- 1a) Fe + CuSO₄ → FeSO₄ + Cu
- 1b) Fe(s) + Cu²⁺(aq) → Fe²⁺(aq) + Cu(s); Iron is oxidized, copper ions are reduced.
- 2) Pb(s) + Cu²⁺(aq) → Pb²⁺(aq) + Cu(s)
- Redox Half-Equations:
- CuO + Mg → MgO + Cu: Reduction: Cu²⁺ + 2e⁻ → Cu; Oxidation: Mg → Mg²⁺ + 2e⁻
- Fe₂O₃ + 2Al → 2Fe + Al₂O₃: Reduction: Fe³⁺ + 3e⁻ → Fe; Oxidation: Al → Al³⁺ + 3e⁻
- CuSO₄ + Zn → ZnSO₄ + Cu: Reduction: Cu²⁺ + 2e⁻ → Cu; Oxidation: Zn → Zn²⁺ + 2e⁻
- 2KBr + Cl₂ → 2KCl + Br₂: Reduction: Cl₂ + 2e⁻ → 2Cl⁻; Oxidation: 2Br⁻ → Br₂ + 2e⁻
- 2NaCl + F₂ → Cl₂ + 2NaF: Reduction: F₂ + 2e⁻ → 2F⁻; Oxidation: 2Cl⁻ → Cl₂ + 2e⁻
- Boost 1:
- H₂S + Cl₂ → S + 2HCl: Oxidation: H₂S → S + 2H⁺ + 2e⁻; Reduction: Cl₂ + 2e⁻ → 2Cl⁻
- Zn + 2HCl → ZnCl₂ + H₂: Oxidation: Zn → Zn²⁺ + 2e⁻; Reduction: 2H⁺ + 2e⁻ → H₂
- Boost 2: Bromine is less reactive than chlorine and cannot displace chloride ions from sodium chloride; fluorine is more reactive and would displace chloride, but bromine lacks sufficient oxidizing power under normal conditions.
Parent Tip: Review the logic above to help your child master the concept of redox reaction worksheet.
