AU2002315563A1

AU2002315563A1 - Reduction of metal oxides in an electrolytic cell

Info

Publication number: AU2002315563A1
Application number: AU2002315563A
Authority: AU
Inventors: Steve Osborn; Ivan Ratchev; Les Strezov
Original assignee: Metalysis Ltd
Current assignee: Metalysis Ltd
Priority date: 2001-06-29
Filing date: 2002-06-28
Publication date: 2003-05-15
Anticipated expiration: 2022-06-28

Description

REDUCTION OF METAL OXIDES IN AN ELECTROLYTIC CELL

The present invention relates to reduction of metal oxides in an electrolytic cell.

The present invention was made during the course of an on-going research project on the electrolytic reduction of titania (Ti0₂) carried out by the applicant.

During the course of the research project the applicant carried out experimental work on 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 cathode that included solid titania.

One objective of the experimental work was to reproduce the results reported in International application PCT/GB99/01781 (Publication no. 099/64638) in the name of Cambridge University Technical Services Limited and in technical papers published by the inventors .

The Cambridge International application discloses two potential applications of a "discovery" in the field of metallurgical electrochemistry.

One application is the direct production of a metal from a metal oxide.

In the context of this application, the "discovery" is the realisation that an electrolytic cell can be used to ionise oxygen contained in a metal oxide so that the oxygen dissolves in an electrolyte. The Cambridge International application discloses that when a suitable potential is applied to an electrolytic cell with a metal oxide as a cathode, a reaction occurs whereby oxygen is ionised and is subsequently able to dissolve in the electrolyte of the cell.

European patent application 9995507.1 derived from the Cambridge International application has been allowed by the European Patent Office.

The allowed claims of the European patent application inter alia define a method of electrolytically reducing a metal oxide (such as titania) that includes operating an electrolytic cell at a potential that is lower than the deposition potential of cations in the electrolyte.

The Cambridge European patent application does not define what is meant by deposition potential and does not include any specific examples that provide values of the deposition potential for particular cations.

However, submissions dated 2 October 2001 to the

European Patent Office by the Cambridge patent attorneys, which pre-dated the lodgement of the claims that were ultimately allowed, indicate that they believe that the decomposition potential of an electrolyte is the deposition potential of a cation in the electrolyte.

Specifically, page 5 of the submissions state that:

"The second advantage described above is achieved in part through carrying out the claimed invention below the decomposi tion potential of the electrolyte . If higher potentials are used then, as noted in Dl and D2 , the cation in the electrolyte deposi ts on the metal or semi - metal compound. In the example of Dl , this leads to calcium deposi tion and therefore consumption of this reactive metal.... During operation of the method, the electrolytic cation is not deposited on the cathode".

Contrary to the findings of Cambridge, the experimental work carried out by the applicant has established that it is essential that the electrolytic cell be operated at a potential that is above the potential at which Ca⁺⁺ cations in the electrolyte can deposit as Ca metal on the cathode.

Specifically, as a consequence of the experimental work, the applicant has invented a method of reducing a metal oxide such as titanium oxides in a solid state in an electrolytic cell which includes an anode, a cathode formed at least in part from the metal oxide, and a molten electrolyte which includes cations of a metal that is capable of chemically reducing the cathode metal oxide, which method includes a step of operating the cell at a potential that is above a potential at which cations of the metal that is capable of chemically reducing the cathode metal oxide deposit as the metal on the cathode, whereby the metal chemically reduces the cathode metal oxide .

The above method is described in Australian provisional application PS3049 in the name of the applicant lodged on 20 June 2002, and the disclosure in the patent specification lodged with the application is incorporated herein by cross-reference.

In addition to the above, the experimental work

(and associated theoretical analysis work) carried out by the applicant has determined a number of important factors that play a role in the actual reduction process .

The relevant experimental data indicates that (i)

Cl₂ gas is removed at the anode of the electrolytic cell at potentials well below the theoretical decomposition potential of the electrolyte CaCl₂, (ii) Ca_xTiyO_z, is present at the cathode during some stages of the electrolysis, and (iii) CaO is formed in the molten electrolyte bath.

In view of the above, the applicant has concluded that a number of steps are involved in the method of reducing titanium oxides and that some of these steps are represented by reactions (1) to (8) mentioned below. Reactions (1) to (8) relate to reduction of titanium oxides using an electrolytic cell with CaCl₂ (containing 0 anions) as the electrolyte and a graphite anode, with their standard potentials at 950°C.

CaCl₂ + 3Ti0₂ = CaTi0₃ + Cl₂ (g) + Ti₂0₃ ... (1)

E° 99550oCc = -1.45 V

CaCl₂ + 2Ti0₂ = CaTi0₃ + Cl₂ (g) + TiO ... (2)

E 995500CC ⁼ -1.63 V

CaCl₂ + 0.5TiO₂ = CaO + Cl₂ (g) + 0.5Ti ... (3)

E 99550θCc = -2.4 V

CaTi0₃ + C = CaO + TiO + CO (g) ... (4)

CaTi0₃ + 2C = CaO + Ti + 2CO(g) ... (5)

E° 99550oCc = -0.96 V

Ti₂0₃ + C = 2TiO + CO(g) ... (6)

TiO + C = Ti + CO(g) ... (7)

[0]Ti + C = CO (gas) ... (8) Reactions (1) to (8) are not an exhaustive list, of the possible reaction and other reactions can take place. Specifically, the applicant suspects that other reactions, involving titanium suboxides, represented by the formula Ti_n0_2n_ι, and calcium titanates, represented by the formula CaTi_n0_3n+ι, can take place.

The potential of reaction (8) in particular varies with the concentration of oxygen in titanium. The following graph illustrates the variation of potential with concentration of oxygen in titanium in a cell operating at 950°C. The graph was prepared by the applicant using published data.

0.001 0.01 0.1 1 Activicy of oxygen in Ti

It is clear from the graph that reaction (8) requires higher potentials at lower concentrations of oxygen and thus there is increased resistance to oxygen removal as the oxygen concentration decreases.

The solubility of different titanium oxides in

CaCl₂ is not taken into consideration in the calculation of the potentials for reactions (1) to (8) . The significance of this is that some of reactions (1) to (8) may take place at potentials that are higher or lower than the potentials stated above at the stated temperature of 950°C.

For example, reduced activity of TiO will reduce the value of the potentials of reactions (2), (4) and (6) (i.e. make the potentials more positive) and at the same time will increase the potential of reaction (7) (i.e. make it more negative) .

In view of the above, the applicant has realised that it is likely to be extremely difficult to reduce titanium oxide in an electrolytic cell to titanium (αTi) of high purity, i.e. low concentration of oxygen (no more than lOOppm oxygen) in a single stage operation.

Specifically, the applicant has realised that it is necessary to refresh the electrolyte and/or to change cell potential in a later stage or in later stages of the operation of the electrolytic cell in order to reduce titanium oxide in an electrolytic cell to α titanium of high purity, ie low concentration of oxygen.

According to the present invention there is provided a method of reducing a titanium oxide in a solid state in an electrolytic cell which includes an anode, a cathode formed at least in part from the titanium oxide, and a molten electrolyte which includes cations of a metal that is capable of chemically reducing the cathode titanium oxide, which method includes operating the cell at a potential that is above a potential at which cations of the metal that is capable of chemically reducing the cathode titanium oxide deposit as the metal on the cathode, whereby the metal chemically reduces the cathode titanium oxide, and which method is characterised by refreshing the electrolyte and/or changing the cell potential in later stages of the operation of the cell as required having regard to the reactions occurring in the cell and the concentration of oxygen in the titanium oxides in the cell in order to produce high purity titanium (αTi) .

The term "high purity" is understood to mean that the concentration of oxygen is no more than lOOppm in the titanium.

In effect, the present invention is concerned with selecting the operating conditions of the cell, including cell potential and/or electrolyte composition, during various stages of the operation in the cell having regard to the reactions that take place in the cell . The applicant envisages at this stage that commercial operations will be at constant currant and that it may not be possible to achieve voltages required to remove oxygen to very low levels because of composition changes in the electrolyte. In these circumstances, refreshing and or changing the electrolyte composition is important in order to produce a high purity α titanium.

The above-described method makes it possible to produce titanium of high purity with respect to oxygen in an electrolytic cell and without refining or otherwise processing the titanium outside the electrolytic cell.

The method may include refreshing the electrolyte by adding new electrolyte to the existing electrolyte or otherwise adjusting the composition of the electrolyte.

In addition, the method may include carrying out the method in a series of electrolytic cell and successively transferring the partially reduced titanium oxide to each of the cells in the series.

The composition of the electrolyte in each cell may be selected having regard to the reactions occurring in the cell and the concentration of oxygen in the titanium oxide in the cell.

The cell potential may be changed at different stages in the method on a continuous or a step-change basis.

Preferably the metal deposited on the cathode is soluble in the electrolyte and can dissolve in the electrolyte and thereby migrate to the vicinity of the cathode titanium oxide.

It is preferred that the electrolyte be a CaCl₂- based electrolyte that includes CaO as one of the constituents of the electrolyte.

In such a situation it is preferred that the cell potential be above the potential at which Ca metal can deposit on the cathode, i.e. the decomposition potential of CaO.

The decomposition potential of CaO can vary over a considerable range depending on factors such as the composition of the anode, the electrolyte temperature and electrolyte composition.

In a cell containing CaO saturated CaCl₂ at 1373K (1100 °C) and a graphite anode this would require a minimum cell potential of 1.34V.

It is also preferred that the cell potential be below the decomposition potential of CaCl₂.

In a cell containing CaO saturated CaCl₂ at 1373 (1100 °C) and a graphite anode this would require that the cell potential be less than 3.5V. The decomposition potential of CaCl₂ can vary over a considerable range depending on factors such as the composition of the anode, the electrolyte temperature and electrolyte composition.

For example, a salt containing 80% CaCl₂ and 20% KC1 at a temperature of 900K (657°C), decomposes to Ca (metal) and Cl₂ (gas) above 3.4V and a salt containing 100% CaCl₂ at 1373K (1100°C) decomposes at 3.0V.

In general terms, in a cell containing CaO-CaCl₂ salt (not saturated) at a temperature in the range of 600- 1100°C and a graphite anode it is preferred that the cell potential be between 1.3 and 3.5V.

The CaCl₂-based electrolyte may be a commercially available source of CaCl₂, such as calcium chloride dihydrate, that partially decomposes on heating and produces CaO or otherwise includes CaO.

Alternatively, or in addition, the CaCl₂-based electrolyte may include CaCl and CaO that are added separately or pre-mixed to form the electrolyte.

It is preferred that the anode be graphite or an inert anode .

The cell may be of the type disclosed in the drawings of the patent specification lodged with Australian provisional application PS3049.

Claims

1. A method of reducing a titanium oxide in a solid state in an electrolytic cell which includes an anode, a cathode formed at least in part from the titanium oxide, and a molten electrolyte which includes cations of a metal that is capable of chemically reducing the cathode titanium oxide, which method includes operating the cell at a potential that is above a potential at which cations of the metal that is capable of chemically reducing the cathode titanium oxide deposit as the metal on the cathode, whereby the metal chemically reduces the cathode titanium oxide, and which method is characterised by refreshing the electrolyte and/or changing the cell potential in later stages of the operation of the cell as required having regard to the reactions occurring in the cell and the concentration of oxygen in the titanium oxides in the cell in order to produce high purity titanium (αTi) .

2. The method defined in claim 1 wherein the metal deposited on the cathode is soluble in the electrolyte and can dissolve in the electrolyte and thereby migrate to the vicinity of the cathode titanium oxide.

3. The method defined in claim 1 or claim 2 wherein the electrolyte is a CaCl₂-based electrolyte that includes CaO as one of the constituents of the electrolyte.

4. The method defined in claim 3 wherein the cell potential be above the potential at which Ca metal can deposit on the cathode, i.e. the decomposition potential of CaO.

5. The method defined in claim 3 or claim 4 wherein the cell potential is below the decomposition potential of CaCl₂.

6. The method defined in any one of claims 3 to 5 wherein at a temperature in the range of 600-1100°C and a graphite anode the cell potential is between 1.3 and 3.5V.

7. The method defined in any one of claims 3 to 6 wherein the CaCl₂-based electrolyte is a commercially available source of CaCl₂, such as calcium chloride dihydrate, that partially decomposes on heating and produces CaO or otherwise includes CaO.

8. The method defined in any one of claims 3 to 7 wherein the CaCl₂-based electrolyte includes CaCl₂ and CaO that are added separately or pre-mixed to form the electrolyte.

9. The method defined in any one of the preceding claims wherein the anode is graphite or an inert anode.