Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation: N2(g)+3H2(g)→ 2NH3(g) Dinitrogen + Dihydrogen → Ammonia

By BYJU'S Exam Prep

Updated on: September 25th, 2023

(i) calculate the mass of ammonia produced if 2.00 × 103 g of 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?

Solution:

(i) The mass of ammonia produced if 2.00 × 103 g of dinitrogen reacts with 1.00 × 103 g of dihydrogen is 2428.57g.

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

(iii) The mass of unreacted dihydrogen is 571.43 g.

Table of content

Ammonia is created when dinitrogen and dihydrogen react with one another.

N2(g)+3H2(g)→ 2NH3(g)

Dinitrogen + Dihydrogen → Ammonia

Molar mass= 28 g 6 g 34 g

(i) Now we have to calculate the mass of ammonia produced

We know that 28g of N2 produces 34g of NH3

1g of N2 will produce = 34/28 g NH3

2000 g of N2 will produce NH3 = 34/28 x 2000

= 2428.57 g of NH3.

Hence. the mass of ammonia produced = 2428.57g.

(ii) Now we have to calculate the amount of H2 reacted :

We have 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.

Ammonia is created when dinitrogen and dihydrogen react with one another.

(iii) Now we have to calculate the mass of unreacted dihydrogen ;

Mass of unreacted dihydrogen = 1000g – 428.57g

= 571.43 g

Summary:

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

N2(g)+3H2(g)→ 2NH3(g)

Dinitrogen + Dihydrogen → Ammonia

(i) The mass of ammonia produced if 2.00 × 103 g of dinitrogen reacts with 1.00 × 103 g of dihydrogen is 2428.57g.

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

(iii) The mass of unreacted dihydrogen is 571.43 g