Extraction of Aluminium by Electrolysis
Edited by Jamie (ScienceAid Editor), SpellBot, Taylor (ScienceAid Editor), Administrator
Please note that this article uses the British English spelling of aluminium, but this is exactly the same as aluminum - this is simply the North American English spelling.
Aluminium has a very high melting point and strong bonding between atoms, so it doesn't readily dissolve in water. Instead, molten cryolite (Na3AIF6) is used.
The pure aluminium is attracted to the cathode, which is a lining of graphite. The oxygen is attracted to the anode, and bubbles through the solution.
At the cathode, reduction takes place as electrons are gained:
Al3+ + 3e- ® Al
At the anode, oxidation takes place as electrons are lost:
2O2- ® O2 + 4e-
At the anode also, the oxygen formed will react with the anode (which is made of carbon) to form carbon dioxide. This means, the anodes must be frequently replaced.
This process uses A lot of electricity and is expensive. Therefore, aluminium is much more expensive than other metals that are easier to extract (like iron, but its desirable characteristics mean that it is still widely used.
Aluminium is the most widely used metal after iron. It is mostly used in an alloy with another metal, this means it is mixed with another metal to produce another compound that has a certain desirable characteristic - like stainless steel.
Some common uses of aluminium include, making cars, trains, and bicycles. Because it's reasonably strong, but not too heavy, your aluminium bicycle won't break and won't be too difficult to ride. Some packaging like foil and cans are also made from aluminium. This is especially important in recycling since some soft drink cans are made from steel rather than aluminium - but they can be sorted using magnets. Cooking utensils are often made from aluminium because it is very good at conducting heat, and will warm the food evenly.
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Categories : Applied
Recent edits by: Taylor (ScienceAid Editor), SpellBot, Jamie (ScienceAid Editor)