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? Answer 1.24:
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Answer:
Na(g)
+
=6.0 g
3 mol
3H
2(g)
→
=34.0 g
2 mol
2NH
3(g)
(i) 28.0 g of N
2
require 6.0 g of H
2
to produce
=34.0 g of NH
3
2.00×10
3
g of N
2
will produce
=
28
34
×2.00×10
3
g of NH
3
=2.43×10
3
g of NH
3
=2430 g NH
3
(ii) Yes, dihydrogen will remain unreacted to some extent
(iii) Amount of hydrogen that remains unreacted.
28.0 g of N
2
require 6.0 g of H
2
2.00 g×10
3
g of N
2
will require
=
28.0
6.0
×2.00×10
3
of H
2
=428.5 g of H
2
∴ Amount of hydrogen that remains unreacted
=[1.00×10
3
−428.5]
g
=571.5 g.
Explanation:
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