Solved Oxidation-Reduction Worksheet For each reaction | Chegg.com - Free Printable

1. Mg + 2HCl → MgCl₂ + H₂
- Atom oxidized: Mg (0 → +2)
- Atom reduced: H (+1 → 0)
- Oxidizing agent: HCl
- Reducing agent: Mg
- Oxidation half-reaction: Mg → Mg²⁺ + 2e⁻
- Reduction half-reaction: 2H⁺ + 2e⁻ → H₂
- Balanced equation: Mg + 2H⁺ → Mg²⁺ + H₂

2. 2Fe + 3V₂O₃ → Fe₂O₃ + 6VO
- Atom oxidized: Fe (0 → +3)
- Atom reduced: V (+3 → +2)
- Oxidizing agent: V₂O₃
- Reducing agent: Fe
- Oxidation half-reaction: 2Fe → 2Fe³⁺ + 6e⁻
- Reduction half-reaction: 6V³⁺ + 6e⁻ → 6V²⁺
- Balanced equation: 2Fe + 6V³⁺ → 2Fe³⁺ + 6V²⁺

3. KMnO₄ + KNO₂ + 2H₂SO₄ → MnSO₄ + 2H₂O + KNO₃ + K₂SO₄
- Atom oxidized: N (+3 → +5)
- Atom reduced: Mn (+7 → +2)
- Oxidizing agent: KMnO₄
- Reducing agent: KNO₂
- Oxidation half-reaction: NO₂⁻ → NO₃⁻ + 2e⁻
- Reduction half-reaction: MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O
- Balanced equation: 5NO₂⁻ + 2MnO₄⁻ + 6H⁺ → 5NO₃⁻ + 2Mn²⁺ + 3H₂O

4. K₂Cr₂O₇ + SnCl₂ + HCl → CrCl₃ + SnCl₄ + KCl + H₂O
- Atom oxidized: Sn (+2 → +4)
- Atom reduced: Cr (+6 → +3)
- Oxidizing agent: K₂Cr₂O₇
- Reducing agent: SnCl₂
- Oxidation half-reaction: Sn²⁺ → Sn⁴⁺ + 2e⁻
- Reduction half-reaction: Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O
- Balanced equation: 3Sn²⁺ + Cr₂O₇²⁻ + 14H⁺ → 3Sn⁴⁺ + 2Cr³⁺ + 7H₂O

5. 2KMnO₄ + 10NaCl + 8H₂SO₄ → 5Cl₂ + K₂SO₄ + 2MnSO₄ + 8H₂O + 5Na₂SO₄
- Atom oxidized: Cl (-1 → 0)
- Atom reduced: Mn (+7 → +2)
- Oxidizing agent: KMnO₄
- Reducing agent: NaCl
- Oxidation half-reaction: 2Cl⁻ → Cl₂ + 2e⁻
- Reduction half-reaction: MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O
- Balanced equation: 10Cl⁻ + 2MnO₄⁻ + 16H⁺ → 5Cl₂ + 2Mn²⁺ + 8H₂O

6. K₂Cr₂O₇ + H₂O + 3S → 3SO₂ + 2KOH + Cr₂O₃
- Atom oxidized: S (0 → +4)
- Atom reduced: Cr (+6 → +3)
- Oxidizing agent: K₂Cr₂O₇
- Reducing agent: S
- Oxidation half-reaction: S → SO₂ + 4e⁻
- Reduction half-reaction: Cr₂O₇²⁻ + 8H⁺ + 6e⁻ → 2Cr³⁺ + 4H₂O
- Balanced equation: 3S + Cr₂O₇²⁻ + 8H⁺ → 3SO₂ + 2Cr³⁺ + 4H₂O

7. 8KClO₃ + 3C₁₂H₂₂O₁₁ → 8KCl + 11H₂O + 12CO₂
- Atom oxidized: C (0 → +4)
- Atom reduced: Cl (+5 → -1)
- Oxidizing agent: KClO₃
- Reducing agent: C₁₂H₂₂O₁₁
- Oxidation half-reaction: C₁₂H₂₂O₁₁ → 12CO₂ + 48e⁻
- Reduction half-reaction: ClO₃⁻ + 6e⁻ → Cl⁻
- Balanced equation: 8ClO₃⁻ + C₁₂H₂₂O₁₁ → 8Cl⁻ + 12CO₂ + 11H₂O

8. 5H₂C₂O₄ + 2K₂MnO₄ → 10CO₂ + 2K₂O + 2Mn₂O₃ + 5H₂O
- Atom oxidized: C (+3 → +4)
- Atom reduced: Mn (+6 → +3)
- Oxidizing agent: K₂MnO₄
- Reducing agent: H₂C₂O₄
- Oxidation half-reaction: H₂C₂O₄ → 2CO₂ + 2e⁻
- Reduction half-reaction: 2MnO₄²⁻ + 8H⁺ + 6e⁻ → Mn₂O₃ + 4H₂O
- Balanced equation: 3H₂C₂O₄ + 2MnO₄²⁻ + 8H⁺ → 6CO₂ + Mn₂O₃ + 8H₂O

9. 2Mn(NO₃)₂ + 5NaBiO₃ + 16HNO₃ → 2HMnO₄ + 5Bi(NO₃)₃ + 5NaNO₃ + 7H₂O
- Atom oxidized: Mn (+2 → +7)
- Atom reduced: Bi (+5 → +3)
- Oxidizing agent: NaBiO₃
- Reducing agent: Mn(NO₃)₂
- Oxidation half-reaction: Mn²⁺ → MnO₄⁻ + 5e⁻
- Reduction half-reaction: BiO₃⁻ + 6H⁺ + 2e⁻ → Bi³⁺ + 3H₂O
- Balanced equation: 2Mn²⁺ + 5BiO₃⁻ + 30H⁺ → 2MnO₄⁻ + 5Bi³⁺ + 15H₂O

10. 5H₂C₂O₄ + 2KMnO₄ → 10CO₂ + K₂O + 2Mn₂O₃ + 5H₂O
- Atom oxidized: C (+3 → +4)
- Atom reduced: Mn (+7 → +3)
- Oxidizing agent: KMnO₄
- Reducing agent: H₂C₂O₄
- Oxidation half-reaction: H₂C₂O₄ → 2CO₂ + 2e⁻
- Reduction half-reaction: 2MnO₄⁻ + 12H⁺ + 8e⁻ → Mn₂O₃ + 6H₂O
- Balanced equation: 5H₂C₂O₄ + 2MnO₄⁻ + 12H⁺ → 10CO₂ + Mn₂O₃ + 11H₂O