Chapter 9, Problem 9.29EP

(a)

Interpretation Introduction

Interpretation:

The substances which act as reducing agent and oxidizing agent in the given redox reactions have to be identified.

${\text{N}}_{\text{2}}{\text{+3H}}_{\text{2}}\underset{}{\to }{\text{2NH}}_{\text{3}}$

Concept Introduction:

Redox reactions:

It is a type of reaction in which both oxidation and reduction happens simultaneously.  One gets oxidized and one gets reduced.

Example:

  ${\text{Zn(s)+2H}}^{\text{+}}\text{(aq)}\to {\text{Zn}}^{\text{2+}}{\text{(aq)+H}}_{\text{2}}\text{(g)}$

    Oxidation of Zinc increased by two and Hydrogen reduced by one;  $\text{Zn}$ is oxidized and hydrogen is reduced here.

Oxidizing agent:

Oxidizing agent will gain electrons but itself will get reduced in the reaction.  Oxygen, Hydrogen peroxide are good oxidizing agent.

Reducing agent:

A compound or an element donates electron in redox reactions.  Reducing agent will get oxidized in a reaction.

Lithium Aluminium Hydride and Sodium borohydride are good reducing agents.

(b)

Interpretation Introduction

Interpretation:

The substances which act as reducing agent and oxidizing agent in the given redox reactions has to be identified.

${\text{Cl}}_{\text{2}}\text{+2KI}\underset{}{\to }{\text{2KCl+I}}_{\text{2}}$

Concept Introduction:

Redox reactions:

Both reduction and oxidation will occur simultaneously in a redox reaction, one will get reduced and the other will get oxidized.

Example:

    ${\text{CuO+H}}_{\text{2}}\stackrel{}{\to }{\text{Cu+H}}_{\text{2}}\text{O}$

Here Cu is reduced and ${\text{H}}_{\text{2}}$ is oxidized.

Oxidizing agent:

The substance which accepts electrons in a redox reaction is known as oxidizing agent.

Hydrogen peroxide, oxygen are examples of oxidizing agent.

Reducing agent:

The substance which donates electrons in a redox reaction is known as reducing agent.

(c)

Interpretation Introduction

Interpretation:

The substances which act as reducing agent and oxidizing agent in the given redox reactions have to be identified.

${\text{Sb}}_{\text{2}}{\text{O}}_{\text{3}}\text{+3Fe}\stackrel{}{\to }\text{2Sb+3FeO}$

Concept Introduction:

Redox reactions:

It is a type of reaction in which both oxidation and reduction happens simultaneously.  One gets oxidized and one gets reduced.

Example:

  ${\text{Zn(s)+2H}}^{\text{+}}\text{(aq)}\to {\text{Zn}}^{\text{2+}}{\text{(aq)+H}}_{\text{2}}\text{(g)}$

    Oxidation of Zinc increased by two and Hydrogen reduced by one;  $\text{Zn}$ is oxidized and hydrogen is reduced here.

Oxidizing agent:

Oxidizing agent will gain electrons but itself will get reduced in the reaction.  Oxygen, Hydrogen peroxide are good oxidizing agent.

Reducing agent:

A compound or an element donates electron in a redox reactions.  Reducing agent will get oxidized in a reaction.

Lithium Aluminium Hydride and Sodium borohydride are good reducing agents.

(d)

Interpretation Introduction

Interpretation:

The substances which act as reducing agent and oxidizing agent in the given redox reaction has to be identified.

${\text{3H}}_{\text{2}}{\text{SO}}_{\text{3}}{\text{+2HNO}}_{\text{3}}\underset{}{\to }{\text{2NO+H}}_{\text{2}}{\text{O+3H}}_{\text{2}}{\text{SO}}_{\text{4}}$

Concept Introduction:

Redox reactions:

Both reduction and oxidation will occur simultaneously in a redox reaction, one will get reduced and the other will get oxidized.

Example:

    ${\text{CuO+H}}_{\text{2}}\stackrel{}{\to }{\text{Cu+H}}_{\text{2}}\text{O}$

Here Cu is reduced and ${\text{H}}_{\text{2}}$ is oxidized.

Oxidizing agent:

The substance which accepts electrons in a redox reaction is known as oxidizing agent.  Hydrogen peroxide, oxygen are examples of oxidizing agent.

Reducing agent:

The substance which donates electrons in a redox reaction is known as reducing agent.