Chapter 19, Problem 19.94QP

a)

Interpretation Introduction

Interpretation:

The strongest oxidizing agent and reducing agent has to be predicted.

Concept introduction:

Standard reduction potential: The voltage associated with a reduction reaction at an electrode when all solutes are 1M and all gases are at 1 atm. The hydrogen electrode is called the standard hydrogen electrode (SHE).

Oxidizing agent: An oxidizing agent gains electron from other species.

Reducing agent: A reducing agent donate electron to other species.

b)

Interpretation Introduction

Interpretation:

The substance that can be oxidized by ${\text{B}}_2$ has to be identified.

Concept introduction:

Standard reduction potential: The voltage associated with a reduction reaction at an electrode when all solutes are 1M and all gases are at 1 atm. The hydrogen electrode is called the standard hydrogen electrode (SHE).

Oxidizing agent: An oxidizing agent gains electron from other species.

Reducing agent: A reducing agent donate electron to other species.

c)

Interpretation Introduction

Interpretation:

The substance that can be reduced by ${\text{B}}^{-}$ has to be predicted.

Concept introduction:

Standard reduction potential: The voltage associated with a reduction reaction at an electrode when all solutes are 1M and all gases are at 1 atm. The hydrogen electrode is called the standard hydrogen electrode (SHE).

Oxidizing agent: An oxidizing agent gains electron from other species.

Reducing agent: A reducing agent donate electron to other species.

d)

Interpretation Introduction

Interpretation:

The overall equation for a cell that delivers a voltage of $2.59\text{V}$ under standard-state conditions has to be written.

Concept introduction:

Procedure for balancing redox equations:

Step 1: Write the unbalanced equation for the reaction in ionic form.

Step 2: Separate the equation into two half-reactions.

Step 3: Balance each half-reactions for number and type of atoms and charges. For reactions in an acidic medium, add ${\text{H}}_{\text{2}}\text{O}$ to balance the O-atoms and H⁺ to balance the H atoms.

Step 4: Add the two half-reactions together and balance the final equation. The equation must be atomically and electrically balanced. In case of different number of electrons, need to multiply one or both half-reactions to equalize the number of electrons.

Step 5: Finally, the number and type of atoms; charges on both sides of the equation must be same and balanced.