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Redox Reaction With Nx Nitrogen Compound

  1. Sep 25, 2008 #1
    1. The problem statement, all variables and given/known data

    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


    2. Relevant equations


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

    3. 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.
     
  2. jcsd
  3. Sep 26, 2008 #2

    Borek

    User Avatar

    Staff: Mentor

    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.
     
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