   Chapter 3, Problem 62E

Chapter
Section
Textbook Problem

What number of molecules (or formula units) are present in 1.00 g of each of the compounds in Exercise 52?

(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 52 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 P4O6 .

Explanation

Given

The mass of P4O6 is 1.00g .

The molar mass of P4O6 is,

(4×30.973+6×15.999)g/mol=219.886g/mol

Formula

The number of moles in P4O6 is calculated as,

MolesofP4O6=MassofP4O6MolarmassofP4O6

Substitute the values of mass and molar mass of P4O6 in above equation.

MolesofP4O6=MassofP4O6MolarmassofP4O6=1.00g219.886g/mol=0.0045mol

The number of molecules in 1

(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 52 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 Ca3(PO4)2 .

(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 52 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 Na2HPO4 .

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