Answer:
3Zn(s) + 2FeCl₃(aq) → 2Fe(s) + 3ZnCl₂ (aq)
Explanation:
This is a redox reaction where solid iron is formed by the reaction of Zn and Iron(III) chloride. We called redox because the iron is reduced and the zinc is oxidized.
The reactants are: Zn(s) and FeCl₃(aq)
The products are: ZnCl₂(aq) and Fe(s)
Zn(s) → Zn²⁺(aq) + 2e⁻ Oxidation
Fe³⁺(aq) + 3e⁻ → Fe(s) Reduction
The e- are unballanced so we multiply the half reactions:
(Zn(s) → Zn²⁺(aq) + 2e⁻) . 3 → 3Zn(s) → 3Zn²⁺(aq) + 6e⁻
(Fe³⁺(aq) + 3e⁻ → Fe(s)) . 2 → 2Fe³⁺(aq) + 6e⁻ → 2Fe(s)
When we sum the half reactions, the electrons can be cancelled:
3Zn(s) + 2Fe³⁺(aq) + 6e⁻ → 2Fe(s) + 3Zn²⁺(aq) + 6e⁻
Balanced equation: 3Zn(s) + 2FeCl₃(aq) → 2Fe(s) + 3ZnCl₂ (aq)
