CA1188360A - Inorganic rechargeable non-aqueous cell - Google Patents
Inorganic rechargeable non-aqueous cellInfo
- Publication number
- CA1188360A CA1188360A CA000415569A CA415569A CA1188360A CA 1188360 A CA1188360 A CA 1188360A CA 000415569 A CA000415569 A CA 000415569A CA 415569 A CA415569 A CA 415569A CA 1188360 A CA1188360 A CA 1188360A
- Authority
- CA
- Canada
- Prior art keywords
- cell
- electrolyte
- cathode
- comprised
- anode
- 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.)
- Expired
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
- H01M10/05—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
- H01M10/0561—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of inorganic materials only
- H01M10/0563—Liquid materials, e.g. for Li-SOCl2 cells
-
- 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
- H01M4/58—Selection of substances as active materials, active masses, active liquids of inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy; of polyanionic structures, e.g. phosphates, silicates or borates
- H01M4/582—Halogenides
-
- 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
Abstract
INORGANIC RECHARGEABLE NON-AQUEOUS CELL
ABSTRACT
A totally inorganic non-aqueous rechargeable cell having an alkali or alkaline earth metal anode such as of lithium, a sulfur dioxide contain-ing electrolyte and a discharging metal halide cathode, such as of CuC12, with said metal halide being substantially totally insoluble in S02.
ABSTRACT
A totally inorganic non-aqueous rechargeable cell having an alkali or alkaline earth metal anode such as of lithium, a sulfur dioxide contain-ing electrolyte and a discharging metal halide cathode, such as of CuC12, with said metal halide being substantially totally insoluble in S02.
Description
This invent~ OD relates to non-aqueous rechar~eable cells and more particularly to such cells having lithium anodes and sulfur dioxide electro-lyte solvents.
The rechargeabllity of non-aqueous cells has been generally hampered by the presence within such cells of mater~als which ~eart either upon ~tanding or during cell discharge and which are not capable of be~ng completely regenerated from ~heir reaction products during cell charginK.
Organic electrolyte solvents utili~.ed in non-aqueous rell~ such as propylene carbonate which ~or~s anode metal carbonates and propylene ga5 are the most common of the :Lncompletely regenerable material~. Ho~everg such organic electrolyte soLvents are generally indispensible for proper operation of the non-aqueous cells particularly cells having sulfur dioxlde electrolyte solvent/cathode depolarizers, since sulfur dioxide alone i6 a poor solvent for electrolyte salt6 except for certain esoteric salts such as clovobora~es and gallium halldes as descrlbed in ~.S. PatentR Nos. 4,020,240 and 4,177,329 respectively. More common salts such as metal halides; e.g., LiBr and tetrachloroaluminat~ e.g., LiAlC14 are ei~her insoluble iD S02 alone or form complexes therewith whereby cell performance is drastically deterior ated. Utilization of the aforemeneloned esoteric 6alts ln order to provide a totally inorganic cell has been e~fective in ~ncreasing the rechargeable efficiency ~f 6uch cells. Ho~ever9 fiome of the e60teric salts, while effective, are nevertheless exceedingly costly whereby construction of an economical cell ~herewith has been generally precluded. Further~ore 7 durlng the increased cycle lif~ in such cells a second cource o~ deteriora-tion of the eells was discover2d. In cells containing the inorganic sulfur dio~ide electrolyte and lnert carbon cathodes said cathode6 tended to lose their structural inte~rity. The formAtion and depletion of cell react~on products with~n the cathode causes detrimental expansion and contraction of the carbon cathode which expansion and contraction could not be accommodated without structural damage to the cathode.
The rechargeabllity of non-aqueous cells has been generally hampered by the presence within such cells of mater~als which ~eart either upon ~tanding or during cell discharge and which are not capable of be~ng completely regenerated from ~heir reaction products during cell charginK.
Organic electrolyte solvents utili~.ed in non-aqueous rell~ such as propylene carbonate which ~or~s anode metal carbonates and propylene ga5 are the most common of the :Lncompletely regenerable material~. Ho~everg such organic electrolyte soLvents are generally indispensible for proper operation of the non-aqueous cells particularly cells having sulfur dioxlde electrolyte solvent/cathode depolarizers, since sulfur dioxide alone i6 a poor solvent for electrolyte salt6 except for certain esoteric salts such as clovobora~es and gallium halldes as descrlbed in ~.S. PatentR Nos. 4,020,240 and 4,177,329 respectively. More common salts such as metal halides; e.g., LiBr and tetrachloroaluminat~ e.g., LiAlC14 are ei~her insoluble iD S02 alone or form complexes therewith whereby cell performance is drastically deterior ated. Utilization of the aforemeneloned esoteric 6alts ln order to provide a totally inorganic cell has been e~fective in ~ncreasing the rechargeable efficiency ~f 6uch cells. Ho~ever9 fiome of the e60teric salts, while effective, are nevertheless exceedingly costly whereby construction of an economical cell ~herewith has been generally precluded. Further~ore 7 durlng the increased cycle lif~ in such cells a second cource o~ deteriora-tion of the eells was discover2d. In cells containing the inorganic sulfur dio~ide electrolyte and lnert carbon cathodes said cathode6 tended to lose their structural inte~rity. The formAtion and depletion of cell react~on products with~n the cathode causes detrimental expansion and contraction of the carbon cathode which expansion and contraction could not be accommodated without structural damage to the cathode.
-2-1~88360 M-3573 It i8 an object of the pre6ent lnventiDD tc prcvlde an improved toeally inor~anic non-aqueous cell which is readily and efficiently recharge-able.
It iR a further object of the present invention to provide such cell with readily obtainable and economical comp~nents.
These and other ob~ects, features and advan~a~es ~f the pre~ent lnvention will be more readily apparent fr~m the followlng discussion and the drawings in which:
Flgure 1 is a discharge-charge graph of cells made in a~cordance with the present invention and Figure 2 is a discharge~charge graph of another embodiment of a cell made in accordance with the present invention.
Generally, the present invention comprl~es ~n efficiently recharge-able totally in~rganic non-aqueous cell consaining an anode of an alkali or alkaline earth metal preferably lithium, including alloys and mixtures, a totally inorganic electrolyte comprified of sulfur dioxide with an electro-lyte salt soluble therein dissolved therein, and an insolu~le (in said sulfur dioxide) metal h~lide cathode which dischar~es during cell operation in preference to the S02. Metal salts such as FeC13 whlch are coluble in S02 are accordingly generally not with$n the purview ~f the present lnven-tion. In order to prevent such S02 discharge snd for greater cell capacity it ls preferred that the metal halide provides a potential greater than that obtainable from the S02 as a cathode depolarl~er. Howeve~, even with metal halides of lower potential the S02 electrolyte solvent is substantially prevented from being discharged in preference to the meta~ halide because the insoluble metal halide cathode does not provide a catalytic surface for the discharge of the S02 as compared to inert carbon cathodes.
In a preferred embodiment of the present invent~on the cell is comprised of a li~hium anode ~nd a coppe~ chloride ~CuC12) cathode. It has been discovered that the previously unsuitable but economical salts such as . LiAlC14 (which ~hlle soluble in the S02 de~rimentally complexed therewith) co~ld be effectively utlllzed in the cells Df the present invention. This utility is believed to be attributable ts the fact that S02 in the cell is not discharged and that its complexing with the salt does nDt a~ a result affect cell capacity or performance. It is therefore preferred from an economic standpoint, to utilize tetrachloroaluminate ~alts such as LiAlC14 as the electrolyte salt. This does not however preclude the util~zation of other salts such aB LiGaC14, Li2BloCllo and the like as electrolyte salts provided that they are soluble in the S02 without the necessity for organic cosolvents. Preferably such 6alts are anode ~etal salts.
Though metal halides such as copper chloride have been utilized as cathodes in non-aqueous cells, such cells have invariably contained organic solvents in which the halides ~uch as copper chlorlde were at least partial-ly soluble. As a result such cells were con6idered to be unsatisfactory because of the inherent problem of self discharge caused by the solvated metal halide. However9 the ~ery deficiency of S02, ehat lt is a poor sol-vent without or~anic cosolvents, renders the present invention operable since the metal halides such as copper chloride are substan~ially totally insoluble in S02 alone.
~he metal halide cathode is preferably made from a compressed ~o mixture of the metal halide~ conductive materials such as graphite or carbon and a binder such as polytetrafluoroethylene. The preferred percentage of ~he metal halide is between 60% to 80% by wei~ht with ~he remainder being the conductive material ~about 30 to 10%) and binder ~about 10%). The higher the intended rate the greater the amount of conductive materials.
In order to more clearly illustrate the efficacy of the present invention, the ~ollowing examples are presented. It is understood that such examples are for illustrati~e purposes only and that spec~fics contained therein are not to be construed as limitations on the present invention.
Unless otherwise indicated all parts and percenta~es are by wei~ht.
EXAMPLE_l Flat cells ~ere made with each having two an~de layers of lith$um foil (1 x 1.6 x 0.020" or 2.54 x 4.06 x O.Q5 cm) pressed onto a copper foil (0.020" or 0.05 cm), ab~ut 25 grams of 0.5 M L-lGaCl~-SO2 electrolyte, and four grams of a compressed (20,000 psi or 1406 Kg/cm ) mi~ture of 60~ CuCl2, 30% graphite and 10% polytetrafluoroethylene ~PTFE) on an expanded nickel grid as the cathode (l x 1.6 x 0.065" Dr 2.54 x 4.06 x 0.16 cm). The anode layers and cathode were individually heat sealed inside sheets Df micrD-porous polypropylene and the anode layerc placed one ~n each 6ide of the cathode. Two cells were each dlscharged at a ra~e of 2~A/cm2 or 40 ~A and thereafter charged in a cycling regimen with a 2 volt cutoff for charging.
The theoretical capacity of the cells was 480mAhrs (limiting cathode capa-city. Anode capacity was about 1800 mAhrs.). Figure 1 depicts the cycling efficiency of the cell~ wlth one cell ~hown by the solid line after the 4th cycle and the broken line indicating the ;~econd cell after the 70th cycle ~a ~h~rt circuit in the first cell prematurely ended itB cycling life after about 60 cycles).~ The 6econd cell was cycled lOl times but wl~h di~ini~hed capacity snd delivered about 67 times the CuC12 capacity on voltage cycling and lô anode turnovers. The average discharge voltage i6 rel~tively high at about 3.3 volts as compared to the discharge voltage of S02 of abDut 2.9 v~lts.
E~AMPLE 2 =
A cell was made as in Example 1 but with a 1 M LlAlC14-S02 elec-troly~e and a 2 gram cathode. The cell was discharged at the same rate of 2ma/cm2 and charged at lma/cm2 with discharge-charge cycling being on a timed basis of 4.9 hr. discharge and 9.~ hr. charge. The cell underwent 23 cycles and Figure 2 depicts the curves for the first cycle (solid line) and twenty-first cycle (broken line~ with the cell actually lmproving over contlnued cycling~
118836~ M-3573 It is u~derstood that ~he above examples are for illustrative purposes only ~nd that changes m~y be made in cell constructiQn and compo-nents without departing from ~he scope of the present invention as defined in the following claims.
It iR a further object of the present invention to provide such cell with readily obtainable and economical comp~nents.
These and other ob~ects, features and advan~a~es ~f the pre~ent lnvention will be more readily apparent fr~m the followlng discussion and the drawings in which:
Flgure 1 is a discharge-charge graph of cells made in a~cordance with the present invention and Figure 2 is a discharge~charge graph of another embodiment of a cell made in accordance with the present invention.
Generally, the present invention comprl~es ~n efficiently recharge-able totally in~rganic non-aqueous cell consaining an anode of an alkali or alkaline earth metal preferably lithium, including alloys and mixtures, a totally inorganic electrolyte comprified of sulfur dioxide with an electro-lyte salt soluble therein dissolved therein, and an insolu~le (in said sulfur dioxide) metal h~lide cathode which dischar~es during cell operation in preference to the S02. Metal salts such as FeC13 whlch are coluble in S02 are accordingly generally not with$n the purview ~f the present lnven-tion. In order to prevent such S02 discharge snd for greater cell capacity it ls preferred that the metal halide provides a potential greater than that obtainable from the S02 as a cathode depolarl~er. Howeve~, even with metal halides of lower potential the S02 electrolyte solvent is substantially prevented from being discharged in preference to the meta~ halide because the insoluble metal halide cathode does not provide a catalytic surface for the discharge of the S02 as compared to inert carbon cathodes.
In a preferred embodiment of the present invent~on the cell is comprised of a li~hium anode ~nd a coppe~ chloride ~CuC12) cathode. It has been discovered that the previously unsuitable but economical salts such as . LiAlC14 (which ~hlle soluble in the S02 de~rimentally complexed therewith) co~ld be effectively utlllzed in the cells Df the present invention. This utility is believed to be attributable ts the fact that S02 in the cell is not discharged and that its complexing with the salt does nDt a~ a result affect cell capacity or performance. It is therefore preferred from an economic standpoint, to utilize tetrachloroaluminate ~alts such as LiAlC14 as the electrolyte salt. This does not however preclude the util~zation of other salts such aB LiGaC14, Li2BloCllo and the like as electrolyte salts provided that they are soluble in the S02 without the necessity for organic cosolvents. Preferably such 6alts are anode ~etal salts.
Though metal halides such as copper chloride have been utilized as cathodes in non-aqueous cells, such cells have invariably contained organic solvents in which the halides ~uch as copper chlorlde were at least partial-ly soluble. As a result such cells were con6idered to be unsatisfactory because of the inherent problem of self discharge caused by the solvated metal halide. However9 the ~ery deficiency of S02, ehat lt is a poor sol-vent without or~anic cosolvents, renders the present invention operable since the metal halides such as copper chloride are substan~ially totally insoluble in S02 alone.
~he metal halide cathode is preferably made from a compressed ~o mixture of the metal halide~ conductive materials such as graphite or carbon and a binder such as polytetrafluoroethylene. The preferred percentage of ~he metal halide is between 60% to 80% by wei~ht with ~he remainder being the conductive material ~about 30 to 10%) and binder ~about 10%). The higher the intended rate the greater the amount of conductive materials.
In order to more clearly illustrate the efficacy of the present invention, the ~ollowing examples are presented. It is understood that such examples are for illustrati~e purposes only and that spec~fics contained therein are not to be construed as limitations on the present invention.
Unless otherwise indicated all parts and percenta~es are by wei~ht.
EXAMPLE_l Flat cells ~ere made with each having two an~de layers of lith$um foil (1 x 1.6 x 0.020" or 2.54 x 4.06 x O.Q5 cm) pressed onto a copper foil (0.020" or 0.05 cm), ab~ut 25 grams of 0.5 M L-lGaCl~-SO2 electrolyte, and four grams of a compressed (20,000 psi or 1406 Kg/cm ) mi~ture of 60~ CuCl2, 30% graphite and 10% polytetrafluoroethylene ~PTFE) on an expanded nickel grid as the cathode (l x 1.6 x 0.065" Dr 2.54 x 4.06 x 0.16 cm). The anode layers and cathode were individually heat sealed inside sheets Df micrD-porous polypropylene and the anode layerc placed one ~n each 6ide of the cathode. Two cells were each dlscharged at a ra~e of 2~A/cm2 or 40 ~A and thereafter charged in a cycling regimen with a 2 volt cutoff for charging.
The theoretical capacity of the cells was 480mAhrs (limiting cathode capa-city. Anode capacity was about 1800 mAhrs.). Figure 1 depicts the cycling efficiency of the cell~ wlth one cell ~hown by the solid line after the 4th cycle and the broken line indicating the ;~econd cell after the 70th cycle ~a ~h~rt circuit in the first cell prematurely ended itB cycling life after about 60 cycles).~ The 6econd cell was cycled lOl times but wl~h di~ini~hed capacity snd delivered about 67 times the CuC12 capacity on voltage cycling and lô anode turnovers. The average discharge voltage i6 rel~tively high at about 3.3 volts as compared to the discharge voltage of S02 of abDut 2.9 v~lts.
E~AMPLE 2 =
A cell was made as in Example 1 but with a 1 M LlAlC14-S02 elec-troly~e and a 2 gram cathode. The cell was discharged at the same rate of 2ma/cm2 and charged at lma/cm2 with discharge-charge cycling being on a timed basis of 4.9 hr. discharge and 9.~ hr. charge. The cell underwent 23 cycles and Figure 2 depicts the curves for the first cycle (solid line) and twenty-first cycle (broken line~ with the cell actually lmproving over contlnued cycling~
118836~ M-3573 It is u~derstood that ~he above examples are for illustrative purposes only ~nd that changes m~y be made in cell constructiQn and compo-nents without departing from ~he scope of the present invention as defined in the following claims.
Claims (14)
1. A totally inorganic rechargeable non-aqueous electrochemical cell comprising, a cathode, an anode of alkali or alkaline earth metal, and an electrolyte comprised of an electrolyte salt dissolved in sulfur dioxide, with said electrolyte being free of organic solvents; characterized in that said cathode is comprised of a cathode active metal halide insoluble in said sulfur dioxide and wherein said metal halide provides a potential greater than that provided by the sulfur dioxide.
2. The cell of claim 1 wherein said anode is comprised of lithium and said potential is greater than 3.0 volts.
3. The cell of claim 1 wherein said electrolyte salt is a gallium halide salt.
4. The cell of claim 1 wherein said electrolyte salt is an aluminum halide salt.
5. A totally inorganic rechargeable non-aqueous electrochemical cell comprising, a cathode, an anode of alkali or alkaline earth metal, and in electrolyte comprised of an electrolyte salt dissolved in sulfur dioxide, with said electrolyte being free of organic solvents; characterized in that said cathode is comprised of a member of the group consisting of CuC12 , CuBr2 and mixture thereof.
6. A totally inorganic rechargeable non-aqueous electrochemical cell comprising a lithium anode and an electrolyte consisting essentially of LiA1C14 dissolved in So 2 characterized in that said cell contains a cathode comprised of CuC1 2 .
7. A totally inorganic rechargeable non-aqueous electrochemical cell comprising a lithium anode and an electrolyte consisting essentially of LiGaCl 4 dissolved in SO 2 characterized in that said cell contains a cathode comprised of CuC1 2 .
8. A totally inorganic rechargeable non-aqueous electrochemical cell comprising, a cathode, an anode of alkali or alkaline earth metal, and an electrolyte comprised of an electrolyte salt dissolved in sulfur dioxide, with said electrolyte being free of organic solvents; characterized in that said cathode is comprised of a cathode active metal halide insoluble in said sulfur dioxide admixed with a conductive carbon material.
9. The cell of claim 8 wherein said metal halide is CuC1 2 or CuBr 2 .
10. The cell of claim 8 wherein said anode is comprised of lithium.
11. The cell of claim 8 wherein said electrolyte salt is a gallium halide salt.
12. The cell of claim 8 wherein said electrolyte salt is an aluminum halide salt.
13. A totally inorganic rechargeable non-aqueous electrochemical cell comprising a lithium anode and electrolyte consisting essentially of LiAlCl 4 dissolved in SO 2 characterized in that said cell contains a cathode comprised of CuCl 2 admixed with a conductive carbon material.
14. A totally inorganic rechargeable non-aqueous electrolyte cell comprising a lithium anode and an electrolyte consisting essentially of LiGaCl 4 dissolved in SO 2 characterized in that said cell contains a cathode comprised of CuCl 2 admixed with a conductive carbon material.
Applications Claiming Priority (2)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US33012881A | 1981-12-14 | 1981-12-14 | |
| US330,128 | 1981-12-14 |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| CA1188360A true CA1188360A (en) | 1985-06-04 |
Family
ID=23288432
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA000415569A Expired CA1188360A (en) | 1981-12-14 | 1982-11-15 | Inorganic rechargeable non-aqueous cell |
Country Status (7)
| Country | Link |
|---|---|
| JP (1) | JPS58117660A (en) |
| BE (1) | BE895143A (en) |
| CA (1) | CA1188360A (en) |
| DE (1) | DE3245859A1 (en) |
| FR (1) | FR2518319B1 (en) |
| GB (1) | GB2113457B (en) |
| IL (1) | IL67250A (en) |
Families Citing this family (14)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| CA1210056A (en) * | 1982-08-09 | 1986-08-19 | Donald L. Foster | Electrochemical cells having low vapor pressure complexed so.sub.2 electrolytes |
| DE3318981A1 (en) * | 1983-05-25 | 1984-11-29 | Duracell International Inc., Tarrytown, N.Y. | Nonaqueous electrochemical cell |
| US4508800A (en) * | 1983-06-30 | 1985-04-02 | Duracell Inc. | Cell with FeBr3 cathode |
| US4508798A (en) * | 1983-06-30 | 1985-04-02 | Duracell Inc. | Cell with CoCl2 cathode |
| FR2548464B1 (en) * | 1983-06-30 | 1987-06-26 | Duracell Int | NON-AQUEOUS ELECTROCHEMICAL CELLS |
| US4513067A (en) * | 1983-06-30 | 1985-04-23 | Duracell Inc. | Inorganic non-aqueous cell |
| US4508799A (en) * | 1983-06-30 | 1985-04-02 | Duracell Inc. | Cell with NiCl2 cathode |
| US4510220A (en) * | 1983-06-30 | 1985-04-09 | Duracell Inc. | Cell with PbCl2 cathode |
| DE3604541A1 (en) * | 1986-02-13 | 1987-08-20 | Finke Hans Dieter Dr | Galvanic cell comprising an alkali-metal negative electrode and a non-aqueous electrolyte containing SO2 for use as a rechargeable battery |
| EP0286990A1 (en) * | 1987-04-17 | 1988-10-19 | Whittaker Technical Products, Inc. | Method of operating and recharging a rechargeable electrochemical cell |
| US4902588A (en) * | 1988-06-06 | 1990-02-20 | Altus Corporation | Electrolyte additives to improve voltage regulation in the lithium-copper chloride rechargeable cell |
| DE3826812A1 (en) * | 1988-08-06 | 1990-02-08 | Heitbaum Joachim | NONWATER, RECHARGEABLE GALVANIC LITHIUM ELEMENT WITH INORGANIC ELECTROLYTE SOLUTION |
| DE10242694A1 (en) * | 2002-09-13 | 2004-03-25 | MAX-PLANCK-Gesellschaft zur Förderung der Wissenschaften e.V. | Compositions used as electrode in lithium battery contain transition metal halide or ruthenium and/or molybdenum oxide, binder and optionally conductive additive or amorphous composition of metal clusters and lithium oxide or fluoride |
| EP3367483A1 (en) * | 2017-02-23 | 2018-08-29 | Alevo International, S.A. | Rechargeable battery cell comprising a separator |
Family Cites Families (11)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| FR1541885A (en) * | 1967-10-25 | 1968-10-11 | American Cyanamid Co | Electrochemical cell |
| GB1258498A (en) * | 1968-06-11 | 1971-12-30 | ||
| US3829330A (en) * | 1969-08-27 | 1974-08-13 | Mallory & Co Inc P R | High rate li/moo3 organic electrolyte cell |
| DE2140146C3 (en) * | 1971-08-11 | 1975-11-06 | Kuehnl, H., Prof. Dr., 3000 Hannover | Galvanic element which can be used as a storage battery and has a negative electrode made of an alkali metal or aluminum and an electrolyte containing SO deep 2 |
| JPS4934086A (en) * | 1972-07-30 | 1974-03-29 | ||
| US3897264A (en) * | 1972-11-13 | 1975-07-29 | Gte Laboratories Inc | Electrochemical cells with inorganic oxyhalide or thiohalide solvent |
| JPS5125230A (en) * | 1974-08-26 | 1976-03-01 | Nissan Motor | |
| US4020240A (en) * | 1975-09-03 | 1977-04-26 | P. R. Mallory & Co., Inc. | Electrochemical cell with clovoborate salt in electrolyte and method of operation and composition of matter |
| US4177329A (en) * | 1978-11-02 | 1979-12-04 | P. R. Mallory & Co. Inc. | Electrolyte salts for non aqueous electrochemical cells |
| US4316777A (en) * | 1979-10-01 | 1982-02-23 | Duracell International Inc. | Rechargeable nonaqueous silver alloy anode cell |
| US4246327A (en) * | 1979-10-01 | 1981-01-20 | Medtronic, Inc. | High energy-density battery system |
-
1982
- 1982-11-12 IL IL67250A patent/IL67250A/en not_active IP Right Cessation
- 1982-11-15 CA CA000415569A patent/CA1188360A/en not_active Expired
- 1982-11-25 BE BE0/209571A patent/BE895143A/en not_active IP Right Cessation
- 1982-11-29 FR FR8219966A patent/FR2518319B1/en not_active Expired
- 1982-12-10 DE DE19823245859 patent/DE3245859A1/en active Granted
- 1982-12-10 JP JP57216769A patent/JPS58117660A/en active Pending
- 1982-12-14 GB GB08235610A patent/GB2113457B/en not_active Expired
Also Published As
| Publication number | Publication date |
|---|---|
| DE3245859C2 (en) | 1991-08-01 |
| FR2518319A1 (en) | 1983-06-17 |
| IL67250A (en) | 1986-01-31 |
| DE3245859A1 (en) | 1983-06-23 |
| IL67250A0 (en) | 1983-03-31 |
| GB2113457B (en) | 1985-08-07 |
| FR2518319B1 (en) | 1986-11-14 |
| GB2113457A (en) | 1983-08-03 |
| JPS58117660A (en) | 1983-07-13 |
| BE895143A (en) | 1983-03-16 |
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