CA1173496A - Nonaqueous cell having a mno.sub.2/poly-carbon fluoride cathode - Google Patents

Nonaqueous cell having a mno.sub.2/poly-carbon fluoride cathode

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Publication number
CA1173496A
CA1173496A CA000385080A CA385080A CA1173496A CA 1173496 A CA1173496 A CA 1173496A CA 000385080 A CA000385080 A CA 000385080A CA 385080 A CA385080 A CA 385080A CA 1173496 A CA1173496 A CA 1173496A
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Prior art keywords
manganese dioxide
poly
cell
cathode
carbon fluoride
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CA000385080A
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French (fr)
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Violeta Z. Leger
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Union Carbide Corp
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Union Carbide Corp
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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
    • H01M4/36—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
    • H01M4/583—Carbonaceous material, e.g. graphite-intercalation compounds or CFx
    • 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
    • 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
    • H01M4/48—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides
    • H01M4/50—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese
    • H01M4/502—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese for non-aqueous 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
    • H01M4/583—Carbonaceous material, e.g. graphite-intercalation compounds or CFx
    • H01M4/5835—Comprising fluorine or fluoride salts
    • 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
    • H01M6/14—Cells with non-aqueous electrolyte
    • H01M6/16—Cells with non-aqueous electrolyte with organic electrolyte
    • 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

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  • Chemical & Material Sciences (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • General Chemical & Material Sciences (AREA)
  • Inorganic Chemistry (AREA)
  • Engineering & Computer Science (AREA)
  • Manufacturing & Machinery (AREA)
  • Battery Electrode And Active Subsutance (AREA)
  • Primary Cells (AREA)

Abstract

12854 NONAQUEOUS CELL HAVING A MnO2/POLY-CARBON FLUORIDE CATHODE ABSTRACT OF THE INVENTION A nonaqueous cell employing an anode such as lithium, a liquid organic electrolyte and a cathode comprising manganese dioxide and a poly-carbon fluoride such as (C2F)n or (CFX)n in which x is greater than 0 up to about 1.1. S P E C I F I C A T I O N 1.

Description

~ 1 73'19~ D 12854-C

Field of the Invention The invention relates to a nonaqueous cell utilizing an active metal anode, a liquid organic electrolyte and a cathode compri~ing manganese dioxide and a poly-carbon fluoride wherein said manganese dioxide contains less than 1 weight per cent water based on the weight of the manganese dioxide and said poly-carbon fluoride has the general formula (CyFX)n wherein y is 1 or 2 and x is greater than 0 up to about 1.1 Background of the Invention The development of high energy battery systems requires the compatability of an electrolyte possessing desirable electrochemical properties with highly reactive anode materials, such as lithium, sodium, and the like, and the efficient use of high energy density cathode materials, such as manganese dioxide. The use of aqueous electrolytes is precluded in these systems since the anode materials are sufficiently active to react with water chemically. It has, therefore, been necessary, in order to realize the high energy density obtainable through use of these highly reactive anodes and high energy density cathodes, to turn to the investigation of nonaqueous electrolyte systems and more particularly to nonaqueous organic electrolyte systems.
The term "nonaqueous organic electrolyte" in the prior art refers to an electrolyte which is composed of a solute, for example, a salt or complex salt of Group I-A, Group II-A or Group III-A elements of the
- 2 - .

~ ~73~9~
D-1285~-C

Periodic Table, dissolved in an appropriate nonaqueous organic solvent. Conventional solvents include propylene carbonate, ethylene carbonate or ~-butyrolactone. The term "Periodic Table" as used herein refers to the Periodic Table of the Elements as set forth on the insi~e back cover of the Handbook of Chemistry and Physics, 48th Edition, the Chemical Rubber Co., Cleveland, Ohio, 1967-1568.

A multitude of solutes is known and recommended for use but the selection of a suitable solvent has been particularly troublesome since many of those solvents which are used to prepare electrolytes sufficiently conductive to permit effective ion migration through the solution are reactive with the highly active anodes mentioned above. Most investigators in this area, in search of suitable solvents, have concentrated on aliphatic and arGmatic nitrogen- and oxygen-containing compounds with some attention given to organic sulfur-, phosphorus- and arsenic-containing compounds. The results of this search have no~ been entirely satisfactory since many of the solvents investigated still could not be used effectively with high energy density cathode materials, such as manganese dioxlde (MnO2), and were sufficiently corrosive to lithium anodes to prevent efficient performance over any length of time.

Although manganese dioxide has been mentioned as a possible cathode for cell applications, manganese dioxide inherently contains an unacceptable amount of water, both of the adsorbed and bound types, which is ~ :~73'l9~ D_l2854-C

sufficient to cause anode (lithium) corrosion along with its associated hydrogen evolution. This type of corrosion that causes gas evolution is a serious problem in sealed cells, particularly in miniature type button cells. In order to maintain overall battery-powered electronic devices as compact as possible, the electronic devices are usually designed with cavities to accommodate the miniature cells as their power source.
The cavities are usually made so that a cell can be snugly positioned therein thus making electronic contact with appropriate terminals within the device. A major potential problem in the use of cell-powered devices of this nature is that if the gas evolution causes the cell to bulge then the cell could become wedged within the cavity. This could result in damage to the device.
Also, if electrolyte leaks from the cell it could cause damage to the device. Thus it is important that the physical dimensions of the cell's housing remain constant during discharge and that the cell will not leak any electrolyte into the device being powered.
U.S. Patent 4,133,856 discloses a process for producing an MnO2 electrode (cathode) for nonaqueous cells whereby the MnO2 is initially heated within a range of 350C to 430C so as to substantially remove both the adsorbed and bound water and then, after beiny formed into an electrode with a conductive agent and binder, it is further heated in a range of 200C to 350C prior to its assembly into a cell. British Patent 1,199,42~ also discloses the heat treatment ot MnO~ in air at 250C to 450C to substantially remove its water component.

~. t~3'l9~
D-12~5~-C

Belgium Patent No. 883,98S discloses a nonaqueous cell employing among other components a
3-methyl-2-oxazolidone-based electrolyte and a manganese dioxide-containing cathode wherein the water content is less than 1 weight per cent based on the weight of the manganese dioxide.
Fluorinated carbon cathodes are disclosed in U.S. Patents 3,536,532 and 3,700,502 as having the formula (CFx)n wherein x varies from 0.5 to about 1Ø The cathodes are stated as being extremely stable and resistive to chemicals over the range of x from 0 to about 1. U.S. Patent 4,139,474 disclosed (C2F)n material.
It is an object of the present invention to provide a nonaqueous cell employing an MnO2/(CyFx)n cathode for nonaqueous cell systems.
It is another object of the present invention to provide an MnO2/(CyFx)n cathode for use with lithium anodes and various liquid organic electrolytes such as 3-methyl-2-oxazolidone in combination with at least one cosolvent and a solute.
It is another object of the present invention to provide a nonaqueous cell with an MnO2 cathode having a layer of (CyFX)n-Summary of the Invention The invention provides a novel high energydensity nonaqueous cell comprising an anode~ an electrolyte and a cathode, said cathode comprising manganese dioxide have a water content of less than 1 weight per cent based on the weight of the manganese -- 5 ~

3 '1 ~ 6 dioxide; the improvement wherein a poly-carbon fluoride is added to the manganese dioxide cat:hode and has the formula (CyFX)n wherein y is 1 or 2, x is greater than 0 up to about 1.1 and n refers tothe number of monomer units which can vary widely.
The poly-carbon fluoride is composed of carbon and fluorine in which the carbon includes graphitic and non-graphitic forms of carbon, such as coke, charcoal or active carbon. Preferably, the poly-carbon fluoride would be those having a y of 1 and an x between about 0.8 and 1.0, and poly-dicarbon monofluoride (C2Fn).
The amount of the poly-carbon fluoride to be used with the manganese dioxide could be 50~ by weight or less based on the weight of the manganese dioxide and poly-carbon fluoride. Preferably, ~he poly-carbon fluoride should be between about 10% by weight and about 30% by weight of the weight o~ the manganese dioxide and poly-carbon fluoride. This range o~ the poly-carbon fluoride would extend the ampere-hour capacity of the manganese dioxide io render the cells more acceptable for a wider range of applications. It has been observed that with the addition of the poly-carbon fluoride to a manganese dioxide-containing cathode, the voltage output remains substantially at the manganese dioxide level which is above the voltage output for a poly-carbon fluoride cathode such as CFX where x is about 0.85 to 1. It has also been observed that the addition of the poly-carbon fluoride will improve the pulse voltage maintenance at high drain rates beyond that obtainable with a manganese dioxide cathode.

~ :l73~9~i The poly-carbon fluoride can be mixed with the manganese dioxide or could be added as a discrete layer disposed preferably aajacent the container interface of the cell.
The water inherently contained in both electrolytic and chemical types o~ manganese dioxide can be substantially removed by various treatments. For example, the manganese dioxide can be heated in air or an inert atmosphere at a temperature up to 380C for about 8 hours or at a lower temperature for a longer period of time. Care should be taken to avoid heating the manganese dioxide above its decomposition temperature which is about 400C in air. In oxygen atmospheres, nigher temperatures may be employed. In accordance with this invention the manganese dioxide should be heated for a sufficient period of time to insure that the water content is reduced below about 1 weight per cent, preferably below about 0.5 and most preferably below about 0.2 weight per cent based on the weight of the manganese dioxide. An amount of water above about 1 weight per cent would react with the highly active metal anode, such as lithium, arld cause it to corrode thereby resulting in hydrogen evolution. As stated above, this could result in physical distortion of the cell and/or electrolyte leakage from the cell during storage or discharge.
To effectively remove the undesirable water from MnO2, or MnO2 ~lixed with a conductive agent and a sultable binder, to the level necessary to prac-tice this invention, it is believed necessary that both the adsorbed and bound water be substantially removed.

_ D-1285~-C
~ ~3~9~
After the water removal treatment has been completed, it is essential that the manganese dioxide be shielded to prevent adsorption of water from the atmosphere. This could ~e accomplished by handling the treated manganese dioxide in a dry box or the like. Alternatively, the treated manganese dioxide or the manganese dioxide combined with a conductive agent and a suitable binder could be heat treated to remove wal:er that could have been adsorbed from the atmosphere.
Preferably, the manganese dioxide should be heat treated to remove its water content to below about 1 weight per cent and then it can be mixed with a conductive agent such as graphite, carbon or the like and a binder such as Te10n (trademark for polytetra-fluoroethylene), ethylene acrylic acid polymer or the like to produce a solid cathode electrode. I desired, a small amount of the electrolyte can be incorporated into the manganese dioxide mix.
An added possible benefit in the removal of substantially all the water from manganese dioxide is that if small amounts of water are present in the cell's electrolyte, then the manganese dioxide will absorb the main portion of the water rom the electrolyte and thereby prevent or substantially delay the reaction of the water with the anode suchn as lithium. In this situation, the manganese dioxide will act as an extracting agent for the water impurities in the organic solvents.
Highly active anodes for use in nonaqueous systems according to this invention would be consumable metals and include aluminum, the alkali metals, alkaline ~ ~73'~9~;
D-1285~-C

earth metals and alloys of alkali metals or alkaline earth metals with each other and othelr metals.
The term "alloys" as used herein and in the appended claims is intended to include mixtures, solid solutions, such as lithlum-magnesium, and the intermetallic compounds, such as lithium, monoaluminide. The preferred anode materials are lithium, sodium, potassium, calcium, magnesium and alloys thereof. Of the preferred anode materials, lithium would be the best because, in addition to being ductile metal that can be easily assembled in a cell, it possesses the highest energy-to-weight ratio of the group of suitable anodes.
In nonaqueous cells, useful organic solvents employed alone or mixed with one or more other solvents for use in preparing electrolytes employed in the cell of this invention include the following classes of compounds:

Alkylene nitriles: e.g., crotonitrile (liquid range -51.1C to 120C) Trialkyl borate: e.g., trimethyl borate, tCH30)3B
(liquid range -29.3C to 67C) Tetraalkyl silicates: e.g.., tetramethyl silicate, (CH30)4Si (boiling point 121C) Nitroalkanes: e.g., nitromethane, CH3N02 (liquid range -17C to 100.8C) Alkylnitriles: e.g. acetonitrile, CH3CN
(liquid range -45C to 81.6C) DiakylamideS: e.g., dimethylformamide, HCON(CH3)2 (liquid range -60.48C to 149C) g ~ :~73~96 Lactams: e.g., N-methylpyrrolidone, C~l2-CH2-C~2-CO-W-CH3 (liquid range -16C to 202C) ~onocarboxylic acid esters: e.g., ethyl acetate (liquid range -83.6 to 77.06C) Orthoesters: e.g., trimethylorthoformate, HC(OCH3)3 (boiling point 103C) Lactones: e.g.,~ -(gamma)butyrolactone, CH2-CH2-CH2-O-CO
(liquid range -42 to 206C) Dialkyl carbonates: e.g., dimethyl carbonate, OC(OCH3)2 (liquid range 2 to 90C) Alkylene carbonates: eOg., propylene carbonate, CH(CH3)CH2-O-CO-O (liquid range -48 to 242C) Monoethers: e.g., diethyl ether (liquid range -116 to 34.5C) Polyethers: e.g., 1,1- and 1,2-dimethoxyethane (liquid ranges -113.2 to 64.5DC and -58 to 83C, respectively) Cyclic ethers: e.g., tetrahydrofuran (liquid range -65 to 67C); 1,3-dioxolane (liquid range -95 to 78C) Nitroaromati^s: e.g., nitrobenzene (liquid range 5.7 to 210.8C~
Aromatic carboxylic acid halides: e.g., benzoyl chloride (liquid ranqe 0 to 197C); benzoyl bromide (liquid range -24 to 218C) Aromatic sulfonic acid halides: e.g., benzene sulfonyl chloride (liquid range 14.5 to 251C) Aromatic phosphonic acid dihalides: e.g., benzene Phosphonyl dichloride (boiling point 258C) 3 ~ 6 Aromatic thiophosphonic acid dihalicles: e.g., benzene thiophosphonyl dichloride (boiling point 124C at 5mm) Cyclic sulfones: e.g., sulfolane, CH2-cH2-cH2-cH2-so2 (meltiny point 22 C);
3-methylsulfolane (melting point: -1C) Alkyl sul~onic acid halides: e.g., methanesul~onyl chloride (boiling point 161C) Alkyl carboxylic acid halides: e.g., acetyl chloride (liquid range -112 to 50.9C); acetyl bromide (liquid range -96 to 76C); propionyl chloride (liquid range -94 to 80C) Saturated heterocyclics; e.g., tetrahydrothiophene (liquid range -96 to 121C); 3-methyl-2-oxa-zolidone (melting point 15.9C) Dialkyl sulfamic acid halides: e.g., dimethyl sulfamyl chloride (boiling point 80C at 16mm) Alkyl halosulfonates: e.g., ethyl chlorosulfonate (boiling point 151C) Unsaturated hetrocyclic carboxylic acid halides:

e.g., 2-furoyl chloride (liquid range -2 to 173C) Five-membered unsaturated heterocyclics: e.g. 9 3,5-dimethylisoxazole (boiling point 140C);
l-methylpyrrole (boiling point 114C~;
2,4-dimethylthiazole (boiling point 144C); furan (liquid range -85.65 to 31.36C) Esters and/or halides of dibasic carboxylic acids; e.g., ethyl oxalyl cnloride (boiling point 135C) Mixed alkyl sul~onic acid halides and carboxylic acid halides, e.g., chlorosulfonyl acetyl chloride (boiling point 98C at lOmm~

3~96 D-1285~ C

Dialkyl sulfoxides: e.g., dimethyl sul~oxicle ~liquid range ~18.4 to 189C) Dialkyl sulfates: e.g., dimethylsulfate (liquid range -31.75 to 188.5C) Dialkyl sulfites: e.g., dimethylsul~ite (boiling point 126C) Alkylene sulfites: e.g., ethylene glycol sulfite (liquid range -11 to 173C) Halogenated alkanes: e.g., methylene chloride (liquid range -95 to 40C); 1,3-dichloropropane (liquid range -9~.5 to 12004C) Of the above, the preferred solvents are sulfolane; crotonitrile; nitrobenzene; tetrahydrofuran;
1,3-dioxolane; 3-methyl-2-oxazolidone; propylene or ethylene carbonate; -butyrolactone; ethylene glycol sulfite, dimethylsulfite; dimethyl sulfoxide; and 1,1-and 1,2-dimethoxyethane. Of the preferred solvents, the best are 3-methyl-2-o~azolidone, propylene or ethylene carbonate, l,2-dimethoxyethane, and 1,3-dioxolane because they ap~ear more chemically inert to battery components and have wide liquid ranges, and especially because they permit highly efficient utilization of the cathode materials.
The ionizing solute for use in the invention may be a simple or double salt or mixtures thereof, e.g., LiCF3S03 or LiC104, which will produce an ionically conductive solution when dissolved in one or more solvents. Useful solutes include complexes of inorganic or organic Lewis acids and inorganic ionizable salts. The only requirements for utility are that the salts, whether simple or complex, be compatible with the ~ ~3~9~
D-12854~C

solvent or solvents being employed and that they yield a solution which is sufficiently ionically conductive.
According to the Lewis or electronic concept ot acids and bases, many substances which contain no active hydrogen can act as acids or acceptors of electron doublets. The basic concept is set forth in the chemical literature (Journal of the Franklin Institute, Vol. 226, July/December 1938, pages 293-313 by G. N. Lewis).
A suggested reaction mechanism for the manner in which these complexes function in a solvent is described in detail in U.S. Patent No. 3,542,602 wherein it is su~gested that the complex or double salt ~ormed between the Lewis acid and the ionizable salt yields an entity which is more stable than either of the components alone~
Typical Lewis acids suitable ~or use in the present invention include aluminum flouride, aluminum bromide, aluminum chloride, antimony pentachloride, zirconium tetrachloride, phosphorus pentachloride, boron fluoride, boron chloride and boron bromide;
Ionizable salts useEul in combination with the Lewis acids include lithium fluoride, lithium chloride, lithium bromide, lithium sulEide, sodium fluoride, sodium chloride, sodium bromide, potassium fluoride, potassium chloride and potassium bromide.
A separator for use in this invention has to be chemically inert and insoluble in the cell system and have a porosity so as to permit the liquid electrolyte to permeate through and contact the anode of the cell, ~ :~73'~9~ D-l2854-c thus establishing an ion trans~er path between the anode and cathode.
The container housing for the cell can be made of stainless steel or some other conductive material that will not corrode or otherwise deteriorate when in contact with the cell materials.
The insulating member disposed between the cover and the can has to be stable in the presence of the cell components and can be selected from such materials as polytetrafluoroethylene (e.g., "Te10n"), fluorinated ethylene-propylene (e.g., FEP), ethylene copolymer with FEP, chlorotrifluoroethylene, perfluoroalkoxy-polymer (e.g., PFA), tetrafluoroethylene, (TFE), polyvinyl polyethylene, polypropylene, polystyrene, nylon, etc.
Figure 1 is a graph of the output voltage and pulse voltage versus time for a nonaqueous cell employing a manganese dioxide-x cathode.
Figure 2 and 3 are graphs of the output voltage and pulse voltage versus time for nonaqueous cells emp~oying a manganese dioxide-CFx cathode in accordance with this invention.

EXA~PLE 1 An experimental cell was constructed using a lithium anode (0.114 gram), a 1.5 cc electrolyte of lM
LiCF3S03 in 40 percent dioxolane, 30 percent dimethoxyethane and 30 percent 3-methyl-2-oxazolidone containing a trace of dimethylisoxaole and 0.3566 gram of a cathode containing 86~ by weight MnO2, 8.5~ dry weight graphite, 2~ by weight acetylene black and 3.5 3 '1 9 ~;

polytetrafluoroethylene. The cell was discharged across a 15-K ohm load and the voltage observed with time is shown plotted in Figure 1. At intervals the cell was discharged across a l-K ohm load for two seconds and the pulse voltages observed are shown on the gra~h of Fig~re 1 as cross l+) marks.

EXAMPLE II
An experimental cell was constructed as in Example I except that the cathode was 0.358 gram of 77.4% by weight MnO2 8~ by weight CFX wherein x was 0.85 to 1, 9.1% acetylene black, and 5.5%
polytetrafluoroethylene. The cell was discharged across a 15-K ohm load and the voltage observed with time is shown plotted in Figure 2. At intervals the cell was disc~arged across a 300 ohm load for two seconds and the pulse voltages observed are shown on the graph of Figure 2 as cross (+) marks.

EXA~P~E III
An experimental cell was constructed as in Example I exce~t that the cathode was 0.362 gram of 69 by weight MnO2, 16% by weight CF~ wherein x was 0.85 to 1, 9% by weight acetylene black an 6~ by weight polytetra~luoroethylene. The cell was discharged across a 15-K ohm load and the voltage observed with time is shown plotted in Figure 2. At intervals the cell was discharged across a l-K ohm load for two seconds and the pulse voltages observed are shown on the graph of Fig~re 3 as cross (+) marks.
As evident from the data obtained from the above examples, the cells of this invention (Examples II

:~ 173'~9~

and III) had a better amphere-hour capacity and pulse voltage maintenance at high drain rates than the cell employing an all-MnO2 cathode ~Example I).
It should be understood that the foregoing disclosure relates to preferred embodimen~s of the invention and it is intended to cover all changes and modifications of the invention which do not depart from the spirit and scope of the appended claims.

Claims (9)

WHAT IS CLAIMED IS:
1. A nonaqueous cell comprising an anode, an electrolyte and a cathode, said cathode comprising manganese dioxide having a water content of less than 1 weight percent based on the weight of the manganese dioxide; the improvement wherein a poly-carbon fluoride is added to the manganese dioxide cathode and has the formula (CyFx)n wherein y is 1 or 2 and x is greater than 0 up to about 1.1.
2. The nonaqueous cell of claim 1 wherein y is 1 and x is between about 0.8 and 1Ø
3. The nonaqueous cell of claim 1 wherein the poly-carbon fluoride is (C2F)n.
4. The nonaqueous cell of claim 1, 2 or 3 wherein the poly-carbon fluoride is present in an amount of 50% by weight or less based on the weight of the manganese dioxide.
5. The nonaqueous cell of claim 1, 2 or 3 wherein the poly-carbon fluoride is present in an amount of between about 10% by weight and 30% by weight based on the weight of the manganese dioxide.
6. The nonaqueous cell of claim 1, 2 or 3 wherein poly-carbon fluoride is mixed with the manganese dioxide.
7. The nonaqueous cell of claim 1, 2 or 3 wherein the poly-carbon fluoride is a layer disposed on the manganese dioxide.
8. The nonaqueous cell of claim 1, 2 or 3 wherein the cathode contains a binder and a conductive agent.
9. The nonaqueous cell of claim 1, 2 or 3 wherein said anode is selected from the group consisting of lithium, potassium, sodium, calcium, magnesium, aluminum and alloys thereof.
CA000385080A 1980-09-29 1981-09-02 Nonaqueous cell having a mno.sub.2/poly-carbon fluoride cathode Expired CA1173496A (en)

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
US191,997 1980-09-29
US06/191,997 US4327166A (en) 1980-09-29 1980-09-29 Nonaqueous cell having a MNO2 /poly-carbon fluoride cathode

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CA1173496A true CA1173496A (en) 1984-08-28

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JP (1) JPS5788671A (en)
AR (1) AR241733A1 (en)
AU (1) AU548405B2 (en)
BR (1) BR8106143A (en)
CA (1) CA1173496A (en)
DE (1) DE3161842D1 (en)
IN (1) IN158482B (en)

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AR241733A1 (en) 1992-11-30
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AU7570481A (en) 1982-04-08
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DE3161842D1 (en) 1984-02-09
EP0049082B1 (en) 1984-01-04

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