Question

In the reaction,
$4N{H}_3(g)+5O_2(g)\to 4NO(g)+6H_{2}O(l)$
When $1$ mole of ammonia and $1$ mole of $O_2$ are made to react to completion, then

• A. 1.0 mole of $H_{2}O$ 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)

$\underset{\text{4 mol}}{4N{H}_3(g)}+\underset{\text{ 5 mol}}{5O_2(g)}⟶\underset{\text{4 mol }}{4NO(g)}+\underset{\text{6 mol}}{6H_{2}O(I)}$
According to equation,
$5$ moles of $O_2$ required $=4$ moles of $N{H}_3$
$1$ mole of $O_2$ requires $=\frac{4}{5}=0.8$ mole of $N{H}_3$
While $1$ mole of $N{H}_3$ requires $=\frac{5}{4}$
$=1.25$ moles of $O_2$
As there is $1$ mole of $N{H}_3$ and 1 mole of $O_2$, so all the oxygen will be consumed.