Chapter 6, Problem 23A

(a)

Interpretation Introduction

Interpretation:

The mass in grams for given sample has to be calculated.

Concept Introduction :

The formula to calculate the number of moles is given as shown below:

  $\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Answer to Problem 23A

The mass of aluminium iodide is $611.55\text{g}$ .

Explanation of Solution

The molar mass of aluminium iodide is $407.7\text{g/mol}$ . Substitute the value of given moles as $1.50$ and molar mass as $407.7\text{g/mol}$ in the above formula and value of mass of given sample is calculated as shown below:

  $\begin{array}{c}\text{1}\text{.50 mol}=\frac{\text{Given mass}}{407.7\text{g/mol}}\\ \text{Given mass}=\text{1}\text{.50 mol}\times 407.7\text{g/mol}\\ =\text{611}\text{.55}\text{g}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The mass in grams for given sample has to be calculated.

Concept Introduction :

The formula to calculate the number of moles is given as shown below:

  $\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Answer to Problem 23A

The mass of benzene is $0.149\text{g}$ .

Explanation of Solution

The molar mass of benzene is $78.11\text{g/mol}$ . Substitute the value of given moles as $1.91\times {10}^{-3}$ and molar mass as $78.11\text{g/mol}$ in the above formula and value of mass of given sample is calculated as shown below:

  $\begin{array}{c}\text{1}\text{.91}\times {\text{10}}^{-3}\text{ mol}=\frac{\text{Given mass}}{78.11\text{g/mol}}\\ \text{Given mass}=\text{1}\text{.91}\times {\text{10}}^{-3}\text{ mol}\times 78.11\text{g/mol}\\ =\text{0}\text{.149}\text{g}\end{array}$

(c)

Interpretation Introduction

Interpretation:

The mass in grams for given sample has to be calculated.

Concept Introduction :

The formula to calculate the number of moles is given as shown below:

  $\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Answer to Problem 23A

The mass of glucose is $720.624\text{g}$ .

Explanation of Solution

The molar mass of glucose is $180.156\text{g/mol}$ . Substitute the value of given moles as $4.00$ and molar mass as $180.156\text{g/mol}$ in the above formula and value of mass of given sample is calculated as shown below:

  $\begin{array}{c}4.00\text{mol}=\frac{\text{Given mass}}{180.156\text{g/mol}}\\ \text{Given mass}=4.00\text{ mol}\times 180.156\text{g/mol}\\ =\text{720}\text{.624}\text{g}\end{array}$

(d)

Interpretation Introduction

Interpretation:

The mass in grams for given sample has to be calculated.

Concept Introduction :

The formula to calculate the number of moles is given as shown below:

  $\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Answer to Problem 23A

The mass of ethanol is $2.1\times {10}^7\text{g}$ .

Explanation of Solution

The molar mass of ethanol is $46.07\text{g/mol}$ . Substitute the value of given moles as $4.56\times {10}^5$ and molar mass as $46.07\text{g/mol}$ in the above formula and value of mass of given sample is calculated as shown below:

  $\begin{array}{c}4.56\times {10}^5\text{mol}=\frac{\text{Given mass}}{46.07\text{g/mol}}\\ \text{Given mass}=4.56\times {10}^5\text{ mol}\times 46.07\text{g/mol}\\ =\text{2}\text{.1}\times {10}^7\text{g}\end{array}$

(e)

Interpretation Introduction

Interpretation:

The mass in grams for given sample has to be calculated.

Concept Introduction :

The formula to calculate the number of moles is given as shown below:

  $\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Answer to Problem 23A

The mass of calcium nitrate is $372.48\text{g}$ .

Explanation of Solution

The molar mass of calcium nitrate is $164.088\text{g/mol}$ . Substitute the value of given moles as $2.27$ and molar mass as $164.088\text{g/mol}$ in the above formula and value of mass of given sample is calculated as shown below:

  $\begin{array}{c}2.27\text{mol}=\frac{\text{Given mass}}{164.088\text{g/mol}}\\ \text{Given mass}=2.27\text{ mol}\times 164.088\text{g/mol}\\ =372.48\text{g}\end{array}$