Chapter 4, Problem 4.94P

(a)

Interpretation Introduction

Interpretation:

The oxidizing agent and the reducing agent in the following reaction are to be determined.

${\text{8H}}^{+}\left(aq\right)+6{\text{Cl}}^{-}\left(aq\right)+\text{Sn}\left(s\right)+4{\text{NO}}_3^{-}\left(aq\right)\to {\text{SnCl}}_6^{2-}\left(aq\right)+4{\text{NO}}_2\left(g\right)+4{\text{H}}_2\text{O}\left(l\right)$

Concept introduction:

A redox reaction is a type of reaction that involves the change in oxidation number of a molecule, atom or ion changes due to the transfer of an electron from one species to another.

An oxidizing agent is a substance that oxidizes another species and itself gets reduced in a chemical reaction. A reducing agent is the one that reduces another species and itself gets oxidized in a chemical reaction.

(b)

Interpretation Introduction

Interpretation:

The oxidizing agent and the reducing agent in the following reaction are to be determined.

${\text{2MnO}}_4^{-}\left(aq\right)+10{\text{Cl}}^{-}\left(aq\right)+{\text{16H}}^{+}\left(aq\right)\to 5{\text{Cl}}_2\left(aq\right)+{\text{2Mn}}^{2+}\left(g\right)+8{\text{H}}_2\text{O}\left(l\right)$

Concept introduction:

A redox reaction is a type of reaction that involves the change in oxidation number of a molecule, atom or ion changes due to the transfer of an electron from one species to another.

An oxidizing agent is a substance that oxidizes another species and itself gets reduced in a chemical reaction. A reducing agent is the one that reduces another species and itself gets oxidized in a chemical reaction.