The loss of electrons needs to be classified as oxidation or reduction. Concept Introduction : In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.

Question

Want to see more full solutions like this?

Answer 1

Question

Chapter 15, Problem 43UTC

(a)

Interpretation Introduction

Interpretation:

The loss of electrons needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.

(a)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

When electrons are lost in a chemical reaction, the type of reaction is said to be an oxidation reaction. In this reaction, oxidation state of the species increases. The oxidation reaction is shown as follows:

A→A++e−

Here, species A get oxidized to A+ by loss of 1 electron.

(b)

Interpretation Introduction

Interpretation:

The reaction of an oxidizing agent needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. When in reaction 1, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(b)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

An oxidizing agent is the chemical species which itself gain electron/s and oxidizes other species. Therefore, the reaction of an oxidizing agent is a reduction reaction.

For example:

A+B+→A++B

Here, B+ is an oxidizing agent as it oxidizes A to A+ and itself gets reduced to B.

(c)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

O2(g)→OH−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, oneof the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(c)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

O2(g)→OH−(aq)

The oxidation state of molecular oxygen is zero. It gets reduced to -2 in OH− thus, oxygen is getting reduced.

Therefore, the above reaction is a reduction reaction.

(d)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Br2(l)→2Br−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(d)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

Br2(l)→2Br−(aq)

Here, in the molecular bromine or Br₂, the oxidation state of bromine is 0.

Now, in Br^-, since, it gets reduced to -1, the bromine undergoes reduction. This takes place by gaining 2 electrons as there are 2 Br atoms in 1 Br₂ molecule.

Therefore, the given reaction is reduction.

(e)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Sn2+(aq)→Sn4+(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(e)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

In the given reaction is as follows:

Sn2+(aq)→Sn4+(aq)

The oxidation state of ‘Sn’ changes from +2 to +4. This means that Sn²+ loses2 electrons to form Sn⁴⁺. The oxidation state of an ion increases due to loss of electron/s thus, the given reaction is an oxidation reaction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Students have asked these similar questions

In the following reaction, identify the reactant that is oxidized and the reactant that is reduced: 2FeO(s) → 2Fe(s) + O2(g) Half-equations: for Fe2+ in FeO: 2Fe2+ + 4e–→ 2Fe for O2– in FeO: 2O2–→ O2 + 4e– A. Fe2+ in FeO is reduced, while O2– in FeO is oxidized. B. Fe2+ in FeO is oxidized, while O2– in FeO is reduced. C. Both Fe2+ and O2– in FeO are oxidized. D. Both Fe2+ and O2– in FeO are reduced.

Glutathione (G-SH), one of the most common tripeptides in animals, plants, and bacteria, is a scavenger of oxidizing agents. In reacting with oxidizing agents, glutathione is converted to G-S-S-G. Q. Write a balanced half-reaction for the reaction of two molecules of glutathione to form a disulfide bond. Is glutathione a biological oxidizing agent or a biological reducing agent?

When Fe+2 is biologically oxidized in mine wastewater, it precipitates as Fe+3 and can remove the red color of rivers. (1) Find the balanced equation for the biological oxidation of Fe+2. Use fs,max and ammonia as the nitrogen source. (2) How many g of oxygen is needed to oxidize 1 g of Fe+2?

Answer 2

Question

Chapter 15, Problem 43UTC

(a)

Interpretation Introduction

Interpretation:

The loss of electrons needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.

(a)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

When electrons are lost in a chemical reaction, the type of reaction is said to be an oxidation reaction. In this reaction, oxidation state of the species increases. The oxidation reaction is shown as follows:

A→A++e−

Here, species A get oxidized to A+ by loss of 1 electron.

(b)

Interpretation Introduction

Interpretation:

The reaction of an oxidizing agent needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. When in reaction 1, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(b)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

An oxidizing agent is the chemical species which itself gain electron/s and oxidizes other species. Therefore, the reaction of an oxidizing agent is a reduction reaction.

For example:

A+B+→A++B

Here, B+ is an oxidizing agent as it oxidizes A to A+ and itself gets reduced to B.

(c)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

O2(g)→OH−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, oneof the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(c)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

O2(g)→OH−(aq)

The oxidation state of molecular oxygen is zero. It gets reduced to -2 in OH− thus, oxygen is getting reduced.

Therefore, the above reaction is a reduction reaction.

(d)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Br2(l)→2Br−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(d)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

Br2(l)→2Br−(aq)

Here, in the molecular bromine or Br₂, the oxidation state of bromine is 0.

Now, in Br^-, since, it gets reduced to -1, the bromine undergoes reduction. This takes place by gaining 2 electrons as there are 2 Br atoms in 1 Br₂ molecule.

Therefore, the given reaction is reduction.

(e)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Sn2+(aq)→Sn4+(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(e)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

In the given reaction is as follows:

Sn2+(aq)→Sn4+(aq)

The oxidation state of ‘Sn’ changes from +2 to +4. This means that Sn²+ loses2 electrons to form Sn⁴⁺. The oxidation state of an ion increases due to loss of electron/s thus, the given reaction is an oxidation reaction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 15, Problem 43UTC

(a)

Interpretation Introduction

Interpretation:

The loss of electrons needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.

(a)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

When electrons are lost in a chemical reaction, the type of reaction is said to be an oxidation reaction. In this reaction, oxidation state of the species increases. The oxidation reaction is shown as follows:

A→A++e−

Here, species A get oxidized to A+ by loss of 1 electron.

(b)

Interpretation Introduction

Interpretation:

The reaction of an oxidizing agent needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. When in reaction 1, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(b)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

An oxidizing agent is the chemical species which itself gain electron/s and oxidizes other species. Therefore, the reaction of an oxidizing agent is a reduction reaction.

For example:

A+B+→A++B

Here, B+ is an oxidizing agent as it oxidizes A to A+ and itself gets reduced to B.

(c)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

O2(g)→OH−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, oneof the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(c)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

O2(g)→OH−(aq)

The oxidation state of molecular oxygen is zero. It gets reduced to -2 in OH− thus, oxygen is getting reduced.

Therefore, the above reaction is a reduction reaction.

(d)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Br2(l)→2Br−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(d)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

Br2(l)→2Br−(aq)

Here, in the molecular bromine or Br₂, the oxidation state of bromine is 0.

Now, in Br^-, since, it gets reduced to -1, the bromine undergoes reduction. This takes place by gaining 2 electrons as there are 2 Br atoms in 1 Br₂ molecule.

Therefore, the given reaction is reduction.

(e)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Sn2+(aq)→Sn4+(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(e)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

In the given reaction is as follows:

Sn2+(aq)→Sn4+(aq)

The oxidation state of ‘Sn’ changes from +2 to +4. This means that Sn²+ loses2 electrons to form Sn⁴⁺. The oxidation state of an ion increases due to loss of electron/s thus, the given reaction is an oxidation reaction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 15, Problem 43UTC

(a)

Interpretation Introduction

Interpretation:

The loss of electrons needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.

(a)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

When electrons are lost in a chemical reaction, the type of reaction is said to be an oxidation reaction. In this reaction, oxidation state of the species increases. The oxidation reaction is shown as follows:

A→A++e−

Here, species A get oxidized to A+ by loss of 1 electron.

(b)

Interpretation Introduction

Interpretation:

The reaction of an oxidizing agent needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. When in reaction 1, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(b)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

An oxidizing agent is the chemical species which itself gain electron/s and oxidizes other species. Therefore, the reaction of an oxidizing agent is a reduction reaction.

For example:

A+B+→A++B

Here, B+ is an oxidizing agent as it oxidizes A to A+ and itself gets reduced to B.

(c)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

O2(g)→OH−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, oneof the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(c)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

O2(g)→OH−(aq)

The oxidation state of molecular oxygen is zero. It gets reduced to -2 in OH− thus, oxygen is getting reduced.

Therefore, the above reaction is a reduction reaction.

(d)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Br2(l)→2Br−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(d)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

Br2(l)→2Br−(aq)

Here, in the molecular bromine or Br₂, the oxidation state of bromine is 0.

Now, in Br^-, since, it gets reduced to -1, the bromine undergoes reduction. This takes place by gaining 2 electrons as there are 2 Br atoms in 1 Br₂ molecule.

Therefore, the given reaction is reduction.

(e)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Sn2+(aq)→Sn4+(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(e)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

In the given reaction is as follows:

Sn2+(aq)→Sn4+(aq)

The oxidation state of ‘Sn’ changes from +2 to +4. This means that Sn²+ loses2 electrons to form Sn⁴⁺. The oxidation state of an ion increases due to loss of electron/s thus, the given reaction is an oxidation reaction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 15, Problem 43UTC

(a)

Interpretation Introduction

Interpretation:

The loss of electrons needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.

(a)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

When electrons are lost in a chemical reaction, the type of reaction is said to be an oxidation reaction. In this reaction, oxidation state of the species increases. The oxidation reaction is shown as follows:

A→A++e−

Here, species A get oxidized to A+ by loss of 1 electron.

(b)

Interpretation Introduction

Interpretation:

The reaction of an oxidizing agent needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. When in reaction 1, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(b)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

An oxidizing agent is the chemical species which itself gain electron/s and oxidizes other species. Therefore, the reaction of an oxidizing agent is a reduction reaction.

For example:

A+B+→A++B

Here, B+ is an oxidizing agent as it oxidizes A to A+ and itself gets reduced to B.

(c)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

O2(g)→OH−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, oneof the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(c)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

O2(g)→OH−(aq)

The oxidation state of molecular oxygen is zero. It gets reduced to -2 in OH− thus, oxygen is getting reduced.

Therefore, the above reaction is a reduction reaction.

(d)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Br2(l)→2Br−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(d)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

Br2(l)→2Br−(aq)

Here, in the molecular bromine or Br₂, the oxidation state of bromine is 0.

Now, in Br^-, since, it gets reduced to -1, the bromine undergoes reduction. This takes place by gaining 2 electrons as there are 2 Br atoms in 1 Br₂ molecule.

Therefore, the given reaction is reduction.

(e)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Sn2+(aq)→Sn4+(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(e)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

In the given reaction is as follows:

Sn2+(aq)→Sn4+(aq)

The oxidation state of ‘Sn’ changes from +2 to +4. This means that Sn²+ loses2 electrons to form Sn⁴⁺. The oxidation state of an ion increases due to loss of electron/s thus, the given reaction is an oxidation reaction.

Answer 6

Chapter 15, Problem 43UTC

(a)

Interpretation Introduction

Interpretation:

The loss of electrons needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.

(a)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

When electrons are lost in a chemical reaction, the type of reaction is said to be an oxidation reaction. In this reaction, oxidation state of the species increases. The oxidation reaction is shown as follows:

A→A++e−

Here, species A get oxidized to A+ by loss of 1 electron.

Answer 7

Chapter 15, Problem 43UTC

(a)

Interpretation Introduction

Interpretation:

The loss of electrons needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction.

Answer 8

(a)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

When electrons are lost in a chemical reaction, the type of reaction is said to be an oxidation reaction. In this reaction, oxidation state of the species increases. The oxidation reaction is shown as follows:

A→A++e−

Here, species A get oxidized to A+ by loss of 1 electron.

Answer 13

(b)

Interpretation Introduction

Interpretation:

The reaction of an oxidizing agent needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. When in reaction 1, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(b)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

An oxidizing agent is the chemical species which itself gain electron/s and oxidizes other species. Therefore, the reaction of an oxidizing agent is a reduction reaction.

For example:

A+B+→A++B

Here, B+ is an oxidizing agent as it oxidizes A to A+ and itself gets reduced to B.

Answer 14

(b)

Interpretation Introduction

Interpretation:

The reaction of an oxidizing agent needs to be classified as oxidation or reduction.

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. When in reaction 1, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

Answer 15

(b)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

An oxidizing agent is the chemical species which itself gain electron/s and oxidizes other species. Therefore, the reaction of an oxidizing agent is a reduction reaction.

For example:

A+B+→A++B

Here, B+ is an oxidizing agent as it oxidizes A to A+ and itself gets reduced to B.

Answer 20

(c)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

O2(g)→OH−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, oneof the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(c)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

O2(g)→OH−(aq)

The oxidation state of molecular oxygen is zero. It gets reduced to -2 in OH− thus, oxygen is getting reduced.

Therefore, the above reaction is a reduction reaction.

Answer 21

(c)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

O2(g)→OH−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, oneof the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

Answer 22

(c)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

The given reaction is as follows:

O2(g)→OH−(aq)

The oxidation state of molecular oxygen is zero. It gets reduced to -2 in OH− thus, oxygen is getting reduced.

Therefore, the above reaction is a reduction reaction.

Answer 27

(d)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Br2(l)→2Br−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(d)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Explanation of Solution

The given reaction is as follows:

Br2(l)→2Br−(aq)

Here, in the molecular bromine or Br₂, the oxidation state of bromine is 0.

Now, in Br^-, since, it gets reduced to -1, the bromine undergoes reduction. This takes place by gaining 2 electrons as there are 2 Br atoms in 1 Br₂ molecule.

Therefore, the given reaction is reduction.

Answer 28

(d)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Br2(l)→2Br−(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and 1 gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

Answer 29

(d)

Expert Solution

Answer to Problem 43UTC

Reduction reaction.

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

The given reaction is as follows:

Br2(l)→2Br−(aq)

Here, in the molecular bromine or Br₂, the oxidation state of bromine is 0.

Now, in Br^-, since, it gets reduced to -1, the bromine undergoes reduction. This takes place by gaining 2 electrons as there are 2 Br atoms in 1 Br₂ molecule.

Therefore, the given reaction is reduction.

Answer 34

(e)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Sn2+(aq)→Sn4+(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

(e)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Explanation of Solution

In the given reaction is as follows:

Sn2+(aq)→Sn4+(aq)

The oxidation state of ‘Sn’ changes from +2 to +4. This means that Sn²+ loses2 electrons to form Sn⁴⁺. The oxidation state of an ion increases due to loss of electron/s thus, the given reaction is an oxidation reaction.

Answer 35

(e)

Interpretation Introduction

Interpretation:

The given reaction needs to be classified as oxidation or reduction:

Sn2+(aq)→Sn4+(aq)

Concept Introduction :

In a redox reaction both oxidation and reduction take place simultaneously. Oxidation takes place by loss of electrons and reduction takes place by gain of electrons. The oxidation state of a species increases on oxidation and decreases on reduction. In a reaction, one of the reactants get oxidized and one gets reduced, this is known as a redox reaction. The species that oxidizes others and itself gets reduced is known as an oxidizing agent.

Answer 36

(e)

Expert Solution

Answer to Problem 43UTC

Oxidation reaction.

Answer 37

(e)

Expert Solution

Answer 38

(e)

Expert Solution

Answer 39

Expert Solution

Answer 40

Explanation of Solution

In the given reaction is as follows:

Sn2+(aq)→Sn4+(aq)

The oxidation state of ‘Sn’ changes from +2 to +4. This means that Sn²+ loses2 electrons to form Sn⁴⁺. The oxidation state of an ion increases due to loss of electron/s thus, the given reaction is an oxidation reaction.