Question

In the reaction,
$4 NH _{3}(g)+5 O _{2}(g) \rightarrow 4 NO (g)+6 H _{2} O (l)$
When $1 $ mole of ammonia and $1$ mole of $O _{2}$ are made to react to completion, then

• A. 1.0 mole of $H_2O$ is produced
• B. 1.0 mole of NO will be produced
• C. all the oxygen will be consumed
• D. all the ammonia will be consumed

Answer 1

Answer: (C)

$\underset{\text{4 mol}}{4 NH _{3}(g)}+\underset{\text{ 5 mol}}{5 O _{2}(g)} \longrightarrow \underset{\text{4 mol }}{4 NO (g)}+\underset{\text{6 mol}}{6 H _{2} O (I)}$
According to equation,
$5$ moles of $O _{2}$ required $=4$ moles of $NH _{3}$
$1 $ mole of $O _{2}$ requires $=\frac{4}{5}=0.8$ mole of $NH _{3}$
While $1$ mole of $NH _{3}$ requires $=\frac{5}{4}$
$=1.25$ moles of $O _{2}$
As there is $1$ mole of $NH _{3}$ and 1 mole of $O _{2}$, so all the oxygen will be consumed.