Ask Question
8 April, 17:43

Balance the oxidation-reduction half reactions for hydrogen peroxide and permanganate ion, respectively. Write the net ionic equation for the reaction between MnO4 - ions and H2O2 in acidic solution.

+3
Answers (1)
  1. 8 April, 18:11
    0
    5 H₂O₂ + 6 H⁺ + 2 MnO₄⁻ → 5 O₂ + 2 Mn²⁺ + 8 H₂O

    Explanation:

    In order to balance a redox reaction, we will use the ion-electron method.

    Step 1: Identify both half-reactions

    Oxidation: H₂O₂ → O₂

    Reduction: MnO₄⁻ → Mn²⁺

    Step 2: Perform the mass balance, adding H⁺ and H₂O where necessary.

    H₂O₂ → O₂ + 2 H⁺

    8 H⁺ + MnO₄⁻ → Mn²⁺ + 4 H₂O

    Step 3: Perform the electrical balance, adding electrons where necessary.

    H₂O₂ → O₂ + 2 H⁺ + 2 e⁻

    8 H⁺ + MnO₄⁻ + 5 e⁻ → Mn²⁺ + 4 H₂O

    Step 4: Multiply both half-reactions by numbers that secure that the number of electrons gained and lost are equal.

    5 * (H₂O₂ → O₂ + 2 H⁺ + 2 e⁻)

    2 * (8 H⁺ + MnO₄⁻ + 5 e⁻ → Mn²⁺ + 4 H₂O)

    Step 5: Add both half-reactions and cancel what is repeated in both sides.

    5 H₂O₂ + 16 H⁺ + 2 MnO₄⁻ → 5 O₂ + 10 H⁺ + 2 Mn²⁺ + 8 H₂O

    5 H₂O₂ + 6 H⁺ + 2 MnO₄⁻ → 5 O₂ + 2 Mn²⁺ + 8 H₂O
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Balance the oxidation-reduction half reactions for hydrogen peroxide and permanganate ion, respectively. Write the net ionic equation for ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers