What is the overall reaction when potassium manganate(VII) is used to oxidize hydrogen peroxide?

The overall reaction when potassium manganate(VII) (or permanganate ion, MnO4-) is used to oxidize hydrogen peroxide (H2O2) is represented accurately by the balanced reaction:

2MnO4- + 6H+ + 5H2O2 → 2Mn2+ + 8H2O + 5O2.

This reaction demonstrates that permanganate acts as a strong oxidizing agent in acidic conditions. The manganese, originally in the +7 oxidation state within the permanganate ion, is reduced to the +2 oxidation state, resulting in the formation of Mn2+ ions. Meanwhile, hydrogen peroxide is oxidized, leading to the production of oxygen gas (O2) and water (H2O).

In this balanced equation, important stoichiometric coefficients reflect the required proportions of reactants and products. For every 2 moles of permanganate ion, 5 moles of hydrogen peroxide are consumed, and these reactants yield 5 moles of oxygen gas and 8 moles of water as products.

Understanding the conditions of this reaction is crucial: it occurs in an acidic environment where protons (H+) are present, facilitating the redox process