Question

(b) Ammonia burns in oxygen and the combustion, in
the presence of a catalyst, may be represented by
2NH2 + 0, → 2NO+ 3H20 (H = 1, N=14, 0 =16)
What mass of steam is produced when 1.5g of nitrogen
monoxide is formed?​

Answer 1

Explanation:

'Ammonia' burns in 'oxygen' and the 'combustion', in the presence of a 'catalyst'. This can be represented by  

$2 \mathrm{NH}_{2}+\mathrm{O}_{2} \rightarrow 2 \mathrm{NO}+3 \mathrm{H}_{2} \mathrm{O}$

Mass of nitrogen monoxide = 1.5 gm

Thus, from the equation,

$2 \mathrm{NH} 2+\mathrm{O} 2 \rightarrow 2 \mathrm{NO}+3 \mathrm{H} 2 \mathrm{O}$

That is  (2x0.75) + (0.75) ⇒ (2x0.75) + (3x0.75)

Thus, mass of steam produced when '1.5g of nitrogen  monoxide is formed' = 3 x 0.75 gm

               = 2.25 gm

Hence, '2.25 gm of steam is produced'.