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?

Related questions
See all questions in Balancing Chemical Equations
Impact of this question
1575 views around the world
You can reuse this answer
Creative Commons License