CA1115488A - Production of anhydrous aluminium chloride - Google Patents
Production of anhydrous aluminium chlorideInfo
- Publication number
- CA1115488A CA1115488A CA336,223A CA336223A CA1115488A CA 1115488 A CA1115488 A CA 1115488A CA 336223 A CA336223 A CA 336223A CA 1115488 A CA1115488 A CA 1115488A
- Authority
- CA
- Canada
- Prior art keywords
- aluminium chloride
- temperature
- chlorination
- range
- anhydrous aluminium
- 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
Links
Classifications
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
- C01F7/00—Compounds of aluminium
- C01F7/48—Halides, with or without other cations besides aluminium
- C01F7/56—Chlorides
- C01F7/58—Preparation of anhydrous aluminium chloride
Abstract
A B S T R A C T
A process for obtaining anhydrous aluminium chloride from aluminium chloride hexahydrate comprises heating the hexahydrate at a temperature in the range 200 - 450°C until it is substantially dehydrated and reacting the dehydrated material at a temperature in the range 350 - 600°C with a gas mixture containing chlorine, carbon monoxide, carbon dioxide and hydrogen, to produce gaseous anhydrous aluminium chloride.
A process for obtaining anhydrous aluminium chloride from aluminium chloride hexahydrate comprises heating the hexahydrate at a temperature in the range 200 - 450°C until it is substantially dehydrated and reacting the dehydrated material at a temperature in the range 350 - 600°C with a gas mixture containing chlorine, carbon monoxide, carbon dioxide and hydrogen, to produce gaseous anhydrous aluminium chloride.
Description
This invention relates to the production of anhydrous aluminium chloride and more particularly to an improved process for the production of this material from aluminium chloride hexahydrate by dehydration followed by chlorination.
Currently aluminium is produced from bauxite using a combination of the Bayer and Hall-Heroult processes. The -Bayer process produces high purity alumina from bauxite which, in the Hall-Heroult process, is continuously dissolved in a fluoride bath (principally cryolite) and reduced electrolyt-ically, and molten aluminium is collected above the carbon cathode which forms the base of the furnace. The electrolytic reduction of alumina which is the basis for the Hall-Heroult process uses very large amounts of electrical energy, typically 13-18 MWh per tonne of metal and also consumes carbon anodes through oxidation by oxygen evolved during the electrolysis.
In recent years, production of aluminium by the electrolysis of anhydrous aluminium chloride dissolved in a molten electrolyte composed of one or more halides of alkali and/or alkaline earth metals has received conslderable attention (U.E. Patent 3,725,222) as this method offers certain potential advantages over the Hall-Heroult process. The advantages which include operation at a lower temperature, lower power consumption (9.5 MWh per tonne of metal) and non-consumption of carbon electrodes indicate significant cost savings over the conventional Hall-Heroult process.
A pre-requisite to the chloride electrolysis process is the production of high purity anhydrous aluminium chloride feed for the electrolysis stage. Although the potential of
Currently aluminium is produced from bauxite using a combination of the Bayer and Hall-Heroult processes. The -Bayer process produces high purity alumina from bauxite which, in the Hall-Heroult process, is continuously dissolved in a fluoride bath (principally cryolite) and reduced electrolyt-ically, and molten aluminium is collected above the carbon cathode which forms the base of the furnace. The electrolytic reduction of alumina which is the basis for the Hall-Heroult process uses very large amounts of electrical energy, typically 13-18 MWh per tonne of metal and also consumes carbon anodes through oxidation by oxygen evolved during the electrolysis.
In recent years, production of aluminium by the electrolysis of anhydrous aluminium chloride dissolved in a molten electrolyte composed of one or more halides of alkali and/or alkaline earth metals has received conslderable attention (U.E. Patent 3,725,222) as this method offers certain potential advantages over the Hall-Heroult process. The advantages which include operation at a lower temperature, lower power consumption (9.5 MWh per tonne of metal) and non-consumption of carbon electrodes indicate significant cost savings over the conventional Hall-Heroult process.
A pre-requisite to the chloride electrolysis process is the production of high purity anhydrous aluminium chloride feed for the electrolysis stage. Although the potential of
- 2 -', .. '' '. "'.' ' - ..
:
:
: - - ;. ~:
: ,. . :.
11-1',4t~r~ 1 aluminium chloride electrolysis as a method of producing aluminium metal has been recognized for a while, the develop-ment of the process to a commercial scale has been inhibited due to the unavailability of an economic process for the prod-uction of high purity anhydrous aluminium chloride. Many processes have been proposed for the production of anhydrous aluminium chloride from bauxite and alumina but to date the suggested methods have not satisfied the objective of commercial production o~ high purity anhydrous aluminium chloride. Chlor-ination of bauxite results in aluminium chloride contaminated with the chlorides of iron, titanium and silicon and the separation of these impurities from aluminium chloride requires complex and costly processing steps. On the other hand, the chlorination of Bayer, alumina, although it results in high purity aluminium chloride, requires an expensive starting material and unlike direct electrolysis of alumina in the Hall cell introduces an extra step of chlorination. Furthermore, Bayler alumina contains about 0.5% of sodium oxide, which during chlorination, will cons~me chlorine to produce NaAlC14.
The formation of the latter compound would not only create problems during chlorination but also result in some loss of chlorine values. Chlorination is generally carried out above 600C (West German Patent No. 1,229,056) using high purity, as such expensive, carbon monoxide as reductant. An alternative to carbon monoxide as reductant is the chlorination of porous alumina particles being intermixed, ., . . ~ . ...... . ~.. ~ . . . .
: .:
.. ;, . .
\
and preferably coated or impregnated, with carbon to provide an average carbon content of about 15-24% by weight and having an average hydrogen content of less than 0.5~ by weight and desirably of less than 0.3% and preferably less than 0.1% (U.S. Patent 3,842,163). The preferred chlorination temperaturesare in the range 650 - 700C.
Unlike many hydrated compounds, aluminium chloride hexahydrate when heated to remove combined water does not yield anhydrous aluminium chloride. Instead, A1203, HCl and H2O are produced according to the following reaction:
2 AlC13 6H2 ~ A1203 + 6HCl + 9H20 According to the studies which have been carried out on the dehydration reaction, decomposition takes place at 180C and heating in a stream of HCl does not prevent the above hydrolysis reaction. Very little loss in weight is observed below this temperature, particularly at 100C.
The literature contains very little information on the dehydration of AlC13.6H2O to AlC13, According to Heap and Newbery tBritish Patents Nos. 130,626 and 131,039~
dehydration of aluminium chloride hexahydrate can be carried out by reacting it with phosgene which has a great affinity for water. These patents do not give any experimental details and results except indicating that aluminium chloride hexa-hydrate was heated at 100C before reacting it with phosgene and that hydrogen was excluded from the chlorinating gas mixture in order to avoid formation of water.
.. : . , ,. .. ~ . .
.~. . .
, ! ..y D'.... ' ,: ,. ~ ' 4~
Thus it may be seen that the dehydration of hexa-hydrate according to the teaching of the above patents would result in the production of a large excess o~ HCl. The amount of HCl produced would be about four times that required to produce aluminium chloride hexahydrate from bauxite or other aluminum containing materials as shown below, representing - an overall loss of chlorine and CO from the system.
2AlC13.6H2O + 12 CO + 12C12 -~ 2AlC13 + 12CO2 + 24HCl A12O3 + 6HCl + 9H2O ' 3 2 Although one of the patents (British Patent 131,039) discloses the use of producer gas (practically free from hydrogen), production of hydrogen-free producer gas is relatively expensive and the presence of nitrogen in the producer gas, although it may not affe¢t the dehydration reaction, would have an adverse effect on the condensation of AlC13 from gas mixture containing AlC13, CO, CO2 and N2 due to the dilution effect of nitrogen further lowering the partial pressure of __ AlC13.
East German Patent ~o. 130,656 describes a two-stage process for the production of anhydrous aluminium chloride wherein, in the first stage aluminium chloride hexahydrate is heated at a temperature between 100 and 500C to remove a major proportion of water and HCl. In the second stage the first stage product (a basic aluminium chloride) is heated at a temperature between 600 and 900C to produce anhydrous : aluminium chloride which is removed by a carrier gas, which ; . :~; :
preferably contains gaseous HCl, and leave a residue o~
~-A12O3. Only some 10-20% of the aluminium present in the starting material emerges as the anhydrou~ chloride product.
The present invention seeks to overcome the disadvantages of the prior art processes and producè high purity anhydrous aluminium chloride which can be used as feed in the electrolytic production of aluminium metal.
More specifically, the primary objective of the present invention is to provide a process whereby high purity anhydrous aluminium chloride is produced from aluminium ehloride hexahydrate by dehydration followed by chlorination at low temperatures.
The invention also aims to avoid the necessity or high purity of the reductant, earbon monoxide, and to use as the -chlorinating medium a gas mixture containing carbon monoxide, carbon dioxide and hydrogen, which is more economical to produce than pure carbon monoxide, without any detriment to the process of production of anhydrous aluminium chloride.
Basieally, the process of the present invention relies upon the removal of most of the water from hexahydrate ,, :: - .
, ' . , at temperatures which are compatable with reasonable rates of water removal and at the same time making sure that the product of dehydration is reactive to chlorine-containing gases at ]ow temperatures, i.e. below 600C.
Thus, according to the present invention, a process for obtaining anhydrous aluminium chloride from aluminium - chloride hexahydrate comprises heating the hexahydrate at a temperature in the range 200 - 450C until it is substantially dehydrated and reacting the dehydrated material at a temperature in the range 350 - 600C with a gas mixture containing chlorine, carbon monoxide, carbon dioxide and hydrogen, to produce gaseous anhydrous aluminium chloride.
Preferably, the dehydration and chlorination steps are both carried out in a fluidized bed reactor. Hence, in accordance with a preferred embodiment of the invention, a process for obtaining anhydrous aluminium chloride from aluminium chloride hexahydrate comprises heating the crystalline hexahydrate in a fluidized bed reactor maintained at a temperature in the range 200 - 450C to substantially dehydrate the crystals, reacting the dehydrated material, in the same or another fluidized bed reactor, which is maintained at a temperature in the range 350 - 600C, with a gas mixture containing chlorine, carbon monoxide, carbon dioxide and hydrogen, condensing anhydrous aluminium chloride from the gases leavLng the fluidized-bed reactor.
Preferred gas mixtures for use in the invention contain, by volume, 30 to 50% chlorine, 30 to 50% carbon monoxide, 5 to 15% hydrogen and 5 to 15% carbon dioxide~
Preferred temperature ranges for the dehydration and chlorination . .
)4~
stages are, respectively, 300 - 400C and 400 - 500C.
Having outlined the invention in broad terms, furthe-r details will be provided by way of specific examples which are provided herein for purposes of illustration only and are not intended to be limiting on the invention.
Reference will be made to the accompanying drawing which is a graph showing chlorine utilisation versus temperature for the chlorination step.
E}~AMPLE 1 lOg of aluminium chloride hexahydrate crystals were dehydrated at 100C for 24 hours. The loss of weight of water corresponded to 3.6% only.
415g of aluminium chloride hexahydrate crystals were dehydrated at 400C in an externally heated fluidized-bed reactor (7.5 cm diameter) for 2 hours. Nitrogen was used as fluidizing gas. The water removed corresponded to 98%.
EX~MPLE 3 20g of samples of the dehydrated material produced in Example 2 were reacted for 72 minutes with a gas mixture consisting of CO + C12 in the ratio of 1:1 (v/v) in a fluidized-bed reactor (2.5 cm diameter) at temperatures of 250, 300, 400, 450, 500 and 600C. The gas flow rate was 200 cm ~min.
The gaseous products from the reactor containing anhydrous aluminium chloride were absorbed in a sodium chloride column heated to 150C and sodium chloroaluminate collected in a flask was analysed for aluminium values. Chlorine utilization ., : ..
.: .. -, : :
:. :: ... :: :
.. .. ..
~''"'''.' ~ ,~' 1~1'"~4~
(calculated from the amount of aluminium in the double salt) at the various temperatures is shown in Figure l. The :results show that chlorine utilization of greater than 85%
is obtained at temperatures above 400C and 450C, chlorine utilization is 97%.
A 20g sample of the dehydrated material from example 2 was reacted with a gas mixture containing, by volume, 43%
Cl2, 47% CO and 10% CO2 at 400C using the procedure of Example 3, but using a flow rate of 230 cm3/min. The chlorine utilization was 88.1%.
A 20g sample of the dehydrated material from example 2 was reacted with a gas mixture containing, by volume, 39%
C12, 47% CG, 9% CO2 and 5% H~ at 400C using the procedure of Example 3, but at a flow rate of 305 cm3/min. The chlorine utilization, including reaction with hydrogen, was 87.1%.
EXAMP_E 6 A 20g sample of the dehydrated material from Example 2 was reacted with a gas mixture containing, by volume, 41%
Cl2, 39% CO, 8% CO2 and 12% H2 at 400C using the procedure of Example 3, but at a flow rate of 360 cm3/min. The chlorine utilization was, includiny reaction with hydro~en, 88.3%.
The experiment of Example 6 was repeated at a temperature of 500C. The chlorine utilization was 94.6%.
Example l clearly shows that dehydration of AlCl3.6H2O
at lO0 C leaves more than 95% of water in the product and - . _ g _ .. . . . . .. . ..... .. . .... . . ..
..
,, . ~
: :
1 1 ~r ~ ~
subsequent reaction of this material with CO and C12, as proposed in the prior art, would result in loss of both the C12 and CO values.
On the other hand Examples 2 to 7 show that dehydration according to the present invention results in a product containing very little water which in turn results in negligible chlorine loss during the chlorination stage. It is also shown that chlorination using a mixture of gases containing C12, CO, CO2 and H2 does not affect the efficiency of chlorination and accordingly the present invention allows the production of anhydrous aluminium chloride economically.
As such it is a very significant improvement over the prior art processes.
.
: 25 .
-- 10 -- .
.. . . .
- . :~, : : .. , ;
- : , :,.. : , . . .
:: :
:
:
: - - ;. ~:
: ,. . :.
11-1',4t~r~ 1 aluminium chloride electrolysis as a method of producing aluminium metal has been recognized for a while, the develop-ment of the process to a commercial scale has been inhibited due to the unavailability of an economic process for the prod-uction of high purity anhydrous aluminium chloride. Many processes have been proposed for the production of anhydrous aluminium chloride from bauxite and alumina but to date the suggested methods have not satisfied the objective of commercial production o~ high purity anhydrous aluminium chloride. Chlor-ination of bauxite results in aluminium chloride contaminated with the chlorides of iron, titanium and silicon and the separation of these impurities from aluminium chloride requires complex and costly processing steps. On the other hand, the chlorination of Bayer, alumina, although it results in high purity aluminium chloride, requires an expensive starting material and unlike direct electrolysis of alumina in the Hall cell introduces an extra step of chlorination. Furthermore, Bayler alumina contains about 0.5% of sodium oxide, which during chlorination, will cons~me chlorine to produce NaAlC14.
The formation of the latter compound would not only create problems during chlorination but also result in some loss of chlorine values. Chlorination is generally carried out above 600C (West German Patent No. 1,229,056) using high purity, as such expensive, carbon monoxide as reductant. An alternative to carbon monoxide as reductant is the chlorination of porous alumina particles being intermixed, ., . . ~ . ...... . ~.. ~ . . . .
: .:
.. ;, . .
\
and preferably coated or impregnated, with carbon to provide an average carbon content of about 15-24% by weight and having an average hydrogen content of less than 0.5~ by weight and desirably of less than 0.3% and preferably less than 0.1% (U.S. Patent 3,842,163). The preferred chlorination temperaturesare in the range 650 - 700C.
Unlike many hydrated compounds, aluminium chloride hexahydrate when heated to remove combined water does not yield anhydrous aluminium chloride. Instead, A1203, HCl and H2O are produced according to the following reaction:
2 AlC13 6H2 ~ A1203 + 6HCl + 9H20 According to the studies which have been carried out on the dehydration reaction, decomposition takes place at 180C and heating in a stream of HCl does not prevent the above hydrolysis reaction. Very little loss in weight is observed below this temperature, particularly at 100C.
The literature contains very little information on the dehydration of AlC13.6H2O to AlC13, According to Heap and Newbery tBritish Patents Nos. 130,626 and 131,039~
dehydration of aluminium chloride hexahydrate can be carried out by reacting it with phosgene which has a great affinity for water. These patents do not give any experimental details and results except indicating that aluminium chloride hexa-hydrate was heated at 100C before reacting it with phosgene and that hydrogen was excluded from the chlorinating gas mixture in order to avoid formation of water.
.. : . , ,. .. ~ . .
.~. . .
, ! ..y D'.... ' ,: ,. ~ ' 4~
Thus it may be seen that the dehydration of hexa-hydrate according to the teaching of the above patents would result in the production of a large excess o~ HCl. The amount of HCl produced would be about four times that required to produce aluminium chloride hexahydrate from bauxite or other aluminum containing materials as shown below, representing - an overall loss of chlorine and CO from the system.
2AlC13.6H2O + 12 CO + 12C12 -~ 2AlC13 + 12CO2 + 24HCl A12O3 + 6HCl + 9H2O ' 3 2 Although one of the patents (British Patent 131,039) discloses the use of producer gas (practically free from hydrogen), production of hydrogen-free producer gas is relatively expensive and the presence of nitrogen in the producer gas, although it may not affe¢t the dehydration reaction, would have an adverse effect on the condensation of AlC13 from gas mixture containing AlC13, CO, CO2 and N2 due to the dilution effect of nitrogen further lowering the partial pressure of __ AlC13.
East German Patent ~o. 130,656 describes a two-stage process for the production of anhydrous aluminium chloride wherein, in the first stage aluminium chloride hexahydrate is heated at a temperature between 100 and 500C to remove a major proportion of water and HCl. In the second stage the first stage product (a basic aluminium chloride) is heated at a temperature between 600 and 900C to produce anhydrous : aluminium chloride which is removed by a carrier gas, which ; . :~; :
preferably contains gaseous HCl, and leave a residue o~
~-A12O3. Only some 10-20% of the aluminium present in the starting material emerges as the anhydrou~ chloride product.
The present invention seeks to overcome the disadvantages of the prior art processes and producè high purity anhydrous aluminium chloride which can be used as feed in the electrolytic production of aluminium metal.
More specifically, the primary objective of the present invention is to provide a process whereby high purity anhydrous aluminium chloride is produced from aluminium ehloride hexahydrate by dehydration followed by chlorination at low temperatures.
The invention also aims to avoid the necessity or high purity of the reductant, earbon monoxide, and to use as the -chlorinating medium a gas mixture containing carbon monoxide, carbon dioxide and hydrogen, which is more economical to produce than pure carbon monoxide, without any detriment to the process of production of anhydrous aluminium chloride.
Basieally, the process of the present invention relies upon the removal of most of the water from hexahydrate ,, :: - .
, ' . , at temperatures which are compatable with reasonable rates of water removal and at the same time making sure that the product of dehydration is reactive to chlorine-containing gases at ]ow temperatures, i.e. below 600C.
Thus, according to the present invention, a process for obtaining anhydrous aluminium chloride from aluminium - chloride hexahydrate comprises heating the hexahydrate at a temperature in the range 200 - 450C until it is substantially dehydrated and reacting the dehydrated material at a temperature in the range 350 - 600C with a gas mixture containing chlorine, carbon monoxide, carbon dioxide and hydrogen, to produce gaseous anhydrous aluminium chloride.
Preferably, the dehydration and chlorination steps are both carried out in a fluidized bed reactor. Hence, in accordance with a preferred embodiment of the invention, a process for obtaining anhydrous aluminium chloride from aluminium chloride hexahydrate comprises heating the crystalline hexahydrate in a fluidized bed reactor maintained at a temperature in the range 200 - 450C to substantially dehydrate the crystals, reacting the dehydrated material, in the same or another fluidized bed reactor, which is maintained at a temperature in the range 350 - 600C, with a gas mixture containing chlorine, carbon monoxide, carbon dioxide and hydrogen, condensing anhydrous aluminium chloride from the gases leavLng the fluidized-bed reactor.
Preferred gas mixtures for use in the invention contain, by volume, 30 to 50% chlorine, 30 to 50% carbon monoxide, 5 to 15% hydrogen and 5 to 15% carbon dioxide~
Preferred temperature ranges for the dehydration and chlorination . .
)4~
stages are, respectively, 300 - 400C and 400 - 500C.
Having outlined the invention in broad terms, furthe-r details will be provided by way of specific examples which are provided herein for purposes of illustration only and are not intended to be limiting on the invention.
Reference will be made to the accompanying drawing which is a graph showing chlorine utilisation versus temperature for the chlorination step.
E}~AMPLE 1 lOg of aluminium chloride hexahydrate crystals were dehydrated at 100C for 24 hours. The loss of weight of water corresponded to 3.6% only.
415g of aluminium chloride hexahydrate crystals were dehydrated at 400C in an externally heated fluidized-bed reactor (7.5 cm diameter) for 2 hours. Nitrogen was used as fluidizing gas. The water removed corresponded to 98%.
EX~MPLE 3 20g of samples of the dehydrated material produced in Example 2 were reacted for 72 minutes with a gas mixture consisting of CO + C12 in the ratio of 1:1 (v/v) in a fluidized-bed reactor (2.5 cm diameter) at temperatures of 250, 300, 400, 450, 500 and 600C. The gas flow rate was 200 cm ~min.
The gaseous products from the reactor containing anhydrous aluminium chloride were absorbed in a sodium chloride column heated to 150C and sodium chloroaluminate collected in a flask was analysed for aluminium values. Chlorine utilization ., : ..
.: .. -, : :
:. :: ... :: :
.. .. ..
~''"'''.' ~ ,~' 1~1'"~4~
(calculated from the amount of aluminium in the double salt) at the various temperatures is shown in Figure l. The :results show that chlorine utilization of greater than 85%
is obtained at temperatures above 400C and 450C, chlorine utilization is 97%.
A 20g sample of the dehydrated material from example 2 was reacted with a gas mixture containing, by volume, 43%
Cl2, 47% CO and 10% CO2 at 400C using the procedure of Example 3, but using a flow rate of 230 cm3/min. The chlorine utilization was 88.1%.
A 20g sample of the dehydrated material from example 2 was reacted with a gas mixture containing, by volume, 39%
C12, 47% CG, 9% CO2 and 5% H~ at 400C using the procedure of Example 3, but at a flow rate of 305 cm3/min. The chlorine utilization, including reaction with hydrogen, was 87.1%.
EXAMP_E 6 A 20g sample of the dehydrated material from Example 2 was reacted with a gas mixture containing, by volume, 41%
Cl2, 39% CO, 8% CO2 and 12% H2 at 400C using the procedure of Example 3, but at a flow rate of 360 cm3/min. The chlorine utilization was, includiny reaction with hydro~en, 88.3%.
The experiment of Example 6 was repeated at a temperature of 500C. The chlorine utilization was 94.6%.
Example l clearly shows that dehydration of AlCl3.6H2O
at lO0 C leaves more than 95% of water in the product and - . _ g _ .. . . . . .. . ..... .. . .... . . ..
..
,, . ~
: :
1 1 ~r ~ ~
subsequent reaction of this material with CO and C12, as proposed in the prior art, would result in loss of both the C12 and CO values.
On the other hand Examples 2 to 7 show that dehydration according to the present invention results in a product containing very little water which in turn results in negligible chlorine loss during the chlorination stage. It is also shown that chlorination using a mixture of gases containing C12, CO, CO2 and H2 does not affect the efficiency of chlorination and accordingly the present invention allows the production of anhydrous aluminium chloride economically.
As such it is a very significant improvement over the prior art processes.
.
: 25 .
-- 10 -- .
.. . . .
- . :~, : : .. , ;
- : , :,.. : , . . .
:: :
Claims (5)
1. A process for obtaining anhydrous aluminium chloride from aluminium chloride hexahydrate comprises heating the hexahydrate at a temperature in the range 200 - 450°C until it is substantially dehydrated and reacting the dehydrated material at a temperature in the range 350 - 600°C with a gas mixture containing chlorine, carbon monoxide, carbon dioxide and hydrogen, to produce gaseous anhydrous aluminium chloride.
2. A process as claimed in Claim 1, wherein one or both of the dehydration and chlorination steps are carried out in a fluidized bed reactor.
3. A process as claimed in Claim 1, wherein the temperature for the dehydration step is in the range 300° - 400°C.
4. A process as claimed in Claim 1, wherein the temperature for the chlorination step is in the range 400° - 500°C.
5. A process as claimed in Claim 1, wherein the gas mixture for the chlorination step contains, by volume:
30 to 50% chlorine 30 to 50% carbon monoxide 5 to 15% hydrogen and 5 to 15% carbon dioxide,
30 to 50% chlorine 30 to 50% carbon monoxide 5 to 15% hydrogen and 5 to 15% carbon dioxide,
Applications Claiming Priority (2)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| AUPD6121/78 | 1978-09-26 | ||
| AU612178 | 1978-09-26 |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| CA1115488A true CA1115488A (en) | 1982-01-05 |
Family
ID=3696633
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA336,223A Expired CA1115488A (en) | 1978-09-26 | 1979-09-24 | Production of anhydrous aluminium chloride |
Country Status (3)
| Country | Link |
|---|---|
| US (1) | US4264569A (en) |
| AU (1) | AU528882B2 (en) |
| CA (1) | CA1115488A (en) |
Families Citing this family (16)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US4465566A (en) * | 1982-07-20 | 1984-08-14 | Atlantic Richfield Company | Method of producing anhydrous aluminum chloride from acid leach-derived ACH and the production of aluminum therefrom |
| US4465659A (en) * | 1982-07-21 | 1984-08-14 | Atlantic Richfield Company | Aluminum production via the chlorination of partially calcined aluminum chloride hexahydrate |
| US4459274A (en) * | 1982-10-25 | 1984-07-10 | Atlantic Richfield Company | Chlorination using partially calcined carbonaceous material as a reductant |
| US4559215A (en) * | 1983-08-03 | 1985-12-17 | Atlantic Richfield Company | Production of anhydrous aluminum chloride from hydrated alumina |
| US4493784A (en) * | 1984-01-30 | 1985-01-15 | Atlantic Richfield Company | Dehydration of aluminum chloride hexahydrate |
| US4943426A (en) * | 1988-06-20 | 1990-07-24 | Aluminum Company Of America | Method for regulating reaction temperature |
| DE4121276C2 (en) * | 1991-06-27 | 1994-02-17 | Metallgesellschaft Ag | Process for the preparation of sulfate-containing, basic polyaluminium chloride solutions |
| EP1869399A2 (en) * | 2005-04-11 | 2007-12-26 | Zetetic Institute | Apparatus and method for in situ and ex situ measurement of spatial impulse response of an optical system using phase-shifting point-diffraction interferometry |
| US7428058B2 (en) * | 2005-05-18 | 2008-09-23 | Zetetic Institute | Apparatus and method for in situ and ex situ measurements of optical system flare |
| WO2007019548A2 (en) * | 2005-08-08 | 2007-02-15 | Zetetic Institute | Apparatus and methods for reduction and compensation of effects of vibrations and of environmental effects in wavefront interferometry |
| WO2007025147A2 (en) * | 2005-08-26 | 2007-03-01 | Zetetic Institute | Apparatus and method for measurement and compensation of atmospheric turbulence effects in wavefront interferometry |
| WO2007059249A2 (en) * | 2005-11-15 | 2007-05-24 | Zetetic Institute | Interferometer with coherent artifact reduction plus vibration and enviromental compensation |
| CN103803621A (en) * | 2012-11-06 | 2014-05-21 | 贵阳铝镁设计研究院有限公司 | Method using double salt method to prepare anhydrous aluminum chloride from crystallization aluminum chloride dehydration |
| CN103936047B (en) * | 2013-01-22 | 2017-07-25 | 贵阳铝镁设计研究院有限公司 | A kind of preparation method of anhydrous Aluminum chloride |
| WO2015179973A1 (en) * | 2014-05-26 | 2015-12-03 | Procede Ethanol Vert Technologie | Process for pure aluminum production from aluminum-bearing materials |
| US10704152B2 (en) | 2018-01-11 | 2020-07-07 | Consolidated Nuclear Security, LLC | Methods and systems for producing a metal chloride or the like |
Family Cites Families (6)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US1304567A (en) * | 1919-05-27 | Paul leon htulin | ||
| US1144304A (en) * | 1915-03-02 | 1915-06-22 | Almer Mcduffie Mcafee | Manufacture of aluminum chlorid. |
| US1331257A (en) * | 1918-08-26 | 1920-02-17 | Heap William | Manufacture of metallic chlorids |
| US3842136A (en) * | 1971-06-30 | 1974-10-15 | Shell Oil Co | Isoamylene extraction |
| DE2201866A1 (en) * | 1972-01-15 | 1973-07-19 | Basf Ag | Regeneration of aluminium chloride solns - by conversion to aluminium oxide and subsequent chlorination |
| DD130656A1 (en) * | 1977-04-18 | 1978-04-19 | Dieter Petzold | PROCESS FOR PREPARING WATER-FREE ALUMINUM CHLORIDE |
-
1978
- 1978-09-26 AU AU50982/79A patent/AU528882B2/en not_active Ceased
-
1979
- 1979-09-24 CA CA336,223A patent/CA1115488A/en not_active Expired
- 1979-09-26 US US06/079,008 patent/US4264569A/en not_active Expired - Lifetime
Also Published As
| Publication number | Publication date |
|---|---|
| AU5098279A (en) | 1980-04-03 |
| AU528882B2 (en) | 1983-05-19 |
| US4264569A (en) | 1981-04-28 |
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