Difference between revisions of "Lunar Aluminum Production"
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[[Anorthite]] could be directly reduced to its component metals using the [[FFC Cambridge Process]]. The [[Anorthite]] is pressed/sintered into a cathode, which is placed in a bath of molten calcium chloride and electrolyzed. The oxygen is stripped out, leaving behind [[Aluminum]], [[Calcium]], and [[Silicon]]. | [[Anorthite]] could be directly reduced to its component metals using the [[FFC Cambridge Process]]. The [[Anorthite]] is pressed/sintered into a cathode, which is placed in a bath of molten calcium chloride and electrolyzed. The oxygen is stripped out, leaving behind [[Aluminum]], [[Calcium]], and [[Silicon]]. | ||
| − | This process has the advantage of inherent simplicity, as well as having only one component to recycle, the calcium chloride, which does not react chemically with the inputs, making recovery much simpler. In addition, this process runs at lower temperatures (900º-1100º C) than many other electrolysis procedures, and inert(non-consumable) anodes have been successfully demonstrated with it<ref>http://www.lpi.usra.edu/meetings/roundtable2006/pdf/tripuraneni.pdf</ref>. On the downside, energy must be expended to split all the components of the [[Anorthite]], not just the [[aluminum]]. Splitting the silicon and calcium adds a significant amount of extra energy to the process, as both of them are strong reducers. However, if the silicon and calcium byproducts were needed for other purposes (calcium is a good [[Electrical Conductors|electrical conductor]], and silicon could be used for solar panels or [[In-Situ Propellant Production | + | This process has the advantage of inherent simplicity, as well as having only one component to recycle, the calcium chloride, which does not react chemically with the inputs, making recovery much simpler. In addition, this process runs at lower temperatures (900º-1100º C) than many other electrolysis procedures, and inert(non-consumable) anodes have been successfully demonstrated with it<ref>http://www.lpi.usra.edu/meetings/roundtable2006/pdf/tripuraneni.pdf</ref>. On the downside, energy must be expended to split all the components of the [[Anorthite]], not just the [[aluminum]]. Splitting the silicon and calcium adds a significant amount of extra energy to the process, as both of them are strong reducers. However, if the silicon and calcium byproducts were needed for other purposes (calcium is a good [[Electrical Conductors|electrical conductor]], and silicon could be used for solar panels or [[In-Situ Propellant Production|rocket fuel]]), this extra energy cost may not be an issue. |
=== Alumina Production === | === Alumina Production === | ||
| − | Many processes used on earth or proposed for Lunar use require [[ | + | Many processes used on earth or proposed for Lunar use require [[alumina]] ([[Aluminum|Al]]<sub>2</sub>[[Oxygen|O]]<sub>3</sub>) as an input. On Earth, alumina is produced from bauxite through the Bayer process. As this process is not feasible using Anorthite, another method must be utilized. |
====Vacuum Distillation==== | ====Vacuum Distillation==== | ||
| Line 48: | Line 48: | ||
=== Direct Calcium Aluminate / Alumina Reduction === | === Direct Calcium Aluminate / Alumina Reduction === | ||
| − | Calcium Aluminate (see above for production) could be simply melted and electrolyzed directly, producing aluminum and calcium oxide.<ref>http://www.moonminer.com/Lunar_Aluminum.html</ref> This has two advantages. First, it requires no imported reagents, and second, only the aluminum is split, reducing the amount of energy needed. The disadvantage is that temperatures of approximately 1600 | + | Calcium Aluminate (see above for production) could be simply melted and electrolyzed directly, producing aluminum and calcium oxide.<ref>http://www.moonminer.com/Lunar_Aluminum.html</ref> This has two advantages. First, it requires no imported reagents, and second, only the aluminum is split, reducing the amount of energy needed. The disadvantage is that temperatures of approximately 1600 ºC are required, making electrode material of prime concern. Carbon electrodes could be utilized at those temperatures, but the anode would continually wear away as oxygen was produced around it, creating carbon monoxide. The carbon would need to be [[Lunar Carbon Production|recovered]] and new anodes made from it. This effectively means that a rare reagent is needed, negating the process's first stated advantage. Finding an anode material that would produce oxygen without wearing away at those temperatures could be quite difficult. |
| − | Alumina could also be directly melted and electrolyzed in the same fashion. However, this would require temperatures of approximately 2000 | + | Alumina could also be directly melted and electrolyzed in the same fashion. However, this would require temperatures of approximately 2000 ºC, bringing with it again the issue of electrode material. |
=== Hall-Heroult Process === | === Hall-Heroult Process === | ||
| − | In the Hall-Heroult process, alumina is dissolved in molten cryolite ([[Sodium]] hexafluoroaluminate, Na<sub>3</sub> AlF<sub>6 </sub>) around 1400 ºC. This mix is electrolyzed to separate two byproducts: aluminium and CO<sub>2</sub>. The carbon comes from the consumption of the carbon anode. | + | In the Hall-Heroult process, alumina is dissolved in molten cryolite ([[Sodium]] hexafluoroaluminate, Na<sub>3</sub> AlF<sub>6 </sub>) around 1400 ºC. This mix is electrolyzed to separate two byproducts: [[aluminium]] and [[Carbon Dioxide|CO<sub>2</sub>]]. The carbon comes from the consumption of the carbon anode. |
| − | This procedure is used extensively on earth for aluminum production, and as such has the advantage of being a very mature technology. The biggest issue is the consumption of the anode, which would require the produced carbon | + | This procedure is used extensively on earth for aluminum production, and as such has the advantage of being a very mature technology. The biggest issue is the consumption of the anode, which would require the produced carbon dioxide to be captured, [[Lunar Carbon Production|converted back into carbon]], and recast into new anodes; an energy intensive process. It is not known if an inert(non-consumable) anode material can be found that would work under these conditions.<ref>http://en.wikipedia.org/wiki/Hall-H%C3%A9roult_process</ref> |
=== Subchloride Process === | === Subchloride Process === | ||
| − | In the subchloride process [[alumina]] is reacted with [[carbon]] and [[chlorine]] to yield [[Al]][[Cl]]<sub>3</sub> and [[Carbon dioxide |CO<sub>2</sub>]]. The [[Al]][[Cl]]<sub>3</sub> is electrolyzed to produce [[ | + | In the subchloride process [[alumina]] is reacted with [[carbon]] and [[chlorine]] to yield [[Al]][[Cl]]<sub>3</sub> and [[Carbon dioxide |CO<sub>2</sub>]]. The [[Al]][[Cl]]<sub>3</sub> is electrolyzed to produce [[aluminum]] while recovering the [[chlorine]]. This has the advantage that conventional [[carbon]] electrodes can be used continuously, as the produced [[chlorine]] does not react with them. However, the [[Carbon dioxide |CO<sub>2</sub>]] byproduct must be [[Lunar Carbon Production|recycled]], adding extra complexity and energy requirements to the system. This makes it similar to the Hall-Heroult process in difficulty, except for two advantages. First, the recycled carbon can be directly used in powdered form, it does not need to be recast into electrodes. Second, due to the low melting point of [[Al]][[Cl]]<sub>3</sub> (120 ºC), the process does not require significant energy to melt, and is more easily handled. <ref>http://www.moonminer.com/Lunar_Aluminum.html </ref> |
=== Carbothermal Reduction === | === Carbothermal Reduction === | ||
| − | Carbon reduction of Alumina is impossible under normal smelting conditions, due to [[aluminum]]s high reduction potential. However, Alumina could be mixed with silica and carbon and melted near 2000 | + | Carbon reduction of Alumina is impossible under normal smelting conditions, due to [[aluminum]]s high reduction potential. However, Alumina could be mixed with silica and carbon and melted near 2000 ºC, which would form an aluminium-silicon alloy, as well as CO<sub>2</sub>. This could be separated by cooling the Al-Si mixture to 700 - 1000 ºC and allowing the silicon to solidify and settle out of the melt.<ref>http://www.moonminer.com/Lunar_Aluminum.html </ref> |
An alternate process involves alumina and carbon processed at high temperatures and low pressure into Al<sub>4</sub>C<sub>3</sub> and carbon monoxide.<ref> [http://en.wikipedia.org/wiki/Aluminium ''Aluminum'' section ''Production and refinement''] </ref> | An alternate process involves alumina and carbon processed at high temperatures and low pressure into Al<sub>4</sub>C<sub>3</sub> and carbon monoxide.<ref> [http://en.wikipedia.org/wiki/Aluminium ''Aluminum'' section ''Production and refinement''] </ref> | ||
| − | <ref> [http://www.moonminer.com/Lunar_Aluminum.html ''Lunar Aluminum'' at ''Moondust index''] </ref> This breaks down into Aluminum and Carbon between 1900 and 2000 | + | <ref> [http://www.moonminer.com/Lunar_Aluminum.html ''Lunar Aluminum'' at ''Moondust index''] </ref> This breaks down into Aluminum and Carbon between 1900 and 2000 ºC.<ref> [http://en.wikipedia.org/wiki/Aluminum_carbide ''Aluminium carbide'' at ''Wikipedia''] </ref>. |
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| + | In either case, CO<sub>2</sub>/CO would have to be recovered and and the [[Lunar Carbon Production|carbon recycled]]. | ||
== See Also == | == See Also == | ||
Latest revision as of 10:38, 10 April 2019
Since Luna lacks any known deposits of bauxite, the ore most commonly used on earth for aluminum production, anorthite (CaAl2Si2O8) is most commonly proposed as a lunar substitute.[1] Anorthite could be separated from the lunar highland material Anorthosite with mechanical methods. It could then be reduced through various chemical and electrochemical methods to produce aluminum.
Anorthite Production
The Anorthosite which makes up the Lunar highlands is a mix of Plagioclases, Olivines, and Pyroxenes. To separate the anorthite, anorthosite must be ground. Then, magnetic separation could leave the non-magnetic anorthite.
The magnetic materials (Ilmenite and iron oxide) could be stored for production of titanium, iron, and oxygen.
Anorthite Refinement
Direct Reduction
Main Article: FFC Cambridge Process
Anorthite could be directly reduced to its component metals using the FFC Cambridge Process. The Anorthite is pressed/sintered into a cathode, which is placed in a bath of molten calcium chloride and electrolyzed. The oxygen is stripped out, leaving behind Aluminum, Calcium, and Silicon.
This process has the advantage of inherent simplicity, as well as having only one component to recycle, the calcium chloride, which does not react chemically with the inputs, making recovery much simpler. In addition, this process runs at lower temperatures (900º-1100º C) than many other electrolysis procedures, and inert(non-consumable) anodes have been successfully demonstrated with it[2]. On the downside, energy must be expended to split all the components of the Anorthite, not just the aluminum. Splitting the silicon and calcium adds a significant amount of extra energy to the process, as both of them are strong reducers. However, if the silicon and calcium byproducts were needed for other purposes (calcium is a good electrical conductor, and silicon could be used for solar panels or rocket fuel), this extra energy cost may not be an issue.
Alumina Production
Many processes used on earth or proposed for Lunar use require alumina (Al2O3) as an input. On Earth, alumina is produced from bauxite through the Bayer process. As this process is not feasible using Anorthite, another method must be utilized.
Vacuum Distillation
Alumina could be produced from Anorthite by boiling out the impurities between 1500 ºC - 2000 ºC under vacuum conditions. The resulting material would be calcium aluminate (CaAlO4). Raising the temperature further could cause alumina to volatilize as well. [3]
Sulfuric Acid Leaching
Another method is to produce calcium aluminate as outlined previously, which is then leached in sulfuric acid, resulting in the following reaction:
CaAl2O4 + 4H2SO4 ==> CaSO4 + Al2(SO4)3 + 4H2O
Aluminium sulfate in hexadecahydrate form (Al2(SO4)3) is then separated from calcium sulphate (CaSO4 + Al2(SO4)3) by filtering and from water by evaporation (and then recovered).
Finally Alumina is obtained by roasting the aluminum sulfate releasing S2.[4]
Hydrochloric Acid Leaching
Another option is to react Anorthite with hydrochloric acid, which results in following reaction:
The calcium chloride and hydrated aluminum chloride dissolve in the solution and are removed. They are then precipitated out of solution, dried, and heated under partial vacuum until the calcium chloride evaporates out of the mix. Temperatures of this range will cause the hydrated aluminum chloride to become alumina, releasing water and hydrogen chloride in the process:
- 2 AlCl3.6 H2O ==> Al2O3 + 6 HCl + 3 H2O
The water and hydrogen chloride are separated from the calcium chloride and fed back into the system. The calcium chloride is then electrolyzed into metallic calcium and chlorine. A portion of the recovered water is then split into hydrogen and oxygen. The hydrogen component is reacted with the evolved chlorine to produce hydrogen chloride, which is then fed back into the main system.
Direct Calcium Aluminate / Alumina Reduction
Calcium Aluminate (see above for production) could be simply melted and electrolyzed directly, producing aluminum and calcium oxide.[5] This has two advantages. First, it requires no imported reagents, and second, only the aluminum is split, reducing the amount of energy needed. The disadvantage is that temperatures of approximately 1600 ºC are required, making electrode material of prime concern. Carbon electrodes could be utilized at those temperatures, but the anode would continually wear away as oxygen was produced around it, creating carbon monoxide. The carbon would need to be recovered and new anodes made from it. This effectively means that a rare reagent is needed, negating the process's first stated advantage. Finding an anode material that would produce oxygen without wearing away at those temperatures could be quite difficult.
Alumina could also be directly melted and electrolyzed in the same fashion. However, this would require temperatures of approximately 2000 ºC, bringing with it again the issue of electrode material.
Hall-Heroult Process
In the Hall-Heroult process, alumina is dissolved in molten cryolite (Sodium hexafluoroaluminate, Na3 AlF6 ) around 1400 ºC. This mix is electrolyzed to separate two byproducts: aluminium and CO2. The carbon comes from the consumption of the carbon anode.
This procedure is used extensively on earth for aluminum production, and as such has the advantage of being a very mature technology. The biggest issue is the consumption of the anode, which would require the produced carbon dioxide to be captured, converted back into carbon, and recast into new anodes; an energy intensive process. It is not known if an inert(non-consumable) anode material can be found that would work under these conditions.[6]
Subchloride Process
In the subchloride process alumina is reacted with carbon and chlorine to yield AlCl3 and CO2. The AlCl3 is electrolyzed to produce aluminum while recovering the chlorine. This has the advantage that conventional carbon electrodes can be used continuously, as the produced chlorine does not react with them. However, the CO2 byproduct must be recycled, adding extra complexity and energy requirements to the system. This makes it similar to the Hall-Heroult process in difficulty, except for two advantages. First, the recycled carbon can be directly used in powdered form, it does not need to be recast into electrodes. Second, due to the low melting point of AlCl3 (120 ºC), the process does not require significant energy to melt, and is more easily handled. [7]
Carbothermal Reduction
Carbon reduction of Alumina is impossible under normal smelting conditions, due to aluminums high reduction potential. However, Alumina could be mixed with silica and carbon and melted near 2000 ºC, which would form an aluminium-silicon alloy, as well as CO2. This could be separated by cooling the Al-Si mixture to 700 - 1000 ºC and allowing the silicon to solidify and settle out of the melt.[8]
An alternate process involves alumina and carbon processed at high temperatures and low pressure into Al4C3 and carbon monoxide.[9] [10] This breaks down into Aluminum and Carbon between 1900 and 2000 ºC.[11].
In either case, CO2/CO would have to be recovered and and the carbon recycled.
See Also
References
- ↑ http://www.permanent.com/l-minera.htm#aluminum
- ↑ http://www.lpi.usra.edu/meetings/roundtable2006/pdf/tripuraneni.pdf
- ↑ http://www.moonminer.com/Lunar_Aluminum.html
- ↑ http://www.moonminer.com/Lunar_Aluminum.html
- ↑ http://www.moonminer.com/Lunar_Aluminum.html
- ↑ http://en.wikipedia.org/wiki/Hall-H%C3%A9roult_process
- ↑ http://www.moonminer.com/Lunar_Aluminum.html
- ↑ http://www.moonminer.com/Lunar_Aluminum.html
- ↑ Aluminum section Production and refinement
- ↑ Lunar Aluminum at Moondust index
- ↑ Aluminium carbide at Wikipedia
