Write the following redox reactions using half equations:

1. Zn_(s) + PbCl_2(aq) → Pb_(s) + ZnCl_2(aq)

2. 2Fe³⁺_(aq) + 2I⁻_(aq) → I_2(aq) + 2Fe²⁺_(aq)

3. 2Na_(s) + Cl_2(g) → 2NaCl_(s)

4. Mg_(s) + Cl_2(g) → MgCl_2(s)

5. Zn_(s) + 2H⁺_(aq) → Zn²⁺_(aq) + H_2(g)

Solution:

1. Zn_(s) → Zn²⁺_(aq) + 2e⁻ (oxidation)

   Pb²⁺_(aq) + 2e⁻ → Pb_(s) (reduction)

2. 2Fe³⁺_(aq) + 2e⁻ → 2Fe²⁺_(aq) (reduction)

   2I⁻_(aq) → I_2(aq) + 2e⁻ (reduction)

3. 2Na_(aq) → 2Na⁺_(aq) + 2e⁻ (oxidation)

   Cl_2(g) + 2e⁻ → 2Cl⁻_(aq) (reduction)

4. Mg_(s) → Mg²⁺_(aq) + 2e⁻ (oxidation)

   Cl_2(g) + 2e⁻ → 2Cl⁻_(aq) (reduction)

5. Zn_(s) → Zn²⁺_(aq) + 2e⁻ (oxidation)

   2H⁺_(aq) + 2e⁻ → H_2(g) (reduction)