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WO2025118033A1 - Procédé métallurgique extractif utilisant des eutectiques de sel fondu - Google Patents

Procédé métallurgique extractif utilisant des eutectiques de sel fondu Download PDF

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Publication number
WO2025118033A1
WO2025118033A1 PCT/AU2024/051320 AU2024051320W WO2025118033A1 WO 2025118033 A1 WO2025118033 A1 WO 2025118033A1 AU 2024051320 W AU2024051320 W AU 2024051320W WO 2025118033 A1 WO2025118033 A1 WO 2025118033A1
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Prior art keywords
metal
iron
eutectic system
ores
eutectic
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English (en)
Inventor
Bjorn Winther-Jensen
Bartlomiej KOLODZIEJCZYK
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Element Zero Pty Ltd
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Element Zero Pty Ltd
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Priority claimed from AU2023903979A external-priority patent/AU2023903979A0/en
Application filed by Element Zero Pty Ltd filed Critical Element Zero Pty Ltd
Publication of WO2025118033A1 publication Critical patent/WO2025118033A1/fr
Pending legal-status Critical Current
Anticipated expiration legal-status Critical

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    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B3/00—Extraction of metal compounds from ores or concentrates by wet processes
    • C22B3/04—Extraction of metal compounds from ores or concentrates by wet processes by leaching
    • C22B3/06—Extraction of metal compounds from ores or concentrates by wet processes by leaching in inorganic acid solutions, e.g. with acids generated in situ; in inorganic salt solutions other than ammonium salt solutions
    • C22B3/10—Hydrochloric acid, other halogenated acids or salts thereof
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
    • C25C3/34—Electrolytic production, recovery or refining of metals by electrolysis of melts of metals not provided for in groups C25C3/02 - C25C3/32
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C7/00—Constructional parts, or assemblies thereof, of cells; Servicing or operating of cells
    • C25C7/005—Constructional parts, or assemblies thereof, of cells; Servicing or operating of cells of cells for the electrolysis of melts
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C7/00—Constructional parts, or assemblies thereof, of cells; Servicing or operating of cells
    • C25C7/02—Electrodes; Connections thereof
    • C25C7/025—Electrodes; Connections thereof used in cells for the electrolysis of melts
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B15/00—Obtaining copper
    • C22B15/0063—Hydrometallurgy
    • C22B15/0065—Leaching or slurrying
    • C22B15/0067—Leaching or slurrying with acids or salts thereof
    • C22B15/0069—Leaching or slurrying with acids or salts thereof containing halogen
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
    • C25C3/06—Electrolytic production, recovery or refining of metals by electrolysis of melts of aluminium
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
    • C25C3/26—Electrolytic production, recovery or refining of metals by electrolysis of melts of titanium, zirconium, hafnium, tantalum or vanadium
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
    • C25C3/30—Electrolytic production, recovery or refining of metals by electrolysis of melts of manganese
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
    • C25C3/32—Electrolytic production, recovery or refining of metals by electrolysis of melts of chromium
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
    • Y02P10/00—Technologies related to metal processing
    • Y02P10/20—Recycling

Definitions

  • the present invention relates to the field of ore processing.
  • the invention relates to processing metal ores to isolate metal.
  • the present invention is suitable for isolation of iron from iron ore.
  • Iron ore is a metal ore that typically comprises iron oxides, the primary forms of which are magnetite (FesC ) and haematite (Fe2O3), goethite (FeO(OH)), limonite (FeO(OH)-/?H2O) or siderite (FeCOa). Almost all (98%) of iron ore is used in steelmaking.
  • Iron is typically recovered from iron ore using a pyrometallurgical process or extractive metallurgy. Extractive metallurgy techniques are commonly grouped into three categories: hydrometallurgy, pyrometallurgy and electrometallurgy including electrorefining and electrowinning. Many of these processes use high operating temperatures and have high inefficiencies.
  • leaching which originates from the Old English word leccan meaning ‘to water’, is a commonly used method in extractive metallurgy and comprises treating metal ore with water and reagents to convert the metal in the ore into soluble salts, while insoluble impurities remain in the ore. The soluble salts are then washed out and processed to provide the pure metal, the remainder being referred to as ‘tailings’.
  • iron oxides in general, have low solubility in water and good solubility in acid, with the acid leaching efficiency of common acids decreasing in the following order: hydrofluoric acid > hydrochloric acid > sulfuric acid > perchloric acid.
  • the main properties that influence iron dissolution for a given acid are temperature, pH, acid concentration, specific surface area, chemical composition, and crystalline habit.
  • the acid may be applied at high temperatures.
  • hydrochloric acid is typically applied to iron ore at temperatures greater than 750°C.
  • United States patent no. 2,723,912 to The United Steel Companies Limited describes one such process for leaching iron in the form of ferric chloride using hot hydrochloric acid gas.
  • the ferric chloride may subsequently be treated with a reductant such as hydrogen gas to produce metallic iron and fresh hydrochloric gas, which can be used to distil more ferric chloride from fresh ore according to the following equations:
  • An object of the present invention is to provide a more commercially convenient method for extracting metals from metal ores, particularly extracting iron from iron ore.
  • a further object of the present invention is to alleviate at least one disadvantage associated with the related art.
  • the method for the extraction of metal from metallic ores including the steps of;
  • ore for use in the present invention is chosen from the group comprising one or more of the following: iron ore including hematite, goethite, magnetite, titanomagnetite and pisolitic ironstone; aluminium containing ores including bauxite, cryolite and corundum; gold ores including gold-polysulfide, gold-quartz, gold-telluride, gold-tetradymite, gold-antimony, gold-bismuth-sulfosalt, gold-pyrrhotite, and gold-fahlore; manganese containing ores such as romanechite, manganite hausmannite and rhodochrosite; lead ores including galena, cerussite and anglesite; zinc ores including calamine and smithsonite; cobalt containing ores; uranium
  • the ore is iron ore, particularly in the form of magnetite (FesC ), hematite (Fe2O3), goethite (FeO(OH)), limonite (FeO(OH)-/?H2O) or siderite (FeCOa).
  • a single metal is extracted using the process of the present invention, however extraction of more than one metal at the same time is also contemplated as being within the scope of the present invention.
  • the metal is leached by a highly oxidative reagent such as an acid or halide gas.
  • the leaching agent may be chosen from HF, HCI, HBr, HI, F2. Br2 or CI2 in liquid or gaseous form.
  • a metal salt extracted by the leaching process is preferably a metal halide.
  • the metal is iron
  • the metal halide leached form the ore is an iron halide such as iron(lll) fluoride or iron(lll) chloride.
  • Iron(lll) fluoride is extremely stable and has a melting point of >1000°C, however iron(lll) chloride is more economically viable to synthesis and to use in downstream processing.
  • Iron(lll) chloride is also considerably more stable than the equivalent bromide salt, reflecting the greater oxidizing power of chlorine. Above 200°C, FeBra decomposes to ferrous bromide according to:
  • Iron(lll) bromide is more stable than iron(lll) iodide because iron(lll) tends to oxidize iodide ions.
  • a eutectic system is a homogeneous mixture that has a melting point lower than the melting points of the components.
  • the eutectic system of the present invention comprises salts, such as halide salts.
  • the eutectic system may include one or more salts chosen from NaCI, KCI, LiCI, CaCh, MgCh, MnCh or other alkali metal halides and alkaline earth metal halides.
  • the optimal composition of the eutectic system will depend on the composition at or near the eutectic system point and the person skilled in the art can identify a suitable eutectic system from the phase diagram for the eutectic system mixture.
  • Carrier salts that is salts that form eutectic systems with metal halide feedstock but are not meant to be reduced; must have higher reduction voltage compared to metal halide feedstock that act as a source for electrodeposited metal. Failure to comply with this requirement will lead to parasitic reactions, consumption of carrier salts, and product contamination.
  • the eutectic system comprises an iron halide, such as iron(lll) chloride, and an alkali metal chloride or alkaline earth metal chloride.
  • Eutectic systems comprising iron(lll) chloride and common alkali metal chlorides such as NaCI, KCI or LiCI are particularly preferred because they have a relatively low melting temperature, typically 150 to 200°C.
  • Eutectic systems formed from iron(lll) chloride with calcium(ll) chloride are particularly advantageous because they melt at ambient temperature and exhibit a low moisture uptake.
  • the eutectic system comprises 40% to 60% NaCI (molar), more preferably -50% NaCI based on the relevant phase diagram.
  • the eutectic system preferably comprises 30% to 60% CaCh (molar), more preferably -50% CaCh.
  • the eutectic system comprises an aluminium halide, such as aluminium(lll) chloride, and an alkali metal chloride or alkaline earth metal chloride.
  • embodiments of the present invention stem from the realization that the known process of dissolution/conversion of metal from metal ores can be greatly enhanced by combination with electrowinning from a molten salt eutectic system.
  • the process of dissolution/conversion of iron oxides by conversion to a salt such as FeCh can be greatly enhanced by combination with electrowinning from a molten chloride salt solution.
  • the prior art uses HCI for dissolving iron ore and hydrogen gas for the reduction of FeCh to Fe
  • the present invention uses electrochemical means.
  • the metal containing eutectic system has a high percentage of target metal ions species that can participate in the electrodeposition process. This is substantially different from aqueous systems (e.g., copper production) where the molarity of the electrowinning solution is often limited to the millimolar range due to risk of sedimentation. It is also different from most molten salt electrowinning processes where the target metal species are only added in small amount to (a eutectic system of) non-depositing salts (e.g., aluminium electrowinning). As such this removes diffusion limitations and provides the foundation for very high current densities;
  • aqueous systems e.g., copper production
  • non-depositing salts e.g., aluminium electrowinning
  • Fig. 1 is a diagram illustrating in general terms, the process of the present invention for the electrochemical production of iron
  • Fig. 2 illustrates, for reference, the phase diagrams for the eutectic systems of FeCh-NaC-Ch (Fig. 2A), FeCh-KCl-Ch (Fig. 2B) and FeCh-LiCI-Ch (Fig. 2C);
  • Fig. 3 illustrates, for reference, the phase diagrams for the eutectic systems of CaCl2-FeCI 3 -Cl2 (Fig. 3A), FeCh-MgCh-Ch (Fig. 3B) and FeCh-MnCh- Cl 2 (Fig. 3C);
  • Fig. 4 is a cyclic voltammogram performed in 1 :1 molar eutectic system of FeCh-NaCI at 250°C with steel cathode and graphite rod anode. Scan rate used in this measurement was 100 mV/s;
  • Fig. 5 is a cyclic voltammogram performed in 1 :1 :1 molar eutectic system of FeCh-NaCI-CaCh at 200°C with steel cathode and graphite rod anode. Scan rate used in this measurement was 100 mV/s.
  • Fig. 6 is a flow diagram depicting the extraction of two different metals from the same ore using chlorine gas leaching and electrowinning from two different molten salts;
  • Fig. 7 is a flow diagram depicting the production of iron from iron ore according to one embodiment of the present invention using molten NaFeCk as the electrolyte for the electrowinning;
  • Fig. 8 illustrates, for reference, the phase diagram for the eutectic system of CaCI 2 -NaCI
  • Fig. 9 depicts for reference, equilibrium phase diagrams between water and alkali metal chlorides or alkaline earth metal chlorides.
  • Fig. 9A is between water and NaCI;
  • Fig. 9B is between water and sylvite (KCI in natural mineral form);
  • Fig. 9C is between water and CaCh; and
  • Fig. 9D is between water and MgCh; and
  • Fig. 10 presents theoretical reduction voltages versus temperature for various alkali metal chlorides and alkaline earth metal chlorides as well as iron chloride, aluminium chloride, alumina, hematite, magnetite, water. [0041] Figs. 2, 3, and 8 are reproduced from FactSageTM thermochemical software and databases.
  • the present invention provides a method for the extraction of metal such as iron from metallic ores, the method including the steps of;
  • the reaction according to the present invention is depicted diagrammatically in Fig. 1 with reference to the extraction of iron from an ore comprising Fe20a.
  • chlorine gas at >400°C is applied to the ore, to extract the iron as iron(lll) chloride, which is combined with NaCI to form a eutectic system.
  • the eutectic system is subjected to electrowinning, such that Fe is deposited from the molten eutectic system on to a cathode.
  • Chlorine gas is formed at the anode and can be fed back into the extraction step.
  • iron ore is leached with HF, to form iron(lll) fluoride, or leached with HCI, or CI2 to iron(lll) chloride, both of which readily form eutectic systems with many alkali metal chlorides or alkaline earth metal chlorides.
  • Eutectic systems comprising iron(lll) chloride and common alkali metal halides, such as NaCI, KCI or LiCI, are particularly preferred because they have relatively low melting temperatures, typically 150 to 200°C.
  • Fig. 2 illustrates for reference, the phase diagrams for the eutectic systems of FeCh-NaCI-Ch (Fig. 2A) and for the eutectic systems of FeCh-KCl-Ch (Fig. 2B).
  • Eutectic systems formed from iron(lll) chloride with calcium(ll) chloride are particularly advantageous because they melt at ambient temperature.
  • FIG. 3 illustrates for reference, the phase diagrams for the eutectic systems of CaCh-FeCh- CI2 (Fig. 3A) and for the eutectic systems of FeCh-MgCh-Ch (Fig. 3B).
  • chlorine extraction from the other metal containing ores may differ from chlorine extraction from iron ores. There are a few practical issues and deviations which may be significant.
  • the difference in melting points of the various metal chlorides can be utilised to facilitate the separation of various metal chloride gases in a multi-step separator or by gradually increasing the temperature in a batch based chlorination leaching step to allow various metal-chlorides to evaporate one-by-one.
  • two or more different metal chlorides can be extracted and separately subjected to electrowinning to recover two different metals.
  • Fig. 6 is an illustration of one such example.
  • bauxite ore (comprising both iron and aluminium) is used as feed into a chlorinator and both iron and aluminium are produced by electrowinning from separate cells.
  • both electrowinning cells use sodium chloride to form eutectic systems and thereby limit the possible formation of gaseous metal chlorides.
  • electrodeposition of aluminium metal from neat molten AlCh is possible when a moderate pressure is applied to the system.
  • chlorine salts that may be formed during the extraction step, are not suitable as precursors for electrowinning from molten chlorides (e.g. NiCh and CuCh). However, they may be valuable as a commercial product in their own right or may be suitable metal salts for use in conventional aqueous electrowinning processes.
  • FeCh gaseous FeCh.
  • FeCh is known to readily sublime
  • the eutectic system is formed in the more FeCh salt rich part of the relevant phase diagram, where more precipitate will form.
  • a eutectic system of NaCI and FeCh will preferably comprise 40% to 60% NaCI (molar), and more preferably about 50% NaCI.
  • a eutectic system of CaCh and FeCh will preferably comprise 30% to 60% CaCh (molar), and more preferably -50% CaCh.
  • the temperature ranges are mainly limited at one end by the temperature at which the eutectic system solidifies, and at the other end by the temperature at which there is a significant chance of producing FeCh gas. It should also be noted that tertiary eutectic systems (e.g., NaCI, KCI, FeCh) may lower the melting temperatures further.
  • Aluminium(lll) chloride and NaCI form eutectic systems similar to those for iron chloride but with a melting temperature that is approximately 50°C lower.
  • EXAMPLE 1 A Electrowinninq from FeCh-NaCI containing eutectic systems
  • Anhydrous FeCh was mixed with pre-dried NaCI (120°C) in a 1 :1 molar ratio and immediately heated to 250°C in a Teflon beaker to form a liquid eutectic system.
  • the eutectic system was subjected to electrowinning at 250°C and 200°C using a mild steel cathode and a glassy carbon anode.
  • Chlorine gas was detected over the anode and the iron deposited was analysed to be of 94% purity.
  • EXAMPLE 1 B Electrowinninq from FeCh-NaCI containing eutectic systems
  • Anhydrous FeCh was mixed with pre-dried NaCI (200°C) in a 1 :1 molar ratio and immediately heated to 250°C in a glass beaker to form a molten eutectic system. Eutectic formation took about 40 minutes without stirring.
  • the eutectic system was subjected to electrowinning at 250°C using a mild steel cathode and a graphite rod anode.
  • Chlorine gas was detected over the anode and the iron deposited was analysed to be of 94% purity.
  • EXAMPLE 1 C Electrowinninq from FeCh-CaCh containing eutectic systems
  • anhydrous FeCh powder was mixed with anhydrous CaCh powder in a 2:1 molar ratio and immediately heated to 100°C in a closed Teflon container.
  • Electrodeposition was again performed at 200°C with similar outcome as for the 2:1 ratio however without any detectable evaporation of FeCh.
  • the deposited iron was washed trice in water at pH 12 to prevent corrosion of the deposited iron then dried at 120°C.
  • EXAMPLE 1 D Electrowinninq from FeCh-NaCI-CaCh tertiary eutectic system
  • Electrodeposition was performed at 200°C by applying constant cell voltage of 2.0 V. The corresponding current density was measured to be about 60 mA/cm 2 . Electrodeposition was performed in glass beaker using a mild steel cathode and a graphite rod anode. Cyclic voltammogram is presented in Fig. 5.
  • the present invention may be carried out in a “closed loop” set up as depicted diagrammatically in Fig. 7, wherein the chlorine/chloride is cycled between the chlorine leaching process and the electrowinning process.
  • Iron ore in the form of hematite was reacted in a chlorinator with chlorine gas at elevated temperature (>700°C) to produce gaseous iron(lll) chloride and oxygen according to the following equation:
  • a eutectic system was formed by adding molten NaFeCk (>160°C) to the FeCh.
  • the eutectic system was used as the electrolyte in the electrowinning cell.
  • chlorine gas was produced (according to the equation, 2CI- - CI2 + 2e _ ) and metallic iron was deposited on the cathode (according to the equation Fe 3+ + 3e _ - Fe°).
  • Figs. 9, 10, 11 and 12 depict an equilibrium phase diagram between water and alkali metal chlorides or alkaline earth metal chlorides. While these phase diagrams are limited to four instances, a clear trend emerges.
  • Alkali metal chlorides, in particular NaCI and KCI require lower temperatures to fully dry and remove any residual water, compared to alkaline earth metal chlorides.
  • alkaline earth metal chlorides particularly CaCh and MgCh
  • NaCI and KCI become anhydrous at temperatures of 108.7°C and 108.6°C, respectively.
  • alkali metal halides in particular NaCI and KCI, seem to be much better candidates for deep eutectic systems used for metal electrodeposition.
  • Carrier salts that is salts that form eutectic systems with metal halide feedstock, but are not meant to be reduced; must have higher reduction voltage compared to metal halide feedstock that act as a source for electrodeposited metal. Failure to comply with this requirement will lead to parasitic reactions, consumption of carrier salts, and product contamination.
  • Fig. 10 shows that reduction voltages for aluminium(lll) chloride and manganese(ll) chloride are not compatible due to similar reduction voltages, which could result in parasitic reaction of manganese reduction and contamination of aluminium product with manganese.
  • aluminium(lll) chloride and manganese(ll) chloride form eutectic systems with very narrow temperature window of liquid phase (this phase diagram is not included in this document). This raises a further question with respect to their compatibility for formation of suitable electroreduction environment.
  • metal halides have lower reduction voltage compared to their oxide counterparts. At least in the case of iron, iron(lll) chloride has reduced reduction voltage by about 0.2 V compared to hematite (Fe2Oa) and magnetite (FeaC ). When it comes to aluminium the benefit is even greater. Depending on temperature, the difference between reduction voltage of alumina and aluminium(lll) chloride can be greater than 0.6 V.
  • salts such as lithium chloride (LiCI), sodium chloride (NaCI), potassium chloride (KCI) and calcium chloride (CaCh) benefit from a very broad electrochemical window. This makes them suitable carrier salt candidates for eutectic systems for a large variety of metal halides.

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  • Life Sciences & Earth Sciences (AREA)
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  • Electrolytic Production Of Metals (AREA)

Abstract

L'invention concerne un procédé d'extraction de métal à partir de minerais métalliques, le procédé comprenant les étapes consistant à : (i) lixivier le minerai pour fournir un sel métallique, (ii) former un système eutectique comprenant le sel métallique et (iii) récupérer le métal à partir du système eutectique par extraction électrolytique, de préférence par dépôt électrochimique. Le procédé de la présente invention présente une application particulière pour le minerai de fer, en particulier l'isolement ou le fer à partir de minerai d'hématite, cependant l'invention peut s'appliquer à l'extraction d'une large gamme de métaux métalliques à partir d'une large gamme correspondante de minerais métalliques.
PCT/AU2024/051320 2023-12-08 2024-12-06 Procédé métallurgique extractif utilisant des eutectiques de sel fondu Pending WO2025118033A1 (fr)

Applications Claiming Priority (2)

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AU2023903979A AU2023903979A0 (en) 2023-12-08 Electrowinning from molten salt
AU2023903979 2023-12-08

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Citations (2)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20200399772A1 (en) * 2019-06-21 2020-12-24 Xerion Advanced Battery Corp. Methods for extracting lithium from spodumene
US20230279572A1 (en) * 2022-04-26 2023-09-07 Case Western Reserve University System and process for sustainable electrowinning of metal

Patent Citations (2)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20200399772A1 (en) * 2019-06-21 2020-12-24 Xerion Advanced Battery Corp. Methods for extracting lithium from spodumene
US20230279572A1 (en) * 2022-04-26 2023-09-07 Case Western Reserve University System and process for sustainable electrowinning of metal

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