Xiang
Xue
a,
Liwen
Zhang
a,
Qi
Fang
c,
Chunjia
Liu
c,
Shuijie
Su
c,
Xiaoli
Xi
*ab and
Zuoren
Nie
ab
aState Key Laboratory of Materials Low-Carbon Recycling, Beijing University of Technology, Beijing 100124, China. E-mail: xixiaoli@bjut.edu.cn
bCollaborative Innovation Center of Capital Resource-Recycling Material Technology, College of Materials Science and Engineering, Beijing University of Technology, Beijing 100124, China
cChina National R&D Center for Tungsten Technology, Xiamen Tungsten Co., Ltd, Xiamen 361005, China
First published on 7th March 2025
As a rare-earth reinforced tungsten alloy, photovoltaic tungsten-based busbars have been extensively employed in silicon production in recent years. The urgent issue at hand is the need to achieve the co-recovery of tungsten and lanthanum from photovoltaic tungsten wire scrap. In this study, the complete recycling of photovoltaic tungsten scrap is achieved for the first time through a brief molten salt electrolysis process, utilizing Na2WO4 as the electrolyte and tungsten wire scrap as the anode. The process involves a graphite crucible as the cathode, ensuring continuous contact with the product to prevent the oxidation of tungsten powder (W) to sodium tungsten bronze (NaxWO3) by Na2WO4 electrolyte. The corundum anode basket promotes the dissolution of La2O3 in the electrolyte to form La2(WO4)3. This compound actively participates in electrochemical reactions to facilitate the simultaneous production of W and La2O3. The regenerated tungsten powder possesses a uniform distribution of La2O3, making it a suitable raw material for the manufacture of photovoltaic tungsten-based busbars. Overall, this approach establishes a sustainable and environmentally friendly tungsten resource recycling ecosystem.
Green foundation1. Photovoltaic tungsten filaments are typically processed through chemical recycling methods, which result in significant contaminant generation. These methods overlook the recovery of rare earth elements and necessitate the reintroduction of La precursors for the production of photovoltaic tungsten wires. In this study, a one-step molten salt electrolysis approach is employed to achieve the co-recovery of tungsten and La2O3 from photovoltaic tungsten wires, with no contaminant formation during the process.2. One-step regeneration of photovoltaic tungsten wires by molten salt electrolysis is realized, and the prepared rare earth tungsten powder can be directly used as a raw material to produce photovoltaic tungsten wires, which shortens the recycling process and eliminates the pollution. 3. Future research should focus on optimizing current efficiency and advancing the development of continuous molten salt electrolysis equipment. |
Photovoltaic tungsten wires are used as cutting tools and are scrapped upon breakage. To enhance their performance, tungsten is typically strengthened with rare-earth oxides.5–7 Therefore, photovoltaic tungsten wire is actually a rare-earth-reinforced tungsten alloy. Rare-earth oxides are uniformly distributed in tungsten powder through physical or chemical methods, followed by sintering and thermal processing to form rare-earth tungsten alloys. The distribution of rare-earth oxide nanoparticles in the grains performs the role of pinning down and accumulating dislocations, enhancing the mechanical properties by the Orowan and pinning mechanisms (oxide dispersion strengthened).8,9 Currently, the yield rate of PV tungsten wires is below 50%, meaning that every 3 tons of tungsten powder yields only 100 million meters of tungsten wire. Consequently, tungsten busbar scrap originates from two sources, production-end scrap and use-end scrap. The accumulation of waste photovoltaic tungsten wires is not only a waste of resources but also a potential risk of environmental pollution when improperly handled. The tungsten content of tungsten busbar is more than 99%, which is much higher than that of the original ore, and the recycling of photovoltaic tungsten busbar scrap can reduce the pollution caused by the original ore mining and smelting, reduce production costs, and promote the sustainable development of the photovoltaic industry. The challenge in reclaiming photovoltaic tungsten wires stems from the co-recovery of tungsten and rare earth oxides and it is difficult to directly convert PV tungsten busbar scrap into tungsten powder with uniformly dispersed rare-earth oxides. Moreover, the exceptional mechanical properties of tungsten wires hinder their regeneration through physical methods. The chemical recycling route stands out as the prevailing technology for recovering tungsten.10 Although the quality of the product prepared by this method is closest to that of the original ore, the process is cumbersome and does not comply with sustainable development. Furthermore, this recovery approach neglects rare-earth oxides, and incorporating the recovery of rare-earth elements would prolong the process and production cycle, leading to heightened environmental and economic burdens. Molten salt electrolysis, a sustainable and efficient tungsten recovery technique, has undergone extensive research and demonstrated success in recovering various tungsten products, such as tungsten (W), tungsten carbide (WC), and cemented carbide (WC-Co).11–13 For example, Xiao et al. recovered cemented carbide scrap by double-cathode and two-stage electrolysis in NaCl–KCl molten salt and obtained cobalt and tungsten carbide, respectively.14 Xi et al. recovered WC-10Co in NaF–KF molten salt and utilized the potential difference to achieve tungsten and cobalt separation, obtaining particles less than 1 μm under 88 mA.15 Realization of the recovery of rare earth oxides in tungsten wires is another research priority. Depending on the existing tungsten wire scrap, the recyclable is La2O3. Conventional molten salt electrolytes use chloride or fluoride salts, and literature has been investigated on species and solubility of La2O3 in these electrolytes. La exists in molten FLiNaK as LaOF and La2O3 with a solubility of 6.81 × 10−4 wt% at 700 °C.16 The solubility of La2O3 could reach 8.71 wt% in molten salts of 50 wt% NaF-50 wt% (44 wt%NaCl + 56 wt%KCl).17 La indeed has solubility in the molten chlorine and fluorine, but achieving uniform distribution of La2O3 in tungsten powder during tungsten wire recovery is challenging. This unique distribution is expected when La3+ participates in electrochemical reactions and produces La2O3. Obviously, it is impossible in chlorine and fluorine salts, where La2O3 dissolves as LaOF, and the excess over the solubility becomes an anodic sludge. Hence, the primary focus of the research is to identify a suitable electrolyte and facilitate the recovery of tungsten and rare-earth oxides (La2O3) efficiently through streamlined processes.
In this study, we develop a recovery pathway for tungsten wires by employing Na2WO4 as electrolyte based on theoretical principles and experimental validation. This approach allows for the simultaneous recovery of tungsten and lanthanum from tungsten wire scrap. A cathodic protection strategy is used to avoid oxidation of tungsten powder by Na2WO4. The utilization of anode basket facilitates the dissolution of La2O3 to generate La2(WO4)3. This compound can engage in the electrochemical reaction, enabling the concurrent production of tungsten powder and La2O3. The regenerated tungsten powder exhibits a homogeneous distribution of La2O3, making it suitable for direct use as a raw material in the manufacturing of photovoltaic tungsten wires. Ultimately, a sustainable ecological framework is established for the recovery of photovoltaic tungsten wires through molten salt electrolysis.
The electrolysis unit consists of photovoltaic tungsten wire anode, graphite crucible cathode and sodium tungstate electrolyte. Pre-treatment of photovoltaic tungsten wire scrap is necessary before it can be used as anode. The tungsten wire is first cleaned with pure water, after drying completely, weighed 20 g and then forged into a rectangular shape (65 × 10 × 6 mm) in a hydraulic press. The anode basket is the crucial point to achieving tungsten-lanthanum co-recovery. The corundum anode basket has a circular opening (∅ 6 mm) at 35 mm from the bottom to ensure ion transport and the photovoltaic tungsten wire scrap is placed in the basket. The graphite crucible serves as both cathode and electrolyte container, and the conductivity of the graphite crucible is achieved by a stainless-steel collector. Before configuring the electrolyte, sodium tungsten needs to be held in a vacuum oven at 200 °C for 48 h to remove water. After the electrolysis unit is assembled, it is placed in furnace (Thermcraft, Winstom-Salem, N.C. U.S.A), and the device needs to be evacuated to a vacuum before the temperature is raised. The electrolysis unit needs to be held at 573 K for 1 h to completely eliminate water interference, and then heated to 1073 K under a dry argon atmosphere. The current density used for the experiment is 15.76 mA cm−2. Electrolysis duration is 3 h, unless otherwise specified. The product is rinsed with deionized water to remove electrolytes, then filtered through a 0.1 μm nylon microporous membrane and washed with ultrapure water until the electrolytes are completely removed. Finally, the product is completely dried in an oven at 100 °C.
E = −ΔG/nF | (1) |
The electrochemical window of the molten salt and the dissolution potential of tungsten are characterized by cyclic voltammetry (CV) and linear sweep voltammetry (LSV) on VersaSTAT 4 electrochemical workstation (Princeton Applied Research, Advanced Measurement Technology Inc., USA). Open circuit chronopotentiometry (OCP) and square wave voltammetry (SWV) are applied to characterize electrochemical reactions. The morphology of products is characterized by scanning electron microscopy (SEM, Sigma 300, Carl Zeiss Microscopy GmbH). The composition of products is characterized by Energy Dispersive Spectroscope (EDS), X-ray photoelectron spectroscopy (XPS, PHI5000 VersaProbe lll), X-ray diffraction (XRD, X'Pert PRO, Malvern Panalytical) and Glow Discharge Mass Spectrometry (GDMS, Element GD Plus GD-MS, Thermo Fisher Scientific Inc.). The XRD uses Co Kα radiation. Each sample is scanned from 10° to 110° and the data is compared with PDF data of MDI Jade 6.0 to determine the crystal shape. The XPS uses Al Kα radiation as the excitation source. The XPS data are processed on Avantage software and the C 1 s peak (284.8 eV) is used as a reference for the calibration of binding energies. The binding energy of elemental is based on the NIST XPS database and literature.7,8,19,20
La2(WO4)3 → 3W + La2O3 + 4.5O2 | (2) |
La2(WO4)3 is not observed when using chloride/fluoride as an electrolyte. Therefore, only oxygenates such as carbonate, tungstate, sulfate, etc., can fulfill the requirements. Based on the principle of excluding impurity ions, the selection of electrolytes is constrained to tungsten oxygenates. Nonetheless, the defect of utilizing tungsten oxygenates electrolyte is that tungsten is easily oxidized to sodium tungsten bronze (NaxWO3) by the tungsten oxygenates, as in reactions (3) and (4).21
(2 − x)W + xNa2WO4 + (3 − 2x)O2 → 2NaxWO3 | (3) |
xW + 3xNa2WO4 + (6 − 4x)WO3 → 6NaxWO3 | (4) |
These reactions promote the anodic electrochemical dissolution of tungsten, but are detrimental to the cathodic preparation of tungsten powders. Due to the specific physicochemical traits of tungsten, the tungsten reduced cathodically tends to detach easily. Once detached, it undergoes oxidation to form NaxWO3 due to interaction with the electrolyte, resulting in compromised product purity and diminished current efficiency. Preventing the oxidation of the product is a critical issue that needs to be resolved when employing tungsten oxygenates as electrolytes. The reaction possibilities of La2O3 and tungsten oxygenates have been calculated, as shown in Fig. 1a. La2O3 is unable to react spontaneously with Na2WO4, which could lead to low solubility in Na2WO4. From the effect of concentration on the actual reduction potential, it can be seen that extremely low solubility prevents La2(WO4)3 from participating in electrochemical processes. But La2O3 can react spontaneously with WO3 or Na2W2O7 to form La2(WO4)3. This does not mean that Na2W2O7 (Na2WO4–WO3) is the ideal choice of electrolyte. The Na2WO4–WO3 molten salt contains a high concentration of WO3, which undoubtedly enhances the reaction (4), resulting in the final product that is not regenerated tungsten powder. Consequently, Na2W2O7 proves unsuitable as an electrolyte.
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Fig. 1 (a) Possible reactions of La2O3 in tungsten oxygenates, (b) the calculation of thermal stability of molten salts, (c) the theoretical potential for possible electrochemical reactions in molten salts, (d) the theoretical electrochemical reduction order at 800 °C, (e) comparison of chemical recycle route10 and molten salt electrolysis route. |
Based on the above analysis, the only alternative electrolyte is Na2WO4. Enhancing the concentration of La2(WO4)3 in the Na2WO4 electrolyte is pivotal for achieving co-recovery of W and La. Meanwhile, the dissolution of La2O3 is critically dependent on the Na2W2O7 content in the electrolyte. Consequently, optimizing the concentration of Na2W2O7 in the electrolyte while ensuring that the product is tungsten powder is the focus of this work. The thermal stability of the molten salt is further calculated as shown in Fig. 1b. La2(WO4)3 and Na2WO4 have excellent thermal stability and do not decompose spontaneously. Na2W2O7 spontaneously decomposes to form Na2WO4 and WO3 at temperatures exceeding 800 °C. The ionic W2O72− reacts more readily with La2O3 than WO3, thus the working temperature should be lower than the decomposition temperature of Na2W2O7. The theoretical potential for possible electrochemical reactions in the electrolyte is further calculated, as in Fig. 1c. The theoretical potentials of reactions decrease with increasing temperature, which means that high temperatures are more favourable for electrochemical processes. The working temperature is chosen to be 800 °C in conjunction with calculations of the thermal decomposition of the molten salt. Fig. 1d shows the prioritization of reactions at operating temperature. At 800 °C, Na2W2O7 exhibits the lowest reduction potential (−0.986 V), but Na2W2O7 spontaneously binds La2O3 to form La2(WO4)3. As a result, its impact on the anticipated sequence of electrochemical reactions is minimal. During the reduction process, La2(WO4)3 preferentially produces W and La2O3 (−1.103 V) rather than W and La (−1.471 V). The theoretical reduction potential of Na2WO4 to W is −1.512 V, ensuring that electrolyte decomposition can be avoided prior to the formation of W and La2O3. Last but not least, the electrochemical window of Na2WO4 is tested using a tungsten rod as the counter electrode and a Pt wire as the reference and working electrode, and the cyclic voltammetry curve and linear voltametric curve is shown in Fig. 2a and b. Notably, sodium tungstate has an electrochemical window of −0.84 V to 1.38 V. A linear voltametric curve, as shown in Fig. 2c, signifies the dissolution potential of tungsten at −0.291 V, confirming the recovery feasibility within sodium tungstate. The aforementioned analysis provides a theoretical foundation for the recovery of photovoltaic tungsten-based busbars scraps through molten salt electrolysis. If proven feasible, this method has the potential to significantly streamline the existing chemical recycling route (Fig. 1e) and pave the way for the development of a rapid and environmentally friendly PV tungsten wire regeneration technology.
In a preliminary investigation of the validity of CPS, the experiment is conducted using photovoltaic tungsten wire scrap as anode, and a comparison is made between graphite crucibles cathode and tungsten rods cathode. Photos of the molten salt and products obtained after the experiment are visualized in Fig. S1.† The XRD patterns of the product are display in Fig. 3. The product when using a tungsten rod cathode is a mixture of tungsten powder and sodium tungsten bronze (Fig. 3a), which suggests that oxidation occurs when the tungsten powder is detached from the cathode. The SEM image of the product is shown in the Fig. 3b, and its morphology is a fragment-type structure of varying sizes. The elements Na, W, and O can be clearly observed on the EDS spectra, further proving that the product is a mixture of sodium tungsten bronze and tungsten powder. To further understand the oxidation process of tungsten, the open circuit chronopotentiometry of tungsten is tested, such as Fig. 2d. Platform A is the reduction potential during electrolysis and corresponds to the WO42− deposition process. At the end of electrolysis, the voltage is polarized from platform A to platform B and stabilized for about 20 s, which corresponds to the oxidation of tungsten to sodium tungsten bronze. La2O3 in the tungsten wires is not detected in the SEM image of the product, and combined with the GDMS results (Table S1†) of the product, suggests that the product does not contain lanthanum. The La2O3 remains dissolved in the electrolyte in the form of La2(WO4)3, as a large amount of sodium tungsten bronze is present in the electrolyte. In contrast, the product is pure tungsten powder when using a graphite crucible cathode (Fig. 3c). The morphology of tungsten powder is shown in Fig. 3d, which exits in stick and sphere shape. The morphology of tungsten obtained from molten salt electrolysis is usually sphere-shaped,22,23 whereas the stick-shaped tungsten obtained in this experiment may be caused by electrochemical dissolution of the tungsten wire during the electrolysis process. The comparative experiment is carried out using tungsten rod and wires as anode, and the products obtained were all tungsten spheres, as shown in Fig. S2a and S2b,† which proves that stick-tungsten comes from the electrochemical dissolution process of tungsten wires. Unfortunately, this tungsten of stick morphology can have a negative effect on the performance of recycled tungsten powder, as it has a relatively large size. Therefore, it is necessary to find a solution to remove this stick-shaped tungsten in subsequent experiments. The GDMS result of tungsten powder is given in Table S1,† which contains about 0.29 wt% La. The La2O3 observed in Fig. 3d is present as particles in the tungsten powder and does not develop a uniform distribution. Combined with theoretical analyses, it can be seen that La2O3 can form La2(WO4)3 only if the molten salt contains WO3 or Na2W2O7. This part of the La2O3 is not produced by electrochemical reduction, but is formed by agglomeration of La2O3 during dissolution of the anode. The desired product should be a uniform distribution of La2O3 in the tungsten powder, thus the strategy in the theoretical analysis needs further verification. The above results show that the oxidation of tungsten powder can be inhibited by avoiding it detaching from the cathode, which is a preliminary proof of the validity of CPS. However, the graphite crucible will provide a portion of the carbon, so that the possibility of a carbothermal reduction reaction between carbon and sodium tungsten bronze cannot be excluded, and the possibility of obtaining pure tungsten powder from such a reaction also exists.24
Therefore, the experiment is carried out using a nickel metal crucible as the cathode, as shown in Fig. S3,† which product remains pure tungsten powder. Repeated experiments are continued for 1.5, 3, 6, and 8 h. The XRD patterns of the products are all pure tungsten powder, as shown in Fig. S4,† which further excludes the effect of carbothermal reaction and proves the effectiveness of the CPS. After confirming the effectiveness of the CPS, electrochemical characterization is necessary to gain a deeper understanding of the reaction process, such as Fig. 2e and f. The number of electrons transferred is obtained by fitting the SWV and calculating viaeqn (5).25
W1/2 = 3.52RT/nF | (5) |
It is clear from the CV that the reduction of WO42− occurs in two steps, while the SWV fitting suggests that WO42− is a six-electron process with a two-step reduction, with two electrons in the first step and four electrons in the second step (W6+ → W4+ → W), which is consistent with literature reports and in line with the theoretical analysis (Fig. 1d).26 Finally, the current efficiency when using graphite crucible cathode is calculated as 90.02% based on the amount of product.
In the subsequent experiments, the structure of the electrolysis unit is modified, as illustrated in Fig. 4a. In this configuration, the photovoltaic tungsten wire is positioned within the anode basket, a design that facilitates the collection of sodium tungsten bronze generated through thermochemical reactions at the anode (reactions (3) and (4)), thereby promoting the dissolution of La2O3. After changing the structure of the electrolysis unit, the XRD spectra of the product are shown in Fig. 4b. The XRD plot reveals that the utilization of the anode basket does not alter the phase of the sample, with the resulting product still being tungsten powder. The regenerated tungsten powder morphology and elemental distribution are further characterized, as shown in Fig. 4f and Fig. S2c.† The SEM demonstrates the absence of stick-shaped tungsten in the samples, with all tungsten shapes appearing spherical, indicating the effective removal of larger grain sizes by the anode basket. This further illustrates that the stick-shaped tungsten originates from the electrochemical dissolution process of the photovoltaic tungsten wires. After employing anode basket, the stick-shaped tungsten was collected and digested in further thermochemical reaction (reaction (3)). The EDS mapping (Fig. 4f) reveals that the regenerated tungsten powder is composed of W, La, and O elements. Notably, La is uniformly distributed in the W, in alignment with previous studies on the synthesis of rare-earth tungsten alloys.7,8,20Fig. 4c, d, and e shows XPS spectra of W 4f, La 3d, and O 1s. Each W, La, and O peaks can be clearly observed, and binding energy is corrected in 284.8 eV. Metallic W (W0) is depicted at 33.44 eV and 31.25 eV in Fig. 4c, and the peaks at 38.01 eV and 35.86 eV are corresponding to W6+, indicating the oxidation of a proportion of the tungsten.27 This oxidation is not reflected in XRD, but areas of oxidized tungsten are clearly observed on EDS mapping (Fig. 4f). The peaks at 835.42 eV and 851.98 eV in Fig. 4d are attributed to La 3d5/2 and La 3d3/2, displaying the typical characteristics of La3+ (La2O3) with an interval ΔE of 16.56 eV.8 Additionally, the peaks at 839.22 eV and 855.76 eV are attributed to La multiplet-split peaks.19,28 Combined with the O 1s peaks in Fig. 4e, it can be concluded that La exists as La2O3 in tungsten powder. The above characterization results indicate that La2O3 is uniformly distributed in the regenerated tungsten powder. This desirable product has been proven to be a suitable raw material for manufacturing photovoltaic tungsten wires and proves the success of the molten salt electrolysis method.
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Fig. 4 (a) Schematic description of the electrolysis unit, (b) XRD pattern of product, XPS spectra at (c) W 4f, (d) La 3d, (e) O 1s, (f) SEM and EDS mapping of product. |
In order to further validate the molten salt electrolysis method for the overall recovery of photovoltaic tungsten wires, the products at different electrolysis durations are studied (Fig. S5†). There is no La distribution in the tungsten at 1 h and 2 h (Fig. S5a and S5b†). This absence can be attributed to the concentration of La2(WO4)3. According to the Nernst equation and Raoult's law (reactions (6) and (7)), concentration influences the actual reduction potential. Lower concentration will make the actual reduction potential rise, resulting in reduction reaction that is less competitive.
EAc = E° + (RT/nF)ln![]() | (6) |
αA = γAxA | (7) |
Notably, the electrolyte can be recycled during industrial applications, thus portion of the lanthanum loss can be ignored. The continuous accumulation of La2O3 during electrolysis may result in a failure to achieve uniform distribution. The electrolysis duration is further extended from 3 h to 8 h and the products are characterized as in Fig. S5c.† La2O3 remains uniformly distributed in the tungsten powders. This is mainly due to the differences between La2O3 generation and the conventional electrochemical reduction process. The electrochemical reduction process involves the transfer of electrons, but there is no transfer of electrons in the production of La2O3. The reduction potential for La2O3 to La is −2.573 V, La2(WO4)3 to La2O3 is −1.103 V, and La2(WO4)3 to La is −1.471 V. These values indicate that the process of generating La monomers is not thermodynamically favorable or competitive. The reduction of WO42− to W produces a large amount of O2−. At this point, La3+ combines with O2− to produce La2O3. The ultimate manifestation is the co-deposition of tungsten and La2O3. The presence of tungsten powder will limit the La2O3 growth. Furthermore, the key to the dissolution of La2O3 is the presence of Na2W2O7. Na2W2O7 exhibits the lowest reduction potential (−0.986 V), which precludes its presence in the cathode. Therefore, the produced La2O3 will not revert to its ionic state. In addition, La is derived exclusively from tungsten wires, and the anodic dissolution, mass transfer, and electrochemical deposition are simultaneous, thus La2O3 can be consistently produced in the tungsten powder.
Ultimately, the current efficiency, estimated by the quantity of products, stands at 46.42%, demonstrating a notable decrease compared to not using anode baskets. This decline primarily arises from mass transfer constraints by anode basket.
In the absence of an anode basket, La2O3 detaches as anode sludge during electrolysis and eventually mixes with regenerated tungsten powder. However, when an anode basket is employed, La2O3 participates in the electrochemical process and is uniformly distributed in the regenerated tungsten powder. The structure of the electrolysis unit significantly influences the migration behavior of La. Specifically, the anodic dissolution of tungsten wires involves two primary mechanisms. The first is electrochemical dissolution, producing WO42−(W + 4O2− → 6e− + WO42−). Concurrently, O2 is generated at the anode (O2− → O2 + 2e−). The second mechanism is thermochemical dissolution, where tungsten wire reacts with oxygen and sodium tungstate (W + O2 + Na2WO4 → NaxWO3), forming NaxWO3. Upon modification of the electrolysis unit structure, the NaxWO3 is confined in the anode basket. At the end of electrolysis, the presence of NaxWO3 can be detected in the anode basket (Fig. 5b and Fig. S6†). NaxWO3, as an intermediate state oxide, can undergo further oxidized by the O2 to form Na2WO4 and WO3.24 These compounds, Na2WO4 and WO3, will spontaneously combine to yield Na2W2O7. Analysis of the molten salt composition in the anode basket reveals a distinct characteristic peak corresponding to Na2W2O7 (Fig. 5b), thereby confirming its presence. Under these conditions, La2O3 and Na2W2O7 will spontaneously react to form La2(WO4)3, which then migrate to the cathode and participates in the electrochemical reaction. This process enables the co-recovery of tungsten (W) and La2O3. A clear graphical representation of the La migration pathway is provided in Fig. 5a.
The conventional chemical recycling route depicted in Fig. 1e involves numerous steps such as oxidation, digestion, calcination, and reduction to yield recycled tungsten powder, along with the emission and disposal of pollutants.10 In sharp contrast, the inputs to the molten salt electrolysis route are tungsten wire scrap, electricity, and heat, the molten salt electrolyte can be recycled, and the output is only the product, thus no pollutants will be generated by the process. In terms of the development and utilization of solar energy, the molten salt electrolysis route can be a perfect match with solar-thermal and solar-electricity, which can build a green and pollution-free tungsten resource recycling ecology, as shown in the Fig. 5c. Energy is a primary factor constraining the practical application of molten salt electrolysis, according to the trend of China's electric power structure, the proportion of green electricity is increasing.29 As a result, the potential for industrial implementation of the molten salt electrolysis route is steadily expanding.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: https://doi.org/10.1039/d5gc00126a |
This journal is © The Royal Society of Chemistry 2025 |