WO2016174394A1 - Pile au lithium-soufre - Google Patents

Pile au lithium-soufre Download PDF

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Publication number
WO2016174394A1
WO2016174394A1 PCT/GB2016/051075 GB2016051075W WO2016174394A1 WO 2016174394 A1 WO2016174394 A1 WO 2016174394A1 GB 2016051075 W GB2016051075 W GB 2016051075W WO 2016174394 A1 WO2016174394 A1 WO 2016174394A1
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WIPO (PCT)
Prior art keywords
lithium
sulfone
cell
anode
electrolyte
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PCT/GB2016/051075
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English (en)
Inventor
Sebastien DESILANI
David Ainsworth
Original Assignee
Oxis Energy Limited
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by Oxis Energy Limited filed Critical Oxis Energy Limited
Priority to GB1719154.5A priority Critical patent/GB2555033B/en
Priority to TW105112830A priority patent/TW201703317A/zh
Publication of WO2016174394A1 publication Critical patent/WO2016174394A1/fr

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    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/62—Selection of inactive substances as ingredients for active masses, e.g. binders, fillers
    • H01M4/624—Electric conductive fillers
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M10/00—Secondary cells; Manufacture thereof
    • H01M10/05—Accumulators with non-aqueous electrolyte
    • H01M10/052—Li-accumulators
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M10/00—Secondary cells; Manufacture thereof
    • H01M10/05—Accumulators with non-aqueous electrolyte
    • H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
    • H01M10/0564—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of organic materials only
    • H01M10/0566—Liquid materials
    • H01M10/0567—Liquid materials characterised by the additives
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M10/00—Secondary cells; Manufacture thereof
    • H01M10/05—Accumulators with non-aqueous electrolyte
    • H01M10/058—Construction or manufacture
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
    • H01M4/134—Electrodes based on metals, Si or alloys
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/36—Selection of substances as active materials, active masses, active liquids
    • H01M4/362—Composites
    • H01M4/366—Composites as layered products
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M10/00—Secondary cells; Manufacture thereof
    • H01M10/05—Accumulators with non-aqueous electrolyte
    • H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
    • H01M10/0564—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of organic materials only
    • H01M10/0566—Liquid materials
    • H01M10/0568—Liquid materials characterised by the solutes
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M10/00—Secondary cells; Manufacture thereof
    • H01M10/05—Accumulators with non-aqueous electrolyte
    • H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
    • H01M10/0564—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of organic materials only
    • H01M10/0566—Liquid materials
    • H01M10/0569—Liquid materials characterised by the solvents
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/36—Selection of substances as active materials, active masses, active liquids
    • H01M4/38—Selection of substances as active materials, active masses, active liquids of elements or alloys
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/36—Selection of substances as active materials, active masses, active liquids
    • H01M4/38—Selection of substances as active materials, active masses, active liquids of elements or alloys
    • H01M4/381—Alkaline or alkaline earth metals elements
    • H01M4/382—Lithium
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/36—Selection of substances as active materials, active masses, active liquids
    • H01M4/38—Selection of substances as active materials, active masses, active liquids of elements or alloys
    • H01M4/40—Alloys based on alkali metals
    • H01M4/405—Alloys based on lithium
    • 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
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/10—Energy storage using batteries
    • 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
    • Y02P70/00—Climate change mitigation technologies in the production process for final industrial or consumer products
    • Y02P70/50—Manufacturing or production processes characterised by the final manufactured product

Definitions

  • the present invention relates to a lithium-sulphur cell.
  • the present invention also relates to a method of assembling a lithium-sulphur cell.
  • a typical lithium-sulphur cell comprises an anode (negative electrode) formed from lithium metal or a lithium metal alloy, and a cathode (positive electrode) formed from elemental sulphur or other electroactive sulphur material.
  • the sulphur or other electroactive sulphur-containing material may be mixed with an electrically conductive material, such as carbon, to improve its electrical conductivity.
  • the carbon and sulphur are ground and then mixed with a solvent and binder to form a slurry.
  • the slurry is applied to a current collector and then dried to remove the solvent.
  • the resulting structure is calendared to form a composite structure, which is cut into the desired shape to form a cathode.
  • a separator is placed on the cathode and a lithium anode placed on the separator. Electrolyte is introduced into the cell to wet the cathode and separator.
  • Lithium-sulphur cells are secondary cells. When a lithium-sulphur cell is
  • the sulphur in the cathode is reduced in two-stages.
  • the sulphur e.g. elemental sulphur
  • polysulphide species S n 2" (n ⁇ 2). These species are generally soluble in the electrolyte.
  • the polysulphide species are reduced to lithium sulphide, L12S, which, may deposit on the surface of the anode.
  • lithium-sulphur secondary cells One consideration when developing lithium-sulphur secondary cells is maximising the useful cycle life of the cell. Other considerations include specific energy.
  • Many lithium sulphur cells employ sulfolane as an organic solvent in the electrolyte. Sulfolane is a good solvent for the polysulphide species that are produced during discharge. However, it is viscous and has a relatively high density.
  • a lithium-sulphur cell comprising
  • an anode comprising lithium metal or lithium metal alloy
  • a cathode comprising a mixture of electroactive sulphur material and solid electroconductive material
  • an electrolyte comprising a lithium salt and an organic solvent comprising 0 to less than 20 weight % of a sulfone
  • the anode comprises a sulfone coating, said coated portion being in contact with the electrolyte.
  • a method of assembling a lithium sulphur cell comprising:
  • the cycle life of a lithium sulphur cell may be improved by pre-treating at least a portion of the anode with a sulfone, such that a sulfone coating is formed on the treated portion of the anode.
  • a solid electrolyte interphase or SEI can be more readily formed on the anode's surface. Without wishing to be bound by any theory, this coating improves the cycle life of the cell.
  • pre-treating the anode in this way cells can be assembled using a wide range of organic solvents, including organic solvents other than sulfones.
  • the anode comprises a lithium metal or lithium metal alloy.
  • the anode comprises a foil formed of lithium metal or lithium metal alloy.
  • lithium alloy include lithium aluminium alloy, lithium magnesium alloy and lithium boron alloy.
  • a lithium metal foil is used.
  • At least a portion of the anode may be pre-treated by contacting the anode with a sulfone, for example, sulfolane.
  • the anode may be pre-treated on one or both sides.
  • the anode e.g. foil
  • the anode may be soaked or dipped in the sulfone.
  • the anode is pre-treated by contacting the anode with a solution of a lithium salt in a sulfone.
  • a coating e.g. an SEI
  • sulfone or derivative e.g. protonated form thereof
  • the anode may be contacted (e.g. soaked or dipped) in a solution of a lithium salt in sulfolane.
  • the lithium salt may be the same or different from the lithium salt employed in the electrolyte of the cell.
  • the lithium salt is the same as the lithium salt employed in the electrolyte of the cell.
  • suitable lithium salts include lithium hexafluorophosphate, lithium hexafluoroarsenate, lithium perchlorate, lithium
  • the lithium salt is lithium trifluoromethanesulphonate (also known as lithium triflate).
  • Combinations of salts may be employed.
  • the salt may be present at a concentration of 0.1 to 5M, preferably, 0.5 to 3M, for example, 1 M in the sulfone.
  • the anode may be coated with any suitable sulfone coating.
  • the sulfone may be an acyclic or cyclic sulfone.
  • Suitable sulfones may have the formula R1SO2R, where Ri and R2 are each independently an alkyl group that is optionally substituted e.g. with an ether group, or Ri and R2 join together to form a 4 to 6 membered ring with the S atom of the SO2 group.
  • Ri and R2 are each independently an alkyl group
  • suitable alkyl groups include methyl, ethyl, propyl (e.g. iso-propyl), butyl (e.g.
  • the sulfone may be a symmetric sulfone where Ri and R2 are the same alkyl group. Alternatively, the sulfone may be asymmetric where R1 and R2 are different alkyl groups. Where the sulfone is a cyclic sulfone, the cyclic sulfone may have a 4-, 5- or 6- membered ring. A preferred sulfone is a sulfolane.
  • the sulfolane may be an unsubstituted sulfolane or a sulfolane that is substituted, for example, with one or more alkyl groups (e.g. a Ci to C6 alkyl group and/or one or more ether groups (e.g. -OCH3).
  • alkyl groups e.g. a Ci to C6 alkyl group and/or one or more ether groups (e.g. -OCH3).
  • Suitable sulfones include
  • the sulfone is a non-polymeric sulfone.
  • the sulfone may contain fewer than 20 carbon atoms, for example, fewer than 15 carbon atoms. In one example, the sulfone contains 2 to 10 carbon atoms. In some embodiments, polyethersulfones may be excluded.
  • the sulfone may be a liquid at room temperature (25 degrees) and pressure (e.g. 101 kPa).
  • the sulfone may have a molecular weight of less than 1000 g/mol, for example, less than 500 g/mol.
  • the sulfone may have a molecular weight of less than 200 g/mol, for example, less than 150 g/mol. In one embodiment may have a molecular weight of 50 to 300 g/mol, for example, 90 to 200 g/mol. Sulfones having a molecular weight of less than 1000g/mol may be conveniently applied to the anode in a pre-treatment step, for example, by dipping or soaking. Lithium salts may also be dissolved or suspended in the sulfone, such that the coating comprises lithium ions and the sulfone.
  • the anode may be contacted with the sulfone or a solution comprising a lithium salt dissolved in sulfone for sufficient time for the sulfone and any optional salt to be deposited on the anode's surface.
  • the contacting step may take at least 5 minutes, preferably at least 30 minutes, more preferably, at least 1 hour. In some examples, the contacting step may take at least 2 hours, for example, at least 5 hours. In some examples, the contacting step may take up to 1 week, for example, up to 3 days.
  • the anode may be contacted with a solution comprising at least 50% sulfone, preferably, at least 90 weight% sulfone, for example, 90 to 100% weight sulfone.
  • the solution may also contain a lithium salt dissolved in the sulfone.
  • the concentration of lithium salt may form 10 weight % or less of the solution.
  • the anode is contacted with contains a lithium salt dissolved in sulfone, whereby the concentration of lithium salt in the sulfone is 0.1 to 5M, preferably, 0.5 to 3M, for example, 1 M.
  • the pre-treated anode may be used to assemble the lithium sulphur cell.
  • the pre-treated anode and a cathode comprising a mixture of electroactive sulphur material and solid electroconductive material with an electrolyte.
  • the anode comprises a coating comprising sulfone and lithium ions.
  • the anode may be an anode that is pre-treated to provide it with such a coating prior to contact with the cell's electrolyte.
  • the organic solvent in the electrolyte may comprise less than 20 weight % sulfolane.
  • the organic solvent comprises less than 10 weight % of a sulfone, more preferably, less than 5 weight %, even more preferably less than 2 weight % sulfone.
  • the organic solvent comprises less than 10 weight % of sulfolane, more preferably, less than 5 weight %, even more preferably less than 2 weight % sulfolane.
  • the organic solvent is substantially devoid of sulfone, for example, substantially devoid of sulfolane.
  • Suitable organic solvents for use in the electrolyte are tetrahydrofurane, 2- methyltetrahydrofurane, dimethylcarbonate, diethylcarbonate, ethylmethylcarbonate, methylpropylcarbonate, methylpropylpropionate, ethylpropylpropionate, methyl acetate, dimethoxyethane, 1 , 3-dioxolane, diglyme (2-methoxyethyl ether), tetraglyme, ethylene carbonate, propylene carbonate, butyrolactone, dioxolane, hexamethyl phosphoamide, pyridine, dimethyl sulfoxide, tributyl phosphate, trimethyl phosphate, and N, N, N, N- tetraethyl sulfamide.
  • the organic solvent comprises an ether.
  • the organic solvent comprises tetraethylene glycol dimethyl ether (TEGDME).
  • the organic solvent comprises TEGDME, dimethoxyethane and, optionally, 1 , 3- dioxolane.
  • TEGDME may form at least 40 v/v%, preferably at least 50% v/v of the organic solvent of the electrolyte.
  • dimethoxyethane may form at least 20 v/v%, preferably at least 30% v/v of the organic solvent of the electrolyte.
  • the organic solvent contains TEGDME, dimethoxyethane and 1 , 3-dioxolane in a v/v ratio of 50:30:20.
  • the organic solvent of the electrolyte may have a viscosity of less than 20cP, preferably less than 10cP, more preferably less than 7cP at 25 degrees C. Where mixtures of organic solvents are employed in the electrolyte, the mixtures may have a viscosity of less than 20cP, preferably less than 10cP, more preferably less than 7cP at 25 degrees C. In one embodiment, the electrolyte may have a viscosity of less than 20cP, preferably less than 10cP, more preferably less than 7cP at 25 degrees C.
  • the electrolyte comprises a lithium salt dissolved in the organic solvent.
  • Suitable lithium salts include lithium hexafluorophosphate, lithium hexafluoroarsenate, lithium nitrate, lithium perchlorate, lithium trifluoromethanesulfonimide, lithium bis(oxalate) borate and lithium trifluoromethanesulphonate.
  • the lithium salt is lithium
  • lithium triflate trifluoromethanesulphonate
  • Combinations of salts may be employed.
  • lithium triflate may be used in combination with lithium nitrate.
  • the lithium salt may be present in the electrolyte at a concentration of 0.1 to 5M, preferably, 0.5 to 3M, for example, 1 M.
  • the electrolyte may also comprise lithium polysulphides.
  • lithium polysulphides may be added to the electrolyte before the cell is discharged.
  • concentration of lithium polysulphide dissolved in the electrolyte may be between 0.1 % and 20% weight % (preferred concentration 1.5%).
  • the cathode of the electrochemical cell includes a mixture of electroactive sulphur material and electroconductive material. This mixture forms an electroactive layer, which may be placed in contact with a current collector, formed for example of metal foil (e.g. Al foil).
  • a current collector formed for example of metal foil (e.g. Al foil).
  • the electroactive sulphur material may comprise elemental sulphur, sulphur-based organic compounds, sulphur-based inorganic compounds and sulphur-containing polymers.
  • elemental sulphur is used.
  • the solid electroconductive material may be any suitable conductive material.
  • this solid electroconductive material may be formed of carbon. Examples include carbon black, carbon fibre, graphene and carbon nanotubes. Other suitable materials include metal (e.g. flakes, filings and powders) and conductive polymers. Preferably, carbon black is employed.
  • the mixture of electroactive sulphur material and electroconductive material may be applied to the current collector in the form of a slurry in a solvent (e.g. water or an organic solvent). The solvent may then be removed and the resulting structure calendared to form a composite structure, which may be cut into the desired shape to form a cathode. A separator may be placed on the cathode and a lithium anode placed on the separator.
  • a solvent e.g. water or an organic solvent
  • Electrolyte may then be introduced into the assembled cell to wet the cathode and separator.
  • the electrolyte may be applied to the separator, for example, by coating or spraying before the lithium anode is placed on the separator.
  • the separator may comprise any suitable porous substrate that allows ions to move between the electrodes of the cell.
  • the separator should be positioned between the electrodes to prevent direct contact between the electrodes.
  • the porosity of the substrate should be at least 30%, preferably at least 50%, for example, above 60%.
  • Suitable separators include a mesh formed of a polymeric material. Suitable polymers include polypropylene, nylon and polyethylene. Non-woven polypropylene is particularly preferred. It is possible for a multi- layered separator to be employed.
  • a lithium foil anode was placed in contact with an electrolyte consisting of a 1 M solution of lithium triflate in sulfolane.
  • the anode was then removed and analysed by photoelectron spectroscopy. .
  • the spectrum shows a strong peak at -169 eV, a distinct shoulder at -167 eV and a broad contribution between 162 and 164 eV.
  • the peaks at 169.3 eV and 167.4 eV were attributed to lithium triflate (CF3SO3 " ) and sulfolane (C4H8O2S), respectively.
  • a lithium sulphur cell was assembled using a lithium foil anode and a cathode formed using a mixture of carbon black and elemental sulphur.
  • the electrolyte was formed of solution containing 1 M LiOTf and 0.5M L1NO3 in TEGDME:DME:DIOX (50:30:20 v/v) and 1.5% wt Li 2 S 8 .
  • the cell was cycled and the capacity of the cell was determined over multiple cycles. The results are shown in Figure 1. As can be seen from the figure, the capacity begins to fade after approximately 30 cycles.
  • Example 2 a cell was assembled according to Example 2 above. However, in this Example, the lithium foil anode was pre-treated by leaving it to soak in 1 M triflate in sulfolane for 48 hours. Once pre-treated, the lithium foil anode was then used as the anode of the cell.
  • the pre-treatment step prolonged the cycle life of the cell to beyond 50 cycles.
  • Example 3 a cell was assembled according to Example 3 above. However, in this Example, the lithium foil anode was pre-treated by leaving it to soak in 1 M triflate in 3- methyl sulfolane for 48 hours. Once pre-treated, the lithium foil anode was then used as the anode of the cell.
  • the pre-treatment step prolonged the cycle life of the cell to beyond 50 cycles.
  • Example 3 a cell was assembled according to Example 3 above. However, in this Example, the lithium foil anode was pre-treated by leaving it to soak in 0.2 M LiBOB (lithium bis(oxalate) borate) in sulfolane for 48 hours. Once pre-treated, the lithium foil anode was then used as the anode of the cell.
  • LiBOB lithium bis(oxalate) borate
  • FIG. 1 is an SEM photograph of the surface of the anode. As can be seen from the SEM photograph, the anode's surface is relatively smooth, indicating that lithium is dissolved and re-deposited onto the anode in an efficient manner.
  • Example 6 was repeated using an untreated lithium foil anode. After 50 cycles, the anode was removed.
  • Figure 3 is an SEM photograph of the surface of the anode. As can be seen from the SEM photograph, lithium dendrites can be seen on the surface of the anode. This indicates poor re-deposition of lithium onto the anode's surface. This has a negative impact on the cycle life of the cell.

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Abstract

La présente invention porte sur une pile au lithium-soufre comprenant une anode comprenant du lithium métallique ou un alliage de lithium métallique, une cathode comprenant un mélange d'un matériau soufré électroactif et d'un matériau électroconducteur solide, et un électrolyte comprenant un sel de lithium et un solvant organique comprenant de 0 à moins de 20 % en poids d'une sulfone ; caractérisée en ce qu'au moins une partie de l'anode comprend un revêtement de sulfone, ladite partie revêtue étant en contact avec l'électrolyte.
PCT/GB2016/051075 2015-04-27 2016-04-19 Pile au lithium-soufre WO2016174394A1 (fr)

Priority Applications (2)

Application Number Priority Date Filing Date Title
GB1719154.5A GB2555033B (en) 2015-04-27 2016-04-19 A lithium-sulphur cell
TW105112830A TW201703317A (zh) 2015-04-27 2016-04-25 鋰－硫電池

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Application Number Priority Date Filing Date Title
EP15165277.3 2015-04-27
EP15165277 2015-04-27

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Cited By (2)

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Publication number Priority date Publication date Assignee Title
CN107293797A (zh) * 2017-07-07 2017-10-24 北京理工大学 锂二次电池
WO2018224374A1 (fr) * 2017-06-09 2018-12-13 Fraunhofer-Gesellschaft zur Förderung der angewandten Forschung e.V. Électrolyte pour batterie alcaline au soufre, batterie alcaline au soufre contenant ledit électrolyte, et utilisations dudit électrolyte

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JP2012156114A (ja) * 2011-01-28 2012-08-16 Toyota Central R&D Labs Inc 非水系空気電池及び非水系空気電池の製造方法

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JP2012156114A (ja) * 2011-01-28 2012-08-16 Toyota Central R&D Labs Inc 非水系空気電池及び非水系空気電池の製造方法

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CHANG D-R ET AL: "Binary electrolyte based on tetra(ethylene glycol) dimethyl ether and 1,3-dioxolane for lithium-sulfur battery", JOURNAL OF POWER SOURCES, ELSEVIER SA, CH, vol. 112, no. 2, 14 November 2002 (2002-11-14), pages 452 - 460, XP004391006, ISSN: 0378-7753, DOI: 10.1016/S0378-7753(02)00418-4 *

Cited By (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2018224374A1 (fr) * 2017-06-09 2018-12-13 Fraunhofer-Gesellschaft zur Förderung der angewandten Forschung e.V. Électrolyte pour batterie alcaline au soufre, batterie alcaline au soufre contenant ledit électrolyte, et utilisations dudit électrolyte
US11594760B2 (en) 2017-06-09 2023-02-28 Fraunhofer-Gesellschaft zur Förderung der angewandten Forschung e.V. Electrolyte for an alkali-sulfur battery, alkali-sulfur battery containing the electrolyte, and uses of the electrolyte
CN107293797A (zh) * 2017-07-07 2017-10-24 北京理工大学 锂二次电池

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GB2555033B (en) 2022-02-09
GB201719154D0 (en) 2018-01-03

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