Provide the coefficients needed to balance the redox reaction given. Choose... Fe(s) + Choose... Cl2(g)→ Choose... Fe3+(aq) + Choose... Cl-(aq)

3 Cl₂(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe³⁺(aq)

Explanation:

Step 1: Write the unbalanced redox reaction

Fe(s) +  Cl₂(g) → Fe³⁺(aq) + Cl⁻(aq)

Step 2: Identify both half-reactions

Reduction: Cl₂(g) → Cl⁻(aq)

Oxidation: Fe(s) → Fe³⁺(aq)

Step 3: Perform the mass balance

Cl₂(g) → 2 Cl⁻(aq)

Fe(s) → Fe³⁺(aq)

Step 4: Perform the charge balance

2 e⁻ + Cl₂(g) → 2 Cl⁻(aq)

Fe(s) → Fe³⁺(aq) + 3 e⁻

Step 5: Multiply both half-reactions by numbers that make that the number of electrons gained and lost are equal

3 × [2 e⁻ + Cl₂(g) → 2 Cl⁻(aq)]

2 × [Fe(s) → Fe³⁺(aq) + 3 e⁻]

Step 6: Add both half-reactions and cancel what is repeated in both sides

6 e⁻ + 3 Cl₂(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe³⁺(aq) + 6 e⁻

3 Cl₂(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe³⁺(aq)