gen-define-balancing-redox-reactions-and-give-one-short-worked-e-e492

Define balancing redox reactions and give one short worked example.

# Balancing Redox Reactions **Definition:** Balancing redox reactions is the process of ensuring that both mass and charge are conserved in oxidation-reduction reactions by equalizing the number of electrons lost (oxidation) and gained (reduction). ## Worked Example Balance this reaction in acidic solution: **MnO₄⁻ + Fe²⁺ → Mn²⁺ + Fe³⁺** ### Step-by-step solution: **1) Split into half-reactions:** - Oxidation: Fe²⁺ → Fe³⁺ - Reduction: MnO₄⁻ → Mn²⁺ **2) Balance electrons:** - Oxidation: Fe²⁺ → Fe³⁺ + e⁻ - Reduction: MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O **3) Equalize electrons (multiply oxidation by 5):** - 5Fe²⁺ → 5Fe³⁺ + 5e⁻ - MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O **4) Add half-reactions together:** ### **MnO₄⁻ + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O** ✓ Atoms balanced: Mn(1), Fe(5), O(4), H(8) ✓ Charge balanced: Both sides = +17