- When iron powder is added to an aqueous solution of copper sulphate, a displacement reaction occurs.
- Initially, the solution is blue in color due to the presence of copper ions.
- As iron powder is added, a red-brown solid forms and settles at the bottom of the container.
- The blue color of the solution fades as copper ions are displaced by iron.

The chemical equation for the reaction can be represented as:
Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)

- This is a single displacement reaction also known as a displacement reaction.
- In this reaction, iron (Fe) displaces copper (Cu) from the copper sulphate solution to form iron sulphate and copper metal.

- In the reaction between iron powder and copper sulphate, iron being more reactive than copper displaces copper from its compound.
- Iron (Fe) loses electrons to form Fe2+ ions, while copper (Cu2+) gains electrons to form solid copper metal.
- The blue color of the copper sulphate solution fades as copper ions are removed from the solution.
- The red-brown solid formed at the bottom of the container is copper metal.
- The iron sulphate formed remains in solution.
- This reaction is an example of the reactivity series, where metals higher in the reactivity series can displace metals lower in the series from their compounds.
- This reaction is a commonly used demonstration of single displacement reactions in chemistry.