Redox reactions in a basic solution? 1/2 reactions

What would be the 1/2 reactions (oxidation and reduction) of this redox problem? And if possible, what is the final answer?

NH3(g) + O2(g) > NO(g) + H2O(g) in a basic solution

Please help, thank you. Any ideas would help. Will award best answer if you answer ASAP

When answering a redox reaction, the half equations refer to the "valence" or charge of the atoms involved in the reaction- only those atoms that change charge need to be recorded, those that don't are "spectator ions" and aren't needed- so your half equations could look something like this :)
Also, I have balanced the equation; like normal reactions, the exchange of electrons has to be balanced- you can't magically create electrons >.<

4NH3(g)+ 5O2(g) => 4NO(g) + 6H20(g)
3-...............................>2+ N is oxidised by 5e-(It has lost 5 electrons)
0...............>2- 0 is reduced by 2e- (It has gained 2 electrons)
Hydrogen's charge doesn't change- it is a spectator ion :)

And to make sure the electrons are balanced:
Electrons oxidised= the number of N atoms x the number of electrons oxidised per atom
4x5= 20 e-
Electrons Reduced= the number of O atoms x the number of electrons reduced per atom
(5x2) x 2 =20 e-
Marvelous :D The electrons are balanced, as is the equation, and the redox reaction has been recorded :D Anything else you wanted bud?