In Ostwald's process of manufacture Nitric acid, Ammonia obtained from Haber's process is oxidised with oxygen. If 17 gram of NH3 is oxidised with 45 gram of oxygen to produce NO and H₂O.
a. Find the limiting reagent
b. How many moles of uncreated reactant left over?
c. What volume of NO are produced at NTP?
d. Calculate the mass of water produced.
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Answer:
Explanation:
The balanced chemical equation is:
4NH
3
(g)+5O
2
(g)→4NO(g)+6H
2
O(g)
The molar masses of ammonia and oxygen are 17 g/mol and 32 g/mol respectively.
5 moles (160 g) of oxygen reacts with 4 moles (68 g) of ammonia.
20 g of oxygen will react with
160
68×20
=8.5 g of ammonia. Hence, oxygen is the limiting regent.
The molar mass of NO is 30 g/mol.
5 moles (160 g) of oxygen will produce 4 moles (120 g) of NO$.
20 g of oxygen will produce
160
120×20
=15g of NO.
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