Edited by Jamie (ScienceAid Editor), Taylor (ScienceAid Editor)
This is an industrial process to reduce iron oxides to obtain iron. It is a continuous process where iron (III) oxide (Fe2O3), coke and limestone are fed into the top of the furnace, and heated by having hot air blown in near the bottom. There is a whole series of reactions taking place in the blast furnace (for a diagram see here).
- 1First of all, the coke reacts with the oxygen in an exothermic reaction to form carbon dioxide.Advertisement
- 2The carbon dioxide then reacts with further coke to make carbon monoxide, which is the reducing agent.
C + O2 ==>> 2CO2 CO2 + C ==>> 2CO
Now at about 1200°C, carbon monoxide reduces most of the iron (III) oxide as follows:
Fe2O3 + 3CO ==>> 2Fe(l) 3COFe2
The the limestone decomposes to form carbon dioxide (which can become carbon monoxide for the above reactions) and calcium oxide and this removes some sand impurities as slag, which is used to make construction materials.
CaCO3 ==>> CaO(s) + CO2 CaO + SiO2 ==>> CaSiO3 (l)
The problem with the iron that is produced from the blast furnace is that it is quite impure. It has to be treated to remove these impurities.
- 1Magnesium is added to the mixture, which reacts with sulphur to form MgS
- 2This forms oxides of phosphorous, manganese etc. which react with CaO to make a slag that floats to the top. However, not all carbon is removed, but this is good because pure iron is too soft and a bit of it makes it stronger but not so much that it is brittle.Oxygen is blown into the the molten mixture with lime added in the Basic Oxygen Process.
It is not possible to extract all metals by this process because rather than form pure metal, they react to form carbides. For example titanium which reacts with carbon to make carbide: TiO2 + 3C ==>> TiC + 2CO
Aluminium is extracted from Bauxite by electrolysis. This is done by dissolving it in molten cryolite. This lowers the required heat to melt Aluminium Oxide from 2000°C to 970°C. At the cathode, aluminium is reduced and at the cathode oxygen is oxidized in the following reactions. Al3+ + 3e- ==>> Al 2O2- ==>> O2 + 4e- In terms of the economics, this process requires a lot of electricity which means it is only done in places where using large amounts of electricity is inexpensive. The process also causes environmental damage because some of the oxygen produced, reacts with the anode (which is carbon) to form carbon monoxide and carbon dioxide. And the waste cryolite could contaminate and cause fluoride pollution.
Titanium is a very useful metal, but unlike iron, having any carbon in it ruins the strength of Titanium, therefore titanium is extracted from a chloride. But the Ore is Titanium Oxide (TiO2) also known as rutile. This is converted into titanium (IV) chloride using chlorine and coke at 900°C in the following reaction.
TiO2 + 2C + 2Cl2 ==>> TiCl4 + 2CO
Titanium Chloride is a colourless liquid and is then purified by fractional distillation. And now to extract the titanium, it is reduced by sodium (or magnesium) at 500°C, but since the reaction is exothermic, the temperature eventually gets up to 1000°C. The reaction is also performed in an atmosphere of argon because it is a noble gas and doesn't react. This is to prevent contamination with oxygen or nitrogen.
TiCl4 + 4Na ==>> Ti + 4NaCl
It is called a batch process because it isn't continuous, and is very expensive because of:
- The extra chemicals that have to be added.
- The high temperatures.
- The danger of TiCl2.
- The argon atmosphere that has to be maintained.
Despite the properties of titanium being more desirable than steel, and its larger abundance compared to iron, it is only used in circumstances when nothing else will do because of the cost of production.
Around the world, but especially in the UK where landfill sites have only a few years left, recycling is being used more and more to prevent wastage and carbon emissions. But here we look at the science and reality of recycling.
Iron and Aluminium are examples of two metals that are extensively recycled. Your soft drink cans are usually made of one of these.
- 1Iron is recycled in a number of ways.
- A large amount is added to the BOS process before the impure iron is added, but this produces carbon dioxide. ##Another method, which is much easier and also doesn't directly produce any carbon dioxide, is to simply melt the scrap.
- 2Because of the expense of extracting it from its ore; melting cans uses only 5% of the energy, compared to extracting the equivalent amount. The quality of this metal is often very good, however, there is an energy cost of collecting and sorting all of the rubbish which also has to be considered before deciding whether recycling or extraction is more efficient.Aluminium, on the other hand is a more desirable metal to recycle.Advertisement
Referencing this Article
If you need to reference this article in your work, you can copy-paste the following depending on your required format:
APA (American Psychological Association)
Metal Extraction. (2017). In ScienceAid. Retrieved Jul 24, 2017, from https://scienceaid.net/chemistry/inorganic/extraction.html
MLA (Modern Language Association) "Metal Extraction." ScienceAid, scienceaid.net/chemistry/inorganic/extraction.html Accessed 24 Jul 2017.
Chicago / Turabian ScienceAid.net. "Metal Extraction." Accessed Jul 24, 2017. https://scienceaid.net/chemistry/inorganic/extraction.html.
Categories : Inorganic
Recent edits by: Jamie (ScienceAid Editor)