EP4400616A2 - Procédé de recyclage à plusieurs étages - Google Patents

Procédé de recyclage à plusieurs étages Download PDF

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Publication number
EP4400616A2
EP4400616A2 EP23000178.6A EP23000178A EP4400616A2 EP 4400616 A2 EP4400616 A2 EP 4400616A2 EP 23000178 A EP23000178 A EP 23000178A EP 4400616 A2 EP4400616 A2 EP 4400616A2
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Prior art keywords
solution
components
nickel
ions
cobalt
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EP23000178.6A
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German (de)
English (en)
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EP4400616A3 (fr
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Tesfu Tadios
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    • 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
    • C22B7/00—Working up raw materials other than ores, e.g. scrap, to produce non-ferrous metals and compounds thereof; Methods of a general interest or applied to the winning of more than two metals
    • C22B7/005—Separation by a physical processing technique only, e.g. by mechanical breaking
    • 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
    • C22B23/00—Obtaining nickel or cobalt
    • C22B23/04—Obtaining nickel or cobalt by wet processes
    • C22B23/0407—Leaching processes
    • C22B23/0415—Leaching processes with acids or salt solutions except ammonium salts solutions
    • C22B23/043—Sulfurated acids or salts thereof
    • 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
    • C22B23/00—Obtaining nickel or cobalt
    • C22B23/04—Obtaining nickel or cobalt by wet processes
    • C22B23/0453—Treatment or purification of solutions, e.g. obtained by leaching
    • C22B23/0461—Treatment or purification of solutions, e.g. obtained by leaching by chemical methods
    • 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
    • C22B26/00—Obtaining alkali, alkaline earth metals or magnesium
    • C22B26/10—Obtaining alkali metals
    • C22B26/12—Obtaining lithium
    • 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
    • C22B3/08—Sulfuric acid, other sulfurated acids or salts thereof
    • 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
    • C22B3/20—Treatment or purification of solutions, e.g. obtained by leaching
    • C22B3/44—Treatment or purification of solutions, e.g. obtained by leaching by chemical processes
    • 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
    • C22B47/00—Obtaining manganese
    • 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
    • C22B59/00—Obtaining rare earth metals
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/01—Products
    • C25B1/02—Hydrogen or oxygen
    • C25B1/04—Hydrogen or oxygen by electrolysis of water
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/01—Products
    • C25B1/21—Manganese oxides
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B9/00—Cells or assemblies of cells; Constructional parts of cells; Assemblies of constructional parts, e.g. electrode-diaphragm assemblies; Process-related cell features
    • C25B9/17—Cells comprising dimensionally-stable non-movable electrodes; Assemblies of constructional parts thereof
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C1/00—Electrolytic production, recovery or refining of metals by electrolysis of solutions
    • C25C1/02—Electrolytic production, recovery or refining of metals by electrolysis of solutions of light metals
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C1/00—Electrolytic production, recovery or refining of metals by electrolysis of solutions
    • C25C1/06—Electrolytic production, recovery or refining of metals by electrolysis of solutions or iron group metals, refractory metals or manganese
    • C25C1/08—Electrolytic production, recovery or refining of metals by electrolysis of solutions or iron group metals, refractory metals or manganese of nickel or cobalt

Definitions

  • the present invention relates to a method for treating components. More specifically, it is a recycling process that is particularly suitable for recovering raw materials from batteries and accumulators, but also from strong magnets and fuel cells.
  • the US Patent Application 2013/0206607 A1 discloses a process for recovering lithium from lithium-ion batteries.
  • the battery material is placed in an acid bath at 50 °C.
  • the European Patent 3 279 343 B1 discloses a method for recovering copper from lithium-ion batteries. The process involves recovering copper by leaching with an acidic solution and then separating it from the solution.
  • the recycling process according to the invention aims to achieve complete recycling, both in terms of the number of recovered raw materials and in terms of their quality.
  • the process should be suitable for batteries but also for other components which contain significant amounts of rare earths in particular.
  • the recycling process according to the invention comprises a large number of individual process steps.
  • the process stands out from other processes in that a particularly high raw material recovery rate can be achieved. For example, a rate of more than 97% (wt. %) of the material supplied can be recovered as raw material that can be further processed.
  • a very high degree of purity can be achieved, in individual cases also a degree of purity of more than 97%, more than 98%, more than 99%, more than 99.5%, more than 99.7 or even more than 99.9 or 99.95% or 99.98 or 99.99%.
  • the first steps of the process can be summarized as physical process steps. These physical process steps include in particular the physical raw material preparation, the discharge of charged cells and physical separation processes, in particular the comminution of the raw materials.
  • the present process is particularly suitable for components that contain metal salts from which metals can be recovered in the course of this process.
  • metal salts from which metals can be recovered in the course of this process.
  • lithium (Li), cobalt (Co), nickel (Ni) and manganese can be recovered from the corresponding metal salts. (Mn).
  • the components can have various compounds with the mentioned and other metals or metal salts, whereby the term metal compound herein also includes the metal itself.
  • the materials to be recycled can be, for example, components from fuel cells or rechargeable batteries or magnets.
  • the recycling of magnets is particularly interesting with regard to their use in electric car engines or wind turbine generators. Strong magnets - and in particular strong magnets that contain rare earths - are a focus here.
  • Rechargeable batteries are often referred to as accumulators, but the word battery and accumulator are used interchangeably here.
  • Larger batteries such as automotive batteries, comprise a large number (more than 100 or typically more than 1,000) of individual battery cells, for example in the form of lithium-ion cells.
  • the individual cells typically have a voltage of 1-5 V and are combined into modules, which in turn have a voltage of 5 V-80 V.
  • These modules in turn form systems, which can have a voltage of 80 V-800 V.
  • Such a system can represent the essential element of an automotive battery.
  • batteries are recycled in this process, it can be assumed that they have a residual charge.
  • the batteries In preparation for the next steps in the process, the batteries must be discharged as completely as possible. Devices with an AC/DC inverter are usually used for this purpose. Discharge protocols are usually also created during the discharge. It is useful if the residual energy that was stored in the batteries is recovered and fed back into the grid.
  • a saline solution discharge can also be used.
  • the saline solution creates a short circuit between the battery poles. This can involve using saline solutions that have such low conductivity that a sudden short-circuit discharge is impossible.
  • a solution, preferably a 6% by weight solution, of NaHCOs and Na 2 CO 3 is used.
  • an early step is disassembly (usually the first step after discharge).
  • This disassembly can be done manually and destructively, for example with angle grinders or chisels. This also separates easily distinguishable components, such as lithium-ion cells and housings and wiring elements or electronic components.
  • the mechanical treatment may also include dismantling the components with a water jet.
  • the physical separation process includes a crushing step as an essential step.
  • the components which are usually pre-crushed manually, are further crushed under high mechanical pressure.
  • shear and tear forces can also act, for example if a working surface (e.g. a roller surface) is provided with corresponding structures (e.g. with teeth).
  • the mechanical separation process is also called shredding.
  • shredding devices can be used.
  • a four-shaft shredding machine is useful. Screening devices can be arranged under this machine. This means that the components are not only shredded into particle sizes of less than 10 mm, but different particle sizes can also be sorted. For example, sorting can be carried out for particle sizes from 5 mm to 0.5 mm.
  • the mechanical separation process should in any case be suitable for producing particles with diameters of less than 10 mm, but also individual particles with diameters of less than 1 mm.
  • Mechanical shredding should generally be carried out under protective gas, such as nitrogen or argon.
  • protective gas such as nitrogen or argon.
  • the residual energy possibly contained in batteries can pose a fire or explosion hazard.
  • electrolyte is usually released from the batteries.
  • anhydrous aprotic solvents are used in lithium-ion batteries. These solvents are purified by distillation.
  • a magnetic separation into ferrous and non-ferrous metals is carried out.
  • a magnetic separator is used for this.
  • the separator works with gravity. Powdery material can fall downwards due to gravity, for example through a grid. In the falling particle stream, however, iron particles are deflected and separated by a strong magnetic field. Such a strong magnetic field can be effectively generated with neodymium magnets. The magnets can also be used to collect the ferrous metals.
  • air flow separation can be used. Gravity also acts in this separation process. Against the direction of gravity - i.e. from below -air is blown in. Heavy parts fall downwards against the air flow, light parts are carried upwards by the air flow. This makes it possible to separate the particles into a light and a heavy fraction.
  • the separation depends on the particle size and the material density. For example, copper and aluminum are easy to separate because of their very different material densities (copper 8.96 g/cm 3 , whereas aluminum 2.7 g/cm 3 ). Metals with similar material densities can often be separated easily because they are in different forms, for example copper is typically present as a metal foil and cobalt is present as a cobalt oxide salt.
  • the particles are then converted into (sulfuric acid) solution.
  • This solution including the particles, is subsequently referred to as the solution.
  • the particles are often referred to as "black mass" when they essentially comprise the cathode material of lithium-ion batteries.
  • the chemical treatment is preferably carried out in a temperature range of 60 to 80°C, particularly conveniently at around 70°C.
  • This decomposition process can be controlled by adding potassium permanganate.
  • Potassium permanganate is used as an oxidizing agent to decompose the metal ions and transfers them into solution. There, further chemical and electrochemical treatment is easily possible.
  • metal sulfates are formed from salts, especially Li, Ni, Mn and Co.
  • Different metal sulfates can be separated from the solution in specific reactions, usually this is done by precipitation.
  • the individual reactions can run in parallel or one after the other.
  • other reactions can be used depending on the raw material used.
  • Precipitation of nickel The precipitation of nickel from the sulfate solution can conveniently be carried out with multidentate ligands, for example with diacetyldioxime or with butanedione dioxime.
  • Separation of cobalt from nickel-containing sulfate solution Separation of cobalt with Cyanex 272 (trihexyltetradecylphosphonium bis(2,4,4-trimethylpentyl)phosphinate) is particularly useful when a nickel-containing sulfate solution is present. Simultaneous electrolysis of cobalt and nickel is practically impossible, since their standard potentials hardly differ (-0.226 volts for nickel and -0.280 volts for cobalt).
  • Ni-Co and Mn ions it is also possible to electrochemically deposit several metal ions, in particular Ni-Co and Mn ions, simultaneously.
  • the raw materials are typically in the form of a metal salt containing the metal to be deposited. As described, this is particularly true for Co, Ni and Mn.
  • the metal can be extracted from the corresponding metal salts by electrolysis, usually by reducing the metal cation to the elemental metal at the cathode.
  • the standard potential for each reaction is also given.
  • the standard potential for nickel and cobalt is very similar. It is therefore not possible to separate nickel and cobalt from a mixed sulfate solution at the same time. With such a mixed sulfate solution, it is advisable to carry out electrolysis only after chemical pretreatment. This pretreatment can be carried out using Cyanex 272. After this pretreatment, cobalt can be extracted from the sulfate solution. Nickel can then be extracted electrochemically in a further separate step.
  • nickel is deposited reductively on the cathode (as described above).
  • manganese dioxide can be deposited simultaneously by oxidation on the anode. This happens when divalent manganese ions are oxidized to trivalent manganese ions. These in turn decompose into divalent and tetravalent manganese ions. From these, manganese dioxide is formed, which is then deposited on the anode.
  • both the anode reaction and the cathode reaction can proceed optimally: 3 volts voltage, 250 amperes/m 2 current density. Temperature of approximately 50°C.
  • Ni, Co and Mn ions it is also possible to electrochemically deposit Ni, Co and Mn ions simultaneously. A chemical post-treatment is then required to separate the metals.
  • the cobalt and nickel deposited on the cathode are dissolved in hydrochloric acid.
  • the divalent ions can be chemically deposited from this hydrochloric acid solution by complex formation with Cyanex 272 for cobalt and diacetyldioxime for nickel.
  • the lithium carbonate can then be purified by recrystallization. Lithium carbonate can then be dissolved in an aprotic solvent (an ionic liquid) and electrochemically deposited as lithium metal.
  • an aprotic solvent an ionic liquid
  • rare earth metals can be separated. This is particularly relevant for the recycling of neodymium, for example from neodymium magnets (such magnets are also often used in wind turbines).
  • the solution usually contains rare earth elements, and neodymium is used in particular in components to be recycled. For example, the recycling of neodymium-iron-boron magnets is considered.
  • a first step two components are added to the sulfate solution with a mixture of metal, semi-metal and rare earth ions: sulfuric acid and sodium hydroxide. It is advisable to use 200 ml of sulfuric acid (concentration 150 g/l) and 665 ml of sodium hydroxide solution (concentration 200 g/l) for 1,000 ml of original solution (sulfate solution). The chemical precipitation takes place thus in a ratio of 2:1:1 milliliter of original solution to milliliter of sulfuric acid to milliliter of NaOH.
  • the pH value In order to achieve precipitation of the rare earths, the pH value must be increased to 2.
  • the addition of sodium sulfate before increasing the pH value is necessary in order to be able to precipitate the rare earths as double sulfate despite leaching with sodium hydroxide solution.
  • organic phase is added to this aqueous solution for extraction; this organic phase consists of a solvent and an organic complexing agent.
  • Kerosene is a suitable solvent.
  • Tri-n-butyl phosphate (TBA) can be used as a complexing agent, particularly for the separation of light rare earth metals, and various ethylhexyl phosphoric acid esters (HDEHP, EHEHPA) can be used for heavier rare earths.
  • the solution obtained in this way is mixed in a mixing system (shaken funnel) by vigorous stirring.
  • the subsequent demixing of the aqueous and organic phases allows these phases to be separated.
  • the organic phase is washed out with an aqueous solution. In this way, an aqueous solution with a single rare earth element, e.g. neodymium, is obtained.
  • This solution with a rare earth element can be subjected to a precipitation reaction, for example by adding oxalic acid. This produces a rare earth oxalate.
  • the rare earth oxalate can in turn easily be converted into a rare earth oxide.
  • Rare earth oxides are common commercial products. The conversion takes place by calcination at approx. 800°C in air with the release of CO 2 .
  • Ionic liquids allow the application of separation processes for a range of valuable substances that are typically dissolved in the (sulfate) solution. For example, it is also possible to obtain neodymium through an electrochemical separation process instead of through precipitation reactions.
  • An ionic liquid is understood here to be an ionically structured aprotic compound with a melting point of less than 100°C. Preferably, the melting point is even below 25°C, so that the ionic liquid is generally in liquid form at room temperature.
  • ionic liquids are also referred to as RTIL (or Room Temperature Ionic Liquids ).
  • RTIL Room Temperature Ionic Liquids
  • a different ionic liquid is appropriate.
  • the metal deposition is generally carried out on an aluminum/titanium cathode and a platinum anode.
  • Neodymium deposition is conveniently carried out in a phosphonium-based ionic liquid at a potential of Nd 3+ / ND of -2.431 volts vs. platinum.
  • a suitable ionic liquid is trihexyltetradecylphosphonium chloride.
  • Electrochemical lithium deposition This is carried out with a piperidinium-based ionic liquid at a potential of -2.3 volts relative to the platinum anode.
  • Electrochemical dysprosium deposition This deposition is conveniently carried out using a guanidinium-based ionic liquid on an aluminum sheet. A potential of -0.7 volts (or less than -0.8 volts...) is applied to the platinum anode. Reduction of Dy(III) to Dy(0) occurs here via a single reaction step.
  • Electrochemical deposition of gold, platinum and ruthenium The metals are dissolved in an ionic liquid, with iron sulfate and/or zinc sulfate added as a reducing agent. This is best done at a temperature of 70°C.
  • the preferred procedure is as follows: platinum, gold and/or ruthenium are dissolved in an ionic liquid (preferably: 1-butyl-1-methylpyrrolidinium bis(trifluoromethanesulfonyl)imide) in the presence of FeSO 4 or ZnSO 4 solution as a reducing agent at a temperature of 70°C.
  • the dissolved divalent noble metal ions are electrochemically reduced to the elemental metal at reduction potentials of platinum, gold and ruthenium at 1.20 V, 1.40 V or 0.45 V on a carrier electrode (aluminum/titanium sheet).
  • the solution can also contain graphite.
  • the process according to the invention can also comprise the chemical and/or electrochemical cleaning of graphite. In particular, aluminum and copper contamination can be removed.
  • the chemical reactions (precipitations) and electrochemical reactions described leave small amounts of metal ions (Li, Co, Mn, Ni, Al) in the solution. These can be electrochemically dialyzed in a neutralization system with a heavy metal separator.
  • FIG.1 A diagram shows an example of a process for extracting raw materials.
  • the process begins with a few, essentially physical steps for raw material preparation, shown in field 10.
  • a first step 12 the raw materials are shredded.
  • a shredder is mainly used. This delivers a raw material powder, which is collected in a container 14. Before shredding, the charged components are usually unloaded.
  • the electrolyte fluid of lithium-ion batteries typically consists of anhydrous, aprotic solvents and a conductive salt, usually lithium hexafluorophosphate.
  • the conductive salt adheres to the raw material powder, so that the addition of an organic solvent (e.g. acetonitrile) can be provided to wash out the conductive salt.
  • an organic solvent e.g. acetonitrile
  • a mixing container for powder and solvent 16 is provided. It is supplemented by a solvent storage container 16A. Extracted electrolyte can be collected in a container 18.
  • the powdered raw materials prepared in this way are physically separated in further process steps. This takes place in the process units in frame 20.
  • a magnetic separation 22 takes place first, in which iron powder is separated from the powder and collected in the container 24.
  • the material is then subjected to an air flow separation 26.
  • aluminum and copper components are separated. These can then be collected in suitable containers, such as a Container 28A for aluminum powder and a container 28B for copper powder.
  • the black mass 30 is obtained from the starting material for the further process steps.
  • This black mass 30 is mixed with other substances in the mixing system 42, especially with sulphuric acid.
  • oxidizing agents can also be added, such as hydrogen peroxide and potassium permanganate.
  • suitable containers for example container 42.
  • the black powder After the black powder has been prepared in the mixing plant, it is transferred to an electrolysis unit 50. Nickel and manganese dioxide electrolysis in particular can take place here.
  • Hydrogen is usually produced during this electrolysis. This hydrogen can be discharged via a pipe and reused in a suitable manner. A cost-effective reuse can take place in a combined heat and power plant 52. In this way, the plant can be operated completely or at least partially in an energy-self-sufficient manner.
  • a substance can be added to the remaining mass from the storage container 62, which allows the recovery of cobalt (II) hydroxide in the container 64.
  • a suitable substance is sodium hydroxide.
  • a substance can be added to the remaining mass from the storage container 66, which allows the extraction of manganese dioxide in the container 68.
  • a suitable substance is potassium permanganate.
  • a substance can be added to the remaining mass from the storage container 70, which allows the extraction of lithium carbonate in the container 72.
  • a suitable substance is sodium carbonate.
  • the added raw materials are almost completely recovered.
  • the residual material is transferred to a neutralization system 80 in which acids and alkalis are neutralized.
  • a neutralization system 80 in which acids and alkalis are neutralized.
  • this also rejects a heavy metal separator.
  • Pure process water can be obtained from the neutralization system 80 and collected in the container 82.
  • the collected process water can also be used in the process itself. For this purpose, it is advantageously led to the mixing system 40, where it can be used to prepare the black mass 30.

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  • Chemical & Material Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Materials Engineering (AREA)
  • Metallurgy (AREA)
  • Organic Chemistry (AREA)
  • Manufacturing & Machinery (AREA)
  • Mechanical Engineering (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Environmental & Geological Engineering (AREA)
  • General Life Sciences & Earth Sciences (AREA)
  • Geology (AREA)
  • Inorganic Chemistry (AREA)
  • General Chemical & Material Sciences (AREA)
  • Geochemistry & Mineralogy (AREA)
  • Manufacture And Refinement Of Metals (AREA)
  • Processing Of Solid Wastes (AREA)
EP23000178.6A 2022-12-15 2023-12-14 Procédé de recyclage à plusieurs étages Pending EP4400616A3 (fr)

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Application Number Priority Date Filing Date Title
DE102022004722.5A DE102022004722A1 (de) 2022-12-15 2022-12-15 Mehrstufiges Recyclingverfahren

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Citations (2)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20130206607A1 (en) 2010-09-29 2013-08-15 Hitachi, Ltd. Lithium Extraction Method, and Metal Recovery Method
EP3279343B1 (fr) 2015-03-31 2021-01-27 JX Nippon Mining & Metals Corporation Procédé d'extraction du cuivre à partir de déchets d'élément de batterie au lithium-ion, et procédé de récupération de métal

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GB1290513A (fr) * 1968-10-23 1972-09-27
CH671780A5 (fr) * 1987-09-28 1989-09-29 Recytec S A C O Orfigest S A
DE102011110083B4 (de) * 2011-08-12 2016-09-01 Technische Universität Braunschweig Carolo-Wilhelmina Verfahren zum Wiedergewinnen von Aktivmaterial aus einer galvanischen Zelle und Aktivmaterial-Separationsanlage, insbesondere Aktivmetall-Separationsanlage
DE102013202976A1 (de) * 2013-02-22 2014-08-28 Siemens Aktiengesellschaft Niedertemperaturverfahren zur Herstellung von Lithium aus schwerlöslichen Lithiumsalzen
DE102015206153A1 (de) * 2015-04-07 2016-10-13 Robert Bosch Gmbh Verwertung von Lithium-Batterien
DE102017216564A1 (de) * 2017-09-19 2019-03-21 Siemens Aktiengesellschaft CO2-freie elektrochemische Herstellung von Metallen und Legierungen davon
US12467152B2 (en) * 2020-03-06 2025-11-11 The Board Of Regents Of The Nevada System Of Higher Education On Behalf Of The University Of Nevada, Las Vegas Lithium recovery from lithium salts dissolved in ionic liquids

Patent Citations (2)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20130206607A1 (en) 2010-09-29 2013-08-15 Hitachi, Ltd. Lithium Extraction Method, and Metal Recovery Method
EP3279343B1 (fr) 2015-03-31 2021-01-27 JX Nippon Mining & Metals Corporation Procédé d'extraction du cuivre à partir de déchets d'élément de batterie au lithium-ion, et procédé de récupération de métal

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