General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 3, Problem 3.42QP

(a)

Interpretation Introduction

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.

Percentbymassofanelement=n×atomicmassofelementmolecularorformulamassofcompound×100%n-Thenumberofelements presentinamoleculeorformulaunitofthecompound

To determine: The percentage mass of nitrogen in urea.

(a)

Expert Solution
Check Mark

Answer to Problem 3.42QP

The richest source of nitrogen by mass is ammonia (NH3)

percentagemassofNinammonia=82.2447%

Explanation of Solution

Molecular mass of urea is calculated as follows:

Molecularformulaofureais(NH2)2CO

Molecular mass of urea=((2×massofN)+(4×massofH)+massofC+massofO)amu=((2×14.0067)+(4×1.00794)+12.0107+15.9994)amu=(28.0134+4.03176+12.0107+15.9994)amu=60.05526amu The molecular mass of urea was calculated by the sum atomic masses nitrogen, hydrogen, carbon and oxygen atoms.

The percentage mass of nitrogen in ammonia is calculated as follows:

PercentbymassofNinUrea=2×atomicmassofNinamumolecularmassofUreainamu×100%=2×14.0067amu60.05526amu×100%=28.0134amu60.05526amu×100%=46.6460%

percentagemassofNinUrea=46.646%

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 Introduction

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.

Percentbymassofanelement=n×atomicmassofelementmolecularorformulamassofcompound×100%n-Thenumberofelements presentinamoleculeorformulaunitofthecompound

To determine: The percentage mass of nitrogen in ammonium nitrate.

(b)

Expert Solution
Check Mark

Explanation of Solution

The molecular mass of ammonium nitrate is calculated as follows:

molecular formula of ammonium nitrate is(NH4NO3)

Molecular mass of Ammonium nitrate=((2×massofN)+(4×massofH)+(3×massofO))amu=((2×14.0067)+(4×1.00794)+(15.9994))amu=(28.0134+4.03176+47.9982)amu=80.0434amu

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:

PercentbymassofNinAmmonium nitrate=2×atomicmassofNinamumolecularmassofAmmonium nitrateinamu×100%=2×14.0067amu80.4336amu×100%=28.0134amu80.4336amu×100%=34.8280%

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 Introduction

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.

Percentbymassofanelement=n×atomicmassofelementmolecularorformulamassofcompound×100%n-Thenumberofelements presentinamoleculeorformulaunitofthecompound

To determine: The percentage mass of nitrogen in urea.

(c)

Expert Solution
Check Mark

Explanation of Solution

Molecular mass of guanidine is calculated as follows:

Molecularformulaofureais (HNC(NH2)2)

Molecular mass of Guanidine=((3×massofN)+(5×massofH)+(1×massofC))amu=((3×14.0067)+(5×1.00794)+12.0107)amu=(42.0201+5.0397+12.0107)amu=59.0705amu

The molecular mass of guanidine was calculated by the sum atomic masses nitrogen, hydrogen, and carbon atoms.

The percentage mass of nitrogen in guanidine is calculated as follows:

PercentbymassofNinGuanidine=3×atomicmassofNinamumolecularmassofGuanidineinamu×100%=3×14.0067amu59.0705amu×100%=42.0201amu59.0705amu×100%=71.1355%

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 Introduction

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.

Percentbymassofanelement=n×atomicmassofelementmolecularorformulamassofcompound×100%n-Thenumberofelements presentinamoleculeorformulaunitofthecompound

To determine: The percentage mass of nitrogen in ammonium nitrate.

(d)

Expert Solution
Check Mark

Explanation of Solution

The molecular mass of ammonia e is calculated as follows:

molecular formula of ammonia is(NH3)

Molecular mass of Ammonia=((1×massofN)+(3×massofH))amu=(14.0067+(3×1.00794))amu=(14.0067+3.02382)amu=17.03052amu

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:

PercentbymassofNinAmmonia=1×atomicmassofNinamumolecularmassofAmmoniainamu×100%=14.0067amu17.03052amu×100%=82.2447%

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

General Chemistry

Ch. 3.4 - Review of Concepts Explain how the mass...Ch. 3.5 - Practice Exercise Calculate the percent...Ch. 3.5 - Prob. 2PECh. 3.5 - Practice Exercise Calculate the number of grams of...Ch. 3.5 - Prob. 1RCCh. 3.6 - Practice Exercise A sample of a compound...Ch. 3.6 - Prob. 1RCCh. 3.7 - Prob. 1PECh. 3.7 - Prob. 1RCCh. 3.8 - Prob. 1PECh. 3.8 - Prob. 2PECh. 3.8 - Prob. 1RCCh. 3.9 - Prob. 1PECh. 3.9 - Consider the following reaction: Starting with...Ch. 3.10 - Prob. 1PECh. 3.10 - Can the percent yield ever exceed the theoretical...Ch. 3 - Prob. 3.1QPCh. 3 - Prob. 3.2QPCh. 3 - Prob. 3.3QPCh. 3 - Prob. 3.4QPCh. 3 - Prob. 3.5QPCh. 3 - 3.6 The atomic masses of and are 6.0151 amu and...Ch. 3 - Prob. 3.7QPCh. 3 - Prob. 3.8QPCh. 3 - Prob. 3.9QPCh. 3 - 3.10 What is the molar mass of an atom? What are...Ch. 3 - Prob. 3.11QPCh. 3 - Prob. 3.12QPCh. 3 - Prob. 3.13QPCh. 3 - Prob. 3.14QPCh. 3 - Prob. 3.15QPCh. 3 - Prob. 3.16QPCh. 3 - 3.17 What is the mass in grams of a single atom of...Ch. 3 - Prob. 3.18QPCh. 3 - Prob. 3.19QPCh. 3 - Prob. 3.20QPCh. 3 - Prob. 3.21QPCh. 3 - Prob. 3.22QPCh. 3 - Prob. 3.23QPCh. 3 - Prob. 3.24QPCh. 3 - Prob. 3.25QPCh. 3 - Prob. 3.26QPCh. 3 - Prob. 3.27QPCh. 3 - Prob. 3.28QPCh. 3 - Prob. 3.29QPCh. 3 - Prob. 3.30QPCh. 3 - Prob. 3.31QPCh. 3 - Prob. 3.32QPCh. 3 - Prob. 3.33QPCh. 3 - Prob. 3.34QPCh. 3 - Prob. 3.35QPCh. 3 - Prob. 3.36QPCh. 3 - Prob. 3.37QPCh. 3 - Prob. 3.38QPCh. 3 - Prob. 3.39QPCh. 3 - Prob. 3.40QPCh. 3 - Prob. 3.41QPCh. 3 - Prob. 3.42QPCh. 3 - Prob. 3.43QPCh. 3 - 3.44 Peroxyacylnitrate (PAN) is one of the...Ch. 3 - Prob. 3.45QPCh. 3 - Prob. 3.46QPCh. 3 - Prob. 3.47QPCh. 3 - Prob. 3.48QPCh. 3 - Prob. 3.49QPCh. 3 - Prob. 3.50QPCh. 3 - Prob. 3.51QPCh. 3 - 3.52 The empirical formula of a compound is CH. If...Ch. 3 - Prob. 3.53QPCh. 3 - Prob. 3.54QPCh. 3 - Prob. 3.55QPCh. 3 - Prob. 3.56QPCh. 3 - Prob. 3.57QPCh. 3 - Prob. 3.58QPCh. 3 - Prob. 3.59QPCh. 3 - Prob. 3.60QPCh. 3 - Prob. 3.61QPCh. 3 - Prob. 3.62QPCh. 3 - Prob. 3.63QPCh. 3 - 3.64 Which of the following equations best...Ch. 3 - Prob. 3.65QPCh. 3 - Prob. 3.66QPCh. 3 - Prob. 3.67QPCh. 3 - Prob. 3.68QPCh. 3 - Prob. 3.69QPCh. 3 - Prob. 3.70QPCh. 3 - Prob. 3.71QPCh. 3 - Prob. 3.72QPCh. 3 - Prob. 3.73QPCh. 3 - Prob. 3.74QPCh. 3 - 3.75 Limestone (CaCO3) is decomposed by heating to...Ch. 3 - Prob. 3.76QPCh. 3 - Prob. 3.77QPCh. 3 - Prob. 3.78QPCh. 3 - 3.79 Define limiting reagent and excess reagent....Ch. 3 - Prob. 3.80QPCh. 3 - Prob. 3.81QPCh. 3 - Prob. 3.82QPCh. 3 - Prob. 3.83QPCh. 3 - Prob. 3.84QPCh. 3 - Prob. 3.85QPCh. 3 - Prob. 3.86QPCh. 3 - Prob. 3.87QPCh. 3 - Prob. 3.88QPCh. 3 - Prob. 3.89QPCh. 3 - Prob. 3.90QPCh. 3 - Prob. 3.91QPCh. 3 - Prob. 3.92QPCh. 3 - Prob. 3.93QPCh. 3 - Prob. 3.94QPCh. 3 - Prob. 3.95QPCh. 3 - Prob. 3.96QPCh. 3 - Prob. 3.97QPCh. 3 - Prob. 3.98QPCh. 3 - Prob. 3.99QPCh. 3 - Prob. 3.100QPCh. 3 - Prob. 3.101QPCh. 3 - Prob. 3.102QPCh. 3 - Prob. 3.103QPCh. 3 - Prob. 3.104QPCh. 3 - Prob. 3.105QPCh. 3 - Prob. 3.106QPCh. 3 - Prob. 3.107QPCh. 3 - Prob. 3.108QPCh. 3 - Prob. 3.110QPCh. 3 - Prob. 3.111QPCh. 3 - Prob. 3.112QPCh. 3 - Prob. 3.113QPCh. 3 - 3.114 In the total synthesis of a natural product,...Ch. 3 - Prob. 3.115QPCh. 3 - Prob. 3.116SPCh. 3 - Prob. 3.117SPCh. 3 - 3.118 A certain metal M forms a bromide containing...Ch. 3 - Prob. 3.119SPCh. 3 - Prob. 3.120SP
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