Fe + CuSO4 → Cu + FeSO4

This reaction represents a single replacement (or single displacement) reaction where iron (Fe) displaces copper (Cu) from copper(II) sulfate (CuSO₄). The products of the reaction are copper (Cu) and iron(II) sulfate (FeSO₄).

To break it down:

• Reactants: Iron (Fe) and Copper(II) sulfate (CuSO₄).
• Products: Copper (Cu) and Iron(II) sulfate (FeSO₄).

The balanced chemical equation is:

\[ \text{Fe (s)} + \text{CuSO}_4 \text{ (aq)} \rightarrow \text{Cu (s)} + \text{FeSO}_4 \text{ (aq)} \]

Key Points:

• Iron is more reactive than copper, which allows it to displace copper from its compound.
• This reaction is also an example of a redox reaction, where iron is oxidized (loses electrons) and copper is reduced (gains electrons).
• In a lab setting, you would observe the formation of solid copper and a change in the color of the solution as the blue copper(II) sulfate solution turns pale yellow due to the formation of iron(II) sulfate.

Make sure to understand the concepts of reactivity series, redox reactions, and balancing chemical equations for your exams!