* Iron becomes coated with copper: You will see a reddish-brown coating forming on the iron. This is because iron is more reactive than copper.
* The blue copper sulphate solution turns pale: The blue color of the copper sulphate solution fades as the copper ions react with the iron.
* The solution may turn slightly green: This is due to the formation of iron(II) sulphate, which is a pale green solution.
Here's why this happens:
1. Displacement Reaction: This is a classic example of a displacement reaction. A more reactive metal (iron) displaces a less reactive metal (copper) from its salt solution.
2. Iron's Reactivity: Iron is higher on the reactivity series than copper. This means it has a stronger tendency to lose electrons and form positive ions.
3. Reaction Equation: The reaction can be represented by the following equation:
```
Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)
```
* Iron (Fe) reacts with copper sulphate (CuSO₄).
* Iron(II) sulphate (FeSO₄) is formed in solution.
* Copper (Cu) is deposited on the iron surface.
In Summary: The iron displaces the copper from the copper sulphate solution, forming iron(II) sulphate and causing a reddish-brown copper coating to form on the iron.
