M & Rodrigues A E, Sep Purif Technol, 45 (2005) Chatzopoulos D, Verma A & Irvine R L, AIChE J, 39 (1993) Mathew A P & Weber Jr W J, AIChE Symp Ser, 166(73) (1976) 91.

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