Redox Reaction With Nx Nitrogen Compound

[BayernBlues]

Homework Statement

Hydroxylammonium chloride reacts with Iron(III)chloride (FeCl3) in solution to produce Iron(II)Chloride, HCL, H2O, and a compound of nitrogen. It was found that 2.0 g of iron(III) chloride reacted in this way with 31 mL of 0.200 M hydroxylammonium chloride.

Suggest a possible formula of the nitrogen compound produced.
This should be a known nitrogen compound

Homework Equations

NH3OHCl + FeCl3 ----> FeCl2 + H2O + X

The Attempt at a Solution

mole FeCl3
2g(1mole/162.2g) = 0.012 mole
mole NH3OHCl
31.0ml(1L/1000mL)(0.2 mole/L) = 0.0062 mole
FeCL3 = 0.012/0.0062 = 1.9 = 2
NH3OHCl = 0.0062/0.0062 = 1

This is the part I'm stuck at. The mol ratio is 2:1 and the compound is supposed to be N2O but I don't know how to arrive at that conclusion.

 

[Borek]

You are OK so far. The only approach I can think off now is to use the information known at this stage (ie you know hydroxylamine is a reactant, you know how many electrons it looses) to write half reaction of hydroxylamine oxidation and then to take random stabs - trying to balance charge, hydrogen and oxygen with H₂O, H⁺ and OH^- and looking at possible products.

 

[Blueshift5]

Based on the reaction and the given information, it is likely that the nitrogen compound produced is nitrous oxide (N2O). This is because the reaction involves the reduction of iron(III) chloride to iron(II) chloride, indicating a redox reaction. Nitrous oxide is a known nitrogen compound that can be produced in this type of reaction. Additionally, the mole ratio of the reactants (FeCl3 and NH3OHCl) is 2:1, which also supports the formation of N2O as it has a 2:1 ratio of nitrogen to oxygen atoms.