Concept explainers
All of the substances listed here are fertilizers that contribute nitrogen to the soil. Which of these is the richest source of nitrogen on a mass percentage basis?
- (a) Urea, (NH2)2CO
- (b) Ammonium nitrate, NH4NO3
- (c) Guanidine, HNC(NH2)2
- (d) Ammonia, NH3
(a)
Interpretation: Based on mass percentage the richest source of nitrogen has to be identified from the given fertilizers.
Concept introduction: The mass percentage of each elements present in a compound is known as the percent composition by mass of the compound.
To determine: The percentage mass of nitrogen in urea.
Answer to Problem 3.40QP
The richest source of nitrogen by mass is ammonia
Explanation of Solution
Molecular mass of urea is calculated as follows:
The percentage mass of nitrogen in ammonia is calculated as follows:
The percentage mass of an element in its compound is calculated by using the atomic mass of that element and molecular mass of the compound.
(b)
Interpretation: Based on mass percentage the richest source of nitrogen has to be identified from the given fertilizers.
Concept introduction: The mass percentage of each elements present in a compound is known as the percent composition by mass of the compound.
To determine: The percentage mass of nitrogen in ammonium nitrate.
Explanation of Solution
The molecular mass of ammonium nitrate is calculated as follows:
The molecular mass of ammonium nitrate was calculated by the sum of atomic masses of nitrogen, hydrogen and oxygen atoms.
The percentage mass of nitrogen in ammonium nitrate is calculated as follows:
The percentage mass of an element in its compound is calculated by using the atomic mass of that element and molecular mass of the compound.
(c)
Interpretation: Based on mass percentage the richest source of nitrogen has to be identified from the given fertilizers.
Concept introduction: The mass percentage of each elements present in a compound is known as the percent composition by mass of the compound.
To determine: The percentage mass of nitrogen in urea.
Explanation of Solution
Molecular mass of guanidine is calculated as follows:
The percentage mass of nitrogen in guanidine is calculated as follows:
The percentage mass of an element in its compound is calculated by using the atomic mass of that element and molecular mass of the compound.
(d)
Interpretation: Based on mass percentage the richest source of nitrogen has to be identified from the given fertilizers.
Concept introduction: The mass percentage of each elements present in a compound is known as the percent composition by mass of the compound.
To determine: The percentage mass of nitrogen in ammonium nitrate.
Explanation of Solution
The molecular mass of ammonia e is calculated as follows:
The molecular mass of ammonia was calculated by the sum atomic masses nitrogen, hydrogen atoms.
The percentage mass of nitrogen in ammonia is calculated as follows:
The percentage mass of an element in its compound is calculated by using the atomic mass of that element and molecular mass of the compound.
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Chapter 3 Solutions
Chemistry
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