Question

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

N2 (g) + 3H2 (g) = 2NH3 (g)

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

(i i) Will any of the two reactants remain unreacted?

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

Answer 1

N2(g) + 3H2(g)--->2NH3(g)
1 mol 3 mol 2 mol
=28.0g = 6.0g = 34.0g
(i) 28.0 g of N2 require 6.0 g of H2 to produce = 34.0 g of NH3
2.00 x 10³g of N2 will produce = (34/28) ×2.00 × 10³g of NH3.
= 2.43×10³g NH3 = 2430 g NH3.
(ii) Yes, dihydrogen will remain unreacted to some extent.
iii) Amount of hydrogen that remains unreacted

28.0 g of N2 require 6.0 g of H2.
2.00 x 10³ g of N2 will require (6/28) × 2.00 × 10³of H2 = 428.5 g of H2
Amount of hydrogen that remains unreacted = [(1.00 × 10³)- 428.5] g = 571.5 g