Chapter 5, Problem 78IAE

Interpretation Introduction

(a)

Interpretation:

The redox reaction given below carried out in an acidic medium needs to be balanced

${\text{Fe}}_{\text{2}}{\text{S}}_{\text{3}}{\text{ + H}}_{\text{2}}{\text{O + O}}_{\text{2}}\to {\text{Fe(OH)}}_{\text{3}}\text{ + S}$

Concept introduction:

• Redox reactions are chemical reactions that are expressed in terms of reduction and oxidation half reactions. They involve transfer of electrons between two species
• Oxidation reaction involves loss of electrons by one of the reactants whereas reduction is accompanied by gain of electrons by the other reactant.

Interpretation Introduction

(b)

Interpretation:

The redox reaction given below carried out in an acidic medium needs to be balanced

${\text{O}}_2^{-}{\text{ + H}}_{\text{2}}\text{O }\to {\text{OH}}^{-}{\text{ + O}}_{\text{2}}$

Concept introduction:

• Redox reactions are chemical reactions that are expressed in terms of reduction and oxidation half reactions. They involve transfer of electrons between two species
• Oxidation reaction involves loss of electrons by one of the reactants whereas reduction is accompanied by gain of electrons by the other reactant.

Interpretation Introduction

(c)

Interpretation:

The redox reaction given below carried out in an acidic medium needs to be balanced

${\text{CrI}}_{\text{3 }}{\text{+ H}}_{\text{2}}{\text{O}}_{\text{2}}\to {\text{ CrO}}_{\text{4}}^{\text{2-}}{\text{ + IO}}_{\text{4}}^{\text{-}}{\text{ + H}}_{\text{2}}\text{O}$

Concept introduction:

• Redox reactions are chemical reactions that are expressed in terms of reduction and oxidation half reactions. They involve transfer of electrons between two species
• Oxidation reaction involves loss of electrons by one of the reactants whereas reduction is accompanied by gain of electrons by the other reactant.

Interpretation Introduction

(d)

Interpretation:

The redox reaction given below carried out in an acidic medium needs to be balanced

${\text{Ag + CN}}^{-}{\text{ + O}}_{\text{2}}{\text{ + OH}}^{-}\to {\text{ [Ag(CN)}}_2{\text{]}}^{-}{\text{ + H}}_{\text{2}}\text{O}$

Concept introduction:

• Redox reactions are chemical reactions that are expressed in terms of reduction and oxidation half reactions. They involve transfer of electrons between two species
• Oxidation reaction involves loss of electrons by one of the reactants whereas reduction is accompanied by gain of electrons by the other reactant.

Interpretation Introduction

(e)

Interpretation:

The redox reaction given below carried out in an acidic medium needs to be balanced

${\text{B}}_{\text{2}}{\text{Cl}}_4{\text{ + OH}}^{-}\to {\text{ BO}}_{\text{2}}^{-}{\text{ + Cl}}^{-}{\text{ + H}}_{\text{2}}{\text{O + H}}_{\text{2}}$

Concept introduction:

• Redox reactions are chemical reactions that are expressed in terms of reduction and oxidation half reactions. They involve transfer of electrons between two species
• Oxidation reaction involves loss of electrons by one of the reactants whereas reduction is accompanied by gain of electrons by the other reactant.