CA2265183C - Magnesium metal production - Google Patents
Magnesium metal production Download PDFInfo
- Publication number
- CA2265183C CA2265183C CA002265183A CA2265183A CA2265183C CA 2265183 C CA2265183 C CA 2265183C CA 002265183 A CA002265183 A CA 002265183A CA 2265183 A CA2265183 A CA 2265183A CA 2265183 C CA2265183 C CA 2265183C
- Authority
- CA
- Canada
- Prior art keywords
- anode
- cell
- magnesium
- chloride
- hydrogen
- 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 - Fee Related
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- FYYHWMGAXLPEAU-UHFFFAOYSA-N Magnesium Chemical compound [Mg] FYYHWMGAXLPEAU-UHFFFAOYSA-N 0.000 title claims abstract description 29
- 238000004519 manufacturing process Methods 0.000 title claims description 22
- TWRXJAOTZQYOKJ-UHFFFAOYSA-L Magnesium chloride Chemical compound [Mg+2].[Cl-].[Cl-] TWRXJAOTZQYOKJ-UHFFFAOYSA-L 0.000 claims abstract description 36
- UFHFLCQGNIYNRP-UHFFFAOYSA-N Hydrogen Chemical compound [H][H] UFHFLCQGNIYNRP-UHFFFAOYSA-N 0.000 claims abstract description 27
- 238000000034 method Methods 0.000 claims abstract description 23
- 229910001629 magnesium chloride Inorganic materials 0.000 claims abstract description 18
- VEXZGXHMUGYJMC-UHFFFAOYSA-N Hydrochloric acid Chemical compound Cl VEXZGXHMUGYJMC-UHFFFAOYSA-N 0.000 claims abstract description 17
- IXCSERBJSXMMFS-UHFFFAOYSA-N hydrogen chloride Substances Cl.Cl IXCSERBJSXMMFS-UHFFFAOYSA-N 0.000 claims abstract description 15
- 229910000041 hydrogen chloride Inorganic materials 0.000 claims abstract description 15
- KZBUYRJDOAKODT-UHFFFAOYSA-N Chlorine Chemical compound ClCl KZBUYRJDOAKODT-UHFFFAOYSA-N 0.000 claims abstract description 11
- VEXZGXHMUGYJMC-UHFFFAOYSA-M Chloride anion Chemical compound [Cl-] VEXZGXHMUGYJMC-UHFFFAOYSA-M 0.000 claims abstract description 6
- 238000005868 electrolysis reaction Methods 0.000 claims abstract description 6
- 239000011777 magnesium Substances 0.000 claims description 20
- 229910052749 magnesium Inorganic materials 0.000 claims description 18
- OKTJSMMVPCPJKN-UHFFFAOYSA-N Carbon Chemical compound [C] OKTJSMMVPCPJKN-UHFFFAOYSA-N 0.000 claims description 10
- 239000003792 electrolyte Substances 0.000 claims description 10
- 229910002804 graphite Inorganic materials 0.000 claims description 7
- 239000010439 graphite Substances 0.000 claims description 7
- 150000003839 salts Chemical class 0.000 claims description 7
- 230000015572 biosynthetic process Effects 0.000 claims description 6
- 239000006227 byproduct Substances 0.000 claims description 6
- 239000012466 permeate Substances 0.000 claims description 6
- 239000011148 porous material Substances 0.000 claims description 6
- 229910052581 Si3N4 Inorganic materials 0.000 claims description 5
- 239000001257 hydrogen Substances 0.000 claims description 5
- 229910052739 hydrogen Inorganic materials 0.000 claims description 5
- 238000011084 recovery Methods 0.000 claims description 5
- HBMJWWWQQXIZIP-UHFFFAOYSA-N silicon carbide Chemical compound [Si+]#[C-] HBMJWWWQQXIZIP-UHFFFAOYSA-N 0.000 claims description 5
- 229910010271 silicon carbide Inorganic materials 0.000 claims description 5
- HQVNEWCFYHHQES-UHFFFAOYSA-N silicon nitride Chemical compound N12[Si]34N5[Si]62N3[Si]51N64 HQVNEWCFYHHQES-UHFFFAOYSA-N 0.000 claims description 5
- 229910052799 carbon Inorganic materials 0.000 claims description 3
- 238000011065 in-situ storage Methods 0.000 claims description 2
- 230000007423 decrease Effects 0.000 description 4
- ZAMOUSCENKQFHK-UHFFFAOYSA-N Chlorine atom Chemical compound [Cl] ZAMOUSCENKQFHK-UHFFFAOYSA-N 0.000 description 3
- 238000006243 chemical reaction Methods 0.000 description 3
- 239000000460 chlorine Substances 0.000 description 3
- 229910052801 chlorine Inorganic materials 0.000 description 3
- 238000000354 decomposition reaction Methods 0.000 description 3
- 239000007789 gas Substances 0.000 description 2
- 239000000463 material Substances 0.000 description 2
- 238000003786 synthesis reaction Methods 0.000 description 2
- 229910001514 alkali metal chloride Inorganic materials 0.000 description 1
- 150000001340 alkali metals Chemical class 0.000 description 1
- 229910001617 alkaline earth metal chloride Inorganic materials 0.000 description 1
- 150000008280 chlorinated hydrocarbons Chemical class 0.000 description 1
- 238000004891 communication Methods 0.000 description 1
- 238000009792 diffusion process Methods 0.000 description 1
- 238000007599 discharging Methods 0.000 description 1
- 230000005611 electricity Effects 0.000 description 1
- 230000007613 environmental effect Effects 0.000 description 1
- -1 for example Substances 0.000 description 1
- 238000013021 overheating Methods 0.000 description 1
- 238000003860 storage Methods 0.000 description 1
Classifications
-
- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
- C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
- C25C3/04—Electrolytic production, recovery or refining of metals by electrolysis of melts of magnesium
Landscapes
- Chemical & Material Sciences (AREA)
- Engineering & Computer Science (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Electrochemistry (AREA)
- Materials Engineering (AREA)
- Metallurgy (AREA)
- Organic Chemistry (AREA)
- Electrolytic Production Of Metals (AREA)
- Manufacture And Refinement Of Metals (AREA)
Abstract
Magnesium metal is produced by electrolysis of magnesium chloride employing a high surface area anode, for example, a porous anode to which hydrogen gas is fed. Hydrogen chloride is formed from the chloride ions at the anode, rather than chlorine gas; the process also has the advantage of operating at a lower voltage with a lower energy requirement than the conventional process in which chlorine gas is generated at the anode.
Description
This invention relates to production of magnesium by electrolysis.
Conventional electrolytic production of magnesium from magnesium chloride dissolved in a molten salt electrolyte in an electrolytic cell results in formation of magnesium at the cathode and chlorine gas at the cathode. The molten salt electrolyte typically comprises one or more alkali metal or alkaline earth metal chlorides in which the magnesium chloride is dissolved.
The production of chlorine as a by-product of the production of magnesium requires auxiliary equipment for recovery and storage of the by-product chlorine gas which typically is reacted with hydrogen gas to form hydrochloric acid. Electrolytic methods for producing magnesium are described in U.S. Patents 4,073,703; 4,192,724; 5,089,094 and 5,665,220. :
This invention seeks to provide a new electrolytic process for the production of magnesium from magnesium chloride, in which hydrogen chloride is produced as the by-product.
This invention also seeks to provide a new electrolytic process for the production of magnesium from magnesium chloride at a lower energy requirement.
In accordance with one aspect of the invention there is provided in a process for the electrolytic production of magnesium from magnesium chloride in an electrolytic cell having an anode and a cathode, and in which magnesium is generated at the cathode, the improvement wherein hydrogen gas is fed to the anode and hydrogen chloride is formed in situ at the anode.
In accordance with another aspect of the invention there is provided a process for the electrolytic production of magnesium comprising: i) electrolysing magnesium chloride in a molten salt electrolyte in an electrolysis cell having a cathode and an anode, with formation of magnesium metal at said cathode, ii) feeding hydrogen gas to said anode and reacting chloride ions at said anode with the hydrogen gas to form hydrogen chloride, iii) recovering the magnesium metal from said cell, and iv) recovering the hydrogen chloride from said cell.
In accordance with still another aspect of the invention there is provided an electrolytic cell for production of magnesium metal from magnesium chloride comprising: a) a cell for housing magnesium chloride in a molten salt electrolyte, said cell having a cathode and an anode, b) means for feeding hydrogen gas to said anode, c) means for recovery from said cell of magnesium metal developed at said cathode, and d) means for recovery from said cell of hydrogen chloride developed at said anode.
In accordance with yet another aspect of the invention there is provided use of hydrogen in an electrolytic cell for the production of magnesium from magnesium chloride with production of by-product hydrogen chloride at the anode.
In particular the anode is a high surface area anode, for example, a porous anode in which case the hydrogen gas permeates the pores of the anode, such as by diffusion, or molten electrolyte containing the magnesium chloride permeates the pores of the anode, to provide the contact between the hydrogen gas and the chloride ions. The hydrogen gas may be fed along a non-porous tube or conduit to the porous anode. If this tube or conduit is in contact with the bath it should not be of a material which will function as an anode for the electrolysis.
As an alternative to a porous anode, any anode having a structure permitting delivery of hydrogen to the cell bath at the anode may be employed, for example, an anode having drilled channels for communication with a source of hydrogen gas. The requirement is that the anode structure deliver hydrogen gas to the cell bath at the anode, so that chloride ions at the anode react with the hydrogen gas to form hydrogen chloride, rather than discharging as chlorine gas.
Conventional electrolytic production of magnesium from magnesium chloride dissolved in a molten salt electrolyte in an electrolytic cell results in formation of magnesium at the cathode and chlorine gas at the cathode. The molten salt electrolyte typically comprises one or more alkali metal or alkaline earth metal chlorides in which the magnesium chloride is dissolved.
The production of chlorine as a by-product of the production of magnesium requires auxiliary equipment for recovery and storage of the by-product chlorine gas which typically is reacted with hydrogen gas to form hydrochloric acid. Electrolytic methods for producing magnesium are described in U.S. Patents 4,073,703; 4,192,724; 5,089,094 and 5,665,220. :
This invention seeks to provide a new electrolytic process for the production of magnesium from magnesium chloride, in which hydrogen chloride is produced as the by-product.
This invention also seeks to provide a new electrolytic process for the production of magnesium from magnesium chloride at a lower energy requirement.
In accordance with one aspect of the invention there is provided in a process for the electrolytic production of magnesium from magnesium chloride in an electrolytic cell having an anode and a cathode, and in which magnesium is generated at the cathode, the improvement wherein hydrogen gas is fed to the anode and hydrogen chloride is formed in situ at the anode.
In accordance with another aspect of the invention there is provided a process for the electrolytic production of magnesium comprising: i) electrolysing magnesium chloride in a molten salt electrolyte in an electrolysis cell having a cathode and an anode, with formation of magnesium metal at said cathode, ii) feeding hydrogen gas to said anode and reacting chloride ions at said anode with the hydrogen gas to form hydrogen chloride, iii) recovering the magnesium metal from said cell, and iv) recovering the hydrogen chloride from said cell.
In accordance with still another aspect of the invention there is provided an electrolytic cell for production of magnesium metal from magnesium chloride comprising: a) a cell for housing magnesium chloride in a molten salt electrolyte, said cell having a cathode and an anode, b) means for feeding hydrogen gas to said anode, c) means for recovery from said cell of magnesium metal developed at said cathode, and d) means for recovery from said cell of hydrogen chloride developed at said anode.
In accordance with yet another aspect of the invention there is provided use of hydrogen in an electrolytic cell for the production of magnesium from magnesium chloride with production of by-product hydrogen chloride at the anode.
In particular the anode is a high surface area anode, for example, a porous anode in which case the hydrogen gas permeates the pores of the anode, such as by diffusion, or molten electrolyte containing the magnesium chloride permeates the pores of the anode, to provide the contact between the hydrogen gas and the chloride ions. The hydrogen gas may be fed along a non-porous tube or conduit to the porous anode. If this tube or conduit is in contact with the bath it should not be of a material which will function as an anode for the electrolysis.
As an alternative to a porous anode, any anode having a structure permitting delivery of hydrogen to the cell bath at the anode may be employed, for example, an anode having drilled channels for communication with a source of hydrogen gas. The requirement is that the anode structure deliver hydrogen gas to the cell bath at the anode, so that chloride ions at the anode react with the hydrogen gas to form hydrogen chloride, rather than discharging as chlorine gas.
By way of example, suitable anodes may be of graphite, silicon carbide or silicon nitride.
It has been found that introducing hydrogen at the anode in the electrolytic cell for magnesium metal production results in a lower energy requirement for the cell, and the cell can be operated at a cell voltage lower than the cell voltage of a corresponding cell having a conventional carbon or graphite anode, without hydrogen gas.
In addition it is found that hydrogen chloride is formed directly at the anode by the reaction:
2C1- + H2(g) = 2HChg) + 2e where (g) indicates the gas phase.
Furthermore, the method has the advantage that this hydrogen chloride gas is produced with minimal, if any, production of chlorine gas.
In conventional cells in which chlorine gas is produced as the by-product, the anode is graphite, and at the high temperatures of operation some chlorinated hydrocarbons are produced by reaction between the chlorine gas and the carbon anode, and this presents environmental problems. Eliminating production of chlorine gas in the present invention can be expected to alleviate these problems.
Table I below shows how the decomposition voltage of the electrolysis decreases, with the process of the invention, as compared with the conventional process and how the minimum voltage required to maintain energy balance changes.
It has been found that introducing hydrogen at the anode in the electrolytic cell for magnesium metal production results in a lower energy requirement for the cell, and the cell can be operated at a cell voltage lower than the cell voltage of a corresponding cell having a conventional carbon or graphite anode, without hydrogen gas.
In addition it is found that hydrogen chloride is formed directly at the anode by the reaction:
2C1- + H2(g) = 2HChg) + 2e where (g) indicates the gas phase.
Furthermore, the method has the advantage that this hydrogen chloride gas is produced with minimal, if any, production of chlorine gas.
In conventional cells in which chlorine gas is produced as the by-product, the anode is graphite, and at the high temperatures of operation some chlorinated hydrocarbons are produced by reaction between the chlorine gas and the carbon anode, and this presents environmental problems. Eliminating production of chlorine gas in the present invention can be expected to alleviate these problems.
Table I below shows how the decomposition voltage of the electrolysis decreases, with the process of the invention, as compared with the conventional process and how the minimum voltage required to maintain energy balance changes.
TABLE I
Reaction E Eadiab. Eadiab. - E
MgC12 4 Mg + C12 2.50 3.60 1.1 MgCl2 + H2 4 Mg + HCI 1.46 2.74 1.28 Difference -1.04 -0.86 0.18 In Table I, Eadiab is the minimum voltage required to carry out the process, assuming 100% current efficiency and that the MgC12 and H2 are fed at room temperature.
In particular, Table I shows the calculated decomposition voltage (1000 K) and adiabatic voltage required to cover the energy requirements of the process without heat losses.
Table I further shows that the decomposition voltage decreases by 1.04V
and that the overall energy requirement decreases by 0.86V. This means that with HCI formation, another 0.18V per mole can be dissipated in the cell without causing overheating. The decrease of 0.86V translates to a reduction of about 25% less electricity consumption for magnesium production. With magnesium cells currently requiring an average of 12.5 MW-hr per tonne, and an average energy cost of 4 cents per KW-hrs, this translates to a savings of about $125 per tonne of magnesium produced in electrical consumption.
Another major cost saving comes from the fact that the cell is producing HC1 rather than chlorine, requiring no HC1 synthesis plant. Chlorine treatment and handling as well as HC1 synthesis can provide for further cost savings.
Environmetal problems associated with chlorine gas production are expected to be alleviated.
The hydrogen gas may be considered to form a hydrogen anode in the cell, for discharge of the chloride ions. In such case an anode structure is provided which, can be of any suitable material, for example, graphite, silicon carbide or silicon nitride.
Reaction E Eadiab. Eadiab. - E
MgC12 4 Mg + C12 2.50 3.60 1.1 MgCl2 + H2 4 Mg + HCI 1.46 2.74 1.28 Difference -1.04 -0.86 0.18 In Table I, Eadiab is the minimum voltage required to carry out the process, assuming 100% current efficiency and that the MgC12 and H2 are fed at room temperature.
In particular, Table I shows the calculated decomposition voltage (1000 K) and adiabatic voltage required to cover the energy requirements of the process without heat losses.
Table I further shows that the decomposition voltage decreases by 1.04V
and that the overall energy requirement decreases by 0.86V. This means that with HCI formation, another 0.18V per mole can be dissipated in the cell without causing overheating. The decrease of 0.86V translates to a reduction of about 25% less electricity consumption for magnesium production. With magnesium cells currently requiring an average of 12.5 MW-hr per tonne, and an average energy cost of 4 cents per KW-hrs, this translates to a savings of about $125 per tonne of magnesium produced in electrical consumption.
Another major cost saving comes from the fact that the cell is producing HC1 rather than chlorine, requiring no HC1 synthesis plant. Chlorine treatment and handling as well as HC1 synthesis can provide for further cost savings.
Environmetal problems associated with chlorine gas production are expected to be alleviated.
The hydrogen gas may be considered to form a hydrogen anode in the cell, for discharge of the chloride ions. In such case an anode structure is provided which, can be of any suitable material, for example, graphite, silicon carbide or silicon nitride.
Claims (17)
1. In a process for the electrolytic production of magnesium from magnesium chloride in an electrolytic cell having an anode and a cathode, and in which magnesium is generated at the cathode, the improvement wherein hydrogen gas is fed to the anode and hydrogen chloride is formed in situ at the anode.
2. A process according to claim 1, wherein the anode is a high surface area anode.
3. A process according to claim 1, wherein the anode is a porous anode and the hydrogen gas permeates the pores of the anode.
4. A process according to claim 1, wherein said magnesium chloride is dissolved in a molten salt electrolyte in said cell, said anode is a porous anode and the molten electrolyte permeates the pores of the porous anode.
5. A process according to claim 1, 2, 3 or 4, wherein the anode is of graphite, silicon carbide or silicon nitride.
6. A process for the electrolytic production of magnesium comprising:
i) ~electrolysing magnesium chloride in a molten salt electrolyte in an electrolysis cell having a cathode and an anode, with formation of magnesium metal at said cathode, ii) ~feeding hydrogen gas to said anode and reacting chloride ions at said anode with the hydrogen gas to form hydrogen chloride, iii) ~recovering the magnesium metal from said cell, and iv) ~recovering the hydrogen chloride from said cell.
i) ~electrolysing magnesium chloride in a molten salt electrolyte in an electrolysis cell having a cathode and an anode, with formation of magnesium metal at said cathode, ii) ~feeding hydrogen gas to said anode and reacting chloride ions at said anode with the hydrogen gas to form hydrogen chloride, iii) ~recovering the magnesium metal from said cell, and iv) ~recovering the hydrogen chloride from said cell.
7. A process according to claim 6, wherein said cell is operated at a cell voltage lower than the cell voltage of a corresponding cell having a carbon anode, without hydrogen gas, in which chlorine gas is developed at the anode.
8. A process according to claim 6 or 7, wherein said anode is a high surface area anode.
9. A process according to claim 6 or 7, wherein said anode is a porous anode and the hydrogen gas permeates from the pores of the anode into the cell.
10. A process according to claim 6 or 7, wherein said anode is a porous anode and the molten electrolyte permeates the pores of the porous anode.
11. A process according to claim 6, 7, 8, 9 or 10, wherein said anode is of graphite, silicon carbide or silicon nitride
12. An electrolytic cell for production of magnesium metal from magnesium chloride comprising:
a) ~a cell for housing magnesium chloride in a molten salt electrolyte, said cell having a cathode and an anode, b) ~means for feeding hydrogen gas to said anode, c) ~means for recovery from said cell of magnesium metal developed at said cathode, and d) ~means for recovery from said cell of hydrogen chloride developed at said anode.
a) ~a cell for housing magnesium chloride in a molten salt electrolyte, said cell having a cathode and an anode, b) ~means for feeding hydrogen gas to said anode, c) ~means for recovery from said cell of magnesium metal developed at said cathode, and d) ~means for recovery from said cell of hydrogen chloride developed at said anode.
13. A cell according to claim 12, further including a conduit for delivery of hydrogen gas to said anode.
14. A cell according to claim 12 or 13, wherein said anode is a high surface area anode.
15 A cell according to claim 12 or 13, wherein said anode is a porous anode.
16. A cell according to claim 12, 13, 14 or 15, wherein said anode is of graphite, silicon carbide or silicon nitride
17. Use of hydrogen in an electrolytic cell for the production of magnesium from magnesium chloride with production of by-product hydrogen chloride at the anode.
Priority Applications (4)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| CA002265183A CA2265183C (en) | 1999-03-11 | 1999-03-11 | Magnesium metal production |
| PCT/CA2000/000248 WO2000053826A1 (en) | 1999-03-11 | 2000-03-09 | Electrolytic production of magnesium |
| AU31390/00A AU3139000A (en) | 1999-03-11 | 2000-03-09 | Electrolytic production of magnesium |
| US09/933,802 US20020014416A1 (en) | 1999-03-11 | 2001-08-22 | Electrolytic production of magnesium |
Applications Claiming Priority (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| CA002265183A CA2265183C (en) | 1999-03-11 | 1999-03-11 | Magnesium metal production |
Publications (2)
| Publication Number | Publication Date |
|---|---|
| CA2265183A1 CA2265183A1 (en) | 2000-09-11 |
| CA2265183C true CA2265183C (en) | 2008-01-08 |
Family
ID=4163374
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA002265183A Expired - Fee Related CA2265183C (en) | 1999-03-11 | 1999-03-11 | Magnesium metal production |
Country Status (4)
| Country | Link |
|---|---|
| US (1) | US20020014416A1 (en) |
| AU (1) | AU3139000A (en) |
| CA (1) | CA2265183C (en) |
| WO (1) | WO2000053826A1 (en) |
Families Citing this family (13)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US8608935B2 (en) * | 2006-03-24 | 2013-12-17 | GM Global Technology Operations LLC | Apparatus and method for synthesis of alane |
| RU2588960C2 (en) | 2011-03-18 | 2016-07-10 | Орбит Элюминэ Инк. | Methods of extracting rare-earth elements from aluminium-containing materials |
| AU2012250460B2 (en) | 2011-05-04 | 2015-11-26 | Orbite Aluminae Inc. | Processes for recovering rare earth elements from various ores |
| AU2012308068B2 (en) | 2011-09-16 | 2015-02-05 | Aem Technologies Inc. | Processes for preparing alumina and various other products |
| WO2013104059A1 (en) | 2012-01-10 | 2013-07-18 | Orbite Aluminae Inc. | Processes for treating red mud |
| CN102534688B (en) * | 2012-01-10 | 2014-12-10 | 华东理工大学 | High-current baffleless magnesium electrolytic tank |
| EP2838848B1 (en) | 2012-03-29 | 2019-05-08 | Orbite Technologies Inc. | Processes for treating fly ashes |
| CA2882181C (en) * | 2012-08-24 | 2019-05-07 | Orbite Aluminae Inc. | Process for treating magnesium-bearing ores |
| US9353425B2 (en) | 2012-09-26 | 2016-05-31 | Orbite Technologies Inc. | Processes for preparing alumina and magnesium chloride by HCl leaching of various materials |
| EP2920114A4 (en) | 2012-11-14 | 2016-03-02 | Orbite Aluminae Inc | Methods for purifying aluminium ions |
| CN105026620B (en) * | 2013-02-14 | 2018-04-24 | 联盟镁公司 | Produce the hydrogen diffusion anodes arrangement of HCl |
| CA2950004A1 (en) * | 2014-05-26 | 2015-12-03 | Procede Ethanol Vert Technologie | Process for pure aluminum production from aluminum-bearing materials |
| US10423746B2 (en) * | 2015-07-23 | 2019-09-24 | Texas Instruments Incorporated | Compensation design of power converters |
Family Cites Families (1)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US5665220A (en) * | 1995-12-26 | 1997-09-09 | General Motors Corporation | Electrolytic magnesium production process |
-
1999
- 1999-03-11 CA CA002265183A patent/CA2265183C/en not_active Expired - Fee Related
-
2000
- 2000-03-09 WO PCT/CA2000/000248 patent/WO2000053826A1/en active Application Filing
- 2000-03-09 AU AU31390/00A patent/AU3139000A/en not_active Abandoned
-
2001
- 2001-08-22 US US09/933,802 patent/US20020014416A1/en not_active Abandoned
Also Published As
| Publication number | Publication date |
|---|---|
| US20020014416A1 (en) | 2002-02-07 |
| WO2000053826A1 (en) | 2000-09-14 |
| CA2265183A1 (en) | 2000-09-11 |
| AU3139000A (en) | 2000-09-28 |
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Legal Events
| Date | Code | Title | Description |
|---|---|---|---|
| EEER | Examination request | ||
| MKLA | Lapsed | ||
| MKLA | Lapsed |
Effective date: 20100311 |
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| MKLA | Lapsed |
Effective date: 20100311 |