Chapter 9, Problem 9.30EP

(a)

Interpretation Introduction

Interpretation:

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

${\text{2Al + 3Cl}}_{\text{2}}\stackrel{}{\to }{\text{ 2AlCl}}_{\text{3}}$

Concept Introduction:

Redox reactions:

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

(b)

Interpretation Introduction

Interpretation:

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

${\text{Zn + CuCl}}_{\text{2}}\underset{}{\to }{\text{ ZnCl}}_2\text{ + Cu}$

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 reaction has to be identified.

${\text{2NiS + 3O}}_{\text{2}}\stackrel{}{\to }{\text{2NiO + 2SO}}_{\text{2}}$

Concept Introduction:

Redox reactions:

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

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

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.