Question

How do you balance the following equation: `?NH_3 + ?O_2 -> ?NO + ?H_2O`?

Answer 1

Overall,

`4NH_3 +5O_2 rarr 4NO +6H_2O`

Explanation:

These are standard redox reactions, nitrogen is oxidized, and oxygen is reduced:

`"Oxidation:"`

`NH_3+H_2Orarr NO + 5H^+ + 5e^-` `(i)`

`"Reduction:"`

`O_2+ 4H^+ +4e^(-)rarr 2H_2O` `(ii)`

We cross multiply and take `4xx(i)+5xx(ii)`

`4NH_3 +5O_2+4H_2O rarr 4NO +10H_2O`

Nitrogens, oxygens, and hydrogens all balance. Charges balance, so this is a valid representation. Of course we can substract 4 equiv of water from EACH side of the equation.

Ammonia might be fully oxidized up to `NO_2`. If you represent this reaction for practice, would you post the balanced equation in this thread?