Question 1: Hydrogen peroxide will be used to oxidize the iron(II) in the comple

Question

Question 1: 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.

Question 2:Part A - The dissolution of iron(II) ammonium sulfate

In the first step of experiment #9, iron(II) ammonium sulafte is desolved in water. Write the equation for this process.

Write the equation for the dissolution of Fe(NH4)2(SO4)2. Include the phases in your equation

Explanation / Answer

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

The halfreactions are:

oxidation: Fe2+ Fe3+

reduction: H2O2 H2O

Balancing the second equation for O and H gives:

2H+ + H2O2 2H2O

Balance both equations for charge with electrons:

Fe2+ Fe3+ + e

2H+ + H2O2 + 2e 2H2O

Now, multiply the first halfreaction by 2 to equalize charge

2Fe2+ 2Fe3+ + 2e

add, and cancel electrons

2Fe2+ + 2H+ + H2O2 2Fe3+ + 2H2O

2. Dissociation of ferrous ammonium sulfate:

(NH4)2Fe(SO4)2 (s) --> 2 NH4+(aq) + Fe+2(aq) + 2 (SO4)-2(aq)

Related Questions

Navigate

• Browse (All)
• Browse Q
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.