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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 5, Problem 59E
Textbook Problem
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What number of molecules (or formula units) are present in 1.00 g of each of the compounds in Exercise 51?

(a)

Interpretation Introduction

Interpretation: The mass of compound is given. By using the mass, the number of molecules present of 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.

Hence,

(6.022×1023 atoms)(12u1atom)=12g1u=16.022×1023 g

To determine: The number of molecules in 1.00g of NH3 .

Explanation of Solution

Given

The mass of NH3 is 1.00g .

The molar mass of NH3 is,

(14.006+3×1.0079)g/mol=17.0297g/mol

Formula

The number of moles in NH3 is calculated as,

MolesofNH3=MassofNH3MolarmassofNH3

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

MolesofNH3=MassofNH3MolarmassofNH3=1.00g17.0297g/mol=0.0587mol

The number of molecules in 1.00g of NH3 is calculated using the formula,

MoleculesofNH3=MolesofNH3(6

(b)

Interpretation Introduction

Interpretation: The mass of compound is given. By using the mass, the number of molecules present of 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.

Hence,

(6.022×1023 atoms)(12u1atom)=12g1u=16.022×1023 g

To determine: The number of molecules in 1.00g of N2H4 .

(c)

Interpretation Introduction

Interpretation: The mass of compound is given. By using the mass, the number of molecules present of 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.

Hence,

(6.022×1023 atoms)(12u1atom)=12g1u=16.022×1023 g

To determine: The number of molecules in 1.00g of (NH4)2Cr2O7 .

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Chapter 5 Solutions

Chemistry: An Atoms First Approach
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