Chemistry
Chemistry
9th Edition
ISBN: 9781133611097
Author: Steven S. Zumdahl
Publisher: Cengage Learning
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Chapter 3, Problem 61E

What number of atoms of nitrogen are present in 1.00 g of each of the compounds in Exercise 51?

(a)

Expert Solution
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Interpretation Introduction

Interpretation: The mass of compound is given. By using the mass, the number of nitrogen atoms present in each of the compound given in exercise 51 is to be determined.

Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.

Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.

The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.

The amount of substance containing 12g of pure carbon is called a mole. One mole of atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

To determine: The number of nitrogen (N) atoms in 1.00g of NH3 .

Explanation of Solution

Given

The mass of NH3 is 1.00g .

The molar mass of NH3 is 17.034g/mol .

Formula

The number of moles of NH3 is calculated as,

MolesofNH3=MassofNH3MolarmassofNH3

Substitute the values of mass and molar mass of NH3 in above equation.

MolesofNH3=MassofNH3MolarmassofNH3=1.00g17.034g/mol=0.0587mol

Since, one mole of NH3 is equal to one mole of nitrogen, Therefore, 0.0587mol of NH3 is equal to 0.0587mol of nitrogen (N) .

The number of nitrogen atoms in NH3 is calculated using the formula,

NumberofNatoms=MolesofNH3×6.022×1023

Substitute the value of number of moles of NH3 in above equation.

NumberofNatoms=MolesofNH3×6.022×1023=0.0587×6.022×1023=3.535×1022atoms_

Conclusion

The number of atoms is calculated by multiplying the number of moles with Avogadro’s number.

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The mass of compound is given. By using the mass, the number of nitrogen atoms present in each of the compound given in exercise 51 is to be determined.

Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.

Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.

The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.

The amount of substance containing 12g of pure carbon is called a mole. One mole of atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

To determine: The number of nitrogen (N) atoms in 1.00g of N2H4 .

Explanation of Solution

Given

The mass of N2H4 is 1.00g .

The molar mass of N2H4 is 32.052g/mol .

Formula

The number of moles of N2H4 is calculated as,

MolesofN2H4=MassofN2H4MolarmassofN2H4

Substitute the values of mass and molar mass of N2H4 in above equation.

MolesofN2H4=MassofN2H4MolarmassofN2H4=1.00g32.052g/mol=0.0312mol

Since, one mole of N2H4 is equal to two moles of nitrogen, Therefore, 0.0311mol of N2H4 is equal to,

2×0.0311mol=0.0623mol of nitrogen (N)

The number of nitrogen atoms in N2H4 is calculated using the formula,

NumberofNatoms=MolesofN2H4×6.022×1023

Substitute the value of number of moles of N2H4 in above equation.

NumberofNatoms=MolesofN2H4×6.022×1023=0.0623mol×6.022×1023=3.758×1022atoms_

Conclusion

The number of atoms is calculated by multiplying the number of moles with Avogadro’s number.

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The mass of compound is given. By using the mass, the number of nitrogen atoms present in each of the compound given in exercise 51 is to be determined.

Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.

Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.

The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.

The amount of substance containing 12g of pure carbon is called a mole. One mole of atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

To determine: The number of nitrogen (N) atoms in 1.00g of (NH4)2Cr2O7 .

Explanation of Solution

Given

The mass of (NH4)2Cr2O7 is 1.00g .

The molar mass of (NH4)2Cr2O7 is 250.28g/mol .

Formula

The number of moles in (NH4)2Cr2O7 is calculated as,

Molesof(NH4)2Cr2O7=Massof(NH4)2Cr2O7Molarmassof(NH4)2Cr2O7

Substitute the values of mass and molar mass of (NH4)2Cr2O7 N2H4 in above equation.

Molesof(NH4)2Cr2O7=Massof(NH4)2Cr2O7Molarmassof(NH4)2Cr2O7=1.00g250.28g/mol=3.99×103mol

Since, one mole of (NH4)2Cr2O7 is equal to two moles of nitrogen, Therefore, 3.99×103mol of (NH4)2Cr2O7 is equal to,

2×3.99×103mol=7.98×103mol of nitrogen (N)

The number of nitrogen atoms in (NH4)2Cr2O7 is calculated using the formula,

NumberofNatoms=Molesof(NH4)2Cr2O7×6.022×1023

Substitute the value of number of moles of (NH4)2Cr2O7 in above equation.

NumberofNatoms=Molesof(NH4)2Cr2O7×6.022×1023=7.98×103mol×6.022×1023=4.81×1021atoms_

Conclusion

The number of atoms is calculated by multiplying the number of moles with Avogadro’s number.

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Chapter 3 Solutions

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