The reactions occurring in the given equations. Introduction: In living organisms, redox reactions are those in which electrons are transferred between an electron donor (known as thereducing agent) and an electron acceptor (known as the oxidizing agent). The tendency of a specific substance to gain an electron is known as its reduction potential. It is denoted as E o .

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Answer 1

Question

Chapter 9, Problem 1Q

Summary Introduction

To review:

The reactions occurring in the given equations.

Introduction:

In living organisms, redox reactions are those in which electrons are transferred between an electron donor (known as thereducing agent) and an electron acceptor (known as the oxidizing agent). The tendency of a specific substance to gain an electron is known as its reduction potential. It is denoted as E^o .

Expert Solution & Answer

Explanation of Solution

The first reaction: Under the appropriateconditions, a redox half-reaction will always reduce any of the half reactions below it in table 9.1. So, the standard redox potential of the production of ethanol is +0.20.The standard potential of the production of cytochrome b (Fe²⁺ ) is 0.075. The standard reduction potential of the reaction is +0.275. As this value is positive, it will not be spontaneous.

The secondreaction: The standard reaction for the production of the cyt (Fe²⁺ ) is –0.075. On the other hand, the standard redox potential of the production of NO₃–will be –0.42.As the standard potential of its reverse reaction is +0.42, the standard potential of the reaction is –0.345. This reaction will be spontaneous.

Conclusion

Therefore, it can be concluded that in redox reactions, the transfer of electrons and protons takes place. If a reaction has a negative redox potential, it will be spontaneous, and if the redox potential of a reaction is positive, it will not be spontaneous. In reaction 1, the reduction potential is positive, and s, ohe reaction is spontaneous. Reaction 2 has a negative reduction potential, and so, it is not spontaneous.

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Answer 2

Question

Chapter 9, Problem 1Q

Summary Introduction

To review:

The reactions occurring in the given equations.

Introduction:

In living organisms, redox reactions are those in which electrons are transferred between an electron donor (known as thereducing agent) and an electron acceptor (known as the oxidizing agent). The tendency of a specific substance to gain an electron is known as its reduction potential. It is denoted as E^o .

Expert Solution & Answer

Explanation of Solution

The first reaction: Under the appropriateconditions, a redox half-reaction will always reduce any of the half reactions below it in table 9.1. So, the standard redox potential of the production of ethanol is +0.20.The standard potential of the production of cytochrome b (Fe²⁺ ) is 0.075. The standard reduction potential of the reaction is +0.275. As this value is positive, it will not be spontaneous.

The secondreaction: The standard reaction for the production of the cyt (Fe²⁺ ) is –0.075. On the other hand, the standard redox potential of the production of NO₃–will be –0.42.As the standard potential of its reverse reaction is +0.42, the standard potential of the reaction is –0.345. This reaction will be spontaneous.

Conclusion

Therefore, it can be concluded that in redox reactions, the transfer of electrons and protons takes place. If a reaction has a negative redox potential, it will be spontaneous, and if the redox potential of a reaction is positive, it will not be spontaneous. In reaction 1, the reduction potential is positive, and s, ohe reaction is spontaneous. Reaction 2 has a negative reduction potential, and so, it is not spontaneous.

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Answer 3

Question

Chapter 9, Problem 1Q

Summary Introduction

To review:

The reactions occurring in the given equations.

Introduction:

In living organisms, redox reactions are those in which electrons are transferred between an electron donor (known as thereducing agent) and an electron acceptor (known as the oxidizing agent). The tendency of a specific substance to gain an electron is known as its reduction potential. It is denoted as E^o .

Expert Solution & Answer

Explanation of Solution

The first reaction: Under the appropriateconditions, a redox half-reaction will always reduce any of the half reactions below it in table 9.1. So, the standard redox potential of the production of ethanol is +0.20.The standard potential of the production of cytochrome b (Fe²⁺ ) is 0.075. The standard reduction potential of the reaction is +0.275. As this value is positive, it will not be spontaneous.

The secondreaction: The standard reaction for the production of the cyt (Fe²⁺ ) is –0.075. On the other hand, the standard redox potential of the production of NO₃–will be –0.42.As the standard potential of its reverse reaction is +0.42, the standard potential of the reaction is –0.345. This reaction will be spontaneous.

Conclusion

Therefore, it can be concluded that in redox reactions, the transfer of electrons and protons takes place. If a reaction has a negative redox potential, it will be spontaneous, and if the redox potential of a reaction is positive, it will not be spontaneous. In reaction 1, the reduction potential is positive, and s, ohe reaction is spontaneous. Reaction 2 has a negative reduction potential, and so, it is not spontaneous.

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Answer 4

Question

Chapter 9, Problem 1Q

Summary Introduction

To review:

The reactions occurring in the given equations.

Introduction:

In living organisms, redox reactions are those in which electrons are transferred between an electron donor (known as thereducing agent) and an electron acceptor (known as the oxidizing agent). The tendency of a specific substance to gain an electron is known as its reduction potential. It is denoted as E^o .

Expert Solution & Answer

Explanation of Solution

The first reaction: Under the appropriateconditions, a redox half-reaction will always reduce any of the half reactions below it in table 9.1. So, the standard redox potential of the production of ethanol is +0.20.The standard potential of the production of cytochrome b (Fe²⁺ ) is 0.075. The standard reduction potential of the reaction is +0.275. As this value is positive, it will not be spontaneous.

The secondreaction: The standard reaction for the production of the cyt (Fe²⁺ ) is –0.075. On the other hand, the standard redox potential of the production of NO₃–will be –0.42.As the standard potential of its reverse reaction is +0.42, the standard potential of the reaction is –0.345. This reaction will be spontaneous.

Conclusion

Therefore, it can be concluded that in redox reactions, the transfer of electrons and protons takes place. If a reaction has a negative redox potential, it will be spontaneous, and if the redox potential of a reaction is positive, it will not be spontaneous. In reaction 1, the reduction potential is positive, and s, ohe reaction is spontaneous. Reaction 2 has a negative reduction potential, and so, it is not spontaneous.

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Answer 5

Chapter 9, Problem 1Q

Summary Introduction

To review:

The reactions occurring in the given equations.

Introduction:

In living organisms, redox reactions are those in which electrons are transferred between an electron donor (known as thereducing agent) and an electron acceptor (known as the oxidizing agent). The tendency of a specific substance to gain an electron is known as its reduction potential. It is denoted as E^o .

Expert Solution & Answer

Explanation of Solution

The first reaction: Under the appropriateconditions, a redox half-reaction will always reduce any of the half reactions below it in table 9.1. So, the standard redox potential of the production of ethanol is +0.20.The standard potential of the production of cytochrome b (Fe²⁺ ) is 0.075. The standard reduction potential of the reaction is +0.275. As this value is positive, it will not be spontaneous.

The secondreaction: The standard reaction for the production of the cyt (Fe²⁺ ) is –0.075. On the other hand, the standard redox potential of the production of NO₃–will be –0.42.As the standard potential of its reverse reaction is +0.42, the standard potential of the reaction is –0.345. This reaction will be spontaneous.

Conclusion

Therefore, it can be concluded that in redox reactions, the transfer of electrons and protons takes place. If a reaction has a negative redox potential, it will be spontaneous, and if the redox potential of a reaction is positive, it will not be spontaneous. In reaction 1, the reduction potential is positive, and s, ohe reaction is spontaneous. Reaction 2 has a negative reduction potential, and so, it is not spontaneous.

Answer 6

Chapter 9, Problem 1Q

Summary Introduction

To review:

The reactions occurring in the given equations.

Introduction:

In living organisms, redox reactions are those in which electrons are transferred between an electron donor (known as thereducing agent) and an electron acceptor (known as the oxidizing agent). The tendency of a specific substance to gain an electron is known as its reduction potential. It is denoted as E^o .

Expert Solution & Answer

Explanation of Solution

The first reaction: Under the appropriateconditions, a redox half-reaction will always reduce any of the half reactions below it in table 9.1. So, the standard redox potential of the production of ethanol is +0.20.The standard potential of the production of cytochrome b (Fe²⁺ ) is 0.075. The standard reduction potential of the reaction is +0.275. As this value is positive, it will not be spontaneous.

The secondreaction: The standard reaction for the production of the cyt (Fe²⁺ ) is –0.075. On the other hand, the standard redox potential of the production of NO₃–will be –0.42.As the standard potential of its reverse reaction is +0.42, the standard potential of the reaction is –0.345. This reaction will be spontaneous.

Conclusion

Therefore, it can be concluded that in redox reactions, the transfer of electrons and protons takes place. If a reaction has a negative redox potential, it will be spontaneous, and if the redox potential of a reaction is positive, it will not be spontaneous. In reaction 1, the reduction potential is positive, and s, ohe reaction is spontaneous. Reaction 2 has a negative reduction potential, and so, it is not spontaneous.

Answer 7

Chapter 9, Problem 1Q

Summary Introduction

To review:

The reactions occurring in the given equations.

Introduction:

In living organisms, redox reactions are those in which electrons are transferred between an electron donor (known as thereducing agent) and an electron acceptor (known as the oxidizing agent). The tendency of a specific substance to gain an electron is known as its reduction potential. It is denoted as E^o .

Answer 8

Expert Solution & Answer

Explanation of Solution

The first reaction: Under the appropriateconditions, a redox half-reaction will always reduce any of the half reactions below it in table 9.1. So, the standard redox potential of the production of ethanol is +0.20.The standard potential of the production of cytochrome b (Fe²⁺ ) is 0.075. The standard reduction potential of the reaction is +0.275. As this value is positive, it will not be spontaneous.

The secondreaction: The standard reaction for the production of the cyt (Fe²⁺ ) is –0.075. On the other hand, the standard redox potential of the production of NO₃–will be –0.42.As the standard potential of its reverse reaction is +0.42, the standard potential of the reaction is –0.345. This reaction will be spontaneous.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Conclusion

Therefore, it can be concluded that in redox reactions, the transfer of electrons and protons takes place. If a reaction has a negative redox potential, it will be spontaneous, and if the redox potential of a reaction is positive, it will not be spontaneous. In reaction 1, the reduction potential is positive, and s, ohe reaction is spontaneous. Reaction 2 has a negative reduction potential, and so, it is not spontaneous.

Answer 12

Ch. 9 - Prob. 1Q Ch. 9 - Prob. 2Q Ch. 9 - Prob. 3Q Ch. 9 - Prob. 4Q Ch. 9 - Prob. 5Q Ch. 9 - Prob. 6Q Ch. 9 - Prob. 7Q Ch. 9 - Prob. 1RQ Ch. 9 - Prob. 2RQ Ch. 9 - Prob. 3RQ

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Explanation of Solution

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