Question

which compound is oxidized in the following reaction: fe(s) + cuso4(aq) → feso4(aq) + cu(s) fe(s) cu(s) cuso4(aq) feso4(aq)

Explanation:

Step1: Determine oxidation states

• For \(Fe(s)\), the oxidation state of \(Fe\) is \(0\).
• In \(FeSO_4(aq)\), the oxidation state of \(Fe\) is \(+2\) (since \(SO_4^{2 -}\) has a charge of \(- 2\) and the compound is neutral).
• For \(Cu(s)\), the oxidation state of \(Cu\) is \(0\).
• In \(CuSO_4(aq)\), the oxidation state of \(Cu\) is \(+2\).

Step2: Analyze oxidation

Oxidation is the loss of electrons (increase in oxidation state).

• \(Fe\) goes from \(0\) (in \(Fe(s)\)) to \(+2\) (in \(FeSO_4(aq)\)). So \(Fe\) is oxidized.
• \(Cu\) goes from \(+2\) (in \(CuSO_4(aq)\)) to \(0\) (in \(Cu(s)\)). So \(Cu\) is reduced.

Answer:

\(Fe(s)\)