Here's the breakdown:
* Reactivity Series: Aluminum is higher on the reactivity series than copper. This means aluminum is more reactive and will displace copper from its compound.
* Reaction: When aluminum is added to a solution of copper(II) sulfate, the aluminum atoms lose electrons and become aluminum ions (Al³⁺). These electrons are then gained by the copper(II) ions (Cu²⁺), reducing them to copper atoms (Cu).
* Products: This reaction produces a solution of aluminum sulfate (Al₂(SO₄)₃) and solid copper.
The chemical equation for the reaction is:
2Al(s) + 3CuSO₄(aq) → Al₂(SO₄)₃(aq) + 3Cu(s)
Key points:
* This reaction is exothermic, meaning it releases heat.
* The copper metal produced will be deposited on the surface of the aluminum, often giving it a reddish-brown color.
* The reaction can be used to demonstrate the concept of the reactivity series and the principles of redox reactions.
