- The reaction \(\mathrm{Fe}+\mathrm{CuSO}_4 \rightarrow \mathrm{FeSO}_4+\mathrm{Cu}\) involves the displacement of copper from copper sulfate by iron.
- This is because iron is more reactive than copper and can displace it from its compound.
- This is an example of a displacement reaction, which is a type of redox (reduction-oxidation) reaction where there is a transfer of electrons between the reactants.
- Iron (Fe) is oxidized to iron(II) sulfate \(\left(\mathrm{FeSO}_4\right)\), and copper \(\left(\mathrm{Cu}^{2+}\right)\) is reduced to copper \((\mathrm{Cu})\). This means there is a transfer of electrons, making it a redox reaction.