Question

In the reaction, $4N{H}_3+5O_2\to 4NO+6H_{2}O$, when one mole of ammonia and one mole of oxygen are allowed to react till completion, which of the following statements is true?

• A. 1.0 mole of $H_{2}O$ is produced
• B. All the oxygen is consumed
• C. 1.5 mole of $NO$ is formed
• D. All the ammonia is consumed

Answer 1

The correct option is B All the oxygen is consumed

Calculation of limiting reactant
$\text{For Ammonia}=\frac{\text{given moles}}{\text{stoichiometric coefficient}}=\frac{1}{4}=0.25\text{mol}$
$\text{For Oxygen}=\frac{\text{given moles}}{\text{stoichiometric coefficient}}=\frac{1}{5}=0.20\text{mol}$
So, Oxygen is the limiting reagent. Hence, it will be totally consumed
As per stoichiometry,
5 mol of oxygen forms 4 mol of $NO$
1 mol will form = $\frac{4}{5}$ = 0.8 mol of $NO$
Similarly,
5 mol of oxygen forms 6 mol of $H_{2}O$
1 mol will form $\frac{6}{5}\times 1=1.2$ mol of $H_{2}O$