FFC_Cambridge_process Knowpia

The FFC Cambridge process is an electrochemical method for producing Titanium (Ti) from titanium oxide by electrolysis in molten calcium salts.^[1]

History edit

A process for electrochemical production of titanium through the reduction of titanium oxide in a calcium chloride solution was first described in a 1904 German patent,^[1]^[2]^[3] and later in a US patent by Carl Marcus Olson.^[4]

The FFC Cambridge process was developed by George Chen, Derek Fray, and Thomas Farthing between 1996 and 1997 at the University of Cambridge. (The name FFC derives from the first letters of the last names of the inventors).^[5] The intellectual property relating to the technology has been acquired by Metalysis, (Sheffield, UK).^{[citation needed]}

Process edit

The process typically takes place between 900 and 1100 °C, with an anode (typically carbon) and a cathode (the oxide being reduced) in a solution of molten CaCl₂. Depending on the nature of the oxide it will exist at a particular potential relative to the anode, which is dependent on the quantity of CaO present in CaCl₂.

Cathode reaction mechanism edit

The electrocalciothermic reduction mechanism may be represented by the following sequence of reactions, where "M" represents a metal to be reduced (typically titanium).

(1) MO
_x+ x Ca → M + x CaO

When this reaction takes place on its own, it is referred to as the "calciothermic reduction" (or, more generally, an example of metallothermic reduction). For example, if the cathode was primarily made from TiO then calciothermic reduction would appear as:

TiO + Ca → Ti + CaO

Whilst the cathode reaction can be written as above it is in fact a gradual removal of oxygen from the oxide. For example, it has been shown that TiO₂ does not simply reduce to Ti. It, in fact, reduces through the lower oxides (Ti₃O₅, Ti₂O₃, TiO etc.) to Ti.

The calcium oxide produced is then electrolyzed:

(2a) x CaO → x Ca²⁺ + x O²⁻

(2b) x Ca²⁺ + 2x e⁻ → x Ca

and

(2c) x O²⁻ → x/2 O₂ + 2x e⁻

Reaction (2b) describes the production of Ca metal from Ca²⁺ ions within the salt, at the cathode. The Ca would then proceed to reduce the cathode.

The net result of reactions (1) and (2) is simply the reduction of the oxide into metal plus oxygen:

(3) MO
_x→ M + x/2 O₂

Anode reaction mechanism edit

The use of molten CaCl₂ is important because this molten salt can dissolve and transport the "O²⁻" ions to the anode to be discharged. The anode reaction depends on the material of the anode. Depending on the system it is possible to produce either CO or CO₂ or a mixture at the carbon anode:

C + 2O²⁻ → CO₂ +4
e⁻

C + O²⁻ → CO + 2
e⁻

However, if an inert anode is used, such as that of high density SnO₂, the discharge of the O²⁻ ions leads to the evolution of oxygen gas. However the use of an inert anode has disadvantages. Firstly, when the concentration of CaO is low, Cl₂ evolution at the anode becomes more favourable. In addition, when compared to a carbon anode, more energy is required to achieve the same reduced phase at the cathode. Inert anodes suffer from stability issues.

2O²⁻ → O₂ + 4
e⁻

References edit

^ ^a ^b Takeda, O.; Ouchi, T.; Okabe, T. H. (2020). "Recent Progress in Titanium Extraction and Recycling". Metall. Mater. Trans. B. 51 (4): 1315–1328. doi:10.1007/s11663-020-01898-6.
^ DE150557C, "Publication of DE150557C"
^ Rideal, Eric Keightley (1919). Industrial Electrometallurgy, Including Electrolytic and Electrothermal Processes. D. Van Nostrand co. p. 137.
^ US2845386A, Marcus, Olson Carl, "Production of metals", issued 1958-07-29
^ Fray, D. J.; Chen, G. Z.; Farthing, T. W. (2000). "Direct Electrochemical Reduction of Titanium Dioxide to Titanium in Molten Calcium Chloride". Nature. 407 (6802): 361–4. Bibcode:2000Natur.407..361C. doi:10.1038/35030069. PMID 11014188. S2CID 205008890.