The following reaction that occurs in acidic solution has to be balanced. N H 4 + + N O 3 − → N 2 O Concept introduction: Procedure for balancing the redox reaction in acidic and basic solution is given below. 1) The oxidation half reaction equation and a reduction half reaction equation of the given reaction have to be separated. 2) The half reaction equation has to be balanced with respect to all atoms other than oxygen and hydrogen. 3) Each half reaction equation has to be balanced with respect to oxygen atoms by adding the suitable number of H 2 O molecules to the side where oxygen atom is deficient. (For metal hydroxides, directly add O H − ions and skip steps 3 – 4. ) 4) In Acidic Solution: Each half reaction equation has to be balanced with respect to hydrogen atoms by adding the suitable number of H + ions to the side deficient in hydrogen atoms. In Basic Solution: Each half reaction has to be balanced with respect to hydrogen atoms by adding a number of H 2 O molecules equal to the number of excess hydrogen atoms to the side deficient in hydrogen atoms and an equal number of O H − ions to the side opposite to the added H 2 O molecules. 5) Each half reaction equation has to be balanced with respect to charge by adding the suitable number of electrons to the side with the excess positive charge. 6) Each half reaction equation has to be multiplied by an integer that makes the number of electrons given by the oxidation half reaction equation equal to the number of electrons taken by the reduction half reaction equation. 7) The complete balanced equation is obtained by adding the two half reaction equations and canceling or combining any like terms.

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Answer 1

Question

Chapter 24, Problem 24.33P

(a)

Interpretation Introduction

Interpretation:

The following reaction that occurs in acidic solution has to be balanced.

NH4++ NO3− →N2O

Concept introduction:

Procedure for balancing the redox reaction in acidic and basic solution is given below.

1) The oxidation half reaction equation and a reduction half reaction equation of the given reaction have to be separated.

2) The half reaction equation has to be balanced with respect to all atoms other than oxygen and hydrogen.

3) Each half reaction equation has to be balanced with respect to oxygen atoms by adding the suitable number of H2O molecules to the side where oxygen atom is deficient. (For metal hydroxides, directly add OH− ions and skip steps 3–4.)

4) In Acidic Solution: Each half reaction equation has to be balanced with respect to hydrogen atoms by adding the suitable number of H+ ions to the side deficient in hydrogen atoms.
In Basic Solution: Each half reaction has to be balanced with respect to hydrogen atoms by adding a number of H2O molecules equal to the number of excess hydrogen atoms to the side deficient in hydrogen atoms and an equal number of OH− ions to the side opposite to the added H2O molecules.

5) Each half reaction equation has to be balanced with respect to charge by adding the suitable number of electrons to the side with the excess positive charge.

6) Each half reaction equation has to be multiplied by an integer that makes the number of electrons given by the oxidation half reaction equation equal to the number of electrons taken by the reduction half reaction equation.

7) The complete balanced equation is obtained by adding the two half reaction equations and canceling or combining any like terms.

(b)

Interpretation Introduction

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).

Expert Solution & Answer

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Answer 2

Question

Chapter 24, Problem 24.33P

(a)

Interpretation Introduction

Interpretation:

The following reaction that occurs in acidic solution has to be balanced.

NH4++ NO3− →N2O

Concept introduction:

Procedure for balancing the redox reaction in acidic and basic solution is given below.

1) The oxidation half reaction equation and a reduction half reaction equation of the given reaction have to be separated.

2) The half reaction equation has to be balanced with respect to all atoms other than oxygen and hydrogen.

3) Each half reaction equation has to be balanced with respect to oxygen atoms by adding the suitable number of H2O molecules to the side where oxygen atom is deficient. (For metal hydroxides, directly add OH− ions and skip steps 3–4.)

4) In Acidic Solution: Each half reaction equation has to be balanced with respect to hydrogen atoms by adding the suitable number of H+ ions to the side deficient in hydrogen atoms.
In Basic Solution: Each half reaction has to be balanced with respect to hydrogen atoms by adding a number of H2O molecules equal to the number of excess hydrogen atoms to the side deficient in hydrogen atoms and an equal number of OH− ions to the side opposite to the added H2O molecules.

5) Each half reaction equation has to be balanced with respect to charge by adding the suitable number of electrons to the side with the excess positive charge.

6) Each half reaction equation has to be multiplied by an integer that makes the number of electrons given by the oxidation half reaction equation equal to the number of electrons taken by the reduction half reaction equation.

7) The complete balanced equation is obtained by adding the two half reaction equations and canceling or combining any like terms.

(b)

Interpretation Introduction

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).

Expert Solution & Answer

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Answer 3

Question

Chapter 24, Problem 24.33P

(a)

Interpretation Introduction

Interpretation:

The following reaction that occurs in acidic solution has to be balanced.

NH4++ NO3− →N2O

Concept introduction:

Procedure for balancing the redox reaction in acidic and basic solution is given below.

1) The oxidation half reaction equation and a reduction half reaction equation of the given reaction have to be separated.

2) The half reaction equation has to be balanced with respect to all atoms other than oxygen and hydrogen.

3) Each half reaction equation has to be balanced with respect to oxygen atoms by adding the suitable number of H2O molecules to the side where oxygen atom is deficient. (For metal hydroxides, directly add OH− ions and skip steps 3–4.)

4) In Acidic Solution: Each half reaction equation has to be balanced with respect to hydrogen atoms by adding the suitable number of H+ ions to the side deficient in hydrogen atoms.
In Basic Solution: Each half reaction has to be balanced with respect to hydrogen atoms by adding a number of H2O molecules equal to the number of excess hydrogen atoms to the side deficient in hydrogen atoms and an equal number of OH− ions to the side opposite to the added H2O molecules.

5) Each half reaction equation has to be balanced with respect to charge by adding the suitable number of electrons to the side with the excess positive charge.

6) Each half reaction equation has to be multiplied by an integer that makes the number of electrons given by the oxidation half reaction equation equal to the number of electrons taken by the reduction half reaction equation.

7) The complete balanced equation is obtained by adding the two half reaction equations and canceling or combining any like terms.

(b)

Interpretation Introduction

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).

Expert Solution & Answer

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Answer 4

Question

Chapter 24, Problem 24.33P

(a)

Interpretation Introduction

Interpretation:

The following reaction that occurs in acidic solution has to be balanced.

NH4++ NO3− →N2O

Concept introduction:

Procedure for balancing the redox reaction in acidic and basic solution is given below.

1) The oxidation half reaction equation and a reduction half reaction equation of the given reaction have to be separated.

2) The half reaction equation has to be balanced with respect to all atoms other than oxygen and hydrogen.

3) Each half reaction equation has to be balanced with respect to oxygen atoms by adding the suitable number of H2O molecules to the side where oxygen atom is deficient. (For metal hydroxides, directly add OH− ions and skip steps 3–4.)

4) In Acidic Solution: Each half reaction equation has to be balanced with respect to hydrogen atoms by adding the suitable number of H+ ions to the side deficient in hydrogen atoms.
In Basic Solution: Each half reaction has to be balanced with respect to hydrogen atoms by adding a number of H2O molecules equal to the number of excess hydrogen atoms to the side deficient in hydrogen atoms and an equal number of OH− ions to the side opposite to the added H2O molecules.

5) Each half reaction equation has to be balanced with respect to charge by adding the suitable number of electrons to the side with the excess positive charge.

6) Each half reaction equation has to be multiplied by an integer that makes the number of electrons given by the oxidation half reaction equation equal to the number of electrons taken by the reduction half reaction equation.

7) The complete balanced equation is obtained by adding the two half reaction equations and canceling or combining any like terms.

(b)

Interpretation Introduction

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).

Expert Solution & Answer

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Answer 5

Chapter 24, Problem 24.33P

(a)

Interpretation Introduction

Interpretation:

The following reaction that occurs in acidic solution has to be balanced.

NH4++ NO3− →N2O

Concept introduction:

Procedure for balancing the redox reaction in acidic and basic solution is given below.

1) The oxidation half reaction equation and a reduction half reaction equation of the given reaction have to be separated.

2) The half reaction equation has to be balanced with respect to all atoms other than oxygen and hydrogen.

3) Each half reaction equation has to be balanced with respect to oxygen atoms by adding the suitable number of H2O molecules to the side where oxygen atom is deficient. (For metal hydroxides, directly add OH− ions and skip steps 3–4.)

4) In Acidic Solution: Each half reaction equation has to be balanced with respect to hydrogen atoms by adding the suitable number of H+ ions to the side deficient in hydrogen atoms.
In Basic Solution: Each half reaction has to be balanced with respect to hydrogen atoms by adding a number of H2O molecules equal to the number of excess hydrogen atoms to the side deficient in hydrogen atoms and an equal number of OH− ions to the side opposite to the added H2O molecules.

5) Each half reaction equation has to be balanced with respect to charge by adding the suitable number of electrons to the side with the excess positive charge.

6) Each half reaction equation has to be multiplied by an integer that makes the number of electrons given by the oxidation half reaction equation equal to the number of electrons taken by the reduction half reaction equation.

7) The complete balanced equation is obtained by adding the two half reaction equations and canceling or combining any like terms.

(b)

Interpretation Introduction

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).

Answer 6

Chapter 24, Problem 24.33P

(a)

Interpretation Introduction

Interpretation:

The following reaction that occurs in acidic solution has to be balanced.

NH4++ NO3− →N2O

Concept introduction:

Procedure for balancing the redox reaction in acidic and basic solution is given below.

1) The oxidation half reaction equation and a reduction half reaction equation of the given reaction have to be separated.

2) The half reaction equation has to be balanced with respect to all atoms other than oxygen and hydrogen.

3) Each half reaction equation has to be balanced with respect to oxygen atoms by adding the suitable number of H2O molecules to the side where oxygen atom is deficient. (For metal hydroxides, directly add OH− ions and skip steps 3–4.)

4) In Acidic Solution: Each half reaction equation has to be balanced with respect to hydrogen atoms by adding the suitable number of H+ ions to the side deficient in hydrogen atoms.
In Basic Solution: Each half reaction has to be balanced with respect to hydrogen atoms by adding a number of H2O molecules equal to the number of excess hydrogen atoms to the side deficient in hydrogen atoms and an equal number of OH− ions to the side opposite to the added H2O molecules.

5) Each half reaction equation has to be balanced with respect to charge by adding the suitable number of electrons to the side with the excess positive charge.

6) Each half reaction equation has to be multiplied by an integer that makes the number of electrons given by the oxidation half reaction equation equal to the number of electrons taken by the reduction half reaction equation.

7) The complete balanced equation is obtained by adding the two half reaction equations and canceling or combining any like terms.

Answer 7

Chapter 24, Problem 24.33P

(a)

Interpretation Introduction

Interpretation:

The following reaction that occurs in acidic solution has to be balanced.

NH4++ NO3− →N2O

Concept introduction:

Procedure for balancing the redox reaction in acidic and basic solution is given below.

1) The oxidation half reaction equation and a reduction half reaction equation of the given reaction have to be separated.

2) The half reaction equation has to be balanced with respect to all atoms other than oxygen and hydrogen.

3) Each half reaction equation has to be balanced with respect to oxygen atoms by adding the suitable number of H2O molecules to the side where oxygen atom is deficient. (For metal hydroxides, directly add OH− ions and skip steps 3–4.)

4) In Acidic Solution: Each half reaction equation has to be balanced with respect to hydrogen atoms by adding the suitable number of H+ ions to the side deficient in hydrogen atoms.
In Basic Solution: Each half reaction has to be balanced with respect to hydrogen atoms by adding a number of H2O molecules equal to the number of excess hydrogen atoms to the side deficient in hydrogen atoms and an equal number of OH− ions to the side opposite to the added H2O molecules.

5) Each half reaction equation has to be balanced with respect to charge by adding the suitable number of electrons to the side with the excess positive charge.

6) Each half reaction equation has to be multiplied by an integer that makes the number of electrons given by the oxidation half reaction equation equal to the number of electrons taken by the reduction half reaction equation.

7) The complete balanced equation is obtained by adding the two half reaction equations and canceling or combining any like terms.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).

Answer 10

Expert Solution & Answer

Answer 11

Expert Solution & Answer

Answer 12

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Answer 13

Ch. 24 - Prob. 24.1P Ch. 24 - Prob. 24.2P Ch. 24 - Prob. 24.3P Ch. 24 - Prob. 24.4P Ch. 24 - Prob. 24.5P Ch. 24 - Prob. 24.6P Ch. 24 - Prob. 24.7P Ch. 24 - Prob. 24.8P Ch. 24 - Prob. 24.9P Ch. 24 - Prob. 24.10P

Videos

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).

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Chapter 24 Solutions

Videos

Interpretation: The following reaction that occurs in basic solution has to be balanced. Fe+O2→ Fe2O3.3 H2O Fe+O2→ Fe2O3 Concept introduction: Refer to part (a).

Want to see the full answer?

Chapter 24 Solutions

Interpretation:

The following reaction that occurs in basic solution has to be balanced.

Fe+O2→ Fe2O3.3 H2O

Fe+O2→ Fe2O3

Concept introduction:

Refer to part (a).