EP1492905A1

EP1492905A1 - Reduction of metal oxides in an electrolytic cell

Info

Publication number: EP1492905A1
Application number: EP03743767A
Authority: EP
Inventors: Les Strezov; Ivan Ratchev; Steve Osborn
Original assignee: BHP Billiton Innovation Pty Ltd
Current assignee: Metalysis Ltd
Priority date: 2002-03-13
Filing date: 2003-03-13
Publication date: 2005-01-05
Also published as: KR20040111408A; CN1650051B; BR0308384A; EP1492905A4; EA007046B1; BR0308384B1; EP2770086A2; NO340277B1; EP2770086A3; CA2479048A1; JP4658479B2; JP2005520045A; KR20110025237A; NZ531467A; EA200401203A1; KR101038701B1; WO2003076690A1; CA2479048C; ZA200407434B; NO20043857L

Abstract

A method of reducing a metal oxide, such as titania in a solid state in an electrolytic cell is disclosed. The electrolytic cell includes an anode, a cathode, and a molten electrolyte. The electrolyte includes cations of a metal that is capable of chemically reducing the metal oxide. The metal oxide in a solid state is immersed in the electrolyte. The 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 metal oxide deposit as the metal on the cathode, whereby the metal chemically reduces the metal oxide.

Description

REDUCTION OF METAL OXIDES IN AN ELECTROLYTIC CELL

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

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

During the course of the research project the applicant carried out experimental work on the reduction of titania using an electrolytic cell that included a graphite crucible that formed an anode of the cell, a pool of molten CaCl₂-based electrolyte in the crucible/ and a range of cathodes that included solid titania.

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 of that International application.

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 at an electrode formed from the metal oxide that is lower than the deposition potential of cations in the electrolyte at a surface of the electrode.

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 decomposition potential of the electrolyte. If higher potentials are used then, as noted in DI and D2, the cation in the electrolyte deposits on the metal or semi - metal compound. In the example of DI, this leads to calcium deposition and therefore consumption of this reactive metaI............Duringr 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.

Accordingly, the present invention provides a method of reducing a metal oxide in a solid state in an electrolytic cell, which electrolytic cell includes an anode, a cathode, a molten electrolyte, the electrolyte includes cations of a metal that is capable of chemically reducing the metal oxide, and the metal oxide in a solid state immersed in the electrolyte, and 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 metal oxide can deposit as the metal on the cathode, whereby the metal chemically reduces the metal oxide.

The applicant does not have a clear understanding of the electrolytic cell mechanism at this stage.

Nevertheless, whilst not wishing to be bound by the comments in this and the following paragraphs, the applicant offers the following comments by way of an outline of a possible cell mechanism.

The experimental work carried out by the applicant produced evidence of Ca metal dissolved in the electrolyte. The applicant believes that, at least during the early stages of operation of the cell, the Ca metal was the result of electrodeposition of Ca⁺⁺ cations as Ca metal on electrically conductive sections of the cathode. The experimental work was carried out using a CaCl₂-based electrolyte at a cell potential below the decomposition potential of CaCl₂. The applicant believes that the initial deposition of Ca metal on the cathode was due to the presence of Ca⁺⁺ cations and O^" anions derived from CaO in the electrolyte. The decomposition potential of CaO is less than the decomposition potential of CaCl₂. In this cell mechanism the cell operation is dependent, at least during the early stages of cell operation, on decomposition of CaO, with Ca⁺⁺ cations migrating to the cathode and depositing as Ca metal and O^" anions migrating to the anode and forming CO and/or C0₂ (in a situation in which the anode is a graphite anode) .

The applicant believes that the Ca metal that deposited on electrically conductive sections of the cathode was deposited predominantly as a separate phase in the early stages of cell operation and thereafter dissolved in the electrolyte and migrated to the vicinity of the titania in the cathode and participated in chemical reduction of titania.

The applicant also believes that at later stages of the cell operation part of the Ca metal that deposited on the cathode was deposited directly on partially deoxidised titanium and thereafter participated in chemical reduction of titanium.

The applicant also believes that the 0^""anions, once extracted from the titania, migrated to the anode and reacted with anode carbon and produced CO and/or C0₂ (and in some instances CaO) and released electrons that facilitated electrolytic deposition of Ca metal on the cathode.

Preferably the cathode is formed at least in part from the metal oxide.

Preferably the method includes operating the cell at the potential that is above the potential at which cations of the metal that is capable of chemically reducing the metal oxide deposit as the metal on the cathode so that the metal deposits on the cathode.

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 metal oxide .

In a situation in which the metal oxide is a titanium oxide, such as titania, it is preferred that the electrolyte be a CaCl₂-based electrolyte that includes CaO as one of the constituents of the electrolyte. In this context, it is noted that the present invention does not require the addition of substantial amounts of CaO to the electrolyte.

In such a situation it is preferred that the cell potential be above a potential at which Ca metal can deposit on the cathode, i.e. at a potential that is above 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 potential at which CI^" anions can deposit on the anode and form chlorine gas, i.e. the decomposition potential of CaCl₂.

In a cell containing CaO saturated CaCl₂ at 1373K (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 CaCl₂ 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 applicant found in the experimental work that there were relatively significant amounts of carbon transferred from the graphite anode to the electrolyte and to a lesser extent, to the titanium produced at the cathode under a wide range of cell operating conditions.

Carbon in the titanium is an undesirable contaminant. In addition, carbon transfer was partially responsible for low energy efficiency of the cell. Both problems could present significant barriers to commercialisation of electrolytic reduction technology.

The applicant also found that the dominant mechanism of carbon transfer is electrochemical rather than erosion and that one way of minimising carbon transfer and therefore contamination of titanium produced at the cathode by electrochemical reduction of titania is to position a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms between the cathode and the anode and thereby prevent migration of carbon to the cathode.

Accordingly, in order to minimise contamination of titanium produced at the cathode resulting from carbon transfer, it is preferred that the electrolytic cell includes a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms positioned between the cathode and the anode to thereby prevent migration of carbon to the cathode.

The membrane may be formed from any suitable material .

Preferably the membrane is formed from a solid electrolyte.

One solid electrolyte tested by the applicant is yttria stabilised zirconia.

According to the present invention there is also provided an electrolytic cell as described above and operating in accordance with the above described method.

The present invention is described further with reference to the following example.

I. Experimental Method and Electrolytic Cell

The electrolytic cell is shown in Figure 1.

With reference to Figure 1, the electrochemical cell included a graphite crucible equipped with a graphite lid. The crucible was used as the cell anode. A stainless steel rod was used to secure electrical contact between a d/c power supply and the crucible. The cell cathode consisted of Kanthal or platinum wire connected at one end to the power supply and Ti0₂ pellets suspended from the other end of the wire. An alumina tube was used as an insulator around the cathode. The cell electrolyte was a commercially available source of CaCl₂, namely calcium chloride dihydrate, that partially decomposed on heating at the operating temperature of the cell and produced CaO. A thermocouple was immersed in the electrolyte in close proximity to the pellets.

Two types of pellets were used. One type was slip-cast and the other type was pressed. Both types of pellets were made from analytical grade Ti0₂ powder. Both types of pellets were sintered in air at 850°C. One pressed and one slip-cast pellet were used in the experiment .

The cell was positioned in a furnace and the experiment was conducted at 950°C. Voltages up to 3V were applied between the crucible wall and the Kanthal or platinum wire. The voltage of 3V is below the potential at which CI^" anions can deposit on the anode at that temperature. In addition, the voltage of 3V is above the decomposition potential of CaO and below the decomposition potential of CaCl₂.

The power-supply maintained a constant voltage throughout the experiment. The voltage and resulting cell current were logged using LabVIEW (TM) data acquisition software.

At the end of the experiment the cell was removed from the furnace and quenched in water. The solid CaCl₂ was dissolved by water and the two pellets were recovered.

II. Experimental Results

With reference to Figures 2 and 3, the constant voltage (3V) used in the experiment produced an initial current of approximately 1.2A. A continuous drop in the current was observed during the initial 2 hours. After that a gradual increase in the current up to 1A was observed.

SEM images of the cross-sections of the two recovered pellets are shown in Figures 4 and 5. The SEM images indicate the presence of metallic titanium in both pellets, thereby establishing that the method successfully electrochemically reduced titania.

The presence of virtually pure metallic titanium in both pellets was confirmed by EPMA analysis. The analysis also showed areas of partially reduced titania. The EPMA results are shown in Figures 6 and 7.

Carbon was detected at various locations within the pellets and its content varied up to 18wt%. Many modifications may be made to the present invention as described above without departing from the the spirit and scope of the invention.

By way of example, whilst the above description of the invention focuses on reduction of titania, the invention is not so limited and extends to reduction of other titanium oxides and to oxides of other metals and alloys. Examples of other potentially important metals are aluminium, silicon, germanium, zirconium, hafnium, magnesium and molybdenum.

Furthermore, whilst the above description focuses on CaCl₂-based electrolyte, the invention is not so limited and extends to any other suitable electrolytes (and mixtures of electrolytes) . Generally, suitable electrolytes will be salts and oxides that are soluble in salts. One example of a potentially suitable electrolyte is BaCl₂.

Claims

CLAIMS :

1. A method of reducing a metal oxide in a solid state in an electrolytic cell, which electrolytic cell includes an anode, a cathode, a molten electrolyte, the electrolyte includes cations of a metal that is capable of chemically reducing the metal oxide, and the metal oxide in a solid state is immersed in the electrolyte, and 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 metal oxide can deposit as the metal on the cathode, whereby the metal chemically reduces the metal oxide .

2. The method defined in claim 1 includes operating the cell that is above the potential at which cations of the metal that is capable of chemically reducing the metal oxide deposit as the metal on the cathode so that the metal deposits on the cathode.

3. The method defined in claim 2 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 metal oxide.

4. The method defined in any one of the preceding claims wherein the metal oxide is a titanium oxide, the electrolyte is a CaCl₂-based electrolyte that includes CaO as one of the constituents of the electrolyte, and the cell potential is above a potential at which Ca metal can deposit on the cathode.

5. The method defined in claim 4 wherein the cell potential is below the decomposition potential for

CaCl₂ to minimise forming Cl₂ gas at the anode.

6. The method defined in claim 4 or claim 5 wherein the cell potential is less than or equal to 3.5V in a cell operating with the electrolyte at 600-1100°C.

7. The method defined in any one of claims 4 to 6 wherein the cell potential is at least 1.3V in a cell operating with the electrolyte at 600-1100°C.

8. The method defined in any one of claims 4 to 7 wherein the CaCl₂-based electrolyte is a commercially available source of CaCl₂ that forms CaO on heating or otherwise includes CaO.

9. The method defined in any one of claims 4 to 7 wherein the CaCl₂-based electrolyte includes CaCl₂ and

CaO that are added separately or pre-mixed to form the electrolyte.

10. The method defined in any one of the preceding claims wherein the anode is graphite.

11. The method defined in any one of the preceding claims wherein the anode is graphite and the electrolytic cell includes a membrane that is permeable to oxygen anions and is impermeable to carbon in ionic and non-ionic forms positioned between the cathode and the anode to thereby prevent migration of carbon to the cathode.

12. The method defined in any one of the preceding claims wherein the cathode is formed at least in part from the metal oxide .

13. An electrolytic cell reducing a metal oxide in a solid state, which electrolytic cell includes an anode, a cathode, a molten electrolyte, which electrolyte includes cations of a metal that is capable of chemically reducing the metal oxide, and a metal oxide in a solid state immersed in the electrolyte, and which electrolytic cell operates at a potential that is above a potential at which cations of the metal that is capable of chemically reducing the metal oxide deposit as the metal on the cathode, whereby the metal chemically reduces the metal oxide .

14. The cell defined in claim 12 wherein the cathode is formed at least in part from the metal oxide.