Reaction:
Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)
Explanation:
* Iron (Fe) is more reactive than copper (Cu). This means iron can displace copper from its compound.
* Copper(II) sulfate (CuSO₄) is a soluble ionic compound, meaning it exists as ions in solution.
* When iron is added to the solution, it reacts with the copper ions (Cu²⁺) to form iron(II) sulfate (FeSO₄), which is also soluble.
* Copper (Cu), now in its elemental form, is less reactive and precipitates out of the solution as a solid.
Observation:
Visually, you'll observe the following:
* The blue color of the copper(II) sulfate solution fades as the reaction proceeds.
* A reddish-brown solid (copper) will form and settle at the bottom of the container.
Net Ionic Equation:
Fe(s) + Cu²⁺(aq) → Fe²⁺(aq) + Cu(s)
This equation focuses only on the species that are directly involved in the reaction.
