NCERT Class XI Chemistry Some Basic Concepts of Chemistry Solutions

Question : 24

Total: 36

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?

Solution:

The balanced chemical equation is N2+3H2 → 2NH3.
Moles of N2 =

2.00×103

= 71.43, Moles of H2 =

1.00×103

= 500
1 mole of N2 required 3 moles of H2 from above equation.
∴ 71.43 mole of N2 will require 3 × 71.43 = 214.29 mole of H2
But moles of H2 actually present = 500 moles
Thus, H2 is in excess and will remain unreacted and N2 is limiting reagent.
(i) 1 mole of N2 reacts with H2 to form NH3 = 2 moles
71.43 moles of N2 react with H2 to form NH3 =

× 71.43
= 142.86 moles
Mass of NH3 produced = 142.86 × 17 = 2428.6 g
(ii) Hydrogen will remain unreacted.
(iii) Moles of H2 remaining unreacted = 500 – 214.29 = 285.71 moles
Mass of H2 left unreacted = 285.71 × 2 = 571.42 g

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