Chapter 7, Problem 74APP

(a)

Interpretation Introduction

Interpretation : The mass percent composition of ${\left({\text{NH}}_{\text{4}}\right)}_{\text{2}}{\text{SO}}_{\text{4}}$ should be calculated.

Concept Introduction : Mass percent composition of each element in the given compound can be given as:

  $\text{Mass percent of element =}\frac{\text{Mass of the element}}{\text{Molar mass of compound}}\text{ x 100}$

Here molar mass of compound is the sum of atomic masses of all constituent atoms in the given formula of molecule.

The relation between moles and grams can be written as:

  $\text{Moles =}\frac{\text{Mass (g)}}{\text{Molar mass (g/mol)}}$

(b)

Interpretation Introduction

Interpretation : The atoms of H should be calculated.

Concept Introduction : Mass percent composition of each element in the given compound can be given as:

  $\text{Mass percent of element =}\frac{\text{Mass of the element}}{\text{Molar mass of compound}}\text{ x 100}$

Here molar mass of compound is the sum of atomic masses of all constituent atoms in the given formula of molecule.

The relation between moles and grams can be written as:

  $\text{Moles =}\frac{\text{Mass (g)}}{\text{Molar mass (g/mol)}}$

(c)

Interpretation Introduction

Interpretation : The mass of oxygen in $4.50\times {10}^{23}$ formula units of compound should be calculated.

Concept Introduction : Mass percent composition of each element in the given compound can be given as:

  $\text{Mass percent of element =}\frac{\text{Mass of the element}}{\text{Molar mass of compound}}\text{ x 100}$

Here molar mass of compound is the sum of atomic masses of all constituent atoms in the given formula of molecule.

The relation between moles and grams can be written as:

  $\text{Moles =}\frac{\text{Mass (g)}}{\text{Molar mass (g/mol)}}$

(d)

Interpretation Introduction

Interpretation : The mass of compound should be calculated.

Concept Introduction : Mass percent composition of each element in the given compound can be given as:

  $\text{Mass percent of element =}\frac{\text{Mass of the element}}{\text{Molar mass of compound}}\text{ x 100}$

Here molar mass of compound is the sum of atomic masses of all constituent atoms in the given formula of molecule.

The relation between moles and grams can be written as:

  $\text{Moles =}\frac{\text{Mass (g)}}{\text{Molar mass (g/mol)}}$