How do you balance the following equation: $? N H_{3} + ? O_{2} \to ? N O + ? H_{2} O$ $?NH_3 + ?O_2 -> ?NO + ?H_2O$ ?

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How do you balance the following equation: $? N H_{3} + ? O_{2} \to ? N O + ? H_{2} O$ $?NH_3 + ?O_2 -> ?NO + ?H_2O$ ?

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Answer 1 · 2017-01-21T08:26:25

Overall,

$4 N H_{3} + 5 O_{2} \to 4 N O + 6 H_{2} O$ $4NH_3 +5O_2 rarr 4NO +6H_2O$

Explanation:

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

$Oxidation:$ $"Oxidation:"$

$N H_{3} + H_{2} O \to N O + 5 H^{+} + 5 e^{-}$ $NH_3+H_2Orarr NO + 5H^+ + 5e^-$ $(i)$ $(i)$

$Reduction:$ $"Reduction:"$

$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$ $O_2+ 4H^+ +4e^(-)rarr 2H_2O$ $(i i)$ $(ii)$

We cross multiply and take $4 \times (i) + 5 \times (i i)$ $4xx(i)+5xx(ii)$

$4 N H_{3} + 5 O_{2} + 4 H_{2} O \to 4 N O + 10 H_{2} O$ $4NH_3 +5O_2+4H_2O rarr 4NO +10H_2O$

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 $N O_{2}$ $NO_2$ . If you represent this reaction for practice, would you post the balanced equation in this thread?

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How do you balance the following equation: $? N H_{3} + ? O_{2} \to ? N O + ? H_{2} O$ $?NH_3 + ?O_2 -> ?NO + ?H_2O$ ?

1 Answer

Explanation:

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How do you balance the following equation: ?NH3+?O2→?NO+?H2O?NH_3 + ?O_2 -> ?NO + ?H_2O?

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How do you balance the following equation: $? N H_{3} + ? O_{2} \to ? N O + ? H_{2} O$ $?NH_3 + ?O_2 -> ?NO + ?H_2O$ ?