allo everyone,

Consider this sentence:
In the presence of hydrogen ions, the hydroxyammonium ion, NH₃OH⁺ will reduce iron(III) ion to iron(II) ion while the NH₃OH⁺ ion itself will be oxidised to dinitrogen oxide.

I wrote a formula equation regarding to the above sentence:
4 Fe³⁺ + 2 NH₃OH⁺ --> 4 Fe²⁺ + N₂O + H₂O + 6H⁺

But my chemistry teacher suggested that the hydrogen ions in my equation should be the reactants(infront of the equation) not the product. So she wrote:
Fe³⁺ + 2 NH₃OH⁺  + 2H⁺ + 5e^- --> Fe²⁺ + N₂O + H₂O + 4 H₂

But I'm totally disagreed with her because as I know(might be wrong) that redox equations should not have e^- (electron charge) present right? It should be cancle off in the redox equation.
Although I disagreed with her equation, I agree of what she said about the hydrogen ions. Yes it should be infront of the equation because it is a acid solution and according to the sentence "with the presence of hydrogen ions".

Anyone have any idea on this redox problem? Or maybe a better and correct equation for this?

BTW, the NH₃OH⁺ ion came from a solution prepared by boiling 4.0 g of hydroxyammonium sulphate, (NH₃OH)₂SO₄ per dm³  with excess iron(III) ammonium sulphate and dilute sulphuric acid.
Later this solution was titre with a solution containing 1.58 g of potassium manganate(VII) KMnO₄ per 500 cm³ to determine the ratio of the number of moles of hydroxyammonium ions to the number of moles of iron(III) ions participating in the reaction.

Hope I made myself clear.
Thx in advance!

allo everyone,

Consider this sentence:
In the presence of hydrogen ions, the hydroxyammonium ion, NH₃OH⁺ will reduce iron(III) ion to iron(II) ion while the NH₃OH⁺ ion itself will be oxidised to dinitrogen oxide.

your reaction is correct.

2 NH3OH(+) --> N2O

2 NH3OH(+) --> N2O + H2O

2 NH3OH(+) --> N2O + H2O + 6 H(+)

2 NH3OH(+) --> N2O + H2O + 6 H(+) + 4 e-

then combined with 4 Fe(3+) + 4 e- --> 4 Fe(2+) will result in your reaction equation.

Maybe the H(+) is a catalist in the reaction.

An interesting side-note:

A reaction like the one described by the teacher could possibly take place in a solution of liquid ammonia as free electrons are solvated by ammonia.  Of course, this is beyond the scope of a high school course and you would not be expected to know this.

Any acid will be said to yield H⁺ in solution

Where does the H⁺ ion came from? Is it from the dilute sulphuric acid that added previously?

Yes. Every acid solution contains them.

Needed as a catalyst?

As sdekivit suggested.

2Fe2(SO4)3 + (NH3OH)2SO4 = 4FeSO4 + N2O + H2O + 3H2SO4

what with the Fe2(SO4)3? the soulution is mixed with iron(III)ammonium sulphate, where is the ammonium?

There is no need to use H2SO4 in the first reaction

maybe as a catalyst?

Im sorry if Im asking a dumb question.
But isnt Fe(3+) + 2NH3OH(+) --> Fe(2+) + N2O + H20 + 6H have balanced the equation already? Why do we still need to add 2 infront of Fe(3+0 and Fe(2+)?

I know I must be wrong. Can someone please correct me?^_^