CuSO₄ (aq) + Fe (s) → FeSO₄ (aq) + Cu (s)
Here's a breakdown of what happens:
* Iron (Fe) is more reactive than copper (Cu). This means iron has a stronger tendency to lose electrons and form positive ions.
* When iron is added to a solution of copper(II) sulfate, the iron atoms displace the copper ions from the solution.
* The iron atoms lose electrons and become iron(II) ions (Fe²⁺), which then combine with the sulfate ions (SO₄²⁻) to form iron(II) sulfate (FeSO₄).
* The copper ions (Cu²⁺) gain electrons and become copper metal (Cu), which precipitates out of the solution.
You can observe this reaction visually:
* The blue color of the copper(II) sulfate solution will fade as the reaction proceeds.
* A reddish-brown deposit of copper metal will form on the surface of the iron.
Important Note: The reaction rate can be increased by:
* Using a more reactive form of iron, like iron filings or powdered iron.
* Heating the solution.
* Increasing the surface area of the iron.
