If a piece of aluminium is added to iron(II) sulphate (FeSO4) solution, what will happen?
Iron will get deposited.
This is a displacement reaction. In the reactivity (activity) series of metals, aluminium lies above iron, meaning aluminium is more reactive than iron. A more reactive metal can displace a less reactive metal from its salt solution.
So aluminium displaces iron from iron(II) sulphate: \(2Al + 3FeSO_4 \rightarrow Al_2(SO_4)_3 + 3Fe\). The displaced iron settles out as a solid deposit, while aluminium goes into solution as aluminium sulphate.
Therefore, iron will get deposited.
Aluminium will not get deposited; it is the metal that dissolves into the solution, not the one that comes out. A blue solution is characteristic of copper(II) salts, not iron(II) sulphate, which is pale green. "No reaction" is incorrect because aluminium is more reactive than iron, so a displacement reaction does occur.
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