Ammonia NH3 (gas) combines with oxygen gas over Pt catalyst to produce Nitric oxide (NO) and water. If 27.2 g of NH3 gas is taken initially then :

Question

Ammonia $\left( NH _{3}\right)$ gas combines with oxygen gas over $Pt$ catalyst to produce Nitric oxide (NO) and water. If $27.2 g$ of $NH _{3}$ gas is taken initially then :

$4 NH _{3}+5 O _{2} \longrightarrow 4 NO +6 H _{2} O$

(A) Volume of oxygen gas required at NTP is $22.4$ litre

(B) Volume of $H _{2} O (\ell)$ produced at $4^{\circ} C$ (assuming density of water as $1000 Kg / m ^{3}$) is $21.6 ml$

(C) Total mass of products obtained is $45.6 g$

(D) Number of moles of NO produced is $1.6$

Answer 1

The correct option of this question will be (D) Number of moles of NO produced is $1.6$