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CATALYSIS, KINETICS AND REACTORS Chinese Journal of Chemical Engineering, 18(5) 730 735 (2010) Kinetics of Reductive Leaching of Low-grade Pyrolusite with Molasses Alcohol Wastewater in H2SO4* SU Haifeng ( )1, LIU Huaikun ( )1, WANG Fan ( )1, LÜ Xiaoyan ( )2 and WEN Yanxuan ( )1,** 1 School of Chemistry and Chemical Engineering, Guangxi University, Nanning 530004, China 2 Educational Administration Department, Guangxi University, Nanning 530004, China Abstract The kinetics of reductive leaching of manganese from low grade pyrolusite in dilute sulfuric acid in the presence of molasses alcohol wastewater was investigated. The shrinking core model was applied to quantify the effects of reaction parameters on leaching rate. The leaching rate increases with reaction temperature, concentra- tions of H2SO4 and organic matter in molasses alcohol wastewater increase and ore particle size decreases. The leaching process follows the kinetics of a shrinking core model and the apparent activation energy is 57.5 kJ·mol–1. The experimental results indicate a reaction order of 0.52 for H2SO4 concentration and 0.90 for chemical oxygen demand (COD) of molasses alcohol wastewater. It is concluded that the reductive leaching of pyrolusite with molasses alcohol wastewater is controlled by the diffusion through the ash/inert layer composed of the associated minerals. Keywords pyrolusite, molasses alcohol wastewater, reductive leaching, kinetics 1 INTRODUCTION With an ever increasing demand for manganese and gradual depletion of high grade manganese ore, many efforts have been made to recover manganese from low-grade pyrolusite. Generally, pyrolusite can be treated by roasting reduction-acid leaching [1] and direct reductive leaching in H2SO4 or HCl solution. The reductive agents in H2SO4 solution include H2O2 [2], H2C2O4 [1], FeSO4 [3] and SO2 [4 6], while the reductive agents in HCl solution include alcoholic [6], nickel matte [7], pyrite [8] and H2O2 [9]. Recently, carbohydrates from agriculture wastes were treated as the potential reducing agents for the leaching of manganese ore in mild acidic solution [10 14]. Molasses alcohol wastewater (MSW), which is generated from the fermentation of cane sugar mo- lasses for production of alcohol [15], has a high re- ducing capacity in acidic medium for its content of melanoidins, caramel and phenolics. In our previous work, MSW was used as reducing agent to leach py- rolusite, and the optimum condition in dilute sulfuric acid solution was reported [16]. In addition, color re- moval is a main problem in the treatment of such wastewater [15]. As indicated in our research [17], leaching is an effective method to remove the organics in MSW by using pyrolusite and its slurry as reducing agent and adsorbent. Meanwhile, a comprehensible understanding of the leaching kinetics is needed for an efficient design of leaching manganese ore. Precious research [18] on the leaching kinetics of MnO2 by SO2 showed that the key step during the leaching process is chemical reac- tion and its apparent activation energy is 35.9 kJ·mol–1. Similarly, the leaching rate of MnO2 with Fe2+ in H2SO4 solution is also controlled by chemical reaction with the apparent activation energy of 28 kJ·mol 1 [19]. Momade and Momade [20] reported that the leaching after 30 min in aqueous methanol-sulfuric acid system can be described by the diffusion controlled shrinking core model. According the investigation of Veglio et al. [12], the leaching in lactose-sulphuric acid follows a shrinking core model with variable activation energy. Lasheen et al. [14] studied the leaching kinetics of manganese oxide ore with molasses in nitric acid so- lution and found that the leaching is controlled by the diffusion through the “product” layer composed of the associated minerals and the apparent activation energy is 27.5 kJ·mol–1. Most works [12, 14, 18 20] on the leaching kinet- ics of pyrolusite mainly focused on the reductive sys- tems of small molecule. However, the reductive agents in MSW are macromolecule with the molecular weight of 2000 9000 [21]. To date, the leaching kinet- ics of pyrolusite by macromolecular reductive agents has not been reported. In this work, we investigated the kinetics of the reductive leaching manganese from pyrolusite by the macromolecular reductive agents of MSW and the main system variables on the leaching rate. The kinetic model and the apparent activation energy were determined. 2 MATERIALS AND METHODS 2.1 Materials Manganese ore was obtained from Mugui Man- ganese Mine, Guangxi, China. The ore samples were crushed to 0.147 mm (–100 meshes). The chemical composition of the manganese ore used are listed in Received 2010-02-24, accepted 2010-05-02. * Supported by the National Natural Science Foundation of China (20866001) and the Natural Science Foundation of Guangxi Province (0832035). ** To whom correspondence should be addressed. E-mail: wenyanxuan@vip.163.com Chin. J. Chem. Eng., Vol. 18, No. 5, October 2010 731 Tables 1 and 2. MSW (Nanning Sugarcane Refinery, Guangxi, China), containing 7.3% organic compounds, 2.9% reducing sugars, CODCr 1.3×105 mg·L–1 and BOD5 7.0×104 mg·L–1, was used in this work. All other chemicals were of analytical grade and used without further purification. Table 1 Chemical composition of the pyrolusite sample Component Mass content/% Mn 22.25 MnO2 31.78 Fe 12.35 SiO2 24.17 Al2O3 11.36 CaO 0.12 MnO 0.12 S 0.005 P 0.078 Table 2 Manganese content of different particle size of pyrolusite Particle size d0/mm Manganese mass content/% 0.134 25.72 0.078 24.10 0.068 9.94 0.046 19.00 2.2 Leaching procedure To investigate the effects of reaction parameters, including stirring speed, particle size, acid concentra- tion, MSW concentration and leaching temperature, the comparative leaching experiments were carried out. The leaching experiments were carried out in a 1000 ml three-neck flask immersed in thermostat water bath with mechanical stirring. In a typical experiment, 5.0 g of ore was added to 500 ml sulfuric acid-MSW solu- tion under stirring (700 r·min–1), and leaching started after manganese ore was added to the solution. After reaction, the slurry was filtered and the residue was washed with distilled water. The filtrate was then di- luted in HNO3 solution (pH 2) for analysis. The Mn concentration during the leaching process was meas- ured by an inductively coupled plasma spectropho- tometer (ICP, Optima 5300 DV, Perkin Elmer). The leaching efficiency was calculated by referring the amount of leached metal in the liquor to its original input quantity. Organic MSW concentration (the mass of the all organic compounds in the dilute sulfate acid solution) is expressed by the COD values. The ratio of liquor to solid was kept as 100 1. The changes of H2SO4 concentration and COD can be neglected dur- ing each leaching test. Unless otherwise specified, the values of temperature, H2SO4 concentration, COD and particle size of manganese ore were selected as 80 °C, 1.0 mol·L–1, 37.7 g·L–1 and 0.0676 mm, respectively. At the end of leaching experiment, the slurry was fil- tered and the filtrate was analyzed for leached man- ganese concentration. All the experiments were re- peated twice, and their relative deviation is always below 1.0 %. 3 RESULTS AND DISCUSSION 3.1 Chemical reaction The reduction and dissolution mechanism of py- rolusite in H2SO4 solution with MSW still remains unclear. The chemical reactions taking place during dissolution of the manganese dioxide in the presence of sucrose [6] or glucose [13] can be described by the following reactions: 2 12 22 11 2 424MnO C H O 24H SO 4 2 224MnSO 12CO 35H O (1) 2 6 12 6 2 412MnO C H O 12H SO 4 2 212MnSO 6CO 18H O (2) In this study, XRD was used to identify the min- eralogical composition of ore samples before and after leachingtreatment. The corresponding XRD patterns are shown in Fig. 1. The raw ore comprises of py- rolusite (MnO2), hematite (Fe2O3), silicon oxide (SiO2) and kaolinite (Al2Si2O5(OH)4), while the leach resi- dues are mainly silicon oxide, kaolinite and some hematite. These results suggested that no insoluble product forms during the leaching processes. So the reaction between pyrolusite and MSW in H2SO4 solu- tion can be written as follows: 2 2 4 4 2 2 (C - H O ) 2 MnO 2 H SO 2 MnSO CO H O x y m m m m m z (3) Figure 1 XRD pattern of pyrolusite and its residue after leaching 1 pyrolusite; 2 residue; MnO2; SiO2; Al2Si2O5(OH)4; Fe2O3 3.2 Effect of parameters Figure 2 shows the effect of stirring speed in the range of 100 1100 r·min–1 on the reductive leaching Chin. J. Chem. Eng., Vol. 18, No. 5, October 2010 732 of pyrolusite. The conversion of manganese first in- creased when stirring speed increased from 100 to 700 r·min–1 due to enhanced diffusion of liquid reactants. However, a slight decrease in the conversion of man- ganese was detected when stirring speed was increased from 700 to 1000 r·min–1, because violent agitation may cause some pyrolusite particles adhered onto the inner wall of three-neck flask and worse contact be- tween particles and liquid reactants, which reduce the leaching efficiency. The most leaching rate is achieved at 700 r·min–1 stirring speed, which was used in the subsequent experiments. The effects of initial particle size of manganese ore, H2SO4 concentration, COD and leaching tem- perature on the leaching of ore are illustrated in Fig. 3, respectively. The results show the conversion of man- ganese increases gradually with the increase of H2SO4 concentration, MSW concentration and leaching tem- perature and with the decrease of the average sizes of particle. 3.3 Kinetic analysis Kinetic modeling yields comprehensive informa- tion regarding leaching mechanisms. In fact, reactions involved in this process are heterogeneous in nature involving mass transport of reactant and product ions. In acidic leaching, the heterogeneous non-catalytic reaction for most manganese ore might be kinetically interpreted by using the shrinking core model (SCM) [18 20]. In the SCM model, the solid reactant is consid- ered as non-porous particle and is initially surrounded by a fluid film through which mass transfer occurs between the solid particle and the bulk of the fluid. As the reaction proceeding, an ash/inert layer forms around the unreacted core. Detailed derivation of the shrinking core model can be found in Refs. [22 24]. The dissolution of pyrolusite can be expressed as follows: A (fluid) bB (solid) fluid products (4) The rate-limiting step, which decides the form of the rate equation, may be one of the following three steps: (1) diffusion through the liquid film surround- ing a solid particle, (2) diffusion through the ash/inert solid layer and (3) chemical reaction on the surface of the unreacted core. The simplified equations of the shrinking core model when liquid film diffusion, ash/inert solid layer diffusion or the surface chemical Figure 2 Manganese extraction vs. time at various stirring speeds 100 r·min–1; 200 r·min–1; 500 r·min–1; 700 r·min–1; 1100 r·min–1 (a) Influence of particle size of manganese ore d0/mm: 0.0134; 0.078; 0.068; 0.046 (b) Influence of sulfuric acid concentrations cH/mol·L 1: 0.4; 0.6; 0.8; 1.0; 1.2 (c) Influence of molasses alcohol wastewater concentration cW/g·L 1: 10.0; 20.0; 30.0; 37.7; 50.0 (d) Influence of leaching temperature T/K: 313; 323; 333; 343; 353; 363 Figure 3 Manganese extraction vs. time at different con- ditions Chin. J. Chem. Eng., Vol. 18, No. 5, October 2010 733 reactions is the slowest step can be expressed as fol- lows, respectively [22]: G S A0 f S 0 3k M x c t k t a r (5) 2 S Aeff A03 d2 S 0 221 1 3 M D cx x t k t a r (6) 1 S c3 A0 r S 0 1 1 M kx c t k t a r (7) where kf, kd and kr are calculated from Eqs. (5), (6) and (7), respectively. To obtain the leaching kinetic equation, the ex- perimental data in Fig. 3 were transformed and fitted to Eqs. (5), (6) and (7), respectively. As shown in Fig. 4, Eq. (6) fitted the data best for the range of experiments and the correlation coefficients (R2) were greater than 0.98. It is suggested that the reductive leaching of py- rolusite was controlled by the diffusion through the ash/inert solid layer. Hence, the insoluble oxide min- erals (hematite, quartz, kaolinite, etc.) associated with pyrolusite may act as the ash/inert layer [2, 14]. Leaching kinetic constant varies with the inverse square of initial particle size for diffusion-controlled reactions in Eq. (6), or the inverse of the size or the surface chemical reaction in Eq. (7). Fig. 5 shows the quantitative relationship between the apparent rate constant (kd) and particle size ( 20r ), indicating the linear relationship between kd and 20r with R 2 of 0.96. It is affirmed that the leaching of pyrolusite with MSW is controlled by the diffusion of reactant through a solid product layer. The apparent activation energy was determined based on the Arrhenius equation: a d 1ln ln E k A R T (8) The plot of lnkd versus 1/T data for the six tempera- tures is linear (Fig. 6). The apparent activation energy (Ea) was, hence, determined to be 57.5 kJ·mol–1, which is about twice of that reported by Lasheen et al. [14]. The reason may be that the diffusion of the mac- romolecular reductive agents in MSW is slower than that of small molecular reductive agents in molasses. To decide the apparent reaction order with re- spect to reagent concentration, the kd values for each H2SO4 concentration and COD were determined from Figs. 3 (b) and 3 (c); and the plots of lnkd versus lncH or lncW were obtained. As shown in Fig. 7, the order of reaction was found be 0.52 with respect to H2SO4 concentration and 0.90 with respect to COD. It seems that the leaching rate of manganese depends more on the concentration of reductive organics. According Eq. (6), the apparent rate constant kd can be expressed as follows: 0.52 0.900 d H W2 0 57500exp kk c c RTr (9) (a) Influence of particle size of manganese ore d0/mm: 0.0134; 0.078; 0.068; 0.046 (b) Influence of sulfuric acid concentrations cH/mol·L–1: 0.4; 0.6; 0.8; 1.0; 1.2 (c) Influence of COD of waste water cW/g·L–1: 10.0; 20.0; 30.0; 37.7; 50.0 (d) Influence of leaching temperature T/K: 313; 323; 333; 343; 353; 363 Figure 4 Plot of 2 321 (1 ) 3 x x vs. time at different conditions and 0k 119.09 mm 2·(mol·L–1)–0.52·(g·L–1)–0.90·s–1 as calculated from the provided data in Fig. 4. Chin. J. Chem. Eng., Vol. 18, No. 5, October 2010 734 Figure 5 Relationship between rate constant and average initial particle diameter Figure 6 Arrhenius plot of reaction rate against reciprocal temperature Figure 7 Determination of reaction order for pyrolusite dissolution with respect to H2SO4 and COD of molasses alcohol wastewater COD; H2SO4 concentrations By the above analysis, the kinetic model of py- rolusite leaching by MSW is: 2 0.52 0.903 H W2 0 2 119.09 575001 1 exp 3 x x c c t RTr (10) To determine the adaptability of Eq. (10), the x values calculated by Eq. (10) were compared with that obtained from the experiments. The calculated con- versions in Fig. 8 agree well with the experimental data with the average relative error of 0.00107. 4 CONCLUSIONS The reductive leaching kinetics of pyrolusite with molasses alcohol wastewater in dilute H2SO4 solution was investigated. The main parameters influencing leaching rate, such as leaching H2SO4 concentration, molasses alcohol wastewater concentration, particle size and stirring speed, were studied. The results re- veal that the leaching rate increases gradually with the increaseof H2SO4 concentration, COD of molasses alcohol wastewater and leaching temperature and with the decrease of the size of particles. The kinetic analysis shows that the leaching process is controlled by diffusion through the insolu- ble layer of the associated minerals. The leaching process follows the kinetic model: 2 0.52 0.903 H W2 0 2 119.09 575001 1 exp 3 x x c c t RTr with apparent activation energy of 57.5 kJ·mol–1. The experimental results also show a reaction order of 0.52 with respect to H2SO4 concentration and a reaction order of 0.90 with respect to molasses alcohol wastewa- ter. The effects of particle size and rate constant further confirm the mechanism of the leaching kinetic model. NOMENCLATURE A constant of the Arrhenius equation b stoichiometric coefficient cA0 concentration of component A in bulk phase, mol·L–1 or g·L–1 cH H2SO4 concentration, mol·L–1 cW COD of molasses alcohol wastewater, g·L–1 DAeff effective diffusion coefficient of component A in the ash/inert solid layer, m·s–2 Ea apparent activation energy, kJ·mol–1 kc chemical kinetic constant, m·s–1 kd apparent rate constant when ash/inert solid layer diffusion con- trols, min–1 kf apparent rate constant when liquid film diffusion controls, min–1 kG mass transfer coefficient of component A in the liquid film, m·s–1 kr apparent rate constant when chemical reaction controls, min–1 k0 kinetic constant, mm2·(mol·L–1)–0.52·(g·L–1)–0.90·s–1 MS molecular weight of MnO2 R gas constant, 8.314 J·mol–1·K–1 r0 initial radius of pyrolusite, mm T reaction temperature, K t reaction time, min x fraction of reacted pyrolusite s pyrolusite density, kg·m–3 Figure 8 Mn extraction (x) of calculation and experiments Chin. J. Chem. Eng., Vol. 18, No. 5, October 2010 735 REFERENCES 1 Sahoo, P.K., Srinivasa, R.K., “Sulphating-roasting of low grade manganese ore: Optimisation by factorial design”, Int. J. Miner. Proc- ess, 25 (1–2), 147 152 (1989). 2 Jiang, T., Yang, Y., Huang, Z., Zhang, B., Qiu, G., “Leaching kinetics of pyrolusite from manganese-silver ores in the presence of hydro- gen peroxide”, Hydrometallurgy, 72 (1-2), 129 138 (2004). 3 Das, S.C., Sahoo, P.K., Rao, P.K., “Extraction of manganese from lowgrade manganese ores by FeSO4 leaching”, Hydrometallurgy, 8 (1), 35 47 (1982). 4 Abbruzzese, C., “Percolating leaching of manganese ores by aque- ous sulphur dioxide”, Hydrometallurgy, 25 (1), 85 97 (1990). 5 Naik, P.K., Sukla, L.B., Das, S.C., “Aqueous SO2 leaching studies on Nishikhal manganese ore through factorial experiment”, Hydro- metallurgy, 54 (2-3), 217 228 (2000). 6 Veglio, F., Toro, L., “Fractional factorial experiments in the devel- opment of manganese dioxide leaching by sucrose in sulphuric acid solutions”, Hydrometallurgy, 36 (2), 215 230 (1994). 7 Chen, H.H., Fu, C., Zheng, D.J., “Reduction leaching of manganese nodules by nickel matte in hydrochloric acid solution”, Hydrometal- lurgy, 28 (2), 269 275 (1992). 8 Kanungo, S.B., “Rate process of the reduction leaching of manga- nese nodules in dilute HCl in presence of pyrite (1) Dissolution be- havior of iron and sulphur species during leaching”, Hydrometal- lurgy, 52 (3), 313 330 (1999). 9 El Hazek, M.N., Lasheen, T.A., Helal, A.S., “Reductive leaching of manganese from low grade Sinai ore in HCl using H2O2 as reduc- tant”, Hydrometallurgy, 84 (3-4), 187 191 (2006). 10 Pagnanelli, F., Garavini, M., Vegliò, F., Toro, L., “Preliminary screening of purification processes of liquor leach solutions obtained from reductive leaching of low-grade manganese ores”, Hydro- metallurgy, 71 (3-4), 319 327 (2004). 11 Trifoni, M., Veglió, F., Taglieri, G., Toro, L., “Acid leaching process by using glucose as reducing agent: A comparison among the effi- ciency of different kinds of manganiferous ores”, Miner. Eng., 13 (2), 217 221 (2000). 12 Veglio, F., Trifoni, M., Pagnanelli, F., Toro, L., “Shrinking core model with variable activation energy: A kinetic model of manganif- erous ore leaching with sulphuric acid and lactose”, Hydrometal- lurgy, 60 (2), 167 179 (2001). 13 Trifoni, M., Toro, L., Veglió, F., “Reductive leaching of manganif- erous ores by glucose and H2SO4: Effect of alcohols”, Hydrometal- lurgy, 59 (1), 1 14 (2001). 14 Lasheen, T.A., El Hazek, M.N., Helal, A.S., “Kinetics of reductive leaching of manganese oxide ore with molasses in nitric acid solu- tion”, Hydrometallurgy, 98 (3-4), 314 317 (2009). 15 Satyawali, Y., Balakrishnan, M., “Wastewater treatment in molas- ses-based alcohol distilleries for COD and color removal: A review”, J. Envir. Manag., 86 (3), 481 497 (2008). 16 Su, H., Wen, Y.X., Wang, F., Li, X., Tong, Z., “Leaching of py- rolusite using molasses alcohol waste water as reductant”, Miner. Eng., 22 (2), 207 209 (2009). 17 Su, H., Li, K., Wen, Y., Tong, Z., “Decolorization and degradation of molasses alcohol waste water by using pyrolusite as oxidant”, Chem. Eng. (China), 37 (6), 66 70 (2009). (in Chinese). 18 Miller, J.D., Wan, R.Y., “Reaction kinetics for the leaching of MnO2 by sulfur dioxide”, Hydrometallurgy, 10 (2), 219 242 (1983). 19 Tekin, T., Bayramoglu, M., “Kinetics of the reduction of MnO2 with Fe2+ in acidic solutions”, Hydrometallurgy, 32 (1), 9 20 (1993). 20 Momade, F.W.Y., Momade, Zs.G., “A study of the kinetics of reduc- tive leaching of manganese oxide ore in aqueous methanol-sulphuric acid medium”, Hydrometallurgy, 54 (1), 25 39 (1999). 21 Takaichi S., “Studies on the colored components in cane final mo- lasses”, Proc. Res. Soc. Japan Sugar, 40 (2), 57 63 (1992). 22 Levenspiel, O., Chemical Reaction Engineering, 3rd edition, Wiley & Sons, New York, 566 588 (1999). 23 Zhou, H.M., Zheng, S.L., Zhang, Y., “Kinetics investigation on the of niobium from a low-grade niobium-tantalum ore by concentrated KOH solution”, Chin. J. Chem. Eng., 12 (2), 202 207 (2004). 24 Li, Y.X., Zhang, S.B., Guo, H.X., “Application of the shrinking core model to the kinetics of zinc oxide desulfurization”, Chin. J. Chem. Eng., 5 (4), 296 303 (1997).
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