Spent Lead-Acid Battery Recycling via Reductive Sulfur-Fixing Smelting and Its Reaction Mechanism in the PbSO4-Fe3O4-Na2CO3-C System

Powered by TCPDF (www.tcpdf.org) This material is protected by copyright and other intellectual property rights, and duplication or sale of all or part of any of the repository collections is not permitted, except that material may be duplicated by you for your research use or educational purposes in electronic or print form. You must obtain permission for any other use. Electronic or print copies may not be offered, whether for sale or otherwise to anyone who is not an authorised user. Li, Yun; Yang, Shenghai; Taskinen, Pekka; He, Jing; Chen, Yongming; Tang, Chaobo; Wang, Yuejun; Jokilaakso, Ari Spent Lead-Acid Battery Recycling via Reductive Sulfur-Fixing Smelting and Its Reaction Mechanism in the PbSO 4 -Fe 3 O 4 -Na 2 CO 3 -C System


INTRODUCTION
Spent lead-acid batteries (LABs) are widely scrapped from automobiles and electric bicycles in urban areas. The reported amounts of scrap LAB annually in China total more than 2.6 million metric tons. 1,2 LABs are a solid waste and classified as hazardous materials in many countries. Their disposal has become a significant environmental concern. 3 Recycling and reuse of LABs are attracting great attention from both the public and materials processing industry. At the same time, the depletion of high-quality lead ores resulting in rising extraction costs presents critical challenges for the lead extractive metallurgical industry. As a result, scrap LABs have become a significant secondary lead source worldwide. 1 Secondary lead produced by recycling is gradually dominating the world's lead market. 4 Typically, a spent LAB consists of four components: waste electrolyte (11-30%), polymeric materials (22-30%), lead alloy grids (24-30%), and lead paste (30-40%). Of these, lead paste is the most difficult part to deal with. 5 However, it is a high-quality secondary lead-bearing material. Around 80-85% of the total secondary lead is recycled from lead paste. 6 Currently, the worldwide LAB recycling technology can be divided into traditional routes such as pyrometallurgy and hydrometallurgy, and advanced approaches including electrowinning, 7 biological techniques, 8,9 and vacuum methods. 5 Pyrometallurgy is presently the predominant route worldwide for recycling LAB, 10 in which high-temperature treatment of spent LABs in a blast, electric, reverberatory, or rotary furnace without pre-desulfurization is employed. 11,12 In the hydrometallurgical process, 13,14 a pre-desulfurization step 15 is necessary. Na 2 CO 3 , NaOH, and K 2 CO 3 solutions or citric acid and citrate salts are usually adopted as desulfurization reagents. However, the JOM https://doi.org/10.1007/s11837-019-03529-1 Ó 2019 The Author(s) treatment of spent LABs involves a potential health and environmental risk. 16,17 At the same time, existing LAB pyrometallurgical processes operated at high temperatures are usually associated with high atmospheric emissions, since dioxins, chloride compounds, and mercury can be generated in the process. Meanwhile, hydrometallurgical processes are accompanied by laborious procedures, generation of large amounts of problematic waste water, and high electricity consumption. 18 As a result, the stringent environmental requirements are increasingly difficult to meet with current pyro-and hydrometallurgical recycling technologies. Therefore, the lead industry is keen to seek advanced technologies 19 which are more economical, minimize environmental pollution, 20 and reduce energy usage and production costs.
In this article, an innovative and environmentally friendly lead-acid battery paste recycling method is proposed. The reductive sulfur-fixing [21][22][23] technique was used to simultaneously extract lead and immobilize sulfur. This novel technique is distinguished from conventional pyrometallurgy techniques such as oxidizing matte smelting and reductive smelting by the use of a reducing atmosphere in the processing combined with sulfur transformation and fixation as a sulfide matte. Iron-containing wastes are also employed as sulfur-fixing agents to immobilize sulfur as FeS. The smelting products obtained contain three products, namely crude metal bullion, matte, and slag. The novelty of this process is the treatment of various iron/lead-bearing wastes, SO 2free sulfur fixation, a much shorter flowsheet, absence of harmful byproducts, and wide adaptability for different secondary materials. 12 This work investigated the detailed lead extraction and sulfurfixing mechanisms in the PbSO 4 -Fe 3 O 4 -Na 2 CO 3 -C system, thermodynamically and experimentally. The phase transformations and microstructural evolution processes were characterized, and the lead extraction and sulfur-fixing reaction mechanisms proposed. Furthermore, bench-scale experiments were carried out to confirm the feasibility and reliability of the new technique.

Materials
In the reaction mechanism investigation, PbSO 4 , Na 2 CO 3 , Fe 3 O 4 , and carbon powder with purity of ‡ 99% were employed to ensure high experimental accuracy. In the batch tests, lead paste separated from LAB scrap was used as raw material. Hematite and coke obtained from Jiuquan Iron & Steel Co., Ltd., Gansu, China were applied as sulfur-fixing agent and reductant, respectively. Their chemical compositions were analyzed by inductively coupled plasma-atomic emission spectrometry (ICP-AES, PerkinElmer, Optima 3000, Norwalk, USA) and are shown in Supplementary Table S-I (Online Supplementary Material). The phase compositions of the lead paste and hematite were characterized by x-ray diffraction (XRD) analysis (D/max 2550PC, Rigaku Co., Ltd., Japan). The results are presented in Supplementary Fig. S

Methods
PbSO 4 was selected as a model compound in the reaction mechanism investigation, since it is the major as well as the most difficult component to deal with in spent lead paste. At the same time, to reveal the reaction paths that may take place in each raw material component, the PbSO 4 -Fe 3 O 4 -Na 2 CO 3 -C system was divided into the PbSO 4 -Na 2 CO 3 , PbSO 4 -Na 2 CO 3 -C, PbSO 4 -Fe 3 O 4 , and PbSO 4 -Fe 3 O 4 -C subsystems. The specimens were mixed carefully and pressed uniaxially under 15 MPa into cylindrical samples of 10 mm diameter. Each specimen was placed in an alumina crucible and pushed slowly into the constant-temperature zone of a horizontal tube furnace (Supplementary Fig. S-2). The temperature was measured using a Pt-Rh thermocouple and controlled using a SHIMADEN SR25 intelligent temperature controller (accuracy ± 1°C). Nitrogen with purity of 99% was applied as protective gas in the reaction mechanism investigations. The N 2 gas flow during the reaction was fixed at 0.5 L/min. After the preset smelting time, the sample was removed rapidly from the furnace and quenched in liquid nitrogen.
In the bench-pilot confirmation experiments, 2000 g LAB paste was mixed thoroughly with a desired proportion of hematite, coke, Na 2 CO 3 , and other fluxes (CaO and SiO 2 ). The specimen was loaded into an alumina crucible and put into a chamber furnace. After the required smelting time, the sample was taken out and cooled down at room temperature. Next, the crucible was broken to carefully separate and weigh the end products obtained, i.e., crude lead, ferrous matte, and slag. Each product was prepared for ICP-AES analysis. The direct recovery rate of Pb (g) and the sulfurfixing rate (c) were calculated based on Eqs. 1 and 2, respectively: The phases and microstructure of the samples were characterized by XRD using Cu K a radiation and scanning electron microscope with energy-dispersive spectroscopy (SEM-EDS, Carl Zeiss LEO 1450, Germany; EDS, INCA Wave 8570, Oxford Instruments, UK). XRD data were collected in the 2h range from 10°to 80°in steps of 1°. The recorded patterns were evaluated using the PDF-2 powder XRD database. 24 Samples for SEM-EDS analysis were mounted in epoxy resin and polished using conventional metallographic grinding and polishing techniques. Figure 1 illustrates the equilibrium compositions of the PbSO 4 -Fe 3 O 4 -Na 2 CO 3 -C reaction system for different carbon additions as simulated using HSC Chemistry software, version 9.2.6, and its database; 25 the phase diagrams of the Al 2 O 3 -SiO 2 -CaO-10 wt.%Na 2 O and Fe-Fe 3 O 4 -FeS systems were calculated using MTDATA version 6.0 26 and MTOX database 8.2. 27 Figure 1a suggests that, without carbon addition, PbSO 4 prefers to react with Na 2 CO 3 to produce Na 2 SO 4 and PbO, even below 200°C. As the temperature is increased above 500°C, some PbO decomposes to metallic lead. In a weakly reductive atmosphere, as shown in Fig. 1b, PbSO 4 is reduced to PbS. At the same time, as the temperature increases, PbS prefers to react further with Fe 3 O 4 , instead of Na 2 CO 3 , generating metallic Pb and FeS. However, when the temperature reaches around 630°C, Na 2 CO 3 gradually reacts with FeS as well as PbS. Thus, the amounts of Pb, Na 2 S, and Fe 3 O 4 products increase, while those of PbS, Na 2 CO 3 , and FeS decrease. However, some PbS remains due to insufficient addition of carbon.  Figure 1c indicates that, at equilibrium conditions, all the lead can be extracted from PbSO 4 and PbS before 800°C when the carbon addition is sufficient. However, when the temperature is increased from 700°C to 800°C, the equilibrium amount of FeS remains steady while the amounts of metallic Pb and Na 2 S increase and, at the same time, those of Na 2 CO 3 as well as PbS decrease. This indicates that Na 2 CO 3 is partly involved in the lead extraction reactions from PbS. When the temperature exceeds 800°C, some FeS will also react with Na 2 CO 3 to generate Na 2 S and Fe 3 O 4 .

THERMODYNAMIC CALCULATIONS
The above thermodynamic equilibrium composition calculations reveal that, in the absence of a reducing agent and below 200°C, PbSO 4 prefers to react with Na 2 CO 3 rather than Fe 3 O 4 to generate PbO and Na 2 SO 4 . Once the temperature is increased and the atmosphere is sufficiently reducing, PbSO 4 will be reduced to PbS. At that point, PbS will prefer to react with Fe 3 O 4 rather than Na 2 CO 3 to produce FeS and PbO. When the temperature exceeds 800°C, the excess Na 2 CO 3 will continue to react with FeS. Thus, the sulfur transfers from the initial PbSO 4 to PbS and then FeS, and finally to Na 2 S. As a result, the presence of Na 2 CO 3 , and a reductant as well as sulfur-fixing agent Fe 3 O 4 , can ensure efficient sulfur fixation and lead extraction at both low and high temperature. No gaseous SO 2 or SO 3 is generated throughout the whole reaction process. All lead can thus be extracted from PbSO 4 and PbS.
The phase diagrams of the Al 2 O 3 -SiO 2 -CaO-10 wt.%Na 2 O system shown in Fig. 1d indicate that the first liquid slag appeared below around 975°C (1248 K), surrounded by liquid wollastonite [(Ca,Fe)SiO 3 ], tridymite (SiO 2 ), and feldspar [(AlCa,NaSi)AlO 8 ]. At that point, PbS, FeS, metallic Pb, Na 2 SO 4 , and Na 2 S were generated in the smelting system, as shown in Fig. 1a-c. They stayed in liquid form, together with the remaining Fe 3 O 4 and liquid Na 2 CO 3 . As the temperature was increased further, more liquid was formed from (Ca,Fe)SiO 3 and other solid smelting materials. When the temperature reached 1200°C (1473 K), more tridymite (SiO 2 ) and feldspar [(AlCa,Na-Si)AlO 8 ] also dissolved in the melt, and the liquid slag region expanded. Figure 1e further reveals that pyrrhotite FeS melts may come into contact with spinel Fe 3 O 4 , halite FeO, or/and FCC-A1 Fe before 1000°C (1273 K). A eutectic iron sulfide-oxide liquid appeared and gradually expanded along with the temperature. At 1200°C (1473 K), FeS was in liquid form. This promoted the generation of FeS and its settling from the smelting system as a separate sulfide melt layer.

Thermogravimetric Behavior of PbSO 4 -Fe 3 O 4 -Na 2 CO 3 -C Mixtures
The thermogravimetric behavior of the reactants and their mixtures was characterized using a thermogravimetric analyzer (TG-DTA, STA 494 F3; Netzsch, Germany) at heating rate of 10°C/min in N 2 flow of 100 mL/min, from 25 to 1000°C. The results are shown in Fig. 2.
It can be observed from Fig. 2a that the weight loss in the PbSO 4 -C, PbSO 4 -Na 2 CO 3 -C, and PbSO 4 -Fe 3 O 4 -C subsystems was greater than that in the PbSO 4 , PbSO 4 -Fe 3 O 4 , and PbSO 4 -Na 2 CO 3 subsystems. This implies that the presence of carbon promoted the conversion of PbSO 4 . Figure 2b further illustrates that T 1 (around 82°C) is associated with loss of crystallographic water from Na 2 CO 3 . T 2 (406°C) is ascribed to the transformation of Fe 3 O 4 into crystal form. T 3 (443°C) corresponds to preliminary decomposition of PbSO 4 . T 4 (563°C) and T 5 (717°C) are associated with the conversion reactions between PbSO 4 and Na 2 CO 3 . The pronounced endothermic peaks detected at T 6 (around 875°C) can be attributed to further decomposition of PbSO 4 . The last obvious endothermic peaks recorded at T 7 (around 980°C) are assumed to be linked with the generation of metallic lead.

Experimental Reaction Mechanisms in the PbSO 4 -Na 2 CO 3 -C Mixture
The experimental phase transformation paths in the different reaction systems and at different temperatures and reaction times were characterized Spent Lead-Acid Battery Recycling via Reductive Sulfur-Fixing Smelting and Its Reaction Mechanism in the PbSO 4 -Fe 3 O 4 -Na 2 CO 3 -C System by XRD and SEM-EDS analyses. The results for the PbSO 4 -Na 2 CO 3 -C system are shown in Fig. 3. It was observed that the reactions between PbSO 4 and Na 2 CO 3 took place below 650°C. PbO and Na 2 SO 4 were detected at 650°C within a 30-min duration. At the same time, when the temperature was increased, more intermediate products were detected, e.g., PbOAEPbSO 4 , 2PbOAEPbSO 4 , and 4PbOAEPbSO 4 . This indicates that the reactions between PbSO 4 and Na 2 CO 3 are a multistage process and follow the shrinking unreacted-core model. The unreacted PbSO 4 core is surrounded by liquid Na 2 CO 3 . The products xPbOAEPbSO 4 (x = 1, 2, or 4) form a boundary layer. When the temperature exceeded 1000°C, the reactions were completed and the final products were stable in PbO and Na 2 SO 4 . No metallic Pb was detected due to the absence of reductant. These results agree well with the thermodynamic calculations presented in Fig. 1. Figure 3b further reveals that the exchange reactions between PbSO 4 and Na 2 CO 3 favorably occur at 850°C quickly, within as little as 5 min. Thus, SO 3 in PbSO 4 was transformed and fixed to Na 2 SO 4 , instead of being emitted to the furnace atmosphere. The presence of Na 2 CO 3 inhibited self-decomposition of PbSO 4 .
Once a reductant was present, as shown in Fig. 3c and d, PbSO 4 was reduced to PbS when the temperature was higher than 750°C. Metallic Pb was also detected. This implies that PbO had been reduced by carbon. Furthermore, as the temperature was increased to 1000°C, the stable sodiumbearing product after 30 min reaction time was Na 2 S, rather than Na 2 SO 4 . This indicates that Na 2 SO 4 had been reduced to Na 2 S. The final products were PbS, Pb, and Na 2 S. The reaction paths in the PbSO 4 -Na 2 CO 3 -C system at 850°C after different reaction times, which are illustrated in Fig. 3d, further reveal that the PbSO 4 and PbO reduction reactions can occur rapidly. PbS and metallic Pb appeared within 5 min reaction time. The presence of carbon thus changes the reaction paths in the PbSO 4 -Na 2 CO 3 system. Only very weak diffraction peaks of PbO, Na 4 CO 3 SO 4 , and Na 2 SO 4 were detected in the reaction products. The reduction of PbSO 4 to PbS dominated the reaction path at 850°C. The sulfur in PbSO 4 would be converted mainly to PbS rather than Na 2 SO 4 . Figure 4 presents the phase evolutions in the PbSO 4 -Fe 3 O 4 -C system. It can be observed in Fig. 4a and b that no reactions took place between PbSO 4 and Fe 3 O 4 in the absence of reductant, as only a decomposition product, viz. PbOAEPbSO 4 from PbSO 4 , was detected. With the addition of a reductant, as illustrated in Fig. 4c, below 650°C, PbSO 4 was still not involved in any reaction with iron oxide during the first 30 min. However, at 750°C, PbS was detected, and PbSO 4 also converted to PbOAEPbSO 4 and further to 2PbOAEPbSO 4 , and metallic Pb emerged. This implies that, without Na 2 CO 3 , PbSO 4 self-decomposition intensified. As the temperature increased to 850°C, the product after 30 min reaction time consisted of PbS, Pb, and Fe 3 O 4 . Figure 4d further illustrates that the PbSO 4 reduction reactions to PbS could take place instantaneously. PbSO 4 disappeared before it was involved in any reaction with Fe 3 O 4 . FeS did not emerge until 1000°C after 30 min reaction time, and was

Microstructural Evolution Mechanisms
Selected samples, produced from simulated smelting systems at different temperatures and reaction times, were further characterized by SEM-EDS analysis. The results are presented in Fig. 5. Figure 5a shows the SEM-EDS results for the PbSO 4 -Na 2 CO 3 -C system at 750°C for 30 min reactions. It was observed that (PbO) x AEPbSO 4 (x = 1, 2, or 4) was close to Na 2 SO 4 particles and a part of PbSO 4 had reduced to PbS. Moreover, PbSO 4 and Na 2 SO 4 were surrounded by PbO and metallic Pb. This confirms that the reactions between PbSO 4 and Na 2 CO 3 follow the shrinking unreacted-core model. PbSO 4 first reacts with Na 2 CO 3 to generate Na 2 SO 4 and PbO. Na 2 CO 3 surrounds and gradually ''erodes'' the PbSO 4 unreacted core, then the PbSO 4 core is disintegrated by molten Na 2 SO 4 . At the same time, the reaction product PbO gradually diffuses out from the unreacted PbSO 4 core. Figure 5b illustrates the SEM-EDS results for the PbSO 4 -Fe 3 O 4 -C system at 850°C after 5 min reaction time. It reveals that PbS was surrounded by FeS. Metallic Pb was located in the center of the PbS particle. A PbFe x O y boundary layer was detected between the metallic Pb and PbS layers. This demonstrates that the reactions between PbS and Fe x O y also follow the shrinking unreacted-core model. A possible phase transformation and  microstructural evolution mechanism for the entire PbSO 4 -Na 2 CO 3 -Fe 3 O 4 -C reaction system is summarized and presented graphically in Fig. 6.

Confirmation Experiments and Characterization of Products
Two bench-scale pilot confirmation experiments with 1800 g lead paste were carried out to determine the reliability of this novel process under the following conditions: W lead paste : W hematite : W Na 2 CO 3 : W coke = 100 g:20 g:4 g:12 g. FeO/SiO 2 = 1.3, CaO/ SiO 2 = 0.4, smelting temperature of 1200°C, and smelting time of 1.5 h. A physical macrograph and corresponding XRD patterns of the smelting products are presented in Fig. 7a and b. It can be observed that three products were obtained, visibly separated as distinct layers by settling, i.e., slag, ferrous matte, and crude lead bullion. The chemical compositions of the different products obtained and the element distribution behavior is presented in Fig. 7c  The matte and slag that were obtained were further characterized by SEM-EDS analysis. The results are shown in Fig. 8. Figure 8a-  magnetite minerals. Metallic Pb was detected, embedded in the FeS and NaFeS 2 minerals. In the slag, as shown in Fig. 8e

CONCLUSION
Effective lead extraction from LAB paste by a reductive sulfur-fixing recycling technique was shown to be feasible, thermodynamically and experimentally. The reaction mechanism investigations revealed that the presence of Na 2 CO 3 helped to transform SO 3 from PbSO 4 to Na 2 SO 4 at low temperatures and in weakly reductive atmospheres. This ensures the conservation of sulfur in the smelting system without emitting gaseous SO 2 to the atmosphere. Once the atmosphere was sufficiently reductive, PbSO 4 was reduced to PbS. Thus, the sulfurfixing agent Fe 3 O 4 reacted with PbS to transfer sulfur to iron matte. Finally, metallic lead was extracted from PbO, and sulfur was fixed as FeS and NaFeS 2 . The lead extraction and sulfur-fixing reactions followed the shrinking unreacted-core model. Furthermore, bench-scale experiments using lead paste as raw material validated the fact that three recycling products were obtained: slag, matte, and crude lead bullion. More than 96.2% of the lead and 98.9% of the sulfur in the raw materials were extracted and fixed. The purity of the crude lead bullion was 98.6% Pb. The lead content in the matte and slag was decreased to 2.6% and 0.5% in the onestep treatment, respectively. This new process can be used for cotreating various iron-containing solid wastes and residues, and for comprehensive recycling of a variety of valuable metals compatible with iron matte and metallic lead.