Reaction:
2 Al(s) + 3 FeSO₄(aq) → Al₂(SO₄)₃(aq) + 3 Fe(s)
Explanation:
* Aluminum (Al) is more reactive than iron (Fe). This means aluminum has a stronger tendency to lose electrons and form positive ions.
* When aluminum is placed in a solution of iron(II) sulfate, it displaces the iron ions from the solution.
* Aluminum (Al) loses electrons and forms aluminum ions (Al³⁺).
* Iron (Fe) ions gain electrons and form iron atoms (Fe).
* The sulfate ions (SO₄²⁻) remain in solution.
* Aluminum sulfate (Al₂(SO₄)₃) is formed, which is soluble in water.
* Iron (Fe) is deposited as a solid.
Observations:
* You would observe the formation of a gray-black solid (iron) at the bottom of the container.
* The solution would change color from light green (FeSO₄) to colorless (Al₂(SO₄)₃).
Note: This reaction is a classic example of a single displacement reaction, and it demonstrates the reactivity series of metals. The more reactive metal will always displace the less reactive metal from its salt solution.
