Concept explainers
(a)
Interpretation :
Mass of hydrogen gas required to react completely with 10 g of nitrogen must be calculated.
Concept Introduction :
1 mol nitrogen gas (28 g) needs 3 moles of hydrogen gas (6 g) to produce 2 moles of ammonia gas (34 g).
(a)
Answer to Problem 4RQ
Mass of hydrogen gas is 2.14 g which is required to react completely with 10 g of nitrogen gas.
Explanation of Solution
The
As per the balanced chemical equation,
1 mol of nitrogen gas reacts with 3 mol of hydrogen gas. Molar mass of nitrogen is 28 g/mol and that of hydrogen gas is 2 g/mol thus, it can be said that:
28 g nitrogen needs 6 g hydrogen.
Or,
1 g nitrogen needs
Thus 10 g nitrogen needs
b)
Interpretation :
Mass of ammonia gas which will be produced from 10 g nitrogen gas and sufficient hydrogen gas must be calculated.
Concept Introduction :
Nitrogen gas is limiting reagent as hydrogen gas is added in sufficient amount.
1 mol nitrogen gas (28 g) produces 2 moles of ammonia gas (34 g).
b)
Answer to Problem 4RQ
12.14 g ammonia gas is produced from 10 g nitrogen gas and sufficient hydrogen gas.
Explanation of Solution
The chemical reaction between nitrogen and hydrogen gas to form ammonia gas is as follows:
The molar mass of ammonia is 17 g/mol.
As per balanced equation 28 g nitrogen gas produces 34 g ammonia gas.
1 g nitrogen gas produces
Thus 10 g nitrogen gas produces
Chapter 9 Solutions
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