   Chapter 18, Problem 59E

Chapter
Section
Textbook Problem

# Answer the following questions using data from Table 17-1 (all under standard conditions).a. Is H+(aq) capable of oxidizing Cu(s) to Cu2+(aq)?b. Is Fe3+ (aq) capable of oxidizing I− (aq)?c. Is H2(g) capable of reducing Ag+(aq)?

(a)

Interpretation Introduction

Interpretation:

Various questions on the oxidizing and reducing tendency of species based on their reduction potential are to be answered.

Concept introduction:

The species with higher reduction potential undergoes reduction at the cathode while the species with lower reduction potential undergoes oxidation at the anode. The change in Gibbs free energy is the useful amount work that can be done and negative value of ΔG° shows that the reaction is spontaneous in nature.

To determine: The ability of H+(aq) to oxidize Cu(s) to Cu2+(aq)

Explanation

Due to negative value of E°cell it is not possible for H+(aq) to oxidize Cu(s) to Cu2+(aq)

The reaction taking place at cathode is,

2H+(aq)+2eH2(g)E°red=0.00V

The reaction taking place at anode is,

Cu(s)Cu2+(aq)+2eE°ox=0.34V

The overall cell potential is calculated as,

E°cell=E°ox+E°red=0

(b)

Interpretation Introduction

Interpretation:

Various questions on the oxidizing and reducing tendency of species based on their reduction potential are to be answered.

Concept introduction:

The species with higher reduction potential undergoes reduction at the cathode while the species with lower reduction potential undergoes oxidation at the anode. The change in Gibbs free energy is the useful amount work that can be done and negative value of ΔG° shows that the reaction is spontaneous in nature.

To determine: The ability of Fe3+(aq) to oxidize I(aq) .

(c)

Interpretation Introduction

Interpretation:

Various questions on the oxidizing and reducing tendency of species based on their reduction potential are to be answered.

Concept introduction:

The species with higher reduction potential undergoes reduction at the cathode while the species with lower reduction potential undergoes oxidation at the anode. The change in Gibbs free energy is the useful amount work that can be done and negative value of ΔG° shows that the reaction is spontaneous in nature.

To determine: The ability of H2(g) to reduce Ag+(aq) .

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