Question

Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation:

$\underset{\mathrm{dinitrogen}}{{\mathrm{N}}_2\left(\mathrm{g}\right)}+\underset{dihydrogen}{3H_2\left(g\right)}\to \underset{ammonia}{2N{H}_3\left(g\right)}$

(i) calculate the mass of ammonia produced if 2.00 × 10³ g dinitrogen reacts with 1.00 × 10³ g of dihydrogen.

(ii) will any of the two reactants remain unreacted? if yes which one ?

(iii) what would be its mass?

Answer 1

Dinitrogen and dihydrogen react with each other to produce ammonia.

$\underset{\mathrm{dinitrogen}}{{\mathrm{N}}_2\left(\mathrm{g}\right)}+\underset{dihydrogen}{3H_2\left(g\right)}\to \underset{ammonia}{2N{H}_3\left(g\right)}$

Molar mass= 28 g 6 g 34 g

(i) Mass of ammonia produced

28g of N₂ produces 34g of NH₃

1g of N₂ will produce = 34/28 g NH₃

2000 g of N₂ will produce NH₃ =$\frac{34}{28}\times 2000$

= 2428.57 g of NH₃.

Hence. the mass of ammonia produced = 2428.57g.

(ii) Amount of H₂ reacted :

28 g of N₂ reacts with 6g of H₂.

1g of N₂ reacts with 6/28 g of H₂

2000g of N₂ will react with 2000 × 6/28

= 428.57 of H₂

but H₂ is given 1 × 10³ g is greater than 428.57 g.

Therefore, dihydrogen (H₂) will remain unreacted to some extent because H₂ is excess,

(iii) Mass of unreacted dihydrogen ;

Mass of unreacted dihydrogen = 1000g - 428.57g

= 571.43 g