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Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

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BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 14, Problem 10E
Textbook Problem
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Name some common oxidizing and reducing agents, and explain their reactions.

Interpretation Introduction

Interpretation:

The most common oxidizing agents and reducing agents, along with their respective reactions, are to be discussed.

Concept Introduction:

Oxidation is the addition of an electronegative element and the removal of an electropositive element in a chemical reaction.

Reduction is the addition of an electropositive element and the removal of an electronegative element in a chemical reaction.

A chemical reaction in which oxidation process and reduction process takes place simultaneously is called a redox reaction.

An oxidizing agent is a substance that has the capacity to oxidize another substance, and to get reduced, in a chemical reaction.

A reducing agent is a substance that has the capacity to reduce another substance, and to get oxidized, in a chemical reaction.

Explanation of Solution

An oxidizing agent is a substance that tends to gain electrons in a redox reaction. It oxidizes the other substance and gets reduced in a redox reaction. It is also known as the electron acceptor and the oxidation state increases. The most common oxidizing agents are oxygen, chlorine, iodine and hydrogen peroxide. Chlorine is used as an oxidizing agent for the production of bleaching powder. It is also used as anantiseptic.

The equation for the reaction of Cl2 with Ca(OH)2 is as follow:

Cl2+Ca(OH)2Ca(OCl)Cl+H2O.

An oxidizing agent gains electron easily while a reducing agent loses electrons easily in a redox reaction.

Cl20+Ca+2(O2H+1)2Ca+2(O2Cl+1)Cl1+H2+1O2.

In this chemical reaction, the oxidation state of Cl2 is increased from 0 to +1, which is accompanied by the loss of electrons. Therefore, Cl2 is the reducing agent.

Oxygen is used as an oxidizing agent for the oxidation of sugar in respiration.

The chemical equation for the respiration reaction is as follow:

C6H12O6+6O26CO2+6H2O

An oxidizing agent gains electron easily while a reducing agent loses electrons easily in a redox reaction.

C60H12+1O62+6O206C+4O22+6H2+1O2

In this chemical reaction, the oxidation state of C6H12O6 is increased from 0 to +4, which is accompanied by the loss of electrons. Therefore, C6H12O6 is the reducing agent.

In this chemical reaction, the oxidation state of O2 is reduced from 0 to 2, which is accompanied by the gain of electrons. Therefore, O2 is the oxidizing agent.

A reducing agent is a substance that tends to lose electrons in an oxidation-reduction reaction. It reduces the other substance and gets oxidized in a redox reaction. It is also known as the electron donor and the oxidation state of the substances decreases.

The common reducing agents are hydrogen, carbon monoxide and carbon.

Hydrogen is used as a reducing agent. It is used for the reduction of nitrogen into ammonia as follow:

N2+3H22NH3

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Chapter 14 Solutions

Chemistry In Focus
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Ch. 14 - Can an oxidation reaction occur without a...Ch. 14 - Why is carbon oxidized in the following reaction...Ch. 14 - Why is bromine reduced in the following reaction...Ch. 14 - What is an oxidizing agent? A reducing agent?Ch. 14 - Name some common oxidizing and reducing agents,...Ch. 14 - Write equations for respiration and...Ch. 14 - Explain how an electrochemical cell works. Include...Ch. 14 - Use chemical equations to explain how an...Ch. 14 - Use chemical equations to describe a Leclanch dry...Ch. 14 - What is a fuel cell? How is it different from a...Ch. 14 - Give a thermodynamic argument for why it is more...Ch. 14 - Use chemical equations to explain how the...Ch. 14 - Use chemical equations to explain how the molten...Ch. 14 - Explain with the help of chemical equations why...Ch. 14 - Explain how each of the following helps prevent...Ch. 14 - How might aging and oxidation be related?Ch. 14 - What are free radicals, and how might they affect...Ch. 14 - What are the chemical similarities among the...Ch. 14 - What are the chemical similarities among the...Ch. 14 - Draw Lewis structures for each chemical reaction,...Ch. 14 - Draw Lewis structures for each chemical reaction,...Ch. 14 - For each reaction, indicate which elements are...Ch. 14 - For each reaction, indicate which elements are...Ch. 14 - For each reaction, indicate which elements are...Ch. 14 - For each reaction, indicate which elements are...Ch. 14 - For each reaction, identify the oxidizing agent...Ch. 14 - For each reaction, identify the oxidizing agent...Ch. 14 - Identify the oxidizing agent and the reducing...Ch. 14 - Identify the oxidizing agent and the reducing...Ch. 14 - Which would you expect to be a better oxidizing...Ch. 14 - Which would you expect to be a better reducing...Ch. 14 - Sum each of the following oxidation and reduction...Ch. 14 - Sum each of the following oxidation and reduction...Ch. 14 - A chemist attempts to protect two pieces of iron...Ch. 14 - A friend tells you that a health-related website...Ch. 14 - Which of the following factors might affect the...Ch. 14 - An engineer suggests using a plastic can instead...Ch. 14 - A molten carbonate fuel cell (MCFC) costs...Ch. 14 - Fossil fuel, nuclear, and hydroelectric power...Ch. 14 - The following diagram shows an electrochemical...Ch. 14 - The following diagram shows a molecular view of...

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