Here's the breakdown of the complete redox reaction between permanganate ion (MnO4-) and hydrogen peroxide (H2O2) under acidic conditions:

1. Identifying Half-Reactions:

* Oxidation Half-Reaction: H2O2 → O2 + 2H+ + 2e-

* Hydrogen peroxide (H2O2) is oxidized to oxygen gas (O2).

* Reduction Half-Reaction: MnO4- + 8H+ + 5e- → Mn2+ + 4H2O

* Permanganate ion (MnO4-) is reduced to manganese(II) ion (Mn2+).

2. Balancing the Number of Electrons:

* Multiply the oxidation half-reaction by 5 and the reduction half-reaction by 2 to equalize the number of electrons transferred:

* 5H2O2 → 5O2 + 10H+ + 10e-

* 2MnO4- + 16H+ + 10e- → 2Mn2+ + 8H2O

3. Combining the Half-Reactions:

* Add the two balanced half-reactions together. Note that the electrons cancel out:

* 5H2O2 + 2MnO4- + 16H+ + 10e- → 5O2 + 10H+ + 10e- + 2Mn2+ + 8H2O

4. Simplifying the Equation:

* Cancel out the common terms on both sides:

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

Complete Redox Reaction:

The complete balanced redox reaction for the reaction of permanganate ion (MnO4-) and hydrogen peroxide (H2O2) in acidic solution is:

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