CA1058284A - Metallic sulfide additives for positive electrode material within a secondary electrochemical cell - Google Patents
Metallic sulfide additives for positive electrode material within a secondary electrochemical cellInfo
- Publication number
- CA1058284A CA1058284A CA250,914A CA250914A CA1058284A CA 1058284 A CA1058284 A CA 1058284A CA 250914 A CA250914 A CA 250914A CA 1058284 A CA1058284 A CA 1058284A
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- CA
- Canada
- Prior art keywords
- electrode
- positive
- active material
- cell
- positive electrode
- Prior art date
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Classifications
-
- 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
- H01M4/581—Chalcogenides or intercalation compounds thereof
-
- 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
- H01M10/39—Accumulators not provided for in groups H01M10/05-H01M10/34 working at high temperature
- H01M10/399—Cells with molten salts
-
- 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
Abstract
An improved active material for use within the positive electrode of a secondary electrochemical cell includes a mixture of iron disulfide and a sulfide of a polyvalent metal. Various metal sulfides, particularly sulfides of cobalt, nickel, copper, cerium and manganese, are added in minor weight proportion in respect to iron disulfide for improving the electrode performance and reducing current collector requirements.
Description
5~2~
METALLIC SULFIDE ADDITIVES FOR POSITIVE ELECTRODE
MATERIAL WIT~TI~ A SECO-L~DARY ELECT~OC~E~ICAL ~L
BACKGROUND OF THE INVENTION
This invention relates to high-temperature, secondary electrochemical cells and batteries of such cells that can be employed as power sources for electrical automobiles, hybrid electric vehicles or for the storage of energy generated during intervals of off-peak power consumption.
It is particularly applicable to electrochemical cells that employ metal sulfides as positive electrode reactan~s and alkali metals as negative electrode reactants.
A substantial amount of work has been done on the development of these types of electrochemical cells and their electrodes. The various type cells showing promise have employed lithium, lithium-aluminum alloy or sodium as the reactant or active material within the negative electrode. In the positive electrode, the chalcogens, ~3S~ZE~
particularly sulfur and sulfur compounds, have been used.
Electrolytes of molten salt, generally containing the ions of the negative reactant, provide ionic conduction between the electrodes. Examples of these secondary, high-temperature cells are disclosed in U. S. patent Nos. 3,887,396 to Walsh et al. entitled "Modular Electrochemical Cell", June 3, 1975;
3,884,715 to Cairns et al. entitled "Secondary Electro-chemical Power Producing Cells Having Mixed Cathode Com-positions, May 20, 1975; 3~827,910 to Cairns et al.
entitled "Homogeneous Cathode Mixtures for Secondary Electrochemical Power-Producing Cells", August 6, 1974;
3,716,409 to Cairns et al., entitled "Cathodes for Secondary Electrochemical Power-Producing Cells", February 13, 1973; and 3,488,221 to Hiroshi Shimotake et al., January 6, 1970. A number of other patents relating to these type cells include U. S. patent No. 3,907,589, September 23, 1975, to Gay and Martino, entitled "Cathode for a Secondary Electrochemical Cell"; and U. S. patent No.
3,947,291, March 30, 1976, to Yao and Walsh, entitled "Electrochemical Cell Assembled in Discharged State".
Each of these patents are assigned to the assignee of -the present application.
The iron sulfides FeS2 and FeS have been found to be particularly attractive sulfur compounds for use as positive electrode reactants. The materials are readily available and are much more easily contained within the cell than elemental sulfur. Although FES2 has a lower equivalent ~1^
~.~3S~328~L
weight and generally performs better within the positive electrodes than FeS, it reacts with and degrades iron com-ponents within the cell to form FeS. Consequently, inert materials such as molybdenum, tungsten or carbon are required for use in current collectors and electrical ter-minals in contact with FeS2 cathode compositions.
Un~ortunately, these materials are difficult to weld and otherwise fabricate into useful structures. Molybdenum in particular has been extensively used as a current collector with FeS2 positive electrodes. This current collector material contributes substantially to the weight and cost of the cell.
Various other problems have been encountered in the development of iron disulfide positive electrodes. A
substantial volume increase occurs as this active positive electrode material reacts with lithium ions within the electrolyte to form lithium sulfide reaction product. The expansion may rupture or deform the electrode contalnment to reduce cell performance. In addition, various inter-mediate phases are formed within the positive electrode,for instance solid phases of Li2FeS2, Li4Fe2S5, etc.
Certain of these phases may inter~ere with the ef~icient utilization of the electrode active materials.
SUMMARY OF THE INVENTION
Therefore, in view of these problems associated wlth the development of iron disul~ide as positive-electrode active material, it is an ob~ect of the present invention to provide an improved composition for use as active ~s~
material within a positive electrode of a secondary electro-chemical cell.
It is a further object to provide improved positive-electrode material that can be employed with a reduced amount of inert metal current collector.
It is also an object to provide a positive-electrode active material including iron disulfide that undergoes reduced expansion on discharge.
It is also an object to provide a positive electrode active material with iron disulfide that exhibits improved utilization of the active material.
In accordance with the present invention, a secondary electrochemical cell is presented that includes a negative electrode with alkali metal as the active material, a positive electrode with an improved active material and a molten salt electrolyte for providing ionic conduction between the electrodes. The improved active material within the positive electrode comprises iron disulfide in a major pro-portion by weight and a sulfide of cobalt in an amount suf-ficient to provide a cobalt to iron atom fraction inexcess of about 0.1.
BRIEF DESCRIPTION OF THE DRAWINGS
The present invention is illustrated in the accom-panying drawings wherein Fig. 1 is a cross-sectional view of a secondary electrochemical cell.
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Fig. 2 is a graph of resiskivity vs atom ~rackion (x) Co in el-xCxS2' Figs. 3A and 3B are graphs of cell voltage vs percent theoretical capacity for several electrochemical cells des-cribed in Example IV. In Fig. 3A the positive-electrode active materials are, in curve A: FeS2, curve B: FeS2-CoS2, curve C: FeS2-~iS and curve D: FeS2-Cu2S. In Fig. 3B the active materials are in curve A: ~eS2, curve E; FeS2-MnS
and curve F: FeS2-Ce2S3.
Fig. 4 is a graph of percent volume increase vs percent theoretical capacity for the positive electrodes of Example V.
DETAILED DESCRIPTION OF T~E PREFERRED EMBODIMENT
Referring now to Fig. 1, a secondary electrochemical cell is illustrated that has been used to demonstrate the present invention. It will be clear that various other cell configurations including many of those illustrated in the patents and applications cited above can also employ the improved positlve-electrode material of the present invention. The cell is shown with an outer housing 11 of stainless steel or other inert material containing kwo negative electrodes 13 and 15 and a centrally disposed positive electrode 17. The electrodes are separated by an electrically insulated mesh, paper or fabric 19, for instance of boron nitride, that is shown enveloping the positive electrode 17. Most o~ the volume of the cell housing 11 not occupied by the electrodes and particularly that volume intermediate the positive and negative elec-~5~8~
trodes is filled with a molten electrolyte for ionic con-duction between the electrodes. For clarity in the drawingr the molten electrolyte is not shown. The electrolyte used in the cell can be selected from known eutectic salt com-positions that are molten at the cell operating temperatures.
Electrolytes such as eutectic compositions of LiCl-KCl or LiCl-LiF-KBr and LiF-LiCl-LiI salts have been found to be suitable for this purpose~ Various other suitable electro-lytic salts can be selected from those listed in U. S.
patent 3,288,221, cited above.
An electrical conductor 21 passes through the housing wall and an opening within the upper negative electrode into electrical contact with the central positive electrode 17.
The conductor is supported and insulated from the cell housing by suitable electrical feedthrough structure 23.
Electrical contact is made to the negative electrodes through the cell housing 11 through conventional elec-trical connections (not shown).
Negative electrodes 13 and 15 can be any one of a number of types such as illustrated in the patents cited in the Background of the Invention. These negative elec-trodes can contain as active material a molten alkali metal such as lithium metal or sodium metal. Also, a solid alloy of lithium-aluminum, lithium-magnesium and other binary and ternary lithium alloys can serve as the ac-tive material.
A molten, negative-electrode, active material will be contained within a porous substrate of, for instance, stain-less steel or nickel. Solid alloy ~5~2~3~
material, for instance lithium-aluminum alloy, can be formed by electrodepositing lithium onto a porous aluminum substrate. In addition, particulate solid alloy material can be distributed throughout a porous metallic substrate in order to provide a negative electrode. Screens or rnesh 25 of an inert material such as stainless steel are illus-trated at the negative electrode surfaces facing the positive electrode for structural support and retention of active material~
The structure of positive electrode 17 is not critical.
It is illustrated in a form generally representative of the type employed in the cells given in the examples. As shown, it is enveloped by the porous~ electrically insu-lative separator 19 of, for instance, boron nitride paper, cloth or fabric. The positive-electrode structure in general will include the positive-electrode active material 27, current collector material 29 and electrolyte.
As illustrated, several layers of current collector 29 are electrically connected to conductor 21 at their center and are embedded within a mixture of the active material and electrolyte. The current collector can be sheets, mesh, screens, foam layers or other forms of electrical conductors. In some embodiments, particulate current collector material can be used in combination with or in place of the illustrated layers. The current collectors are of an electrically conductive materlal that will not extensively corrode in contact with the electrolyte and electrode materials at the electrode potential, for ~C~S~3Z8~
instance of molybdenum, molybdenum alloys, tungsten or carbon.
The positive-electrode active material 27 can also be provlded in a number of structural forms, for example, as solid particulate material or as a solid structure with porosity. In each instance, electrolyte is mixed or inter-spersed with or through the active material to provide ionic conduction to the current collector. In other struc-tures, a porous current collector such as a felt or foam can be filled with the active material and electrolyte.
The active positive electrode material is a com-position including a maJor weight proportion of iron disulfide and a minor proportlon by weight of one or more other polyvalent metal sulfides. Each of the polyvalent metals, like iron, is capable of combining with sulfur in more than one state of oxidation. For example, sulfides of cobalt include CoS, CoS2, Co3S4 and Co2S3 Often a polyvalent sulfide is conveniently provided and can be employed as a mixture of several stoichiometric compounds, e.g. mixtures of CoS and Co3S4.
The composition of lron disulfide and the polyvalent sulfide can be prepared initially by a number of methods.
In a typical manner employed for the cells described in the examples below, particulate mixtures of iron disulfide and the polyvalent metal sulfide were prepared and subsequently flooded with molten electrolyte.within the cell. On cycling o~ the cell at the elevated operating temperature of 400 to 450 C., other ternary and perhaps more complicated ~5~Z84 systems of iron, polyvalent metal, sulfur and possibly other constikuents are indicated. It is therefore contem-plaked that the positive-electrode active material can be prepared initially in various forms of ternary systems including a sulfide compound or berthollide with polyvalent metal substituted for a portion of the iron, a solid solu-tion of the polyvalent metal sulfide and the iron dlsulfide~
a eutectic composition of the constituents or various single and polyphase systems including the constituents.
A number of polyvalent metal sulfide additives have been found which can be combined with iron disulfide to improve the performance of the positive electrode. Addi-tives such as sulfides of cobalt, cerium and nickel are highly conductive materials that reduce the resistance of the electrode. Some of these, such as cobalt and nickel sulfides as well as other sulfides that have higher resis-tivities, may react durlng cycllng of the cell to provide an electrically conductive metal, e.g. Co, Ni~ Cu. These polyvalent metal sulfides exhibit thermodynamic equili-brium potentials within the cell operating range, e.g.
between 1.3 to 2.3 volts, IR free, versus lithium metal, in the formation of lithium sulfide and the electrically conductive metal. Other metal sulfides, such as those of manganese and cerium, that do not exhibit similar equili-brium potentials can possibly improve cell performance in combination with other electrode materials. A number of the polyvalent metal sulfides may interact with other materials within the posikive electrode at operating _ g _ 5~32~
temperature and potential to form electrically conductive phases or merely phases that exhibit reduced diffusional resistance within the positive electrode.
The improved active materials with low ohmic resis-tance (as opposed to diffusional resistance) can operate with reduced amounts of expensive current collector material at increased power output. Reduction in diffusional resis-tance leads to improved utilization of the active material.
Table I lists a number of metal sulfide additives that are contemplated for combining with iron disulfide to reduce both ohmic and dif~usion resistance of a positive electrode.
Resistivities are given where available for comparison with the resistivity o~ FeS2 which is 3.88 x 10 2 at 340 C.
TABLE I
Resistivity Additive Ohm-cm at 450C.
TiS2 1.0 x 10 2 Ti S3 ~~
Ti~ -- 4 CoS 2.2 x 10 Co S
v2~S4 102 Cr ~ 0.1 Mn~ 3 10 (single crystal of ~C-MnS~
MnS2 CdS 10 -6 ZnS 2 x 10 4 CceesS3 1.4 x 1~ 4 Cu S 3 x 10 (400C.) sb2s 2.7 (5103.) Pb~ 3 6.1 x 10 1 (340 C.) MoS~ 2.1 x 10 (102 C.) NiS23 o~2 NiS2 1.6 x 10 ~)S8Z~
Ni3S4 --Ni3S2 One manner of determining the amount of metal sulfide addltive to be included is through the reduction in resis-tivity of the mixture of the positive-electrode active material. Literature values for the Fel Co S2 system indicate that cobalt sulfide additions up to about 0.10 atom fraction produce a substantial reduction in resistivity, while a somewhat more gradual reduction is produced by additions beyond 0.10 atom fraction. This relationship is clearly shown in the graph of Fig. 2. For this ternary system o~ Fe-Co-S2, atom and weight ~raction of iron and cobalt are approximately the same.
In order to demonstrate the present development, a number of electrochemical cells have been operated in the laboratory with various positive-electrode, active materials.
These cells are illustrated in the ~ollowing examples.
Reduction in Current Collector EXAMPLE I
Two laboratory electrochemical cells~ each having a single negative electrode and a single positive electrode, were assembled for operation with a particulate mixture of FeS2 and Co2S3 as positive-electrode, active material. One of the cells (FC-l) employed three molybdenum screens brazed to a central molybdenum rod as a positive electrode current collector. An external molybdenum basket maintained at positive potential, but separated from the electrode active material by a zirconia fabric, was used to define the elec-~l~5~
trode geometry.
The second cell (FC-2) used a single molybdenum screen and central molybdenum rod to test the effect of reduced amounts of current collector material. This electrode a~so eliminated the molybdenum basket through use of a stainless steel basket maintained at negative electrode potential.
Other characteristics of the two cells are given below in Table II.
TABLE II
Cell FC-l FC-2 Positiye Electrode FeS2 20.5 g 19.95 g C02S3 2.0 g 2.21 g Area 23.1 cm2 22-.8 cm2 Volume 23 cm2 20.6 cm2 Current Collector 3 Mo screens 1 Mo screens Capacity ~FeS2) 18.3 A-hr 17.8 A-hr Capacity (C02S3) 1.5 A-hr 1.66 A-hr Negative Electrode Material Li-Al Li-Al Capacity 27.2 A-hr 26.71 A-hr Area - 38.3 cm 38.3 cm Operating Temperature 450C. l~50C
Both the cells were operated through nearly identical cycling programs with discharge voltages of about 1.6 to 0.7, capacity densities of 0.7 to 0.2 A-hr/cm and current densities ranging from 20 ma/cm2 to 700 ma/cm2. These measurements showed there was no significant difference ~358Z~14 between the performance of the two cells. The operationof these cells shows that a substantial reduction in the amount of molybdenum current collector can be made with cells employing iron disulfide with a sulfide of cobalt additive as positive-electrode, active material.
Comparative Resistance and Capacity EXAMPLE II
Two electrochemical cells similar in construction to the cell illustrated in Fig. 1 were operated for extended periods of time in excess of 1500 hours and 70 cycles each.
In the first cell (W-5) only FeS2 was employed as the positive electrode active material, while the second cell included a particulate mixture of FeS2 and about 10 weight percent of a sulfide of cobalt having a nominal composition of Co2S3. Analysis indicated the composition was pre-dominantly CoS with small quantities of Co3S4. Additional data regarding the two cells is given below in Table III.
~5~
o ~ ~ CO
o . . . ~;
~1 0 ~ O ~ ~ O O U~ ~ ~1 1 0 0 ~ O
~r~
~ , oc) o V
~ O O ~1 ~ ~1 ~ O L~ l ~1 1 ~1 0 ~ O
H bD
~1 O
m ¢
~d .
a) ~0 a>
C) a~ o s~
C~ s o ,~
¢
~Q ~
o ~ ~ C~ o o ~
S
O :~
a) ~ c) c) ~ ~
O ~ r-l o ~ OH rl c~ ~ h td^ C> S~
c) ^ ~7 ~I c) u~ ~ ta ~ a) c~ C~ q O c) ~ ~, ~ bO ~0 a) ~d ~ ~ ~ ~ a~ ~ h a) ~ ~: ~a) ~ ~: ~ ~ ~ a~ ~d 4~ ~ ~ a) ~ ~ b~ ~ bD
O O ~ c) O O o o ~ c) ~ ~D O ~ c a~ ~ ~d ~ ~1 . ~ ~
O ~ ~ ~ ~ S ~ ~~ ~ ~ ~ rC O ~ ~ ~ ~rl z; ~ ~ 3~ ~ ~ ~ c~
,~ ~ ~ c) ~ o C~ ~ Z L~ O
~5~
As shown in the table, the cells include essentially the same mass of molybdenum current collector material.
Resistance measurements made on the cells in the charged state showed an ohmic resistance of 8 milliohms in cell W-5 and only 5 milliohms in cell W-10. This reduction in ohmic resistance is attributed to the increased conduc-tivity of the positive-electrode active material including the sulfide of cobalt. Table III also shows a substantially lower charge cutoff voltage for cell W-10 than for cell W-5.
The lower charge potential reduces the corrosivity of the electrode environment and may permit use of a less noble current collector material than molybdenum. Notwithstanding the lower charge cutoff along with higher discharge cutoffs, cell W-10 exhibited a capacity of about 115 amp hours at 5 and 7 amperes discharge and 450C. operating temperature throughout a ma~or portion of its life. This corresponds to a utilization of approximately 77 percent. At these same current levels, cell W-5 without the sulfide of cobalt additive produced only 80 to 90 amp hours corresponding to a utilization of about 57 percent. This increase in capacity withi.n a reduced range o~ cutof~ voltages is attributed to the sulfide of cobalt additive within the positive-electrode active material.
EXAMPLE III
A third cell (W-ll~ of a construction substantially the same as that illustrated in ~ig. 1 and described in Example II included a positive-electrode active material of FeS2 - 10 wt. % Co2S3 (nominal composition). However, ~SE~Z84 only 1/3 the number of current collector layers and 1/2the mass of molybdenum material was included in the positive electrode compared to the positive electrodes of cells W-5 and W-10. Resistance measurements made on this cell showed an ohmic resistance in the charged state of 4.5 milliohms. This clearly indicates that through use of the positive-electrode active material of the present inven-tion a substantial reduction in the mass of current collector material can be made without detrimental effects.
Other-Additive Materials EXAMPLE I~
A number of experimental cells were operated, each having one positive and one negative electrode with LiCl-KCl electrolyte between the electrodes. The negative electrodes were of Li-Al alloy electrochemically formed on a porous compact of aluminum wire with a theoretical capacity of about 19 A~hr. The aluminum wire compacts were about 7.6 cm diameter and contained about 25 grams of aluminum. Each of the positive electrodes were about 20 cm square area and an average thickness of about 3/4 cm. Each included particulate active material, electrolyte and one layer of molybdenum mesh as current collector material. The active material was of particle sizes of between 75 and 180 U. S. standard mesh.
The positive-electrode, active material in the first cell was FeS2 alone. In each subsequent cell, ~ metal sulfide additive in an amount of 15 atom % was included with the FeS2. In each cell, the total weight of the positive-elec-trode active material was 14 grams.
~L~S~284~
During the test the cells were operated between 20and 40 cycles for about 300 to 550 hours at di~ferent current levels tlA, 2A or 3A) and two temperature levels (typically 400 C. and 450C.). Various characteristics of each o~ the cells are tabulated below in Table IV.
~s~
c~ h r~
~ ~ ~ o o~ o O ~ o L~ td o~ ~ ~ ~ ~ o ~ ~ ~ ~ o P~
C~
'U
a~
r ~ ~d ¢ ~ ~ ~D O O~ ~ ~ ~ O~ CO O ~
............
~ ~ O O ~ O ~ O ~ O cr~
M ~1 ~ H ~1 H ~ ~I r-l O
. . ::~
.
:
i .
.~ * ~p *
h L~\ ~Lr~ o ~ ~~ oo o C) ~ ~ ~ ~ ~ ~ ~ ~1 ~1 ~1 -~:
~ Q) H td p ~d C~ ~ ~
~ . , . ~ td m o . ~ c~
¢ ~ ~ ~
E~ ~ : ~ ~
~: o . ~ ~:
p~ ~
.' td~
~ ~ ~ ~ o~ o Lr~ ~o ~
'~ N N ~i ~ J ~i~i 0 O r~l ~1 HH H r-lH N r~J ~1 ~ rl ~ rl S
~ ~q ,aP
a) ~
P a ~
~ CO
rl ~ N N ~ V~ S:
N CQ N
~ O rl O ~ ~ u~ o '~ v c~ ~ ~ Z ~ *
D5~Z~3~
The results of these tests for the positive-electrode, active material including FeS2 alone and five of the more promising additive materials are shown in Figs. 3A and 3B.
These figures are discharge curves at 2 amps current and 450 C. showing utilization as a percentage of theoretical capacity versus cell discharge voltage. In Fig. 3A, curve A corresponds to FeS2, curve B to FeS2-CoS2, curve C to FeS2-NiS, curve D to FeS2-Cu2S, and in Fig. 3B curve A
again corresponds to FeS2, curve E to FeS2-MnS, curve F to FeS2-Ce2S3 as the positive-electrode actlve material within the respective cells.
Most of the remaining cells having other positive electrode additive materials exhibited performances not substantially better than that of FeS2 alone. However, the cell including zinc sulfide additlve did provide good improvement in the percent utilization of active material at the lower voltage plateau of 1.2 volts and below.
It is therefore seen from the results presented in Figs. 3A and 3B that the addition of each of the sulfides of five polyvalent metals provides a substantial and unexpected improvement in the utllization of actlve material in a positive electrode including a ma~or proportion of ~eS2 .
Reduced Electrode Swelling EXAMPLE V
Two electrochemical cells, each with Li-Al alloys as negative electrode material and LiCl-KCl electrolyte were operated through their first discharge cycle at ~S82i3~
50 ma/cm at a temperature of ~25C. Measurements ofaxial expansion were made on the positive electrode of each cell during this first cycle of operation. The first cell included particulate FeS2 as the active positive electrode material, while the second cell included FeS2 - 16 wt. %
Co2S3. The results of these tests are shown in Fig. 4 with the cell employing FeS2-Co2S3 as active material exhibiting both a higher utilization of active material as well as about a 15 to 20% reduction in volume expansion.
It will be clear from the above that the present inven-tion provides an electrochemical cell including an lmproved positive electrode active material. The use of this active material provides a number of unexpected benefits not realized by previous cells employing only particulate FeS2.
Among these benefits are improved utilization of the active material, reduced swellin~ of the electrode and reduced electrode resistance which can result in higher power output and a reduction in the required amount of current collector material.
METALLIC SULFIDE ADDITIVES FOR POSITIVE ELECTRODE
MATERIAL WIT~TI~ A SECO-L~DARY ELECT~OC~E~ICAL ~L
BACKGROUND OF THE INVENTION
This invention relates to high-temperature, secondary electrochemical cells and batteries of such cells that can be employed as power sources for electrical automobiles, hybrid electric vehicles or for the storage of energy generated during intervals of off-peak power consumption.
It is particularly applicable to electrochemical cells that employ metal sulfides as positive electrode reactan~s and alkali metals as negative electrode reactants.
A substantial amount of work has been done on the development of these types of electrochemical cells and their electrodes. The various type cells showing promise have employed lithium, lithium-aluminum alloy or sodium as the reactant or active material within the negative electrode. In the positive electrode, the chalcogens, ~3S~ZE~
particularly sulfur and sulfur compounds, have been used.
Electrolytes of molten salt, generally containing the ions of the negative reactant, provide ionic conduction between the electrodes. Examples of these secondary, high-temperature cells are disclosed in U. S. patent Nos. 3,887,396 to Walsh et al. entitled "Modular Electrochemical Cell", June 3, 1975;
3,884,715 to Cairns et al. entitled "Secondary Electro-chemical Power Producing Cells Having Mixed Cathode Com-positions, May 20, 1975; 3~827,910 to Cairns et al.
entitled "Homogeneous Cathode Mixtures for Secondary Electrochemical Power-Producing Cells", August 6, 1974;
3,716,409 to Cairns et al., entitled "Cathodes for Secondary Electrochemical Power-Producing Cells", February 13, 1973; and 3,488,221 to Hiroshi Shimotake et al., January 6, 1970. A number of other patents relating to these type cells include U. S. patent No. 3,907,589, September 23, 1975, to Gay and Martino, entitled "Cathode for a Secondary Electrochemical Cell"; and U. S. patent No.
3,947,291, March 30, 1976, to Yao and Walsh, entitled "Electrochemical Cell Assembled in Discharged State".
Each of these patents are assigned to the assignee of -the present application.
The iron sulfides FeS2 and FeS have been found to be particularly attractive sulfur compounds for use as positive electrode reactants. The materials are readily available and are much more easily contained within the cell than elemental sulfur. Although FES2 has a lower equivalent ~1^
~.~3S~328~L
weight and generally performs better within the positive electrodes than FeS, it reacts with and degrades iron com-ponents within the cell to form FeS. Consequently, inert materials such as molybdenum, tungsten or carbon are required for use in current collectors and electrical ter-minals in contact with FeS2 cathode compositions.
Un~ortunately, these materials are difficult to weld and otherwise fabricate into useful structures. Molybdenum in particular has been extensively used as a current collector with FeS2 positive electrodes. This current collector material contributes substantially to the weight and cost of the cell.
Various other problems have been encountered in the development of iron disulfide positive electrodes. A
substantial volume increase occurs as this active positive electrode material reacts with lithium ions within the electrolyte to form lithium sulfide reaction product. The expansion may rupture or deform the electrode contalnment to reduce cell performance. In addition, various inter-mediate phases are formed within the positive electrode,for instance solid phases of Li2FeS2, Li4Fe2S5, etc.
Certain of these phases may inter~ere with the ef~icient utilization of the electrode active materials.
SUMMARY OF THE INVENTION
Therefore, in view of these problems associated wlth the development of iron disul~ide as positive-electrode active material, it is an ob~ect of the present invention to provide an improved composition for use as active ~s~
material within a positive electrode of a secondary electro-chemical cell.
It is a further object to provide improved positive-electrode material that can be employed with a reduced amount of inert metal current collector.
It is also an object to provide a positive-electrode active material including iron disulfide that undergoes reduced expansion on discharge.
It is also an object to provide a positive electrode active material with iron disulfide that exhibits improved utilization of the active material.
In accordance with the present invention, a secondary electrochemical cell is presented that includes a negative electrode with alkali metal as the active material, a positive electrode with an improved active material and a molten salt electrolyte for providing ionic conduction between the electrodes. The improved active material within the positive electrode comprises iron disulfide in a major pro-portion by weight and a sulfide of cobalt in an amount suf-ficient to provide a cobalt to iron atom fraction inexcess of about 0.1.
BRIEF DESCRIPTION OF THE DRAWINGS
The present invention is illustrated in the accom-panying drawings wherein Fig. 1 is a cross-sectional view of a secondary electrochemical cell.
~V51~
Fig. 2 is a graph of resiskivity vs atom ~rackion (x) Co in el-xCxS2' Figs. 3A and 3B are graphs of cell voltage vs percent theoretical capacity for several electrochemical cells des-cribed in Example IV. In Fig. 3A the positive-electrode active materials are, in curve A: FeS2, curve B: FeS2-CoS2, curve C: FeS2-~iS and curve D: FeS2-Cu2S. In Fig. 3B the active materials are in curve A: ~eS2, curve E; FeS2-MnS
and curve F: FeS2-Ce2S3.
Fig. 4 is a graph of percent volume increase vs percent theoretical capacity for the positive electrodes of Example V.
DETAILED DESCRIPTION OF T~E PREFERRED EMBODIMENT
Referring now to Fig. 1, a secondary electrochemical cell is illustrated that has been used to demonstrate the present invention. It will be clear that various other cell configurations including many of those illustrated in the patents and applications cited above can also employ the improved positlve-electrode material of the present invention. The cell is shown with an outer housing 11 of stainless steel or other inert material containing kwo negative electrodes 13 and 15 and a centrally disposed positive electrode 17. The electrodes are separated by an electrically insulated mesh, paper or fabric 19, for instance of boron nitride, that is shown enveloping the positive electrode 17. Most o~ the volume of the cell housing 11 not occupied by the electrodes and particularly that volume intermediate the positive and negative elec-~5~8~
trodes is filled with a molten electrolyte for ionic con-duction between the electrodes. For clarity in the drawingr the molten electrolyte is not shown. The electrolyte used in the cell can be selected from known eutectic salt com-positions that are molten at the cell operating temperatures.
Electrolytes such as eutectic compositions of LiCl-KCl or LiCl-LiF-KBr and LiF-LiCl-LiI salts have been found to be suitable for this purpose~ Various other suitable electro-lytic salts can be selected from those listed in U. S.
patent 3,288,221, cited above.
An electrical conductor 21 passes through the housing wall and an opening within the upper negative electrode into electrical contact with the central positive electrode 17.
The conductor is supported and insulated from the cell housing by suitable electrical feedthrough structure 23.
Electrical contact is made to the negative electrodes through the cell housing 11 through conventional elec-trical connections (not shown).
Negative electrodes 13 and 15 can be any one of a number of types such as illustrated in the patents cited in the Background of the Invention. These negative elec-trodes can contain as active material a molten alkali metal such as lithium metal or sodium metal. Also, a solid alloy of lithium-aluminum, lithium-magnesium and other binary and ternary lithium alloys can serve as the ac-tive material.
A molten, negative-electrode, active material will be contained within a porous substrate of, for instance, stain-less steel or nickel. Solid alloy ~5~2~3~
material, for instance lithium-aluminum alloy, can be formed by electrodepositing lithium onto a porous aluminum substrate. In addition, particulate solid alloy material can be distributed throughout a porous metallic substrate in order to provide a negative electrode. Screens or rnesh 25 of an inert material such as stainless steel are illus-trated at the negative electrode surfaces facing the positive electrode for structural support and retention of active material~
The structure of positive electrode 17 is not critical.
It is illustrated in a form generally representative of the type employed in the cells given in the examples. As shown, it is enveloped by the porous~ electrically insu-lative separator 19 of, for instance, boron nitride paper, cloth or fabric. The positive-electrode structure in general will include the positive-electrode active material 27, current collector material 29 and electrolyte.
As illustrated, several layers of current collector 29 are electrically connected to conductor 21 at their center and are embedded within a mixture of the active material and electrolyte. The current collector can be sheets, mesh, screens, foam layers or other forms of electrical conductors. In some embodiments, particulate current collector material can be used in combination with or in place of the illustrated layers. The current collectors are of an electrically conductive materlal that will not extensively corrode in contact with the electrolyte and electrode materials at the electrode potential, for ~C~S~3Z8~
instance of molybdenum, molybdenum alloys, tungsten or carbon.
The positive-electrode active material 27 can also be provlded in a number of structural forms, for example, as solid particulate material or as a solid structure with porosity. In each instance, electrolyte is mixed or inter-spersed with or through the active material to provide ionic conduction to the current collector. In other struc-tures, a porous current collector such as a felt or foam can be filled with the active material and electrolyte.
The active positive electrode material is a com-position including a maJor weight proportion of iron disulfide and a minor proportlon by weight of one or more other polyvalent metal sulfides. Each of the polyvalent metals, like iron, is capable of combining with sulfur in more than one state of oxidation. For example, sulfides of cobalt include CoS, CoS2, Co3S4 and Co2S3 Often a polyvalent sulfide is conveniently provided and can be employed as a mixture of several stoichiometric compounds, e.g. mixtures of CoS and Co3S4.
The composition of lron disulfide and the polyvalent sulfide can be prepared initially by a number of methods.
In a typical manner employed for the cells described in the examples below, particulate mixtures of iron disulfide and the polyvalent metal sulfide were prepared and subsequently flooded with molten electrolyte.within the cell. On cycling o~ the cell at the elevated operating temperature of 400 to 450 C., other ternary and perhaps more complicated ~5~Z84 systems of iron, polyvalent metal, sulfur and possibly other constikuents are indicated. It is therefore contem-plaked that the positive-electrode active material can be prepared initially in various forms of ternary systems including a sulfide compound or berthollide with polyvalent metal substituted for a portion of the iron, a solid solu-tion of the polyvalent metal sulfide and the iron dlsulfide~
a eutectic composition of the constituents or various single and polyphase systems including the constituents.
A number of polyvalent metal sulfide additives have been found which can be combined with iron disulfide to improve the performance of the positive electrode. Addi-tives such as sulfides of cobalt, cerium and nickel are highly conductive materials that reduce the resistance of the electrode. Some of these, such as cobalt and nickel sulfides as well as other sulfides that have higher resis-tivities, may react durlng cycllng of the cell to provide an electrically conductive metal, e.g. Co, Ni~ Cu. These polyvalent metal sulfides exhibit thermodynamic equili-brium potentials within the cell operating range, e.g.
between 1.3 to 2.3 volts, IR free, versus lithium metal, in the formation of lithium sulfide and the electrically conductive metal. Other metal sulfides, such as those of manganese and cerium, that do not exhibit similar equili-brium potentials can possibly improve cell performance in combination with other electrode materials. A number of the polyvalent metal sulfides may interact with other materials within the posikive electrode at operating _ g _ 5~32~
temperature and potential to form electrically conductive phases or merely phases that exhibit reduced diffusional resistance within the positive electrode.
The improved active materials with low ohmic resis-tance (as opposed to diffusional resistance) can operate with reduced amounts of expensive current collector material at increased power output. Reduction in diffusional resis-tance leads to improved utilization of the active material.
Table I lists a number of metal sulfide additives that are contemplated for combining with iron disulfide to reduce both ohmic and dif~usion resistance of a positive electrode.
Resistivities are given where available for comparison with the resistivity o~ FeS2 which is 3.88 x 10 2 at 340 C.
TABLE I
Resistivity Additive Ohm-cm at 450C.
TiS2 1.0 x 10 2 Ti S3 ~~
Ti~ -- 4 CoS 2.2 x 10 Co S
v2~S4 102 Cr ~ 0.1 Mn~ 3 10 (single crystal of ~C-MnS~
MnS2 CdS 10 -6 ZnS 2 x 10 4 CceesS3 1.4 x 1~ 4 Cu S 3 x 10 (400C.) sb2s 2.7 (5103.) Pb~ 3 6.1 x 10 1 (340 C.) MoS~ 2.1 x 10 (102 C.) NiS23 o~2 NiS2 1.6 x 10 ~)S8Z~
Ni3S4 --Ni3S2 One manner of determining the amount of metal sulfide addltive to be included is through the reduction in resis-tivity of the mixture of the positive-electrode active material. Literature values for the Fel Co S2 system indicate that cobalt sulfide additions up to about 0.10 atom fraction produce a substantial reduction in resistivity, while a somewhat more gradual reduction is produced by additions beyond 0.10 atom fraction. This relationship is clearly shown in the graph of Fig. 2. For this ternary system o~ Fe-Co-S2, atom and weight ~raction of iron and cobalt are approximately the same.
In order to demonstrate the present development, a number of electrochemical cells have been operated in the laboratory with various positive-electrode, active materials.
These cells are illustrated in the ~ollowing examples.
Reduction in Current Collector EXAMPLE I
Two laboratory electrochemical cells~ each having a single negative electrode and a single positive electrode, were assembled for operation with a particulate mixture of FeS2 and Co2S3 as positive-electrode, active material. One of the cells (FC-l) employed three molybdenum screens brazed to a central molybdenum rod as a positive electrode current collector. An external molybdenum basket maintained at positive potential, but separated from the electrode active material by a zirconia fabric, was used to define the elec-~l~5~
trode geometry.
The second cell (FC-2) used a single molybdenum screen and central molybdenum rod to test the effect of reduced amounts of current collector material. This electrode a~so eliminated the molybdenum basket through use of a stainless steel basket maintained at negative electrode potential.
Other characteristics of the two cells are given below in Table II.
TABLE II
Cell FC-l FC-2 Positiye Electrode FeS2 20.5 g 19.95 g C02S3 2.0 g 2.21 g Area 23.1 cm2 22-.8 cm2 Volume 23 cm2 20.6 cm2 Current Collector 3 Mo screens 1 Mo screens Capacity ~FeS2) 18.3 A-hr 17.8 A-hr Capacity (C02S3) 1.5 A-hr 1.66 A-hr Negative Electrode Material Li-Al Li-Al Capacity 27.2 A-hr 26.71 A-hr Area - 38.3 cm 38.3 cm Operating Temperature 450C. l~50C
Both the cells were operated through nearly identical cycling programs with discharge voltages of about 1.6 to 0.7, capacity densities of 0.7 to 0.2 A-hr/cm and current densities ranging from 20 ma/cm2 to 700 ma/cm2. These measurements showed there was no significant difference ~358Z~14 between the performance of the two cells. The operationof these cells shows that a substantial reduction in the amount of molybdenum current collector can be made with cells employing iron disulfide with a sulfide of cobalt additive as positive-electrode, active material.
Comparative Resistance and Capacity EXAMPLE II
Two electrochemical cells similar in construction to the cell illustrated in Fig. 1 were operated for extended periods of time in excess of 1500 hours and 70 cycles each.
In the first cell (W-5) only FeS2 was employed as the positive electrode active material, while the second cell included a particulate mixture of FeS2 and about 10 weight percent of a sulfide of cobalt having a nominal composition of Co2S3. Analysis indicated the composition was pre-dominantly CoS with small quantities of Co3S4. Additional data regarding the two cells is given below in Table III.
~5~
o ~ ~ CO
o . . . ~;
~1 0 ~ O ~ ~ O O U~ ~ ~1 1 0 0 ~ O
~r~
~ , oc) o V
~ O O ~1 ~ ~1 ~ O L~ l ~1 1 ~1 0 ~ O
H bD
~1 O
m ¢
~d .
a) ~0 a>
C) a~ o s~
C~ s o ,~
¢
~Q ~
o ~ ~ C~ o o ~
S
O :~
a) ~ c) c) ~ ~
O ~ r-l o ~ OH rl c~ ~ h td^ C> S~
c) ^ ~7 ~I c) u~ ~ ta ~ a) c~ C~ q O c) ~ ~, ~ bO ~0 a) ~d ~ ~ ~ ~ a~ ~ h a) ~ ~: ~a) ~ ~: ~ ~ ~ a~ ~d 4~ ~ ~ a) ~ ~ b~ ~ bD
O O ~ c) O O o o ~ c) ~ ~D O ~ c a~ ~ ~d ~ ~1 . ~ ~
O ~ ~ ~ ~ S ~ ~~ ~ ~ ~ rC O ~ ~ ~ ~rl z; ~ ~ 3~ ~ ~ ~ c~
,~ ~ ~ c) ~ o C~ ~ Z L~ O
~5~
As shown in the table, the cells include essentially the same mass of molybdenum current collector material.
Resistance measurements made on the cells in the charged state showed an ohmic resistance of 8 milliohms in cell W-5 and only 5 milliohms in cell W-10. This reduction in ohmic resistance is attributed to the increased conduc-tivity of the positive-electrode active material including the sulfide of cobalt. Table III also shows a substantially lower charge cutoff voltage for cell W-10 than for cell W-5.
The lower charge potential reduces the corrosivity of the electrode environment and may permit use of a less noble current collector material than molybdenum. Notwithstanding the lower charge cutoff along with higher discharge cutoffs, cell W-10 exhibited a capacity of about 115 amp hours at 5 and 7 amperes discharge and 450C. operating temperature throughout a ma~or portion of its life. This corresponds to a utilization of approximately 77 percent. At these same current levels, cell W-5 without the sulfide of cobalt additive produced only 80 to 90 amp hours corresponding to a utilization of about 57 percent. This increase in capacity withi.n a reduced range o~ cutof~ voltages is attributed to the sulfide of cobalt additive within the positive-electrode active material.
EXAMPLE III
A third cell (W-ll~ of a construction substantially the same as that illustrated in ~ig. 1 and described in Example II included a positive-electrode active material of FeS2 - 10 wt. % Co2S3 (nominal composition). However, ~SE~Z84 only 1/3 the number of current collector layers and 1/2the mass of molybdenum material was included in the positive electrode compared to the positive electrodes of cells W-5 and W-10. Resistance measurements made on this cell showed an ohmic resistance in the charged state of 4.5 milliohms. This clearly indicates that through use of the positive-electrode active material of the present inven-tion a substantial reduction in the mass of current collector material can be made without detrimental effects.
Other-Additive Materials EXAMPLE I~
A number of experimental cells were operated, each having one positive and one negative electrode with LiCl-KCl electrolyte between the electrodes. The negative electrodes were of Li-Al alloy electrochemically formed on a porous compact of aluminum wire with a theoretical capacity of about 19 A~hr. The aluminum wire compacts were about 7.6 cm diameter and contained about 25 grams of aluminum. Each of the positive electrodes were about 20 cm square area and an average thickness of about 3/4 cm. Each included particulate active material, electrolyte and one layer of molybdenum mesh as current collector material. The active material was of particle sizes of between 75 and 180 U. S. standard mesh.
The positive-electrode, active material in the first cell was FeS2 alone. In each subsequent cell, ~ metal sulfide additive in an amount of 15 atom % was included with the FeS2. In each cell, the total weight of the positive-elec-trode active material was 14 grams.
~L~S~284~
During the test the cells were operated between 20and 40 cycles for about 300 to 550 hours at di~ferent current levels tlA, 2A or 3A) and two temperature levels (typically 400 C. and 450C.). Various characteristics of each o~ the cells are tabulated below in Table IV.
~s~
c~ h r~
~ ~ ~ o o~ o O ~ o L~ td o~ ~ ~ ~ ~ o ~ ~ ~ ~ o P~
C~
'U
a~
r ~ ~d ¢ ~ ~ ~D O O~ ~ ~ ~ O~ CO O ~
............
~ ~ O O ~ O ~ O ~ O cr~
M ~1 ~ H ~1 H ~ ~I r-l O
. . ::~
.
:
i .
.~ * ~p *
h L~\ ~Lr~ o ~ ~~ oo o C) ~ ~ ~ ~ ~ ~ ~ ~1 ~1 ~1 -~:
~ Q) H td p ~d C~ ~ ~
~ . , . ~ td m o . ~ c~
¢ ~ ~ ~
E~ ~ : ~ ~
~: o . ~ ~:
p~ ~
.' td~
~ ~ ~ ~ o~ o Lr~ ~o ~
'~ N N ~i ~ J ~i~i 0 O r~l ~1 HH H r-lH N r~J ~1 ~ rl ~ rl S
~ ~q ,aP
a) ~
P a ~
~ CO
rl ~ N N ~ V~ S:
N CQ N
~ O rl O ~ ~ u~ o '~ v c~ ~ ~ Z ~ *
D5~Z~3~
The results of these tests for the positive-electrode, active material including FeS2 alone and five of the more promising additive materials are shown in Figs. 3A and 3B.
These figures are discharge curves at 2 amps current and 450 C. showing utilization as a percentage of theoretical capacity versus cell discharge voltage. In Fig. 3A, curve A corresponds to FeS2, curve B to FeS2-CoS2, curve C to FeS2-NiS, curve D to FeS2-Cu2S, and in Fig. 3B curve A
again corresponds to FeS2, curve E to FeS2-MnS, curve F to FeS2-Ce2S3 as the positive-electrode actlve material within the respective cells.
Most of the remaining cells having other positive electrode additive materials exhibited performances not substantially better than that of FeS2 alone. However, the cell including zinc sulfide additlve did provide good improvement in the percent utilization of active material at the lower voltage plateau of 1.2 volts and below.
It is therefore seen from the results presented in Figs. 3A and 3B that the addition of each of the sulfides of five polyvalent metals provides a substantial and unexpected improvement in the utllization of actlve material in a positive electrode including a ma~or proportion of ~eS2 .
Reduced Electrode Swelling EXAMPLE V
Two electrochemical cells, each with Li-Al alloys as negative electrode material and LiCl-KCl electrolyte were operated through their first discharge cycle at ~S82i3~
50 ma/cm at a temperature of ~25C. Measurements ofaxial expansion were made on the positive electrode of each cell during this first cycle of operation. The first cell included particulate FeS2 as the active positive electrode material, while the second cell included FeS2 - 16 wt. %
Co2S3. The results of these tests are shown in Fig. 4 with the cell employing FeS2-Co2S3 as active material exhibiting both a higher utilization of active material as well as about a 15 to 20% reduction in volume expansion.
It will be clear from the above that the present inven-tion provides an electrochemical cell including an lmproved positive electrode active material. The use of this active material provides a number of unexpected benefits not realized by previous cells employing only particulate FeS2.
Among these benefits are improved utilization of the active material, reduced swellin~ of the electrode and reduced electrode resistance which can result in higher power output and a reduction in the required amount of current collector material.
Claims (2)
1. In a secondary electrochemical cell including a negative electrode with alkali metal as active material, a positive electrode with a positive-electrode, active material and a molten salt electrolyte intermediate said positive and negative electrodes, the improvement wherein said positive-electrode, active material comprises iron disulfide in a major proportion by weight and a sulfide of cobalt in an amount sufficient to provide a cobalt to iron atom fraction in excess of about 0.1.
2. The electrochemical cell of claim 1 wherein said sulfide of cobalt is included in a sufficient amount to provide a cobalt to iron atom fraction of about 0.1 to 0.15.
Applications Claiming Priority (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US05/596,044 US3992222A (en) | 1975-07-15 | 1975-07-15 | Metallic sulfide additives for positive electrode material within a secondary electrochemical cell |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| CA1058284A true CA1058284A (en) | 1979-07-10 |
Family
ID=24385768
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA250,914A Expired CA1058284A (en) | 1975-07-15 | 1976-04-23 | Metallic sulfide additives for positive electrode material within a secondary electrochemical cell |
Country Status (6)
| Country | Link |
|---|---|
| US (1) | US3992222A (en) |
| JP (1) | JPS5264634A (en) |
| CA (1) | CA1058284A (en) |
| DE (1) | DE2631892A1 (en) |
| FR (1) | FR2318511A1 (en) |
| GB (1) | GB1494164A (en) |
Families Citing this family (36)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US4086396A (en) * | 1977-02-23 | 1978-04-25 | The United States Of America As Represented By The United States Department Of Energy | Electrochemical cell with powdered electrically insulative material as a separator |
| US4076905A (en) * | 1977-05-05 | 1978-02-28 | Rockwell International Corporation | Electrode for electrical energy storage device |
| US4132547A (en) * | 1977-05-27 | 1979-01-02 | Westinghouse Electric Corp. | Method of producing self-supporting fully activated iron electrodes by thermal reduction-sintering |
| US4172926A (en) * | 1978-06-29 | 1979-10-30 | The United States Of America As Represented By The United States Department Of Energy | Electrochemical cell and method of assembly |
| DE2837980C2 (en) * | 1978-08-31 | 1983-11-10 | Gerhard Dr. 7301 Deizisau Berger | Activation additive for iron electrodes in alkaline batteries |
| US4233378A (en) * | 1978-12-11 | 1980-11-11 | Great Lakes Carbon Corporation | Process for manufacture of positive electrode for lithium/metal sulfide secondary cell |
| US4228224A (en) * | 1979-04-12 | 1980-10-14 | Rockwell International Corporation | Positive electrode for electrical energy storage device |
| US4233375A (en) * | 1979-08-02 | 1980-11-11 | Exxon Research & Engineering Co. | High energy density plural chalcogenide cathode-containing cell |
| US4264688A (en) * | 1979-08-13 | 1981-04-28 | Catanzarite Vincent Owen | Electrochemical cell |
| JPS57152673A (en) * | 1981-03-18 | 1982-09-21 | Toshiba Corp | Organic solvent battery |
| US4356101A (en) * | 1981-04-16 | 1982-10-26 | Westinghouse Electric Corp. | Iron active electrode and method of making same |
| US4409168A (en) * | 1981-05-22 | 1983-10-11 | Mrazek Franklin C | Method of forming components for a high-temperature secondary electrochemical cell |
| US4379815A (en) * | 1981-06-29 | 1983-04-12 | Union Carbide Corporation | Cell having mixed solid cathode materials for controlling cell expansion on discharge |
| US4390604A (en) * | 1981-06-29 | 1983-06-28 | Union Carbide Corporation | Complex metal sulfide cathodes for nonaqueous cells |
| FR2513817B1 (en) * | 1981-09-30 | 1987-02-06 | Europ Agence Spatiale | IMPROVEMENTS ON BATTERIES |
| GB2121596B (en) * | 1982-05-28 | 1986-03-26 | Us Energy | Feedthrough terminal |
| ZA837601B (en) * | 1982-10-20 | 1984-06-27 | South African Inventions | Electrochemical cell |
| US4761487A (en) * | 1986-06-10 | 1988-08-02 | The United States Of America As Represented By The United States Department Of Energy | Method for improving voltage regulation of batteries, particularly Li/FeS2 thermal batteries |
| US4728590A (en) * | 1986-07-28 | 1988-03-01 | The United States Of America As Represented By The United States Department Of Energy | Electrochemical cell with high discharge/charge rate capability |
| JPS63211566A (en) * | 1988-02-08 | 1988-09-02 | Sanyo Electric Co Ltd | Manufacture of positive electrode for nonaqueous electrolyte battery |
| DE69710787T2 (en) | 1996-05-22 | 2002-11-21 | Moltech Corp | COMPOSITE CATHODES, ELECTROCHEMICAL CELLS WITH COMPOSITE CATHODES AND METHOD FOR THE PRODUCTION THEREOF |
| JP2010509725A (en) * | 2006-11-14 | 2010-03-25 | コーニンクレッカ フィリップス エレクトロニクス エヌ ヴィ | Electrochemical energy source having a cathode electrode having at least one non-oxide active species, and an electrical device having such an electrochemical energy source |
| US8153296B2 (en) * | 2008-08-27 | 2012-04-10 | The Gillette Company | Lithium cell with cathode containing metal doped iron sulfide |
| US8304116B2 (en) * | 2008-10-02 | 2012-11-06 | The Gillette Company | Battery |
| WO2010054305A1 (en) * | 2008-11-07 | 2010-05-14 | Eaglepicher Technologies, Llc | Non-aqueous cell having amorphous or semi-crystalline copper manganese oxide cathode material |
| US8663825B2 (en) * | 2009-03-05 | 2014-03-04 | Eaglepicher Technologies, Llc | End of life indication system and method for non-aqueous cell having amorphous or semi-crystalline copper manganese oxide cathode material |
| EP2409348B1 (en) * | 2009-03-18 | 2015-07-01 | EaglePicher Technologies, LLC | Non-aqueous electrochemical cell having a mixture of at least three cathode materials therein |
| EP2417658B1 (en) * | 2009-04-06 | 2015-08-19 | Eaglepicher Technologies, Llc | Thermal battery electrolyte compositions, electrode-electrolyte composites, and batteries including the same |
| WO2010117956A1 (en) | 2009-04-06 | 2010-10-14 | Eaglepicher Technologies, Llc | Thermal battery cathode materials and batteries including same |
| US8652674B2 (en) | 2010-06-24 | 2014-02-18 | Eaglepicher Technologies, Llc | Thermal battery cathode materials containing nickel disulfide and batteries including same |
| CN102544482A (en) * | 2010-12-20 | 2012-07-04 | 梅岭化工厂 | Formula of thermal battery CoS2 cathode material and processing technology |
| US8697279B2 (en) | 2011-01-14 | 2014-04-15 | General Electric Company | Composition and energy storage device |
| US9825310B2 (en) | 2014-04-25 | 2017-11-21 | Greatbatch Ltd. | High capacity cathode material with improved operating voltage |
| US20160104890A1 (en) * | 2014-10-14 | 2016-04-14 | General Electric Company | Electrode compositions and related energy storage devices |
| CN104393353B (en) * | 2014-11-28 | 2016-08-24 | 南开大学 | A kind of high magnification and long-life fill room temperature sode cell and preparation method thereof |
| CN115332519A (en) * | 2022-09-09 | 2022-11-11 | 郑州大学 | Preparation method and application of lithium-sulfur battery positive electrode material |
Family Cites Families (2)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US3898096A (en) * | 1973-06-11 | 1975-08-05 | Rockwell International Corp | Lithium-molten salt cell with transition metal chalcogenide positive electrode |
| US3997363A (en) * | 1974-10-07 | 1976-12-14 | Electric Power Research Institute | Modular electrical energy storage device |
-
1975
- 1975-07-15 US US05/596,044 patent/US3992222A/en not_active Expired - Lifetime
-
1976
- 1976-04-23 CA CA250,914A patent/CA1058284A/en not_active Expired
- 1976-04-26 GB GB16841/76A patent/GB1494164A/en not_active Expired
- 1976-07-15 FR FR7621684A patent/FR2318511A1/en active Granted
- 1976-07-15 DE DE19762631892 patent/DE2631892A1/en not_active Withdrawn
- 1976-07-15 JP JP51084481A patent/JPS5264634A/en active Pending
Also Published As
| Publication number | Publication date |
|---|---|
| GB1494164A (en) | 1977-12-07 |
| FR2318511B1 (en) | 1981-10-30 |
| FR2318511A1 (en) | 1977-02-11 |
| JPS5264634A (en) | 1977-05-28 |
| DE2631892A1 (en) | 1977-02-10 |
| US3992222A (en) | 1976-11-16 |
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