If 242 gm of dye nitrogen is made from 8gm of hydrogen, then what is the amount of marginal reagent and product?
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Answer:
The balanced chemical equation is as follows:
N
2
+3H
2
→2NH
3
The molar masses of nitrogen, hydrogen and ammonia are 28 g/mol, 2 g/mol and 17 g/mol respectively.
28 g of nitrogen reacts with 6 g of hydrogen to form 34 g of ammonia.
2.00×10
3
g of nitrogen will react with
28
6
×2.00×10
3
=428.6 g hydrogen.
However, 1.00×10
3
g of dihydrogen are present.
Hence, nitrogen is the limiting reagent.
(i) Mass of ammonia produced =
28
34
×2×10
3
=2428.57 g
(ii) Hydrogen is the excess reagent. Hence, it will remain unreacted.
(iii) Mass of dihydrogen left unreacted =1.00×10
3
−428.6=571.4 g
Explanation:
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