Question

Consider the reaction between MnO₄⁻ and C₂O₄²⁻:

MnO₄⁻(aq) + C₂O₄²⁻(aq) → Mn²⁺(aq) + CO₂ (aq)
Balance the redox reaction. a) MnO₄⁻(aq) + 5C₂O₄²⁻(aq) → Mn²⁺(aq) + 10CO₂(aq) + 8H₂O(l)
b) 2MnO₄⁻(aq) + 5C₂O₄²⁻(aq) → 2Mn²⁺(aq) + 10CO₂(aq) + 8OH⁻(aq)
c) 2MnO₄⁻(aq) + 5C₂O₄²⁻(aq) → 2Mn²⁺(aq) + 10CO₂(aq)
d) MnO₄⁻(aq) + 2C₂O₄²⁻(aq) → Mn²⁺(aq) + 4CO₂(aq) + 2H₂O(l)

Answer 1

To balance the redox reaction between MnO₄⁻ and C₂O₄²⁻, the correct balanced equation is 2MnO₄⁻(aq) + 5C₂O₄²⁻(aq) → 2Mn²⁺(aq) + 10CO₂(aq) + 8OH⁻(aq).

Step-by-step explanation:

To balance the redox reaction between MnO₄⁻ and C₂O₄²⁻, we need to make sure that the number of each element and the total charge is balanced on both sides of the equation. By comparing the oxidation states of each element in the reactants and products, we can determine the coefficients. The correct balanced equation is option b) 2MnO₄⁻(aq) + 5C₂O₄²⁻(aq) → 2Mn²⁺(aq) + 10CO₂(aq) + 8OH⁻(aq).

The balanced redox reaction between MnO₄⁻ and C₂O₄²⁻ in an acidic medium is 2MnO₄⁻ + 5C₂O₄²⁻ + 16H⁺ → 2Mn²⁺ + 10CO₂ + 8H₂O.

To balance the redox reaction between permanganate ion (MnO₄⁻) and oxalate ion (C₂O₄²⁻), we have to separately balance the oxidation and reduction half-reactions for atoms and charge, especially in an acidic medium. The correct balanced redox equation in an acidic solution is represented as 2MnO₄⁻(aq) + 5C₂O₄²⁻(aq) + 16H⁺(aq) → 2Mn²⁺(aq) + 10CO₂(g) + 8H₂O(l). This reaction shows permanganate ion being reduced to Mn²⁺ and oxalate ion being oxidized to carbon dioxide (CO₂).