Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
Question
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Chapter 18, Problem 18.21QE

(a)

Interpretation Introduction

Interpretation:

The balanced equation for the reaction has to be given and also has to specify the species which are oxidised and reduced.

  H2+O2H2O

(a)

Expert Solution
Check Mark

Explanation of Solution

The given reaction is as follows:

  H2+O2H2O

The two half-cell reactions can be written as below:

  H2H2OO2H2O

Steps for balancing half –reactions are given below:

  1. 1. Balance all atoms except H and O in half reaction.

    H2H2OO2H2O

  2. 2. Balance O atoms by adding water to the side missing O atoms.

    H2H2OO22H2O

  3. 3. Balance the H atoms by adding H+ to the side missing H atoms.

    H2+H2OH2O+2H+O2+4H+2H2O

  4. 4. Balance the charge by adding electrons to side with more total positive charge.

H2+H2OH2O+2H++2eO2+4H++4e2H2O

  1. 5. Make the number of electrons the same in both half- reactions by multiplication, while avoiding fractional number of electrons.

    2H2+2H2O2H2O+4H++4eO2+4H++4e2H2O

  2. 6. The half reactions can be added together and then same species on opposite side of the arrow can be cancelled for simplifying the equation:

    2H2+O22H2O

Therefore, the balanced reaction is as follows.

2H2+O22H2O

The change in oxidation state of reactants and products are given below:

2H20+O202H2+1O2

Oxidation state of hydrogen increases in the reaction and thus it is oxidised. Oxidation state of oxygen decreases in the reaction and thus it is reduced.

(b)

Interpretation Introduction

Interpretation:

The balanced equation for the reaction has to be given and also has to specify the species which are oxidised and reduced.

  Fe+O2Fe2O3

(b)

Expert Solution
Check Mark

Explanation of Solution

The given reaction is as follows:

  Fe+O2Fe2O3

The two half-cell reactions can be written as below:

  FeFe2O3O2H2O

Steps for balancing half –reactions are given below:

  1. 1. Balance all atoms except H and O in half reaction.

    2FeFe2O3O22H2O

  2. 2. Balance O atoms by adding water to the side missing O atoms.

    2Fe+3H2OFe2O3O22H2O

  3. 3. Balance the H atoms by adding H+ to the side missing H atoms.

    2Fe+3H2OFe2O3+6H+O2+4H+2H2O

  4. 4. Balance the charge by adding electrons to side with more total positive charge.

2Fe+3H2OFe2O3+6H++6eO2+4H++4e2H2O

  1. 5. Make the number of electrons the same in both half- reactions by multiplication, while avoiding fractional number of electrons.

    4Fe+6H2O2Fe2O3+12H++12e3O2+12H++12e6H2O

  2. 6. The half reactions can be added together and then same species on opposite side of the arrow can be cancelled for simplifying the equation:

    4Fe+3O22Fe2O3

Therefore, the balanced reaction is as follows.

4Fe+3O22Fe2O3

The change in oxidation state of reactants and products are given below:

4Fe0+3O202Fe+32O32

Oxidation state of iron increases in the reaction and thus it is oxidised. Oxidation state of oxygen decreases in the reaction and thus it is reduced.

(c)

Interpretation Introduction

Interpretation:

The balanced equation for the reaction has to be given and also has to specify the species which are oxidised and reduced.

  Al2O3+CAl+CO2

(c)

Expert Solution
Check Mark

Explanation of Solution

The given reaction is as follows:

  Al2O3+CAl+CO2

The two half-cell reactions can be written as below:

  CCO2Al2O3Al

Steps for balancing half –reactions are given below:

  1. 1. Balance all atoms except H and O in half reaction.

    CCO2Al2O32Al

  2. 2. Balance O atoms by adding water to the side missing O atoms.

    C+2H2OCO2Al2O32Al+3H2O

  3. 3. Balance the H atoms by adding H+ to the side missing H atoms.

    C+2H2OCO2+4H+Al2O3+6H+2Al+3H2O

  4. 4. Balance the charge by adding electrons to side with more total positive charge.

C+2H2OCO2+4H++4eAl2O3+6H++6e2Al+3H2O

  1. 5. Make the number of electrons the same in both half- reactions by multiplication, while avoiding fractional number of electrons.

    3C+6H2O3CO2+12H++12e2Al2O3+12H++12e4Al+6H2O

  2. 6. The half reactions can be added together and then same species on opposite side of the arrow can be cancelled for simplifying the equation:

    3C+2Al2O33CO2+4Al

Therefore, the balanced reaction is as follows.

3C+2Al2O33CO2+4Al

The change in oxidation state of reactants and products are given below:

3C0+2Al2+3O233C+4O22+4Al0

Oxidation state of carbon increases in the reaction and thus it is oxidised. Oxidation state of aluminium decreases in the reaction and thus it is reduced.

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Chapter 18 Solutions

Chemistry: Principles and Practice

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