What stoichiometric coefficients are used in combustion reactions? How do represent the comproportionation of ammonium nitrate to nitrous oxide?

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What stoichiometric coefficients are used in combustion reactions? How do represent the comproportionation of ammonium nitrate to nitrous oxide?

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Answer 1 · 2017-03-04T19:03:19

Usually, the desirable option is the simplest WHOLE number ratio.....

Explanation:

As for myself, often I reject this rule in favour of half-integral coefficients. For example,............the combustion of ethane,

$H_{3} C - C H_{3} (g) + \frac{7}{2} O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)$ $H_3C-CH_3(g) + 7/2O_2(g) rarr 2CO_2(g) + 3H_2O(l)$ ,

versus,

$2 H_{3} C - C H_{3} (g) + 7 O_{2} (g) \to 4 C O_{2} (g) + 6 H_{2} O (l)$ $2H_3C-CH_3(g) + 7O_2(g) rarr 4CO_2(g) + 6H_2O(l)$ ,

both are balanced; I would prefer the former because it is easier to address the stoichiometry, even tho I know that you cannot have a half an oxygen molecule. You can have, however, $half a mole$ $"half a mole"$ of dioxygen molecules.

For your reaction,

$N H_{4} N O_{3} \to N_{2} O + 2 H_{2} O$ $NH_4NO_3 rarrN_2O + 2H_2O$

which is in fact a $comproportionation reaction$ $"comproportionation reaction"$ , would be the preferred option.

$3 N H_{4} N O_{3} \to 3 N_{2} O + 6 H_{2} O$ $3NH_4NO_3 rarr3N_2O + 6H_2O$ is not the simplest whole number ratio. If I have missed your point I apologize............

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What stoichiometric coefficients are used in combustion reactions? How do represent the comproportionation of ammonium nitrate to nitrous oxide?

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