Need help writing the net ionic equation for NH3 + O2 -- NO + H2O

Question

Need help writing the net ionic equation for NH3 + O2 --> NO + H2O

unklerhaukus · Answer

$$NH_3+O_2\rightarrow NO+H_2O$$first Balance the equation

unklerhaukus · Answer

$$4NH_3+5O_2\rightarrow 4NO+6H_2O$$

anonymous · Answer

ima guess that nitric oxide is what your looking to focus on...

anonymous · Answer

$$4NH _{3} + 5O _{2} \rightarrow 4NO + 3H _{2}O$$
correct?

anonymous · Answer

oh.. you already did it. haha

anonymous · Answer

you got too many reactant hydrogen

unklerhaukus · Answer

wrong number of water molecules

unklerhaukus · Answer

next step is to find the ions

anonymous · Answer

$$N ^{+3} + H _{3}^{-3} \rightarrow 4NO ^{-1} + 6H _{2}O$$
I don't think this is correct but I gave it my best shot.

anonymous · Answer

thats a rather advanced way to write ions... :O

anonymous · Answer

The steps my teacher gave us says we're supposed to delete ions that don't change. Is there anything I'm supposed to delete here? I don't see any that stayed the same from the reactant side to the product side.

anonymous · Answer

4NH3+5O2-> 4NO+6H2O
here how id do it:
4NH3+5O2-> 4NO+6H2O
break ions:
4N- + 4H3+ + 5O2 -> 4NO +6H2+ + 6O-
keep the 4NO because its your wanted product
so cancel all the other crap and theres no charge on the O because its a diatomic
4N- + 2O2 -> 4NO

btaylor · Answer

The net ionic equation is the balanced chemical equation. 
4NH3+5O2→4NO+6H2O
This is because NH3, NO, and O2 are gases, not aqueous solutions. and H2O only slightly ionizes into H+ and OH-. The general rule for net ionics is to only include extensive ionization (past 0.1 M), which doesn't apply to any compounds in this equation.

anonymous · Answer

I knew that........ :D

anonymous · Answer

My brain. It feels betrayed. Haha thanks everyone.