Hey guys! Stuck on some Redox Reactions. I tried my best to put as much work as I could, but I'm super stuck on these ones. Thanks for any help:
1) Balance the equation as written, what is the coefficient for O2?
NH4+ + O2-->NO2− + H2O (in basic solution)
Maybe answer:
I tried treating it as an acid so I know I have to change the H+ ions at the end but I don't remember how to do that.
2(NH4+2H20->NO2-+8H+6e-)
3(4e-+O2+4H+->2H2O)
2NH4++4H2O+3O2+12H+->6H2O+2NO2-+16H+
(What do I do from here? Sorry!)
2) Balance the equation as written, what is the coefficient for Cu2+?
Cu + HNO3-->Cu2+ + NO
Maybe work:
All I know is
Cu->Cu2++2e-
I can't figure out HNO3--> Sorry!
3)Balance the equation as written, what is the coefficient for O2?
CH3CH2OH + O2-->CH3CO2H + H2O (in acidic solution)
Maybe work:
I'm confused by this one, I know it is in acid so I can use the symbolic equation 2H++"O"->H2O somewhere, but I'm super lost! Sorry!
4) A 1.5000 g sample of impure iron (II) ammonium sulfate was found to require 27.03 ml of 0.01876 M potassium permanganate (in excess acid) to reach the end point. What is the percentage of Fe in the sample?
Maybe answer:
Fe(NH4)2(SO4)2 and KMnO4
Fe2+->Fe3++e-
MnO4-+8H++5e- -->Mn2+4H2O
Balanced equation for this reaction:
5Fe2++MnO4-+8H+->5Fe3++Mn2++4H20
Moles MnO4-=.02703l*.01876M=5.07*10^-4
Moles Fe2+=5*5.07*10^-4=.002535414 mol
Mass of Fe2+=.0025mols*55.85g/mol=.1416g
Percent of Fe=.1416/1.5g*100=9.440% (my answer)
2 answers