Chapter 14, Problem 10E

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.

Answer to Problem 10E

Solution:

The most common oxidizing agents are oxygen, chlorine and hydrogen peroxide. Oxygen is used as an oxidizing agent in redox reactions, such as the combustion of gasoline in automobiles and the burning of wood in the presence of fire. Chlorine is used as an oxidizing agent in the formation of bleaching powder, which is used as a disinfectant in drinking water.

The most common reducing agents are carbon, hydrogen and carbon monoxide. Hydrogen is used as a reducing agent in the reduction of nitrogen into ammonia. Carbon is a reducing agent; it is used in the reduction of metal ores into their respective metals. Carbon monoxide is a reducing agent. It is used in the reduction of iron oxide into iron.

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 ${\text{Cl}}_2$ with $\text{Ca}{\left(\text{OH}\right)}_2$ is as follow:

${\text{Cl}}_2+\text{Ca}{\left(\text{OH}\right)}_2\to \text{Ca}\left(\text{OCl}\right)\text{Cl}+{\text{H}}_2\text{O}$.

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

$\underset{0}{{\text{Cl}}_2}+\underset{+2}{\text{Ca}}{\left(\underset{-2}{\text{O}}\underset{+1}{\text{H}}\right)}_2\to \underset{+2}{\text{Ca}}\left(\underset{-2}{\text{O}}\underset{+1}{\text{Cl}}\right)\underset{-1}{\text{Cl}}+\underset{+1}{{\text{H}}_2}\underset{-2}{\text{O}}$.

In this chemical reaction, the oxidation state of ${\text{Cl}}_2$ is increased from $0$ to $+1$, which is accompanied by the loss of electrons. Therefore, ${\text{Cl}}_2$ 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:

${\text{C}}_6{\text{H}}_{12}{\text{O}}_6+6{\text{O}}_2\to 6{\text{CO}}_2+6{\text{H}}_2\text{O}$

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

$\underset{0}{{\text{C}}_6}\underset{+1}{{\text{H}}_{12}}\underset{-2}{{\text{O}}_6}+6\underset{0}{{\text{O}}_2}\to 6\underset{+4}{\text{C}}\underset{-2}{{\text{O}}_2}+6\underset{+1}{{\text{H}}_2}\underset{-2}{\text{O}}$

In this chemical reaction, the oxidation state of ${\text{C}}_6{\text{H}}_{12}{\text{O}}_6$ is increased from $0$ to $+4$, which is accompanied by the loss of electrons. Therefore, ${\text{C}}_6{\text{H}}_{12}{\text{O}}_6$ is the reducing agent.

In this chemical reaction, the oxidation state of ${\text{O}}_2$ is reduced from $0$ to $-2$, which is accompanied by the gain of electrons. Therefore, ${\text{O}}_2$ 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:

${\text{N}}_2+3{\text{H}}_2\to 2{\text{NH}}_3$.

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

$\underset{0}{{\text{N}}_2}+\underset{0}{3{\text{H}}_2}\to 2\underset{-3}{\text{N}}\underset{+1}{{\text{H}}_3}$

In this chemical reaction, the oxidation state of ${\text{H}}_2$ is increased from $0$ to $+1$, which is accompanied by the loss of electrons. Therefore, ${\text{H}}_2$ is oxidized.

In this chemical reaction, the oxidation state of ${\text{N}}_2$ is reduced from $0$ to $-1$, which is accompanied by the gain of electrons. Therefore, ${\text{N}}_2$ is reduced.

Carbon monoxide is used as a reducing agent. It is used for the reduction of iron ore into iron.

The equation for the reaction of ${\text{Fe}}_{\text{2}}{\text{O}}_3$ with $\text{CO}$ is as follow:

${\text{4Fe}}_2{\text{O}}_3+\text{CO}\to 2\text{Fe}+3{\text{CO}}_2$

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

$\text{4}\underset{+3}{{\text{Fe}}_2}\underset{-2}{{\text{O}}_3}+\underset{+2}{\text{C}}\underset{-2}{\text{O}}\to 2\underset{0}{\text{Fe}}+3\underset{+4}{\text{C}}\underset{-2}{{\text{O}}_2}$

In this chemical reaction, the oxidation state of $\text{CO}$ is increased from $+2$ to $+4$, which is accompanied by the loss of electrons. Therefore, $\text{CO}$ is the reducing agent.

In this chemical reaction, the oxidation state of ${\text{Fe}}_2{\text{O}}_3$ is reduced from $+3$ to $0$, which is accompanied by the gain of electrons. Therefore, ${\text{Fe}}_2{\text{O}}_3$ is the oxidizing agent.

Carbon is used as a reducing agent. It is used for the reduction of nickel oxide into nickel.

The equation for the reaction of $\text{NiO}$ with $\text{C}$ is as follow:

$\text{NiO}+\text{C}\to \text{Ni}+\text{}\text{CO}$.

Oxidation is the loss of electrons and gain of oxygen in a chemical reaction. Reduction is the gain of electrons and loss of oxygen in a chemical reaction.

$\underset{+2}{\text{Ni}}\underset{-2}{\text{O}}+\underset{0}{\text{C}}\to \underset{0}{\text{Ni}}+\text{}\underset{+2}{\text{C}}\underset{-2}{\text{O}}$

In this chemical reaction, the oxidation state of $\text{C}$ is increased from 0 to $+2$, which is accompanied by the gain of oxygen. Therefore, $\text{C}$ is oxidized.

In this chemical reaction, the oxidation state of $\text{Ni}$ is reduced from $+2$ to $0$, which is accompanied the loss of oxygen. Therefore, $\text{Ni}$ is reduced.

Conclusion

Oxygen, chlorine and hydrogen peroxide are the most common oxidizing agents, whereas the most common reducing agents are hydrogen, carbon monoxide and carbon.