Home NCERT Solutions NCERT Exemplar CBSE Sample Papers NCERT Books Class 12 Class 10
Question 24

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


N2(g) + H2(g) → 2NH3(g)


(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?


(iii) If yes, which one and what would be its mass?


(i) Balancing the given chemical equation,



Total mass of Ammonia = 2((14) +3(1))= 34 g

From the chemical equation,we can write

28gm of N2 reacts with 6gm of H2 to produce ammonia= 34g

Or  1 gm of  N2 reacts with 1gm of H2 to produce ammonia= 34/28*1

Or  when 2.00x103 g of  N2 reacts with 1.00x103 gm of H2 to produce ammonia


=34/28 *2.00x103=2428.57g


hence 2.00 × 103 g of dinitrogen will react with  1.00x103 g of dihydrogen to give 2428.57 g of ammonia

Given,  Amount of dihydrogen = 1.00 × 103 g

Hence, N2 is the limiting reagent.


(ii) N2 is the limiting reagent and H2 is the excess reagent. Hence, H2 will remain unreacted.


(iii) Mass of dihydrogen left unreacted = 1.00 × 103 g – 428.6 g

= 571.4 g

Popular Questions of Class Chemistry

Recently Viewed Questions of Class Chemistry

9 Comment(s) on this Question

Write a Comment: