CA2479050A1 - Minimising carbon transfer in an electrolytic cell - Google Patents
Minimising carbon transfer in an electrolytic cell Download PDFInfo
- Publication number
- CA2479050A1 CA2479050A1 CA002479050A CA2479050A CA2479050A1 CA 2479050 A1 CA2479050 A1 CA 2479050A1 CA 002479050 A CA002479050 A CA 002479050A CA 2479050 A CA2479050 A CA 2479050A CA 2479050 A1 CA2479050 A1 CA 2479050A1
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- Prior art keywords
- cell
- cathode
- potential
- carbon
- anode
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- 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.)
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Classifications
-
- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
- C25C7/00—Constructional parts, or assemblies thereof, of cells; Servicing or operating of cells
- C25C7/005—Constructional parts, or assemblies thereof, of cells; Servicing or operating of cells of cells for the electrolysis of melts
-
- C—CHEMISTRY; METALLURGY
- C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
- C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
- C22B34/00—Obtaining refractory metals
- C22B34/10—Obtaining titanium, zirconium or hafnium
- C22B34/12—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08
- C22B34/129—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining metallic titanium from titanium compounds by dissociation, e.g. thermic dissociation of titanium tetraiodide, or by electrolysis or with the use of an electric arc
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- Chemical & Material Sciences (AREA)
- Engineering & Computer Science (AREA)
- Organic Chemistry (AREA)
- Metallurgy (AREA)
- Materials Engineering (AREA)
- Mechanical Engineering (AREA)
- Electrochemistry (AREA)
- Geology (AREA)
- Life Sciences & Earth Sciences (AREA)
- General Life Sciences & Earth Sciences (AREA)
- Environmental & Geological Engineering (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Manufacturing & Machinery (AREA)
- Electrolytic Production Of Metals (AREA)
- Electrodes For Compound Or Non-Metal Manufacture (AREA)
- Inert Electrodes (AREA)
- Electrolytic Production Of Non-Metals, Compounds, Apparatuses Therefor (AREA)
- Electrical Discharge Machining, Electrochemical Machining, And Combined Machining (AREA)
- Battery Electrode And Active Subsutance (AREA)
Abstract
An electrolytic cell for reducing a metal oxide, such as titania, in a solid state is disclosed. The electrolytic cell includes an anode formed from carbon and a cathode formed at least in part from the metal oxide. The electrolytic cell also includes a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms positioned between the cathode and the anode to thereby prevent migration of carbon to the cathode.
Description
MINIMISING CARBON TRANSFER IN AN ELECTROLYTIC CELL
The present invention relates to reduction of metal oxides in a solid state in an electrolytic cell.
The present invention was made during the course of an on-going research project on solid state reduction of titania (Ti02) carried out by the applicant.
During the course of the research project the applicant carried out experimental work on the reduction of titania using an electrolytic cell that included a graphite crucible that formed an anode of the cell, a pool of molten CaCl2-based electrolyte in the crucible, and a range of cathodes that included solid titania.
The CaCl2-based electrolyte was a commercially available source of CaCl2, namely calcium chloride dihydrate, that partially decomposed on heating and produced CaO.
The applicant operated the electrolytic cell at a potential above the decomposition potential of Ca0 and below the decomposition potential of CaCl2.
The applicant found that the cell could electrochemically reduce titania to titanium with very low concentrations of oxygen.
The applicant does not have a clear understanding of the electrolytic cell mechanism at this stage.
Nevertheless, whilst not wishing to be bound by the comments in this and the following paragraphs, the applicant offers the following comments by way of an outline of a possible cell mechanism.
The experimental work carried out by the applicant produced evidence of Ca metal dissolved in the electrolyte. The applicant. believes that, at least during the early stages of operation of the cell, the Ca metal was the result of electrodeposition of Ca~+ cations as Ca metal on electrically conductive sections of the cathode.
The experimental work was carried out using a CaCl2-based electrolyte at a cell potential below the decomposition potential of CaCl2. The applicant believes that the initial deposition of Ca metal on the cathode was due to the presence of Ca++-cations and O-- anions derived from CaO in the electrolyte. The decomposition potential of Ca0 is less 'than the decomposition potential of CaClz.
In this cell mechanism the-.cell operation is dependent, at least during the early stages of cell operation, on decomposition of CaO, with Ca++ cations migrating to the cathode and depositing as Ca metal and O-- anions migrating to the anode and forming CO and/or COz (in a situation, in which the anode is a graphite anode).
The applicant believes that the Ca metal that deposited on electrically conductive sections of the cathode was deposited predominantly as a separate phase in the early stages of cell operation and thereafter dissolved in the electrolyte and migrated to the vicinity of the titania in the cathode and participated in chemical reduction of titania.
The applicant also believes that at later stages of the cell operation part of the Ca metal that deposited on the cathode was deposited directly on partially deoxidised titanium and thereafter participated in chemical reduction of titanium.
The applicant also believes that the O'- anions, once extracted from the titania, migrated to the anode and reacted with anode carbon and produced CO and/or C02 (and in some instances Ca0) and released electrons that facilitated electrolytic deposition of Ga metal on the cathode.
However, notwithstanding that the cell could electrochemically reduce titania to titanium with very low concentrations of oxygen, the applicant also found that there were relatively significant amounts of carbon transferred from the anode to the electrolyte and to the titanium produced at the cathode under a wide range of cell operating conditions.
Carbon in the titanium is an undesirable contaminant. In addition, carbon transfer was partially responsible for low energy efficiency of the cell. Both problems are significant barriers to commercialisation of electrolytic reduction technology.
The applicant carried out experimental work to identify the mechanism for carbon transfer and to determine how to minimise carbon transfer and/or to minimise the adverse effects of carbon transfer.
The experimental work indicated that the mechanism of carbon transfer is electrochemical rather than erosion and that one way of minimising carbon transfer and therefore contamination of titanium produced at the cathode by electrochemical reduction of titania at the cathode is to position a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms between the cathode and the anode anal thereby prevent migration of carbon to the cathode.
Accordingly, the present invention provides an electrolytic cell for reducing a metal oxide in a solid state, which electrolytic cell includes an anode formed from carbon, a cathode formed at least in part from the g _ metal oxide, and a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms positioned between the cathode and the anode to thereby prevent migration of carbon to the cathode.
material.
Preferably, the anode is formed from graphite.
The membrane may be formed from any suitable Preferably, the membrane is formed from a solid electrolyte.
One suitable solid electrolyte tested by the applicant is yttria stabilised zirconia.
Preferably, the cathode also includes an electrical conductor.
The present invention also provides a method of reducing a metal oxide in a solid state using the above-described electrolytic cell.
Preferably, the method includes a step of operating the cell at a potential that is above a decomposition potential of at least one of the constituents of the electrolyte so that there are rations of a metal other than that of the metal oxide in the electrolyte.
In a situation in which the metal oxide is a titanium oxide, such as titania, it is preferred that the electrolyte be a CaClz-based electrolyte that includes Ca0 as one of constituents.
In such a situation it is preferred that the cell potential be above the decomposition potential for CaO.
It is also preferred that the cell potential be below the decomposition potential for CaCl2.
It is preferred that the cell potential be less than or equal to 3.0 V.
It is preferred particularly that the cell potential be below 2.5 V, It is preferred more particularly that the cell potential be below 2.0 V.
It is preferred that the cell potential be above 1.5 V.
The CaCl2-based electrolyte may be a commercially available source of CaCl2, such as calcium chloride dehydrate, that partially decomposes on heating and produces Ca0 or otherwise includes CaO.
Alternatively, or in addition, the CaClz-based electrolyte may include CaClz and Ca0 that are added separately or pre-mixed to form the electrolyte.
The present invention is described further with reference to the following Example that relates to experimental work on the above-described electrolytic cell.
As indicated above, the cell included a high density graphite crucible that formed the anode of the cell, a pool of molten CaCl2 electrolyte in the crucible, and a cathode that included solid titanic. In the initial experimental set-up the solid titanic was in the form of titanic pellets connected to a lower end of a Kanthal or stainless steel electrically conductive wire.
As indicated above, experimental work on the cell identified carbon transfer as a significant issue in terms of contamination of cathode titanium and causing low energy efficiency of the cell. Tn addition, as indicated above, the experimental work established that carbon transfer was caused by an electrochemical reaction at the anode.
Thereafter the applicant carried out experimental work to investigate whether it was possible to prevent migration of carbon from the anode to the cathode.
One experiment investigated the impact of a solid ionic barrier on carbon migration.
The ionic barrier was in the form of a yttria stabilised zirconia membrane positioned between the anode and the cathode, thereby dividing the cell into an outer anode chamber and an inner cathode chamber.
Figure 1 is a schematic of the cell set-up for the experiment. With reference to the Figure, the cell included a graphite crucible 3 that formed the anode, a pool 19 of molten CaCl2 electrolyte in the crucible, titania pellets 5 and an electrically conductive wire 7 that formed the cathode immersed in the electrolyte, and a yttria stabilised zirconia membrane 9 immersed in the electrolyte between the anode and the cathode. The cell was located in a resistance furnace 11 heated to a temperature to maintain the electrolyte in a molten state.
The experimental set-up also included gas monitoring, cleaning, and analysis equipment. The cell was operated at an applied potential of 3V for a period of 35 hours, during which time there was continuous monitoring of the off-gas from the furnace. At the conclusion of the experiment, the cell was cooled and the solidified electrolyte, the membrane, the anode and the cathode were analysed.
Figure 2 is a summary of the results of the experiment.
Figure 2 shows measured voltage, current, CO and C02 composition of the off-gas for the experiment.
Visual and analytical examination of the cathode and the cathode chamber indicated that there was no carbon on the cathode and in the cathode chamber.
In addition, the visual and analytical examination of the cathode indicated that titania was reduced to titanium. It follows from this finding that the yttria stabilised zirconia membrane did not restrict migration of O-- anions from the cathode to the anode.
Many modifications may be made to the present invention as described above without departing from the spirit and scope of the invention.
By way of example, whilst the above description of the invention focuses on reduction of titania, the invention is not so limited and extends to electrolytic reduction of other titanium oxides and to oxides of other metals and alloys.
Examples of other potentially important meals are aluminium, silicon, germanium, hafnium, magnesium, and molybdenum.
Furthermore, whilst the above description focuses on CaCl2-based electrolyte, the invention is not so limited and extends to any other suitable electrolytes.
_ g _ Generally, suitable electrolytes will be salts and oxides that are soluble in salts. One example of a potentially suitable electrolyte is BaCl2.
The present invention relates to reduction of metal oxides in a solid state in an electrolytic cell.
The present invention was made during the course of an on-going research project on solid state reduction of titania (Ti02) carried out by the applicant.
During the course of the research project the applicant carried out experimental work on the reduction of titania using an electrolytic cell that included a graphite crucible that formed an anode of the cell, a pool of molten CaCl2-based electrolyte in the crucible, and a range of cathodes that included solid titania.
The CaCl2-based electrolyte was a commercially available source of CaCl2, namely calcium chloride dihydrate, that partially decomposed on heating and produced CaO.
The applicant operated the electrolytic cell at a potential above the decomposition potential of Ca0 and below the decomposition potential of CaCl2.
The applicant found that the cell could electrochemically reduce titania to titanium with very low concentrations of oxygen.
The applicant does not have a clear understanding of the electrolytic cell mechanism at this stage.
Nevertheless, whilst not wishing to be bound by the comments in this and the following paragraphs, the applicant offers the following comments by way of an outline of a possible cell mechanism.
The experimental work carried out by the applicant produced evidence of Ca metal dissolved in the electrolyte. The applicant. believes that, at least during the early stages of operation of the cell, the Ca metal was the result of electrodeposition of Ca~+ cations as Ca metal on electrically conductive sections of the cathode.
The experimental work was carried out using a CaCl2-based electrolyte at a cell potential below the decomposition potential of CaCl2. The applicant believes that the initial deposition of Ca metal on the cathode was due to the presence of Ca++-cations and O-- anions derived from CaO in the electrolyte. The decomposition potential of Ca0 is less 'than the decomposition potential of CaClz.
In this cell mechanism the-.cell operation is dependent, at least during the early stages of cell operation, on decomposition of CaO, with Ca++ cations migrating to the cathode and depositing as Ca metal and O-- anions migrating to the anode and forming CO and/or COz (in a situation, in which the anode is a graphite anode).
The applicant believes that the Ca metal that deposited on electrically conductive sections of the cathode was deposited predominantly as a separate phase in the early stages of cell operation and thereafter dissolved in the electrolyte and migrated to the vicinity of the titania in the cathode and participated in chemical reduction of titania.
The applicant also believes that at later stages of the cell operation part of the Ca metal that deposited on the cathode was deposited directly on partially deoxidised titanium and thereafter participated in chemical reduction of titanium.
The applicant also believes that the O'- anions, once extracted from the titania, migrated to the anode and reacted with anode carbon and produced CO and/or C02 (and in some instances Ca0) and released electrons that facilitated electrolytic deposition of Ga metal on the cathode.
However, notwithstanding that the cell could electrochemically reduce titania to titanium with very low concentrations of oxygen, the applicant also found that there were relatively significant amounts of carbon transferred from the anode to the electrolyte and to the titanium produced at the cathode under a wide range of cell operating conditions.
Carbon in the titanium is an undesirable contaminant. In addition, carbon transfer was partially responsible for low energy efficiency of the cell. Both problems are significant barriers to commercialisation of electrolytic reduction technology.
The applicant carried out experimental work to identify the mechanism for carbon transfer and to determine how to minimise carbon transfer and/or to minimise the adverse effects of carbon transfer.
The experimental work indicated that the mechanism of carbon transfer is electrochemical rather than erosion and that one way of minimising carbon transfer and therefore contamination of titanium produced at the cathode by electrochemical reduction of titania at the cathode is to position a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms between the cathode and the anode anal thereby prevent migration of carbon to the cathode.
Accordingly, the present invention provides an electrolytic cell for reducing a metal oxide in a solid state, which electrolytic cell includes an anode formed from carbon, a cathode formed at least in part from the g _ metal oxide, and a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms positioned between the cathode and the anode to thereby prevent migration of carbon to the cathode.
material.
Preferably, the anode is formed from graphite.
The membrane may be formed from any suitable Preferably, the membrane is formed from a solid electrolyte.
One suitable solid electrolyte tested by the applicant is yttria stabilised zirconia.
Preferably, the cathode also includes an electrical conductor.
The present invention also provides a method of reducing a metal oxide in a solid state using the above-described electrolytic cell.
Preferably, the method includes a step of operating the cell at a potential that is above a decomposition potential of at least one of the constituents of the electrolyte so that there are rations of a metal other than that of the metal oxide in the electrolyte.
In a situation in which the metal oxide is a titanium oxide, such as titania, it is preferred that the electrolyte be a CaClz-based electrolyte that includes Ca0 as one of constituents.
In such a situation it is preferred that the cell potential be above the decomposition potential for CaO.
It is also preferred that the cell potential be below the decomposition potential for CaCl2.
It is preferred that the cell potential be less than or equal to 3.0 V.
It is preferred particularly that the cell potential be below 2.5 V, It is preferred more particularly that the cell potential be below 2.0 V.
It is preferred that the cell potential be above 1.5 V.
The CaCl2-based electrolyte may be a commercially available source of CaCl2, such as calcium chloride dehydrate, that partially decomposes on heating and produces Ca0 or otherwise includes CaO.
Alternatively, or in addition, the CaClz-based electrolyte may include CaClz and Ca0 that are added separately or pre-mixed to form the electrolyte.
The present invention is described further with reference to the following Example that relates to experimental work on the above-described electrolytic cell.
As indicated above, the cell included a high density graphite crucible that formed the anode of the cell, a pool of molten CaCl2 electrolyte in the crucible, and a cathode that included solid titanic. In the initial experimental set-up the solid titanic was in the form of titanic pellets connected to a lower end of a Kanthal or stainless steel electrically conductive wire.
As indicated above, experimental work on the cell identified carbon transfer as a significant issue in terms of contamination of cathode titanium and causing low energy efficiency of the cell. Tn addition, as indicated above, the experimental work established that carbon transfer was caused by an electrochemical reaction at the anode.
Thereafter the applicant carried out experimental work to investigate whether it was possible to prevent migration of carbon from the anode to the cathode.
One experiment investigated the impact of a solid ionic barrier on carbon migration.
The ionic barrier was in the form of a yttria stabilised zirconia membrane positioned between the anode and the cathode, thereby dividing the cell into an outer anode chamber and an inner cathode chamber.
Figure 1 is a schematic of the cell set-up for the experiment. With reference to the Figure, the cell included a graphite crucible 3 that formed the anode, a pool 19 of molten CaCl2 electrolyte in the crucible, titania pellets 5 and an electrically conductive wire 7 that formed the cathode immersed in the electrolyte, and a yttria stabilised zirconia membrane 9 immersed in the electrolyte between the anode and the cathode. The cell was located in a resistance furnace 11 heated to a temperature to maintain the electrolyte in a molten state.
The experimental set-up also included gas monitoring, cleaning, and analysis equipment. The cell was operated at an applied potential of 3V for a period of 35 hours, during which time there was continuous monitoring of the off-gas from the furnace. At the conclusion of the experiment, the cell was cooled and the solidified electrolyte, the membrane, the anode and the cathode were analysed.
Figure 2 is a summary of the results of the experiment.
Figure 2 shows measured voltage, current, CO and C02 composition of the off-gas for the experiment.
Visual and analytical examination of the cathode and the cathode chamber indicated that there was no carbon on the cathode and in the cathode chamber.
In addition, the visual and analytical examination of the cathode indicated that titania was reduced to titanium. It follows from this finding that the yttria stabilised zirconia membrane did not restrict migration of O-- anions from the cathode to the anode.
Many modifications may be made to the present invention as described above without departing from the spirit and scope of the invention.
By way of example, whilst the above description of the invention focuses on reduction of titania, the invention is not so limited and extends to electrolytic reduction of other titanium oxides and to oxides of other metals and alloys.
Examples of other potentially important meals are aluminium, silicon, germanium, hafnium, magnesium, and molybdenum.
Furthermore, whilst the above description focuses on CaCl2-based electrolyte, the invention is not so limited and extends to any other suitable electrolytes.
_ g _ Generally, suitable electrolytes will be salts and oxides that are soluble in salts. One example of a potentially suitable electrolyte is BaCl2.
Claims (14)
1. An electrolytic cell for reducing a metal oxide in a solid state, which electrolytic cell includes an anode formed from carbon, a cathode formed at least in part from the metal oxide, and a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms positioned between the cathode and the anode to thereby prevent migration of carbon to the cathode.
2. The cell defined in claim 1 wherein the anode is formed from graphite.
3. The cell defined in claim 1 or claim 2 wherein the membrane is formed from a solid electrolyte.
4. The cell defined in claim 3 wherein the solid electrolyte is yttria stabilised zirconia.
5. The cell defined in any one of the preceding claims wherein the cathode also includes an electrical conductor.
6. A method of reducing a metal oxide in a solid state using an electrolytic cell that includes an anode formed from carbon, a cathode formed at least in part from the metal oxide, and a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms positioned between the cathode and the anode to thereby prevent migration of carbon to the cathode, which method includes operating the cell at a potential that electrolytically reduces the metal oxide.
7. The method defined in claim 6 includes operating the cell at a potential that is above a decomposition potential of at least one of the constituents of the electrolyte so that there are cations of a metal other than that of the metal oxide in the electrolyte.
8. The method defined in claim 6 or claim 7 wherein the metal oxide is a titanium oxide, such as titania and the electrolyte is a CaCl2-based electrolyte that includes CaO as one of constituents.
9. The method defined in claim 8 includes operating the cell at a potential that is above the decomposition potential for CaO.
10. The method defined in claim 8 or claim 9 includes operating the cell at a potential that is below the decomposition potential for CaCl2.
11. The method defined in any one of claims 6 to 10 wherein the cell potential is less than or equal to 3.0 V.
12. The method defined in claim 11 wherein the cell potential is below 2.5 V.
13. The method defined in claim 12 wherein the cell potential is below 2.0 V.
14. The method defined in any one of claims 6 to 13 wherein the cell potential is above 1.5 V.
Applications Claiming Priority (3)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| AUPS1170 | 2002-03-13 | ||
| AUPS1170A AUPS117002A0 (en) | 2002-03-13 | 2002-03-13 | Minimising carbon transfer in an electrolytic cell |
| PCT/AU2003/000305 WO2003076692A1 (en) | 2002-03-13 | 2003-03-13 | Minimising carbon transfer in an electrolytic cell |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| CA2479050A1 true CA2479050A1 (en) | 2003-09-18 |
Family
ID=3834768
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA002479050A Abandoned CA2479050A1 (en) | 2002-03-13 | 2003-03-13 | Minimising carbon transfer in an electrolytic cell |
Country Status (12)
| Country | Link |
|---|---|
| US (1) | US20050092129A1 (en) |
| EP (1) | EP1483431B1 (en) |
| JP (1) | JP2005520046A (en) |
| CN (1) | CN1650052A (en) |
| AT (1) | ATE367461T1 (en) |
| AU (1) | AUPS117002A0 (en) |
| CA (1) | CA2479050A1 (en) |
| DE (1) | DE60314999D1 (en) |
| MX (1) | MXPA04008886A (en) |
| RU (1) | RU2302482C2 (en) |
| WO (1) | WO2003076692A1 (en) |
| ZA (1) | ZA200407433B (en) |
Families Citing this family (5)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| AU2002951962A0 (en) * | 2002-10-09 | 2002-10-24 | Bhp Billiton Innovation Pty Ltd | Electrolytic reduction of metal oxides |
| AU2002952083A0 (en) | 2002-10-16 | 2002-10-31 | Bhp Billiton Innovation Pty Ltd | Minimising carbon transfer in an electrolytic cell |
| BRPI0512782A (en) * | 2004-06-28 | 2008-04-08 | Bhp Billiton Innovation Pty | method for producing ready-to-use or semi-finished titanium metal and ready-to-use titanium metal products |
| EA014138B1 (en) * | 2005-08-01 | 2010-10-29 | БиЭйчПи БИЛЛИТОН ИННОВЕЙШН ПТИ ЛТД. | Electrochemical reduction of metal oxides |
| WO2007092398A2 (en) * | 2006-02-06 | 2007-08-16 | E. I. Du Pont De Nemours And Company | Method for electrolytic production of titanium and other metal powders |
Family Cites Families (11)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| JPH07113158B2 (en) * | 1984-04-14 | 1995-12-06 | 新日本製鐵株式会社 | Method of cleaning molten steel |
| JPH03115592A (en) * | 1989-09-28 | 1991-05-16 | Osaka Titanium Co Ltd | Molten salt electrolytic cell |
| US5670270A (en) * | 1995-11-16 | 1997-09-23 | The Dow Chemical Company | Electrode structure for solid state electrochemical devices |
| GB9812169D0 (en) * | 1998-06-05 | 1998-08-05 | Univ Cambridge Tech | Purification method |
| US6187168B1 (en) * | 1998-10-06 | 2001-02-13 | Aluminum Company Of America | Electrolysis in a cell having a solid oxide ion conductor |
| EP1257678B1 (en) * | 2000-02-22 | 2007-09-05 | Metalysis Limited | Method for the manufacture of metal foams by electrolytic reduction of porous oxidic preforms |
| GB2359564B (en) * | 2000-02-22 | 2004-09-29 | Secr Defence | Improvements in the electrolytic reduction of metal oxides |
| US6540902B1 (en) * | 2001-09-05 | 2003-04-01 | The United States Of America As Represented By The United States Department Of Energy | Direct electrochemical reduction of metal-oxides |
| JP4089944B2 (en) * | 2001-11-30 | 2008-05-28 | 財団法人電力中央研究所 | Electrolytic reduction apparatus and method |
| KR101038701B1 (en) * | 2002-03-13 | 2011-06-02 | 비에이치피 빌리튼 이노베이션 피티와이 리미티드 | Reduction of metal oxides in an elecrolytic cell |
| JP4252531B2 (en) * | 2004-12-15 | 2009-04-08 | 株式会社大阪チタニウムテクノロジーズ | Metal manufacturing method |
-
2002
- 2002-03-13 AU AUPS1170A patent/AUPS117002A0/en not_active Abandoned
-
2003
- 2003-03-13 AT AT03743766T patent/ATE367461T1/en not_active IP Right Cessation
- 2003-03-13 RU RU2004130453/02A patent/RU2302482C2/en not_active IP Right Cessation
- 2003-03-13 JP JP2003574884A patent/JP2005520046A/en active Pending
- 2003-03-13 CN CNA038092743A patent/CN1650052A/en active Pending
- 2003-03-13 DE DE60314999T patent/DE60314999D1/en not_active Expired - Lifetime
- 2003-03-13 CA CA002479050A patent/CA2479050A1/en not_active Abandoned
- 2003-03-13 MX MXPA04008886A patent/MXPA04008886A/en not_active Application Discontinuation
- 2003-03-13 WO PCT/AU2003/000305 patent/WO2003076692A1/en active IP Right Grant
- 2003-03-13 EP EP03743766A patent/EP1483431B1/en not_active Expired - Lifetime
-
2004
- 2004-09-10 US US10/939,001 patent/US20050092129A1/en not_active Abandoned
- 2004-09-16 ZA ZA200407433A patent/ZA200407433B/en unknown
Also Published As
| Publication number | Publication date |
|---|---|
| EP1483431B1 (en) | 2007-07-18 |
| DE60314999D1 (en) | 2007-08-30 |
| RU2302482C2 (en) | 2007-07-10 |
| ATE367461T1 (en) | 2007-08-15 |
| ZA200407433B (en) | 2005-10-10 |
| US20050092129A1 (en) | 2005-05-05 |
| RU2004130453A (en) | 2005-06-10 |
| JP2005520046A (en) | 2005-07-07 |
| AUPS117002A0 (en) | 2002-04-18 |
| EP1483431A1 (en) | 2004-12-08 |
| MXPA04008886A (en) | 2004-11-26 |
| EP1483431A4 (en) | 2006-06-28 |
| WO2003076692A1 (en) | 2003-09-18 |
| CN1650052A (en) | 2005-08-03 |
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Legal Events
| Date | Code | Title | Description |
|---|---|---|---|
| FZDE | Discontinued |