EP1230707A1 - Cellule electrochimique de stockage d'energie - Google Patents

Cellule electrochimique de stockage d'energie

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Publication number
EP1230707A1
EP1230707A1 EP00941876A EP00941876A EP1230707A1 EP 1230707 A1 EP1230707 A1 EP 1230707A1 EP 00941876 A EP00941876 A EP 00941876A EP 00941876 A EP00941876 A EP 00941876A EP 1230707 A1 EP1230707 A1 EP 1230707A1
Authority
EP
European Patent Office
Prior art keywords
cell according
electrochemical cell
cathode
anode
metal
Prior art date
Legal status (The legal status 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 status listed.)
Withdrawn
Application number
EP00941876A
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German (de)
English (en)
Inventor
Werner Henze
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)
Individual
Original Assignee
Individual
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 Individual filed Critical Individual
Publication of EP1230707A1 publication Critical patent/EP1230707A1/fr
Withdrawn legal-status Critical Current

Links

Classifications

    • 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
    • H01M10/36—Accumulators not provided for in groups H01M10/05-H01M10/34
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M12/00—Hybrid cells; Manufacture thereof
    • H01M12/08—Hybrid cells; Manufacture thereof composed of a half-cell of a fuel-cell type and a half-cell of the secondary-cell type
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M6/00—Primary cells; Manufacture thereof
    • H01M6/24—Cells comprising two different electrolytes
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M12/00—Hybrid cells; Manufacture thereof
    • H01M12/08—Hybrid cells; Manufacture thereof composed of a half-cell of a fuel-cell type and a half-cell of the secondary-cell type
    • H01M12/085—Zinc-halogen cells or batteries
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M16/00—Structural combinations of different types of electrochemical generators
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M8/00—Fuel cells; Manufacture thereof
    • H01M8/18—Regenerative fuel cells, e.g. redox flow batteries or secondary fuel cells
    • H01M8/184—Regeneration by electrochemical means
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M8/00—Fuel cells; Manufacture thereof
    • H01M8/18—Regenerative fuel cells, e.g. redox flow batteries or secondary fuel cells
    • H01M8/184—Regeneration by electrochemical means
    • H01M8/188—Regeneration by electrochemical means by recharging of redox couples containing fluids; Redox flow type batteries
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M8/00—Fuel cells; Manufacture thereof
    • H01M8/22—Fuel cells in which the fuel is based on materials comprising carbon or oxygen or hydrogen and other elements; Fuel cells in which the fuel is based on materials comprising only elements other than carbon, oxygen or hydrogen
    • 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
    • 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
    • Y02E60/30—Hydrogen technology
    • Y02E60/50—Fuel cells

Definitions

  • the invention relates to an electrochemical energy-storing cell according to the preamble of claim 1 and an energy storage system according to claim 33.
  • Electrochemical energy stores should generally meet the following requirements:
  • the object of the invention is to provide an electrochemically operating cell in which reversible electrical energy can be converted into chemical energy and which meets the requirements mentioned above much better than conventional rechargeable batteries and accumulators.
  • the cell according to the invention consists of a partial cell on the cathode side and an anode side. There is a hydrogen electrode between the two cell parts.
  • the cathode forms the negative electrode (negative pole).
  • the positively charged ions migrate to the cathode, pick up the missing electrons there and become electrically neutral. The process is reversed when unloading.
  • the anode forms the positive electrode (positive pole).
  • the negatively charged ions migrate to the anode and give off their excess electrons there. The process is reversed when unloading.
  • the cathode-side sub-cell consists of a cathode-side electrolyte and a memory which contains a base metal in crystalline or dissolved form.
  • This memory is referred to below as a metal memory.
  • the metal storage consists of a crystalline metal
  • the metal itself forms the cathode.
  • the solution and an adjoining intermediate electrode form the metal store.
  • the solution is delimited by the cathode on the opposite side of the intermediate electrode.
  • Such a solution of anhydrous ammonia and an alkali metal has a very high electrical conductivity.
  • the effective part of the intermediate electrode consists of at least one graphite layer. A graphite electrode can also be used as the cathode.
  • the electrolyte on the cathode side which is arranged between the hydrogen electrode and the metal store, has a different composition depending on the type of metal store. If a crystalline metal is used as the metal store, the cathode-side electrolyte contains, in addition to the solvent, for example water, at least one additive which increases the conductivity, preferably potassium hydroxide or ammonia. This enables the electrolytic processes.
  • the cathode-side electrolyte consists of an anhydrous solvent, preferably ammonia, and an additive which increases the conductivity, for example an alkali metal amide, which can be both electrolytically formed and decomposed ,
  • the anode-side sub-cell consists of an anode-side electrolyte and a memory which is able to store halogens, for example fluorine.
  • This storage will be referred to as gas storage in the following.
  • the anode-side electrolyte consists of a halogen-containing water-free solvent, for example hydrogen fluoride, in which to increase the conductivity and to accelerated course of the electrolytic processes at least one salt, for example ammonium fluoride or potassium fluoride, is dissolved.
  • a halogen-containing water-free solvent for example hydrogen fluoride
  • Free halogens are known to be very aggressive and toxic. With the exception of bromine and iodine, they can only be stored as gas under great pressure, for example in steel bottles.
  • the gas storage device is capable of chemically binding halogens and storing them in graphite.
  • the gas storage therefore consists of a mixture of graphite particles and at least one halogen compound which can easily add and release further halogen atoms, the value of the binding partner atom changing.
  • These compounds include, for example, manganese (III) fluoride, manganese (IV) fluoride, bromine fluoride or bromine trifluoride.
  • Halogen atoms are stored in the crystal lattice of the graphite particles during charging and released again when discharging.
  • the embedded halogens are partly ionically bound in the crystal lattice of the graphite and partly exist atomically or molecularly. In this way it is possible to store larger quantities of an otherwise gaseous halogen.
  • Another point to consider is the liquid state of aggregation of the cathode-side and anode-side electrolytes in the operating temperature range, e.g. -20 ° C to + 50 ° C.
  • the melting point of the saline solution can be lowered sufficiently by a sufficient proportion of the halogen solvent in the anode-side electrolyte.
  • the boiling point of the cathode-side sub-cell is increased by adding, for example, an alkali amide and by setting an atmospheric pressure above the liquid.
  • the alkali amide ensures the ionic conductivity of the respective solution.
  • the electrodes between the cathode and anode are intermediate electrodes and must have the following properties:
  • Ionic conductivity (metal storage / electrolyte for alkali metal ions), (Hydrogen electrode, if possible only for hydrogen ions),
  • All properties can be met by using at least one graphite layer, preferably retort graphite, on a carrier material, for example silicon carbide or Teflon.
  • a carrier material for example silicon carbide or Teflon.
  • a platinum or palladium layer is more suitable.
  • Fig. 1 shows the basic structure of a cell that a metal memory made of crystalline metal, e.g. made of zinc Zn,
  • Fig. 2 shows the basic structure of a cell that a metal memory made of dissolved alkali metal, e.g. Sodium, has,
  • Fig. 12 the ion charge exchange and transport in a graphite layer
  • FIG. 13 shows the schematic representation of the electrochemical energy-storing cell according to the invention.
  • Fig. 1 shows the basic structure of the cell according to the invention, which has a metal storage made of crystalline base metal.
  • FIG. 2 shows the basic structure of the cell according to the invention, in which the metal storage contains an alkali metal dissolved in anhydrous ammonia NH 3 .
  • FIGS. 3 to 10 The electrochemical processes when charging and discharging the cells are shown in FIGS. 3 to 10.
  • the chemical reactions between two electrodes for charging or discharging the cell are considered separately.
  • the quantitative changes occurring between the substances between the electrodes are shown in a table.
  • the numerical values given in the tables correspond to the chemical reaction equations given between the electrodes and represent the number of atoms or molecules added or formed and those withdrawn or entered into the reaction.
  • the cathode K consists of zinc Zn.
  • the cathode K has a very large surface area and this is advantageous in part when charging the cell and is used successively. This can be achieved by electrically connecting parts in the form of layers via external resistors and only the furthest when charging the cell the layer removed from the hydrogen electrode El, serves as a cathode connection.
  • the electrolyte ELI consists of water H 2 0 as solvent, potassium hydroxide KOH and the complex salt K [Zn (OH) 3 (H 2 0)].
  • the hydrogen electrode E1 consists, for example, of at least one graphite, palladium or platinum layer.
  • the hydrogen electrode El must be able to absorb electrochemically generated hydrogen H, ionically bind it and also release it again.
  • the hydrogen electrode El must be conductive, i.e. electrons must be able to flow in the conduction band.
  • the precious metals themselves are not attacked by hydrogen fluoride HF and by fluorine F in the operating temperature range of the cell (approx. -20 ° C to + 50 ° C).
  • the hydrogen electrode E1 consists of a graphite layer, it is necessary, at least when charging and discharging the cell, to ensure that a sufficient amount of hydrogen H is previously in the crystal lattice of the hydrogen electrode El was stored.
  • the half element K / ELl / El can also be loaded for a sufficient time and the recovered electrical energy can be supplied after conversion of the half cell E1 / EL2 / A.
  • the hydrogen concentration in the hydrogen electrode El no longer changes, because when charging on the anode-side surface of the hydrogen electrode El the same amount of hydrogen is generated as is consumed on its cathode-side surface, and when discharging only the assignment of generation and consumption to those Electrode surfaces change.
  • Porous silicon carbide SiC which is not attacked by acids and alkalis, can be used as the carrier material for the graphite, palladium or platinum layers.
  • FIG. 3 shows the electrochemical processes taking place in the electrolyte ELI during charging and in FIG. 4 when the Zn / F cell is discharged.
  • Z Zn is deposited on the cathode during charging.
  • the concentration of the complex salt K + [Zn (OH) 3 H 2 0] " decreases because complexed zinc ions reduce Zn 2+ and the ligands water H 2 0 and hydroxide ions OH " are released again.
  • the reverse process takes place when unloading.
  • Zinc Zn goes into solution from the cathode K and again forms the complex salt K + [Zn (OH) 3 H 2 0] " with water H 2 0 and the hydroxide ions OH " and the potassium ions K + .
  • the hydrogen electrode El supplies the hydrogen H necessary for the chemical reaction during charging. When discharged, this is generated on the cathode-side surface of the hydrogen electrode El and from there is stored in the graphite grid of the hydrogen electrode El.
  • Elemental sodium Na is deposited on the cathode K shown in FIG. 2, as illustrated in FIG. 5, which is then dissolved in the electrolyte EL0.
  • a particular advantage here is that no short circuits between cathode K and hydrogen electrode El can occur during charging.
  • the physical nature of the cathode K no longer changes, and thus all related electrodes, including cathode K and anode A, are not energy sources.
  • the sodium amide content in the electrolyte EL0 does not change during charging and discharging.
  • the intermediate electrode E0 is practically a sodium electrode.
  • the electrolyte EL0 also has a very high electrical conductivity due to the sodium Na dissolved in it, this applies to a greater extent to the charged state of the cell.
  • Fig.2 is between the hydrogen electrode E1 and the sodium electrode E0 the electrolyte ELI, which is comparable in terms of cell structure with that in Fig.l.
  • the concentration of sodium amide NaNH 2 is reduced when the cell is charged and increases again when it is discharged, ie the concentration of sodium ion Na + is in the electrolyte ELI lower in the charged state than in the discharged state of the cell.
  • the proportion of the ammonia NH 3 solvent increases during charging and decreases during unloading.
  • sodium ions Na + are discharged on the anode-side surface of the electrode E0 and taken up by the crystal lattice of the graphite.
  • the sodium Na supplied via electrode E0 combines with the discharged NH 2 " ions [NH 2 ] to form sodium amide NaNH 2.
  • the behavior of the NH 2 " ions dissolved in ammonia NH 3 is comparable to that of the hydroxide ions OH " in water H 2 0.
  • iron Fe or, for example, a platinum or palladium layer can be used in the graphite crystal lattice of the hydrogen electrode El.
  • These latter two metals also have the desired property of only absorbing hydrogen H and thus act as a filter against other substances.
  • the catalytically active metals do not form a permanent chemical compound with the solvent ammonia NH 3 and the dissolved sodium amide NaNH 2 .
  • the electrolyte EL2 is composed of the anhydrous hydrogen fluoride solvent HF and a salt, preferably ammonium fluoride NH 4 F or potassium fluoride KF. A salt mixture can also be used.
  • ammonium fluoride NH 4 F is best suited to achieve the electrolyte EL2 a low melting point
  • ammonia NH 3 that forms combines with hydrogen fluoride HF to form ammonium fluoride NH 4 F.
  • Fluorine F is formed on the cathode-side surface of the intermediate electrode E2 and is taken up by the intermediate electrode E2.
  • the property of the hydrogen fluoride HF to accumulate in a chain has an advantageous effect. This ensures that each RF molecule formed on an electrode surface is deposited in the EL2 electrolyte.
  • the intermediate electrode E2 fluorine F When discharging, the intermediate electrode E2 fluorine F is withdrawn, which again forms ammonium fluoride NH 4 F with the discharged NH 4 + ion [NH 4 ] or with the hydrogen H formed therefrom.
  • the concentration of the dissolved salt does not change.
  • hydrogen fluoride HF is decomposed during the charging process and is formed again during the discharging process.
  • fluorine F reacts on the cathode-side surface of the intermediate electrode E2 with ammonium fluoride NH 4 F to form nitrogen trifluoride NF 3 in the following manner.
  • the gas storage GSP in Fig.l and Fig. 2 between the graphite anode A and the intermediate electrode E2 consists of a mixture of very small graphite particles and a fluorinating agent.
  • the chemical compounds manganese (III) fluoride MnF 3 and manganese (IV) fluoride MnF 4 as well as bromine fluoride BrF and bromine trifluoride BrF 3 are particularly suitable for taking up fluorine F during loading and releasing fluorine F during unloading.
  • manganese (II) fluoride MnF 2 and bromopentafluoride BrF 5 are also suitable.
  • the proportion can be increased further by occasionally reacting fluorine atoms F to carbon monofluoride CF during the production in the crystal lattice of the graphite particles, whereby the lattice spacing of the graphite layers is increased.
  • the circulation can e.g. thermally.
  • the mixture conducts the electrical current very well, because on the one hand graphite belongs to the first class conductors and on the other hand the fluorinating agent has electrical conductivity.
  • gas storage device GSP is comparable in terms of its electrical conductivity to the electrolyte EL0 in FIG. 2.
  • the heat losses due to the low ohmic resistance in the gas storage GSP are therefore low when charging and discharging the cell.
  • the mixture of bromofluoride BrF and bromotrifluoride BrF 3 has a lower atomic weight than the manganese fluorides, which is associated with a greater energy density / mass unit.
  • the fluorinating agents manganese (III) fluoride MnF 3 and manganese (IV) fluoride MnF 4 In this case, the gas storage GSP forms a solid gas storage.
  • liquid fluorinating agent compared to the solid gas storage is that even in connection with very large liquid tanks, in extreme cases only one cell according to the construction in FIG. 2 can be used.
  • a further development provides that a metallic conductor connected to the graphite anode A does not corrode. Since the anode A consisting of graphite shown in FIG. 1 and FIG. 2 stores fluorine F in the graphite grid, it is in principle possible that, for example, the copper contact of the anode A corrodes by reaction with fluorine F.
  • FIG. 11 shows how, during charging, fluoride ions F "of the electrolyte EL2 are discharged on the cathode-side surface of the intermediate electrode E2 and are transported ionically through them into the gas store GSP.
  • Carbon atoms C on the surface of the intermediate electrode E2, which face the electrolyte EL2, are positively charged by electron withdrawal via the anode A.
  • a charge exchange takes place between positively charged carbon atoms C + and neighboring fluoride ions F " .
  • the charge exchange is associated with a transport of the fluorine atom F into the graphite lattice because atoms or molecules of different polarity attract each other.
  • the positive charge passes from anode A to a (C + + F " ) pair.
  • the negatively charged fluorine atom F " migrates the positively charged carbon atom C + , which was created by electron withdrawal via anode A.
  • the positively charged carbon atom C + of the original (C + + F " ) pair discharges with the closest fluoride ion F " of the electrolyte EL2, as a result of which the fluorine atom F is embedded in the graphite lattice.
  • Example B shows how the process described in Example A can also be carried out with many fluorine atoms F or fluoride ions F " .
  • fluorine atoms F On the surface of the intermediate electrode E2, which faces the gas storage device GSP, discharge of fluoridions F " results in fluorine atoms F which leave the intermediate electrode E2 and are taken up by the gas storage device GSP.
  • the fluorine atoms F can again be used as fluoride ions F " in the gas storage device GSP.
  • manganese (III) fluoride MnF 3 can be converted into manganese (IV) fluoride MnF 4 and the graphite particles in the gas storage GSP can absorb fluorine atoms F.
  • the electrons e extracted from the intermediate electrode E2 serve to transport the fluoride ions in the gas storage unit GSP.
  • the hydrogen is also transported through the intermediate electrode E1 and the sodium is transported through the intermediate electrode E0.
  • a prerequisite for storing fluorine F in the gas storage unit GSP is that unhindered fluoride ion transport can take place in the entire storage unit.
  • the gas storage unit GSP must therefore not consist entirely of graphite. This means that the transport must not be increasingly hampered by the fact that the left part of the above Equation prevails.
  • the fluorinating agent can release fluorine F during loading of the cell on graphite particles as well as when discharging and that the fluorinating agent can resume and that Graphite particles form a very large surface in their entirety, which allow the storage of fluoride ions F " .
  • the transport of the fluorine atoms F in the gas storage GSP during charging at an arbitrarily selected location is given below.
  • the removal of electrons on the anode side produces positively charged atoms or molecules, the geometrical position of which is denoted by x below and which faces the anode A.
  • the electrons supplied via the cathode K result in atoms or molecules which have been negatively charged with respect to the location x and which have already taken up fluorine atoms F, in the position designated x + 1.
  • E2 cathode cathode Depending on the case of contact, the charges will balance as the fluorine atom F is transported. There are four possible cases.
  • the fluorine atoms F will be spatially balanced. Fluorine atoms F on the surface of the graphite particles, which are currently in the atomic state, react with manganese (III) fluoride MnF 3 to form manganese (IV) fluoride MnF 4 and fluoride ions F " , which result from the decay of manganese (IV) - fluoride MnF 4 to manganese (III) fluoride MnF 3 + F " emerge, are taken up by graphite particles. Ultimately, a state of equilibrium will occur which corresponds to the state of charge of the gas storage unit GSP.
  • the structure of the electrochemical energy-storing cell is shown schematically in FIG.
  • the cell comprises a cathode (K) and an anode (A) and is divided into sub-cells, between which there is a hydrogen electrode (El).
  • the partial cell on the cathode side comprises a metal storage and an electrolyte (ELI).
  • the anode-side sub-cell comprises a gas storage (GSP) and an electrolyte (EL2).
  • the total voltage is:
  • the total voltage is:
  • the cell chambers in which the electrolyte EL2 and the gas storage GSP are located must be sealed gas-tight.
  • Silicon carbide SiC or B ⁇ 3 C 2 as well as Teflon (CF 2 ) n and carbon monographite (CF ⁇ , ⁇ 2 ) can be used as materials for the production of housings and containers in the gas storage unit GSP.
  • hydrogen fluoride-resistant plastics are suitable for holding the EL2 electrolyte.
  • Porous silicon carbide SiC or Teflon is suitable as a carrier material for the graphite electrodes El, E2 and A in Fig.l and K, E0, E2 and A in Fig.2.
  • the resulting end products are therefore potassium fluoride KF, zinc fluoride ZnF 2 , free hydrogen H 2 and free oxygen 0 2 , with zinc fluoride ZnF 2 being difficult to dissolve in water H 2 0.
  • the electrolytes EL0, ELI and EL2 and the GSP will react with one another mainly when the electrodes E0, El and E2 are destroyed and form the following connections:

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  • Engineering & Computer Science (AREA)
  • Manufacturing & Machinery (AREA)
  • Chemical & Material Sciences (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • General Chemical & Material Sciences (AREA)
  • Hybrid Cells (AREA)

Abstract

La présente invention concerne une cellule électrochimique de stockage d'énergie, comprenant une cathode (K) et une anode (A). Ladite cellule est divisée en cellules partielles, entre lesquelles se trouve une électrode à hydrogène (E1). Les cellules partielles situées côté cathode comprennent un dispositif de stockage de métal et un électrolyte (EL1) et les cellules partielles situées côté anode comprennent un dispositif de stockage de gaz (GSP) et un électrolyte (EL2).
EP00941876A 1999-11-19 2000-04-14 Cellule electrochimique de stockage d'energie Withdrawn EP1230707A1 (fr)

Applications Claiming Priority (3)

Application Number Priority Date Filing Date Title
DE19955960 1999-11-19
DE19955960 1999-11-19
PCT/DE2000/001218 WO2001039312A1 (fr) 1999-11-19 2000-04-14 Cellule electrochimique de stockage d'energie

Publications (1)

Publication Number Publication Date
EP1230707A1 true EP1230707A1 (fr) 2002-08-14

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EP00941876A Withdrawn EP1230707A1 (fr) 1999-11-19 2000-04-14 Cellule electrochimique de stockage d'energie

Country Status (4)

Country Link
EP (1) EP1230707A1 (fr)
AU (1) AU5670800A (fr)
DE (1) DE10083651D2 (fr)
WO (1) WO2001039312A1 (fr)

Families Citing this family (1)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
DE10131822A1 (de) * 2001-06-30 2002-09-19 Werner Henze Elektrochemische energiespeichernde Zelle

Family Cites Families (8)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US3092516A (en) * 1960-05-06 1963-06-04 Standard Oil Co Electrochemical reaction apparatus
US3427207A (en) * 1966-10-28 1969-02-11 Us Army Batteries with halogen fluoride electrolyte
US3573987A (en) * 1969-07-28 1971-04-06 Milton A Knight Electrochemical electric power generator
FR2412174A1 (fr) * 1977-12-16 1979-07-13 Aerospatiale Pile du type solution de lithium-gaz oxydant
US4296184A (en) * 1980-01-03 1981-10-20 Stachurski John Z O Electrochemical cell
DE4025699A1 (de) * 1990-08-14 1992-02-20 Reten Electronic Gmbh & Co Akkumulator
US5591538A (en) * 1995-07-07 1997-01-07 Zbb Technologies, Inc. Zinc-bromine battery with non-flowing electrolyte
JP2956027B2 (ja) * 1997-02-04 1999-10-04 康男 馬路 電 池

Non-Patent Citations (1)

* Cited by examiner, † Cited by third party
Title
See references of WO0139312A1 *

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Publication number Publication date
AU5670800A (en) 2001-06-04
WO2001039312A1 (fr) 2001-05-31
DE10083651D2 (de) 2002-11-07

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