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Zhao, H., Wu, H., Hu, H., Li, Y., Li, J., and Zhang, X. (2018). "Cooperative decomposition of hydrogen peroxide by lignin-combined transition metals in pulp bleaching," BioRes. 13(2), 3922-3931.

Abstract

The effects of lignin-combined manganese ion, iron ion, and lignin-combined iron and manganese on the decomposition of hydrogen peroxide were investigated. Elemental analysis and inductively coupled plasma-atomic emission spectrometry were used to analyze the chemical features of the lignin composites and the amount of metal ions present in the solution or adsorbed on lignin, respectively. The results showed that the main transition metal elements remaining in the precipitated lignin were Fe, Mn, and Cu. The hydrogen peroxide decomposition in the presence of lignin-combined transition metal was represented by pseudo-first-order kinetics, and the pseudo-first-order rate constant (kobs) of peroxide decomposition with lignin-combined iron was 0.0068 min-1, while it was 0.0063 min-1 in the presence of lignin-combined manganese. A synergistic effect of manganese and iron combined with lignin on peroxide decomposition was demonstrated, and a kobs value of 0.0053 min-1 was obtained. The mixed addition of magnesium sulfate (MgSO4), sodium silicate (Na2SiO3), and ethylene diamine tetraacetic acid disodium salt (Na2EDTA) resulted in an optimal reduction in peroxide decomposition when single lignin-combined metal ion existed. However, adding Na2EDTA alone had an optimal effect on the reduction of peroxide decomposition in the presence of lignin-combined iron and manganese, with a kobs value of 0.0004 min-1.


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Cooperative Decomposition of Hydrogen Peroxide by Lignin-combined Transition Metals in Pulp Bleaching

Huifang Zhao,a,* Haibiao Wu,b Haowei Hu,a Yan Li,a Jing Li,a and Xuejin Zhang a

The effects of lignin-combined manganese ion, iron ion, and lignin-combined iron and manganese on the decomposition of hydrogen peroxide were investigated. Elemental analysis and inductively coupled plasma-atomic emission spectrometry were used to analyze the chemical features of the lignin composites and the amount of metal ions present in the solution or adsorbed on lignin, respectively. The results showed that the main transition metal elements remaining in the precipitated lignin were Fe, Mn, and Cu. The hydrogen peroxide decomposition in the presence of lignin-combined transition metal was represented by pseudo-first-order kinetics, and the pseudo-first-order rate constant (kobs) of peroxide decomposition with lignin-combined iron was 0.0068 min-1, while it was 0.0063 min-1 in the presence of lignin-combined manganese. A synergistic effect of manganese and iron combined with lignin on peroxide decomposition was demonstrated, and a kobs value of 0.0053 min-1 was obtained. The mixed addition of magnesium sulfate (MgSO4), sodium silicate (Na2SiO3), and ethylene diamine tetraacetic acid disodium salt (Na2EDTA) resulted in an optimal reduction in peroxide decomposition when single lignin-combined metal ion existed. However, adding Na2EDTA alone had an optimal effect on the reduction of peroxide decomposition in the presence of lignin-combined iron and manganese, with a kobs value of 0.0004 min-1.

Keywords: Decomposition; Hydrogen peroxide; Lignin-combined transition metals; Reaction kinetics; Bleaching stabilizers

Contact information: a: School of Biological and Chemical Engineering /School of Light Industry, Zhejiang University of Science & Technology, Hangzhou, 310023, China; b: Hangzhou Huawang New Material Technology Co. Ltd., Lin’ an, 311300, China; *Corresponding author: zhf9966@163.com

INTRODUCTION

With the increasing awareness in society of environment protection issues, elemental chlorine free (ECF) and totally chlorine free (TCF) bleaching technologies have become important trends in the field of pulp bleaching. Hydrogen peroxide is the most important total-chlorine-free bleaching agent and is widely used for pulp bleaching due to its higher efficiency, lower cost, and better operability (Sixta 2006). Unfortunately, transition metals present in pulp are active in catalysis of the decomposition of hydrogen peroxide under certain bleaching conditions. Several studies involving transition metal induced peroxide decomposition have been conducted to try and control the unwanted decomposition of peroxide in the bleaching process, especially for iron ions and manganese ions (Wekesa and Ni 2003, 2011; Popov et al. 2007; Zhang et al. 2015, 2016).

Previous studies have shown that transitional metals are present in many different states during the bleaching process. These states include the “non-equilibrium” suspended particles, oligomer dynamic equilibrium with carboxylic groups of fiber, and the oligomer chelated with residual lignin by forming coordinate bonds with phenolic groups (Cardona-Barrau et al. 2001; Norberg et al. 2001; Zhang et al. 2010; Wekesa et al. 2011). In the case of high yield pulping, peroxide bleaching is performed together with the pulping process, with a certain content of dissolved lignin in waste liquor or residual lignin in pulp. Lignin is an amorphous, polyphenolic, highly cross-linked polymer consisting of certain numbers of active carboxyl and hydroxyl (phenolic or non-phenolic) sites that can be available for complexation with metal ions. According to several studies, lignin has been found to be suitable for transition metal removal from wastewater (Guo et al. 2008; Li et al. 2015). Various studies have investigated the mechanisms of interaction between transition metal and lignin (Merdy et al. 2002; Huang et al. 2015; Lin et al. 2016). Lignin can adsorb Fe (III) strongly at low pH (<3) while Mn(II) forms far less stable surface complexes at pH = 8.0. Redox processes take place as the metal ions are adsorbed onto lignin (Merdy et al. 2002). An outer-sphere complex is formed between Cr(III) and lignin, with the carbonyl groups as the predominant sites. In contrast to Cr(III), a reduction reaction has occurred in the case of Cr(VI) with the carbonyl and phenolic groups in lignin (Lin et al. 2015). Metal ions bound to lignin show less catalytic activity than the corresponding free ions in the solution (Zhang et al. 2016). The effect of different stabilizers on peroxide in the presence of both dissolved lignin and transition metals might change with the external conditions. For instance, the presence of calcium ion can decrease the adsorption of manganese onto lignin (Merdy et al. 2002), which may alter the catalytic action of peroxide decomposition. Therefore, further understanding of the effects of complexation between transition metals and lignin on decomposition of peroxide is important for the accurate characterization and effective control of the invalid decomposition of peroxide during the bleaching process.

In this study, lignin was prepared from the black liquor of a eucalyptus pulping process using hydrochloric acid without further purification, to simulate the dissolved lignin in the bleaching process. Ethylene diamine tetraacetic acid disodium salt (Na2EDTA), sodium silicate (Na2SiO3), and magnesium sulfate (MgSO4) were chosen as stabilizers for peroxide. The chemical composition of the precipitated lignin was studied using modern analytical methods, and the effects of different lignin-combined transition metals and different stabilizers on hydrogen peroxide decomposition were studied.

EXPERIMENTAL

Materials

All the reagents used in this study were of analytical grade and used without further purification. Manganese sulfate (MnSO4•H2O) and ammonium ferric sulfate (NH4Fe(SO4)2•12H2O) were supplied by Dongguan Dongjiang Chemical Reagent Co., Ltd. (Dongguan, China). The black liquor was purchased from Guangxi Jingui Pulp & Paper Co., Ltd. (Qinzhou, China). The pH level was adjusted by a standard sodium hydroxide solution. Milli-Q (Millipore Corporation, Billerica, MA, USA) deionized water was used throughout the experiments.

Methods

Separation of precipitated lignin

In the initial experimental process, precipitated lignin was separated from the black liquor of eucalyptus pulping. Firstly, the black liquor was diluted to 10% concentration by deionized water. Then, the black liquor was screened to obtain 400-mesh fraction. The filtrate was acidified to a pH of 2 to 2.5 using hydrochloric acid, and then stirred for 1 h. The liquid-sediment suspension was then transferred to a centrifugal tube, and the acid liquor was separated at a centrifugal speed of 5000 rpm. The solid was freeze dried under a vacuum. The dried solid was washed with deionized water (20 g•L-1), shaken on an end-over-end shaker for 3 h, separated by centrifugation, and then freeze-dried. This washing and drying procedure was repeated twice, and the solid obtained was termed “precipitated lignin”, which was used throughout the experiments.

Processing-complexation reaction of transition metal by precipitated lignin

The suspension of the precipitated lignin sample was magnetically and vigorously stirred for 2 h to hydrate the sample prior to the introduction of the metal ion. A standard stock solution of manganese ion was prepared by dissolving manganese sulfate into deionized water with 0.1 M HCl solution. A complexation process of metal ions by precipitated lignin took place prior to the peroxide decomposition reaction. The complexation reaction was conducted under the following conditions: metal concentration of 2 ppm, precipitated lignin concentration of 5 g•L-1, reaction temperature of 60 C, and 160 r•min-1 for 24 h. The mixed solutions were cooled sequentially to room temperature using a mixture of ice and water.

Decomposition of hydrogen peroxide

All hydrogen peroxide decomposition processes were conducted in 50-mL polyethylene bottles maintained in a constant temperature water bath at a temperature of 60 °C. The decomposition processes were performed under the following conditions: pH level of 11.0, initial hydrogen peroxide concentration of 2.777 g•L-1 (2.5% on oven-dry (o.d.) pulp at 10% consistency), metal concentration of 2 ppm, precipitated lignin concentration of 5g•L-1, or without any precipitated lignin.

Decomposition of hydrogen peroxide with stabilizers

The stabilities of the additives during the hydrogen peroxide decomposition process were studied. Magnesium sulfate (MgSO4) (0.25% on o.d. pulp at 10% consistency), sodium silicate (Na2SiO3) (2.5% on o.d. pulp at 10% consistency), and Ethylenediamine-tetraacetic acid disodium salt (Na2EDTA) (0.05% on o.d. pulp at 10% consistency) were selected as stabilizers to inhibit the decomposition of hydrogen peroxide, either individually or in combination. The addition-sequence of these chemicals was as follows: Na2EDTA, Na2SiO3, MgSO4, and hydrogen peroxide. There was a 5 min interval and some stirring between the addition of each chemical.

Measurements and Characterization

The content of C, H, N, and S elements in the precipitated lignin was quantified by dry combustion in an autoanalyzer (Vario MAX cube, Elementar Analysensysteme GmbH, Hanau, Germany). X-ray diffraction (XRD; D/max-IIIA, Rigaku Corporation, Tokyo, Japan) was used to identify the crystalline structure of the freeze-dried samples. The amount of metal was determined using inductively coupled plasma-atomic emission spectrometry with an iCAP6300 (ICP-AES; Thermo Electron Corporation, Waltham, MA, USA). The peroxide concentration was measured according to standard iodometric titration using ammonium molybdate solution as a catalyst.

RESULTS AND DISCUSSION

Elemental Analysis of Precipitated Lignin

The concentrations of metal ions in the lignin precipitate are shown in Table 1. The elemental analysis and inductively coupled plasma-atomic emission spectrometry showed that the precipitated lignin had the following percentage composition: C, 41.66%; H, 4.92%; N, 0.90%; S, 2.21%; ash, 23.16%; Ca, 0.254%; Mg, 0.06%; Fe, 0.02%; Cu, 0.0022%; and Mn, 0.0074%. The results were different from those recorded in related literature. In one study, the target lignin contained Ca, 0.06%; Na, 1.4%; Mg, 0.01%; Fe, 0.007%; and Al, 0.03% (Guo et al. 2008). In another study, the target lignin contained Ca, 0.18%; Mg, 0.019%; Fe, 0.0058%; and Mn, 0.0057% (Svärd et al, 2016). These differences are likely due to the different pulping chemicals and process water. Table 1 also showed clearly that the main transition metal elements in the precipitated lignin were Fe, Mn, and Cu, which may have been adsorbed strongly onto lignin through chelation.

Table 1. Characterization of Precipitated Lignin

XRD of Fresh Manganese and Fresh Iron

It is well known that Mn2+ starts to hydrolyze when the pH level is greater than 8, forming Mn(OH)2 precipitate or mixed manganese precipitate in the presence of O(Morgan 2005). The results of the XRD phase analysis of fresh manganese precipitates are given in Fig. 1. The phases present in the fresh manganese sample were identified in accordance with the powder diffraction data contained in the portable document format (PDF) cards. The XRD powder patterns of fresh manganese were ascribed to Mn3O4 according to the Joint Committee Powder Diffraction Standards (JCPDS card 75-1560), Mn3O4 (JCPDS card 18-0803), 7Mn(OH)2·2MnSO4·H2O (JCPDS card 18-0788), and Mn(OH)2 (JCPDS card 73-1133). The patterns indicated that the precipitates of fresh manganese were mixed crystal, composed of Mn3O4, Mn(OH)2, and 7Mn(OH)2·2MnSO4·H2O, and consisted of two kinds of Mn-OH.

Fig. 1. XRD of fresh manganese

Generally speaking, the iron ion starts to hydrolyze when pH value exceeds 1; Fe(OH)i3-i is formed initially, and then polynuclear hydrolyzed species are formed within milliseconds (Schneider 1988; Deng 1997). The iron ions precipitated in the early stage are gradually transformed to crystalline iron (III) hydroxides. Additionally, different kinds of mononuclear or polynuclear complexes can be generated at a higher pH. As a result, different states of iron can be formed during the hydrolysis and oxidizing process, such as FeO(OH) and Fe2O3. The results of the XRD phase analysis of fresh iron precipitates are presented in Fig 2.

Fig. 2. XRD of fresh iron

The XRD powder patterns were just ascribed to thenardite (JCPDS card 37-1465), without any XRD of iron appearance, which indicated that the hydrolysis products of the iron ion were only amorphous iron without any crystalline phases. The result is similar to the previous studies; that is, there was not enough time to transform from amorphous iron to crystalline iron (III) hydroxides (Deng 1997).

Decomposition of Alkaline Hydrogen Peroxide with Manganese and Lignin

To quantify the invalid decomposition of hydrogen peroxide induced by metal ions combined with lignin, a kinetic model was firstly proposed. Under alkaline conditions, hydrogen peroxide decomposition in the presence of manganese or iron was represented by pseudo-first-order kinetics (Ni et al. 2000; Saisaha et al. 2013; Zeineb et al. 2015),

ln([H2O2] / [H2O2]0) = –kobst (1)

where kobs is the pseudo-first-order rate constant for the decomposition of hydrogen peroxide and t is time (min).

Table 2. Pseudo-first-order Rate Constant for the Decomposition of Hydrogen Peroxide with Manganese and in presence of Lignin

The crystallization of manganese hydroxides showed noticeable activity in the hydrogen peroxide decomposition in the previous research (Ryabova et al. 2016). At high pH value (pH>10), the Mn(Ⅱ) can be oxidized by H2Oto form MnO2 (Calull et al. 1988). The pseudo-first-order rate constants for the decomposition of hydrogen peroxide with manganese and lignin at pH level of 11.0 are illustrated in Table 2. The results showed that the stabilizers had a positive effect on decreasing peroxide decomposition whether they were added individually or at the same time. Lignin is also a complex organic ligand, which would form stable complex such as [lignin-Mn-OH], and would promote the catalytic decomposition of hydrogen peroxide (Calull et al. 1988). The mixed addition of MgSO4, Na2SiO3, and Na2EDTA had the most positive effect on the reduction of peroxide decomposition with free manganese ions, having a kobs value of 0.0010 min-1. The kobs for the decomposition of alkaline hydrogen peroxide with manganese and lignin without any additives was 0.0063 min-1.

Decomposition of Alkaline Hydrogen Peroxide with Iron and Lignin

The pseudo-first-order rate constants for the decomposition of hydrogen peroxide with iron and lignin are presented in Table 3. It was confirmed that the addition of Na2EDTA, MgSO4, and Na2SiO3, in combination or individually, improved the stability of peroxide under alkaline conditions. The addition of a mixture of MgSO4, Na2SiO3, and Na2EDTA had the most positive effect on reducing peroxide decomposition, with a kobs value of 0.0006 min-1. The kobsof decomposition of alkaline hydrogen peroxide was only 0.0068 min-1 with the existence of lignin-combined iron, which was higher than 2.2×10-3 min-1 in the presence of magnetite particles under different conditions (Zebardast et al. 2013). In addition, the present results revealed that iron (Ⅲ) caused more catalytic decomposition than Mn(II), which was in good agreement with the effect in peroxide bleaching process in the presence of pulp (Lapierre et al. 1995; Körlü et al. 2008).

Table 3. Pseudo-first-order Rate Constant for the Decomposition of Hydrogen Peroxide with Iron and Lignin

Decomposition of Alkaline Hydrogen Peroxide with Iron,Manganese, and Lignin

The pseudo-first-order rate constants for the decomposition of hydrogen peroxide with mixed addition of iron, manganese, and lignin are shown in Table 4. A synergistic effect between manganese and iron combined with lignin on peroxide decomposition was demonstrated. The pseudo-first-order rate constant (kobs) in the absence of any stabilizers was 0.0053 min-1, which was less than the kobs value of 0.0063min-1 in the presence of lignin and manganese and the kobs value of 0.0068min-1 in the presence of lignin and iron. This might be attributed to the positive effect between manganese and iron on the adsorption of lignin, or the stronger ligands were formed, which were more stable for hydrogen peroxide. It could also be concluded that decomposition of alkaline hydrogen peroxide in the presence of mixed metals and lignin, including stabilizers, was different from that in the presence of single metal and lignin. The addition of Na2EDTA individually had the most positive effect on reducing peroxide decomposition in the presence of iron and manganese, having a kobs value of 0.0004 min-1.

Table 4. Pseudo-first-order Rate Constant for the Decomposition of Hydrogen Peroxide with Iron, Manganese, and Lignin

CONCLUSIONS

  1. The precipitated lignin was separated from the black liquor of eucalyptus pulping without further purification. The precipitated lignin still included transition metal elements such as Fe, Mn, and Cu according to the results of elemental analyses. The precipitates of fresh manganese ion were mixed crystal, containing Mn3O4, Mn(OH)2, and 7Mn(OH)2·2MnSO4·H2O, and consisted of two kinds of Mn-OH, as indicated by the results of XRD. The hydrolysis products of the fresh iron ion were only amorphous iron without any crystalline phases.
  2. The pseudo-first-order rate constant for the decomposition of hydrogen peroxide in the presence of manganese was 0.0053 min-1, which was the smallest rate constant compared to that in the presence of lignin-combined iron or lignin-combined manganese.
  3. The addition of Na2EDTA, MgSO4, and Na2SiO3, in combination or individually, had favorable effect on peroxide stability in the presence of transition metals and lignin under alkaline conditions. Mixed addition of MgSO4, Na2SiO3, and Na2EDTA had the most positive effect on reducing the decomposition of peroxide in the presence of single metal ion and lignin. The kobs was 0.0010 min-1 for manganese and 0.0006 min-1 for iron. The best effect on the reduction of peroxide decomposition in the presence of iron and manganese occurred when Na2EDTA was added individually, with a kobsvalue of 0.0004 min-1.

ACKNOWLEDGEMENTS

The authors would like to acknowledge the support from the Zhejiang Provincial Natural Science Foundation of China (Grant No. LQ13C160001), the Key Research & Development Project of Zhejiang Province (Grant No. 2017C03045) and the Zhejiang Provincial Key Laboratory of Chemical and Biological Processing Technology of Form Products (No. 2016KF0030).

REFERENCES CITED

Calull, M., Marcé, R. M., Piscina, P. R. D. L., Homs, N., Torres, J., and Borrull, F. (1988). “Kinetic-thermometric study of hydrogen peroxide decomposition in basic media catalyzed by Mn(II): Influence of several organic ligands,” Thermochimica Acta 125(88), 319-325. DOI: 10.1016/0040-6031(88)87231-9

Cardona-Barrau, D., Lachenal, D., and Chirat, C. (2001). “Affinity of metal ions for kraft pulps studied by ESR. Inhibition of their catalytic action in oxygen bleaching,” Journal of Wood Chemistry and Technology 21(3), 247-261. DOI: 10.1081/WCT-100105375

Deng, Y. (1997). “Formation of iron(III) hydroxides from homogeneous solutions,” Water Research 31(6), 1347-1354. DOI: 10.1016/S0043-1354(96)00388-0

Guo, X., Zhang, S., and Shan, X. (2008). “Adsorption of metal ions on lignin,” Journal of Hazardous Materials 151(1), 134-142. DOI: 10.1016/j.jhazmat.2007.05.065

Huang, G. L., Wang, D., Ma, S. L., Chen, J. L., Jiang, L., and Wang, P. Y. (2015). “A new, low-cost adsorbent: Preparation, characterization, and adsorption behavior of Pb(II) and Cu(II),” Journal of Colloid and Interface Science 445, 294-302. DOI: 10.1016/j.jcis.2014.12.099

Körlü,  A. E., and Bilgin, E. (2008). “Cotton fabric damage due to metal ion catalysis of hydrogen peroxide decomposition during bleaching,” Aatcc Review 8(4): 44-48

Lapierre, L., Bouchard, J., Berry, R. M., and Lierop, B. V. (1995). “Chelation prior to hydrogen peroxide bleaching of kraft pulps: An overview,” Journal of Pulp & Paper Science 21(8), 268-273.

Li, Z., Xiao, D., Ge, Y., and Koehler, S. (2015). “Surface-functionalized porous lignin for fast and efficient lead removal from aqueous solution,” ACS Applied Materials and Interfaces 7(27), 15000-15009. DOI: 10.1021/acsami.5b03994

Lin, Y.C., and Wang S.L. (2015). “Cr K-edge X-ray absorption and FTIR spectroscopic study on the reaction mechanisms of Cr(III) and Cr(VI) with lignin,” Desalination and Water Treatment 1317(1), 1-12. DOI: 10.1080/19443994.2015.1119754

Merdy, P., Guillon, E., and Aplincourt, M. (2002). “Iron and manganese surface complex formation with extracted lignin. Part 1: Adsorption isotherm experiments and EPR spectroscopy analysis,” New Journal of Chemistry 26(11), 1638-1645. DOI: 10.1039/B206352B.

Morgan, J. J. (2005). “Kinetics of reaction between O2 and Mn(II) species in aqueous solutions,” Geochimicaet Cosmochimica Acta69(1), 35-48. DOI:10.1016/j.gca.2004.06.013

Ni, Y., Ju, Y., and Ohi, H. (2000). “Further understanding of the manganese-induced decomposition of hydrogen peroxide,” Journal of Pulp and Paper Science 26(3), 90-94.

Norberg, C., Lidén, J., and Öhman, L. O. (2001). “Modelling the distribution of free, complexed and precipitated metal ions in a pulp suspension using Donnan equilibria,” Journal of Pulp and Paper Science 27(9), 296-301.

Popov, E., Välisaari, J., Vuorenpalo, V. M., Aksela, R., and Eloranta, J. (2007). “Stabilization of H2O2 in the presence of Fe (II) and Mn (II) impurities under alkaline conditions,” Holzforschung 61(5), 543-547. DOI: 10.1515/HF.2007.109

Ryabova, A. S., Bonnefont A., Zagrebin P., Poux T., Sena R. P., Hadermann J., Abakumov A. M., Kéranguéven, G., Istomin, S. Y., Antipov, E. V., Tsirlina, G. A., and Savinova, E. R. (2016). “Study of hydrogen peroxide reactions on manganese oxides as a tool to decode the oxygen reduction reaction mechanism,” ChemElectroChem 3, 1667-1677. DOI: 10.1002/celc.201600236

Saisaha, P., de Boer, J. W., and Browne, W. R. (2013). “Mechanisms in manganese catalysed oxidation of alkenes with H2O2,” Chemical Society Reviews 42(5), 2059-2074. DOI: 10.1039/C2CS35443H

Schneider, W. (1988). “Iron hydrolysis and the biochemistry of iron—the interplay of hydroxide and biogenic ligands,” Chimia 19(24), 9-20.

Sixta, H. (2006). Handbook of Pulp, Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim, Germany. DOI: 10.1002/9783527619887

Svärd, A., Sevastyanova, O., Dobele, G., Jurkjane, V., and Brännvall, E. (2016). “COST Action FP1105: Effect of raw materials and pulping conditions on the characteristics of dissolved kraft lignins,”Holzforschung 70(12), 1105-1114. DOI: 10.1515/hf-2016-0057

Wekesa, M., Habtewold, A., and Mirdaniali, J. (2011). “Stabilization of manganese (Mn)-induced peroxide decomposition,” African Journal of Pure and Applied Chemistry 5(7), 176-180.

Wekesa, M., and Ni, Y. (2003). “Further understanding of the chemistry of manganese-induced peroxide decomposition,” Canadian Journal of Chemical Engineering 81(5), 968-972. DOI: 10.1002/cjce.5450810507

Wekesa, M., and Ni, Y. (2011). “Decreasing the peroxide decomposition in the magnesia slurry,” Canadian Journal of Chemical Engineering 89(4), 864-868. DOI: 10.1002/cjce.20463

Zebardast, H. R., Rogak, S., Asselin, E. (2013). “Kinetics of decomposition of hydrogen peroxide on the surface of magnetite at high temperature,” Journal of Electroanalytical Chemistry 705, 30-36. DOI: 10.1016/j.jelechem.2013.06.019

Zhang, X., Li, Y., Lu, R., and Hou, Y. (2010). “Effect of free and adsorbed Fe (Ⅲ) on decomposition of hydrogen peroxide,” CIESC Journal 61(6), 1457-1462.

Zhang, X., Li, Y., Wang, L., Sha, L., and Hu, Z. (2015). “Investigation of manganese hydrolysis particles and decomposition of hydrogen peroxide in the pulp bleaching process,” Nordic Pulp and Paper Research Journal 30(4), 578-583. DOI: 10.3183/NPPRJ-2015-30-04-p578-583

Zhang, X., Wang, L., Li, Y., and Lei, L. (2016). “Decomposition of hydrogen peroxide by manganese in the presence of lignin,” Appita Journal 69(3), 241-246.

Article submitted: January 23, 2018; Peer review completed: March 6, 2018; Revised version received: April 5, 2018; Accepted: April 6, 2018; Published: April 17, 2018.

DOI: 10.15376/biores.13.2.3922-3931