Question

Hydrogen peroxide will be used to oxidize the iron(II) in the complex ion to iron(III). Several things happen in this reaction: Iron(II) is oxidized to iron(III) The oxalate ions that were attached to the iron(II) in the complex ion return to the solution (as oxalate ions) Each hydrogen peroxide molecule is reduced to form two hydroxide ions Part A - Oxidation of iron(II) to iron(III). Write a balanced net ionic equation for the oxidation of the iron(II) complex ion with hydrogen peroxide. Make certain that your equation depicts all three things described in the introduction and that is it blanced for nujmber of electrons transferred (charge) as well as for atoms. Write a balanced net ionic equation for this redox reaction. Include the phases.

Answer 1

oxidation of the iron(II) complex ion with hydrogen peroxide

(i) oxidation half reaction will be

oxidation: Fe²⁺ (aq) → Fe³⁺(aq)

Reduction half reaction will be

reduction: H₂O₂ (aq) + 2e → 2OH-(aq)

The two half equaitons will be

Fe²⁺ → Fe³⁺ + e⁻

H₂O₂ + 2e⁻ → 2OH^-

Balancing two half reactions for electrons ,

2Fe²⁺ → 2Fe³⁺ + 2e⁻

Overall equation will be

2Fe²⁺ (aq)+ H₂O₂(aq) → 2Fe³⁺(aq) + 2HO-(aq)

Or

[Fe(C2O4)] (s) + H2O2(aq) ---> [Fe(C2O4)]+(aq) + 2HO-(aq)