Chapter 22, Problem 107A

a.

Interpretation Introduction

Interpretation: To balance the given redox reaction.

Concept Introduction: Redox reaction is the one in which oxidation and reduction take place together.

Answer to Problem 107A

The balanced redox reaction is represented as follows:

  ${\text{2 C}}_{\text{3}}{\text{H}}_{\text{7}}\text{OH}\left(l\right)+{\text{ 9 O}}_{\text{2}}\left(g\right)\to {\text{ 6 CO}}_{\text{2}}\left(g\right)+{\text{ 8 H}}_{\text{2}}\text{O}\left(l\right)$

Explanation of Solution

For balancing a redox reaction, some steps must be followed that are discussed as follows:

1. Write the reaction in an unbalanced form.
2. Identify the atoms that are oxidized or reduced while looking at their oxidation numbers.
3. Differ the reaction by determining where oxidation or reduction takes place.
4. Write the coefficients wherever required.
5. Then, finally, write a balanced redox reaction.

The unbalanced redox reaction is given as follows:

  ${\text{C}}_{\text{3}}{\text{H}}_{\text{7}}\text{OH}\left(l\right)+{\text{O}}_{\text{2}}\left(g\right)\to {\text{CO}}_{\text{2}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

The oxidation numbers must be assigned to each element in a reaction.

  ${\text{C}}_{\text{3}}{}^{-2}{\text{H}}_{\text{7}}{\text{O}}^{-2}\text{H}\left(l\right)+{\text{O}}_{\text{2}}{}^0\left(g\right)\to {\text{C}}^4{\text{O}}_{\text{2}}{}^{-2}\left(g\right)+{\text{H}}_{\text{2}}{\text{O}}^{-2}\left(l\right)$

The balanced redox reaction is represented as follows:

Writing coefficients in front of atoms wherever required in order to balance the reaction.

  ${\text{2 C}}_{\text{3}}{\text{H}}_{\text{7}}\text{OH}\left(l\right)+{\text{ 9 O}}_{\text{2}}\left(g\right)\to {\text{ 6 CO}}_{\text{2}}\left(g\right)+{\text{ 8 H}}_{\text{2}}\text{O}\left(l\right)$

b.

Interpretation Introduction

Interpretation: To balance the given redox reaction

Concept Introduction: Redox reaction is the one in which oxidation and reduction take place together.

Answer to Problem 107A

The balanced redox reaction is represented as follows:

  $\text{3 BaO}\left(s\right)+\text{ 2 Al}\left(s\right)\to {\text{Al}}_{\text{2}}{\text{O}}_3\left(s\right)+\text{ 3 Ba}\left(s\right)$

Explanation of Solution

For balancing a redox reaction, some steps must be followed that are discussed as follows:

1. Write the reaction in an unbalanced form.
2. Identify the atoms that are oxidized or reduced while looking at their oxidation numbers.
3. Differ the reaction by determining where oxidation or reduction takes place.
4. Write the coefficients wherever required.
5. Then, finally, write a balanced redox reaction.

The unbalanced redox reaction is given as follows:

  $\text{ BaO}\left(s\right)+\text{Al}\left(s\right)\to {\text{Al}}_{\text{2}}{\text{O}}_3\left(s\right)+\text{Ba}\left(s\right)$

The oxidation numbers must be assigned to each element in a reaction.

  ${\text{ Ba}}^3\text{O}\left(s\right)+{\text{Al}}^0\left(s\right)\to {\text{Al}}_{\text{2}}{}^3{\text{O}}_3\left(s\right)+{\text{Ba}}^0\left(s\right)$

The balanced redox reaction is represented as follows:

Writing coefficients in front of atoms wherever required in order to balance the reaction.

  $\text{3 BaO}\left(s\right)+\text{ 2 Al}\left(s\right)\to {\text{Al}}_{\text{2}}{\text{O}}_3\left(s\right)+\text{ 3 Ba}\left(s\right)$