USRE31286E - Production of electrolytic battery active manganese dioxide - Google Patents
Production of electrolytic battery active manganese dioxide Download PDFInfo
- Publication number
- USRE31286E USRE31286E US06/152,505 US15250580A USRE31286E US RE31286 E USRE31286 E US RE31286E US 15250580 A US15250580 A US 15250580A US RE31286 E USRE31286 E US RE31286E
- Authority
- US
- United States
- Prior art keywords
- ore
- manganese dioxide
- product
- anodes
- manganese
- 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 - Lifetime
Links
Images
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
- H01M4/48—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
-
- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B1/00—Electrolytic production of inorganic compounds or non-metals
- C25B1/01—Products
- C25B1/21—Manganese oxides
-
- 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
- H01M6/04—Cells with aqueous electrolyte
- H01M6/06—Dry cells, i.e. cells wherein the electrolyte is rendered non-fluid
Definitions
- the major application of the manganese dioxide product is in its use as the cathode depolariser in the conventional Leclanche dry cell battery.
- This high grade ⁇ --MnO 2 is ideally suited for dry cell applications because of its high electrochemical activity.
- Finely divided synthetic manganese dioxide is also used in ferrite manufacture and for pigments. Other applications are in ceramics, welding rods and the general chemical industry.
- the conventional process for the production of ⁇ --MnO 2 from a manganese dioxide feed ore consists of the following steps:
- This invention may be conducted in a cell containing three essential elements
- a cathode compartment which contains a slurry of particulate MnO 2 , the Mn content of which is being selectively leached by a reducing environment attributable to the cathode;
- an anode compartment comprising a manganese containing electrolyte (either the sulphate, chloride or nitrate) from which an MnO 2 product is being produced;
- FIG. 1 A typical such cell is illustrated in FIG. 1, this figure being provided to facilitate understanding of the process and is not to be considered in any way limiting this invention.
- the conditions in the anolyte compartment may be controlled to produce a variety of MnO 2 products. For example, at 90°-98° C., a dense anode deposit of ⁇ -MnO 2 may be deposited, whilst at 15°-25° C., a particulate product may be formed. Typical materials suitable for use at the anode include carbon, lead and titanium, all of which are currently used within the industry.
- the temperature conditions in the catholyte are by necessity similar to those selected for the anodic product formation step. However, markedly different solution conditions may be attained by control of the diaphragm material and electrolysis conditions.
- a solution manganese content of about 20 g/l Mn to about 200 g/l Mn, with a preferred value of 80 to 130 g/l, as this ensures a high deposit efficiency>95%; an operating solution acidity of up to about 5N, with a preferred acidity of about 2N; and an anode current density of about 30 to about 250 Amp/m 2 for an adherent high temperature deposit and of about 1000 to 4000 Amp/m 2 for a particulate deposit.
- the preferred current density range is 30 to 120 A/m 2 for titanium anodes and 80 to 140 A/m 2 for carbon anodes to obtain a conventional adherent deposit.
- the high preferred manganese concentrations facilitate operation at high current densities.
- the cathode solution conditions are related to those in the anolyte by the relative rates of electrolytic generation or consumption and diffusion through the diaphragm.
- the nominated solution temperatures are as given for the anode, namely 15° C. to the solution boiling point; nominated dissolved manganese contents are from 30 g/l to about 220 g/l Mn; nominated solution acidities are from about pH7 to pH0 with a value of about pH4 to pH0.5 preferred. In fact low catholyte acidities are particularly important in avoiding the dissolution of nonmanganese elements.
- a solids loading of about 20 to 350 g/l may be used whilst the preferred range is about 50 to 200 g/l.
- the ore feed should preferably be finely ground, say >95% less than 50 ⁇ m, to attain high dissolution efficiency, but the process is operable with larger particle sizes.
- selection of the cathode material and current density are particularly important to control the selective leaching of MnO 2 and to prevent the dissolution of impurities.
- Typical cathode current densities of 5 to 400 Amp/m 2 may be used with preferred current densities of 25 to 100 Amp/m 2 .
- the adherent MnO 2 product was stripped from the titanium anodes and the catholyte slurry filtered to recover the residue.
- the simplest process flow sheet (FIG. 2) is the addition of ground ore to an electrolytic cell containing a prepared electrolyte, and the batchwise or semi-batchwise dissolution of ore occurs.
- the electrolysis is ceased because of ore depletion of sludge accumulation, the manganese deficient residue is separated from the solution and the solution is returned to the cell and the process repeated.
- the anode may be removed periodically and the adherent deposit stripped at any time throughout the batch dissolution. Modifications of the above, including continuous ore addition to a non-flow cell or a continuous flow system via a multiple series of cells, are obvious to those skilled in the art.
- a refinement of the above single cell is the continuous removal of a portion of the catholyte, and the return of the solution, after filtration, to the cell, for example to the anolyte (FIG. 3). If desired, some form of purification treatment, e.g. pH adjustment, may be carried out before returning the electrolyte to the cell.
- some form of purification treatment e.g. pH adjustment, may be carried out before returning the electrolyte to the cell.
Landscapes
- Chemical & Material Sciences (AREA)
- Inorganic Chemistry (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Electrochemistry (AREA)
- General Chemical & Material Sciences (AREA)
- Engineering & Computer Science (AREA)
- Materials Engineering (AREA)
- Metallurgy (AREA)
- Organic Chemistry (AREA)
- Electrolytic Production Of Non-Metals, Compounds, Apparatuses Therefor (AREA)
- Inorganic Compounds Of Heavy Metals (AREA)
- Battery Electrode And Active Subsutance (AREA)
Abstract
This process concerns the direct electroconversion of low grade manganese ores to high purity manganese dioxide product, which, among other applications, is ideally suited for use in dry cells. The process operating conditions are controlled such that impurities in the ore are substantially eliminated from the product. A decrease in impurity levels in excess of 100 fold can be achieved between the product and the ore feed.
Description
The major application of the manganese dioxide product is in its use as the cathode depolariser in the conventional Leclanche dry cell battery. This high grade γ--MnO2 is ideally suited for dry cell applications because of its high electrochemical activity. Finely divided synthetic manganese dioxide is also used in ferrite manufacture and for pigments. Other applications are in ceramics, welding rods and the general chemical industry.
The conventional process for the production of γ--MnO2 from a manganese dioxide feed ore consists of the following steps:
1. High temperature reduction roasting of the natural MnO2 to MnO.
2. Acid dissolution of this MnO in the spent electrolyte.
3. Purification of the pregnant leach liquors (a) with a base, to remove iron, and (b) with a sulphide, to remove heavy metal impurities.
4. Electrolysis of the filtered electrolyte to produce a high purity MnO2 product at the anode according to equation (2) and hydrogen at the cathode.
2H.sup.+ +2e.sup.- →H.sub.2
Notable disadvantages of the conventional process are: (a) the need for pretreatment (reduction roasting) of the feed ore which is an energy consuming step with polluting side effects; (b) the evolution of hydrogen from the hot (80°-100° C.) electrolytic cells causes appreciable heat losses due to the greatly increased evaporation of water and can also produce an acid mist which yields an unpleasant working environment and building corrosion; (c) depletion of the solution Mn2+ content.
In essence, the process herein described concerns the electrorefining of manganese dioxide to produce a high grade synthetic product from natural ore. The principal equations describing the cathode and anode reactions are:
Cathode MnO.sub.2 +4H.sup.+ +2e.sup.- →Mn.sup.2+ +2H.sub.2 O (1)
Anode Mn.sup.2+ +2H.sub.2 O→MnO.sub.2 +4H.sup.+ +2e.sup.-( 2)
As these equations balance each other in consumption and formation of species, only make-up quantities of other materials are required. This novel process has simultaneously overcome all the disadvantages of the conventional process and has markedly reduced the extent of purification required due to the selectivity of the leach. A further advantage of this novel process is a reduction in the cell operating voltage through the high anolyte Mn2+ concentrations and the lower cathode potential of the dissolution reaction compared with that for H2 evolution, this giving a notable reduction in power consumption.
As this process is based upon two reversible equations, the nature of the anodic species is only significant to the extent at which alternate reactions may occur at the electrodes. Thus, it must be noted that while sulphate, chloride and nitrate solutions may be used, sulphate solutions are preferred at these present least operating difficulties.
This invention may be conducted in a cell containing three essential elements
1. a cathode compartment which contains a slurry of particulate MnO2, the Mn content of which is being selectively leached by a reducing environment attributable to the cathode;
2. an anode compartment comprising a manganese containing electrolyte (either the sulphate, chloride or nitrate) from which an MnO2 product is being produced;
3. an ion-permeable diaphragm, which is impermeable to the particulate MnO2 slurry, separating the anode and cathode regions.
A typical such cell is illustrated in FIG. 1, this figure being provided to facilitate understanding of the process and is not to be considered in any way limiting this invention.
The conditions in the anolyte compartment may be controlled to produce a variety of MnO2 products. For example, at 90°-98° C., a dense anode deposit of γ-MnO2 may be deposited, whilst at 15°-25° C., a particulate product may be formed. Typical materials suitable for use at the anode include carbon, lead and titanium, all of which are currently used within the industry. The temperature conditions in the catholyte are by necessity similar to those selected for the anodic product formation step. However, markedly different solution conditions may be attained by control of the diaphragm material and electrolysis conditions. Correct selection of the diaphragm material is essential for the control of anolyte/catholyte acidities as the anode reaction is acid producing and Mn2+ ion consuming, whilst the cathode reaction is acid consuming and Mn2+ ion producing.
The conditions under which this invention operates are:
i. Anode Compartment A temperature from about 15° C. to the solution boiling point (about 120° C.), with a preferred temperature range of 80°-100° C. for the production of an adherent anode deposit of γ-MnO2, and of 15°-25° C. for a particulate product; a solution manganese content of about 20 g/l Mn to about 200 g/l Mn, with a preferred value of 80 to 130 g/l, as this ensures a high deposit efficiency>95%; an operating solution acidity of up to about 5N, with a preferred acidity of about 2N; and an anode current density of about 30 to about 250 Amp/m2 for an adherent high temperature deposit and of about 1000 to 4000 Amp/m2 for a particulate deposit. Whilst from a capital investment standpoint, high current densities are desirable, product properties, current efficiencies and cell operating conditions are superior at intermediate current densities, thus the preferred current density range is 30 to 120 A/m2 for titanium anodes and 80 to 140 A/m2 for carbon anodes to obtain a conventional adherent deposit. As those skilled in the art are well aware, the high preferred manganese concentrations facilitate operation at high current densities.
ii. Cathode Compartment The cathode solution conditions are related to those in the anolyte by the relative rates of electrolytic generation or consumption and diffusion through the diaphragm. The nominated solution temperatures are as given for the anode, namely 15° C. to the solution boiling point; nominated dissolved manganese contents are from 30 g/l to about 220 g/l Mn; nominated solution acidities are from about pH7 to pH0 with a value of about pH4 to pH0.5 preferred. In fact low catholyte acidities are particularly important in avoiding the dissolution of nonmanganese elements.
A solids loading of about 20 to 350 g/l may be used whilst the preferred range is about 50 to 200 g/l. The ore feed should preferably be finely ground, say >95% less than 50 μm, to attain high dissolution efficiency, but the process is operable with larger particle sizes. Together with catholyte acidity, selection of the cathode material and current density are particularly important to control the selective leaching of MnO2 and to prevent the dissolution of impurities. Typical cathode current densities of 5 to 400 Amp/m2 may be used with preferred current densities of 25 to 100 Amp/m2.
The following example is provided to illustrate this invention but should not be construed as limiting this invention in any way whatsoever.
1200 g of MnO2 ore was agitated in 81 of MnSO4 solution (105 g/l Mn2+ and 2.9 g/l H2 SO4) in a diaphragm cell containing three titanium anodes, each 12 cm×10 cm submerged area and enclosed in polypropylene cloth diaphragm bags, and four graphite cathodes, each 12 cm×10 cm submerged area, external to the diaphragm bags.
Current was passed at 60A /m2 of anode area for 96 hours at a temperature of 90° C. The average cell voltage was 2.1 Volt. The power consumption was 1.24 KWH/Kg.
The adherent MnO2 product was stripped from the titanium anodes and the catholyte slurry filtered to recover the residue.
In Table 1 below, it can be seen that product of high purity is formed and a large reduction in impurity level, one hundred fold in the case of Fe, can be obtained between feed ore and product.
TABLE 1
______________________________________
ANALYTICAL RESULTS
Com- Pro- Resi- Electrolyte
ponent Ore duct due Start Finish
______________________________________
H.sub.2 SO.sub.4
-- -- -- 2.9 g/l
Ano- Catho-
lyte lyte
98.0 g/l
9.8 g/l
Mn 45% 62% 20% 9.5% 9.3%
Fe 20,000 200 35,000
190 mg/l 320 mg/l
ppm ppm ppm
Cu 150 20 250 8 6
Pb 100 50 200 14 14
Zn 70 20 100 78 70
Ni 100 20 200 130 110
Co 70 30 100 114 100
Cr 60 10 100 2 4
Mo 440 -- 1,000 -- --
Ca 16,000 200 30,000
100 400
Mg 10,000 -- 25,000
240 600
K 5,500 200 12,000
40 120
Na 1,040 20 2,300 40 200
Number
of grams
1,200 675 560 -- --
______________________________________
In Table 2, it can be seen that product of high electrochemical activity can be prepared. The product prepared has been compared with a standard electrolytic manganese dioxide from Japan. The method used to determine the electrochemical activity was by the Kornfeil test. Manganese dioxide sample (0.50 g) and acetylene black (0.20 g) are mixed as a slurry with electrolyte solution (Kornfeil 2 solution) to a standard moisture level. This mix is then added into the Kornfeil cell and the wet black mix compressed with the carbon cathode rod by loading with a 2 kg weight. The resulting Kornfeil pellet was maintained under this load and discharged between the carbon and zinc electrodes at constant current drains. The residual cell voltage was determined as a function of time by a pulseinterrupt technique, to a final voltage of 1.00 volts. The time of discharge is taken as a measure of the electrochemical activity of the manganese dioxide.
TABLE 2
______________________________________
ELECTROCHEMICAL ACTIVITY OF PRODUCT-continued
Time to 1.0V at high
Time to 1.0V at
current drain of
low current
Product 60mA drain of 12mA
______________________________________
Standard Electrolytic
4,000 sec. 25,200 sec.
MnO.sub.2 (Japan)
Example product
4,300 27,000
______________________________________
Whilst this invention concerns a process for the electrorefining of MnO2, it must be noted that a variety of process flow sheets are possible, the following illustrations of which are provided but in no way should be considered limiting.
The following discussion has been limited to the formation of a high temperature (80°-100° C.) adherent γ-MnO2 product for illustrative purposes only.
The simplest process flow sheet (FIG. 2) is the addition of ground ore to an electrolytic cell containing a prepared electrolyte, and the batchwise or semi-batchwise dissolution of ore occurs. When the electrolysis is ceased because of ore depletion of sludge accumulation, the manganese deficient residue is separated from the solution and the solution is returned to the cell and the process repeated. The anode may be removed periodically and the adherent deposit stripped at any time throughout the batch dissolution. Modifications of the above, including continuous ore addition to a non-flow cell or a continuous flow system via a multiple series of cells, are obvious to those skilled in the art.
A refinement of the above single cell is the continuous removal of a portion of the catholyte, and the return of the solution, after filtration, to the cell, for example to the anolyte (FIG. 3). If desired, some form of purification treatment, e.g. pH adjustment, may be carried out before returning the electrolyte to the cell.
Claims (10)
1. A process for the production of high grade γMnO2 from manganese dioxide ore in an electrochemical cell having one or more inert anodes, immersed in an aqueous anolyte having a solution manganese content of 20 g/l Mn to 200 g/l Mn and an acidity of up to 5N, and one or more inert cathodes, immersed in a slurry consisting of particulate manganese dioxide ore and an aqueous catholyte having a solution manganese content of 30 g/l Mn to 220 g/l Mn and a pH below 7, the anodes and cathodes disposed on opposite sides of one or more porous diaphragms, the process consisting of applying a direct current potential between the anodes and cathodes to reduce the manganese dioxide slurry to ionic manganese which diffuses through the diaphragms and is oxidised at the anodes where γMnO2 is formed, the anode current density being 20 to 250 Amp/m2 at a cell temperature of from .[.15 to 25° C..]. .Iadd.80° to 100° C. .Iaddend.or 1,000 to 4,000 Amp/m2 at a cell temperature of .Badd..[.80° to 100° C..]..Baddend. .Iadd.15° to 25° C. .Iaddend.and the cathode current density being 5 to 400 Amps/m2.
2. A process as in claim 1 in which the electrolyte comprises the anion group, sulphate.
3. A process as claimed in claim 1 in which the electrolyte comprises the anion group, chloride.
4. A process as claimed in claim 1 in which the electrolyte comprises the anion group, nitrate.
5. A process as claimed in claim 1 in which the current density is from about 30 to 140 Amp/m2.
6. A process as claimed in claim 1 in which the anolyte contains about 80 to 130 g/l Mn and about 2N acid.
7. A process as claimed in claim 1 in which the cathode current density is 25 to 100 Amp/m2.
8. A process as claimed in claim 1 in which the ore content of the catholyte is about 20 to 350 g/l.
9. A process as claimed in claim 1 in which the ore content of the catholyte is about 50 to 200 g/l.
10. A process as claimed in claim 1, in which the acid content is such that the pH is in the range of about pH4 to pH0.5.
Applications Claiming Priority (2)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| AU607173 | 1973-12-20 | ||
| AU6071/73 | 1973-12-20 |
Related Parent Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| US05/531,800 Reissue US3951765A (en) | 1973-12-20 | 1974-12-11 | Production of electrolytic battery active manganese dioxide |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| USRE31286E true USRE31286E (en) | 1983-06-21 |
Family
ID=3696572
Family Applications (2)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| US05/531,800 Expired - Lifetime US3951765A (en) | 1973-12-20 | 1974-12-11 | Production of electrolytic battery active manganese dioxide |
| US06/152,505 Expired - Lifetime USRE31286E (en) | 1973-12-20 | 1980-05-22 | Production of electrolytic battery active manganese dioxide |
Family Applications Before (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| US05/531,800 Expired - Lifetime US3951765A (en) | 1973-12-20 | 1974-12-11 | Production of electrolytic battery active manganese dioxide |
Country Status (3)
| Country | Link |
|---|---|
| US (2) | US3951765A (en) |
| JP (1) | JPS50113498A (en) |
| GB (1) | GB1487418A (en) |
Cited By (2)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US4997531A (en) * | 1988-12-26 | 1991-03-05 | Japan Metals & Chemical Co. Inc. | Process for manufacturing electrolytic manganese oxide |
| US6168888B1 (en) * | 1997-06-19 | 2001-01-02 | Tosoh Corporation | Spinel-type lithium-manganese oxide containing heteroelements, preparation process and use thereof |
Families Citing this family (17)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US4083757A (en) * | 1977-07-26 | 1978-04-11 | Levan Nikolaevich Dzhaparidze | Electrochemical process for producing manganese dioxide |
| US4183792A (en) * | 1979-02-16 | 1980-01-15 | Amax Inc. | Method and cell for electrolytic oxidation of Ni(OH)2 with stationary bed electrode |
| US4405419A (en) * | 1979-12-13 | 1983-09-20 | Japan Metal And Chemical Co., Ltd. | Method for producing electrolytic manganese dioxide |
| EP0037863A1 (en) * | 1980-04-01 | 1981-10-21 | Union Carbide India Limited | Process for making manganous sulphate solution |
| US4597957A (en) * | 1984-03-06 | 1986-07-01 | Japan Metals And Chemicals Co., Ltd. | Process for electrolytically producing metallic oxide for ferrite |
| ES2119000T3 (en) * | 1993-09-30 | 1998-10-01 | Mitsui Mining & Smelting Co | COMPOSITION OF CATHODIC ACTIVE MATERIAL FOR DRY BATTERIES, METHOD FOR PREPARATION AND ALKALINE ACCUMULATORS. |
| US6214198B1 (en) * | 1998-12-21 | 2001-04-10 | Kerr-Mcgee Chemical Llc | Method of producing high discharge capacity electrolytic manganese dioxide |
| US6610263B2 (en) * | 2000-08-01 | 2003-08-26 | Enviroscrub Technologies Corporation | System and process for removal of pollutants from a gas stream |
| JP4940503B2 (en) * | 2001-03-23 | 2012-05-30 | 東ソー株式会社 | Electrolytic manganese dioxide powder and method for producing the same |
| US7232782B2 (en) * | 2002-03-06 | 2007-06-19 | Enviroscrub Technologies Corp. | Regeneration, pretreatment and precipitation of oxides of manganese |
| US20030059460A1 (en) * | 2001-09-27 | 2003-03-27 | Yasuhiko Tabata | Hybrid material for regeneration of living body tissue |
| CN1620334A (en) * | 2001-12-21 | 2005-05-25 | 环境清洁技术公司 | Pretreatment and regeneration of oxides of manganese |
| US20040101457A1 (en) * | 2002-06-11 | 2004-05-27 | Pahlman John E. | Disassociation processing of metal oxides |
| CN1761520A (en) * | 2003-01-28 | 2006-04-19 | 环境清洁技术公司 | Oxides of manganese processed in continuous flow reactors |
| US7488464B2 (en) * | 2003-07-31 | 2009-02-10 | Enviroscrub Technologies Corporation | Metal oxide processing methods and systems |
| US20220333253A1 (en) * | 2021-04-08 | 2022-10-20 | Francois Cardarelli | Electrochemical preparation of vanadium electrolytes and sulfates of multivalent transition metals |
| CN114457355B (en) * | 2021-12-30 | 2023-10-27 | 广西汇元锰业有限责任公司 | Electrolytic method of electrolytic manganese dioxide and electrolytic manganese dioxide |
Citations (1)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US272391A (en) * | 1883-02-13 | Antonin thiolliee |
-
1974
- 1974-12-11 US US05/531,800 patent/US3951765A/en not_active Expired - Lifetime
- 1974-12-17 JP JP49144117A patent/JPS50113498A/ja active Pending
- 1974-12-18 GB GB54754/74A patent/GB1487418A/en not_active Expired
-
1980
- 1980-05-22 US US06/152,505 patent/USRE31286E/en not_active Expired - Lifetime
Patent Citations (1)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US272391A (en) * | 1883-02-13 | Antonin thiolliee |
Cited By (3)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US4997531A (en) * | 1988-12-26 | 1991-03-05 | Japan Metals & Chemical Co. Inc. | Process for manufacturing electrolytic manganese oxide |
| US6168888B1 (en) * | 1997-06-19 | 2001-01-02 | Tosoh Corporation | Spinel-type lithium-manganese oxide containing heteroelements, preparation process and use thereof |
| US6670076B1 (en) * | 1997-06-19 | 2003-12-30 | Tosoh Corporation | Spinel-type lithium-manganese oxide containing heteroelements preparation process and use thereof |
Also Published As
| Publication number | Publication date |
|---|---|
| JPS50113498A (en) | 1975-09-05 |
| US3951765A (en) | 1976-04-20 |
| GB1487418A (en) | 1977-09-28 |
Similar Documents
| Publication | Publication Date | Title |
|---|---|---|
| USRE31286E (en) | Production of electrolytic battery active manganese dioxide | |
| US4204922A (en) | Simultaneous electrodissolution and electrowinning of metals from simple sulphides | |
| EP1310008A1 (en) | Vanadium electrolyte preparation using asymmetric vanadium reduction cells and use of an asymmetric vanadium reduction cell for rebalancing the state of charge of the electrolytes of an operating vanadium redox battery | |
| US3065155A (en) | Electrolytic manganese dioxide process | |
| US6210558B1 (en) | Steel pickling process in which the oxidation of the ferrous ion formed is carried out electrolytically | |
| US4627899A (en) | Electrolytic cell and methods combining electrowinning and electrochemical reactions employing a membrane or diaphragm | |
| EP0184319B1 (en) | Suspension bath and process for production of electrolytic manganese dioxide | |
| US5181994A (en) | Process for the preparation of chromic acid | |
| US4632738A (en) | Hydrometallurgical copper process | |
| CA1049952A (en) | Production of electrolytic battery active manganese dioxide | |
| US4451340A (en) | Method for the electrolytic production of lead | |
| de Araujo et al. | Reuse of furnace fines of ferro alloy in the electrolytic manganese production | |
| US4339312A (en) | Continuous process for the direct conversion of potassium chloride to potassium chlorate by electrolysis | |
| US2417259A (en) | Electrolytic process for preparing manganese and manganese dioxide simultaneously | |
| Maja et al. | Dissolution of pastes in lead-acid battery recycling plants | |
| EP0268319B1 (en) | Method for extracting mn metal and manganese dioxide from divalent mn salt solutions | |
| US4115222A (en) | Method for electrolytic winning of lead | |
| CS268673B2 (en) | Method of zinc production from ores and concentrates | |
| US4124460A (en) | Electrowinning of copper in presence of high concentration of iron | |
| Fink et al. | Anodes for the Electrowinning of Manganese | |
| CN1188548C (en) | Process for directly producing metal zinc by suspension electrolysing high-iron sphalerite | |
| US4626327A (en) | Electrolytic process for manufacturing potassium peroxydiphosphate | |
| Jacobs et al. | Electrowinning of manganese from chloride electrolytes | |
| DE1567586A1 (en) | Process for the production of alkali metal chlorates by electrolytic means and equipment for carrying out the process | |
| Ettel | Electrochemical aspects of hydro-electrometallurgy |