Chapter 19, Problem 19.35CP

Interpretation Introduction

(a)

Interpretation:

The strongest oxidizing agent and reducing agent should be chosen from the given reactions.

Concept introduction:

The standard reduction potential is the tendency of a chemical species to be reduced at standard conditions. The standard conditions are the temperature at $298\text{ K}$, $1\text{ M}$ concentration for each ion in the reaction and partial pressure of $1\text{ atm}$ for each gas present.

Interpretation Introduction

(b)

Interpretation:

Which substances can be oxidized by ${\text{B}}^{2+}$ and which can be reduced by $\text{D}$ should be determined.

Concept introduction:

The standard reduction potential is the tendency of a chemical species to be reduced at standard conditions. The standard conditions are the temperature at $298\text{ K}$, $1\text{ M}$ concentration for each ion in the reaction and partial pressure of $1\text{ atm}$ for each gas present.

Interpretation Introduction

(c)

Interpretation:

A balanced equation for the overall cell reaction needs to be determined.

Concept introduction:

The standard reduction potential is the tendency of a chemical species to be reduced at standard conditions. The standard conditions are the temperature at $298\text{ K}$, $1\text{ M}$ concentration for each ion in the reaction and partial pressure of $1\text{ atm}$ for each gas present.

The standard cell potential of the overall reaction is given by the sum of the standard half-cell potentials for oxidation and reduction.

${\text{E}}_{overall}^0={\text{E}}_{ox}^0+{\text{ E}}_{red}^0$