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

1 Answer
anor277
Jan 21, 2017

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?

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