Chapter 19, Problem 19.61QP

(a)

Interpretation Introduction

Interpretation:

For each of the given redox reactions, the half-cell reactions, the completely balanced cell reaction and the direction of spontaneous reactions has to be found.

Concept Introduction:

Redox reactions are the reactions in which both oxidation and reduction takes place simultaneously.  Oxidation is the removal electron from an atom or ion.  Oxidation process increases the oxidation number.  Reduction is the addition of electron to an atom or ion.  Reduction process decreases the oxidation number.  The electrochemical reaction of zinc with copper sulphate is an example of redox reaction.

  ${\text{Zn}}_{\text{(s)}}{\text{+ CuSO}}_{\text{4}}{}_{\text{(aq)}}\to {\text{ZnSO}}_{\text{4}}{\text{+ Cu}}_{\text{(s)}}$

Standard reduction potential is the measure of the tendency of a species to undergo reduction.  It is measured in terms of volts.  The substance which is having high positive value will easily undergo reduction.

The standard electrode potential of a cell${\text{(E}}^{°}{}_{\text{cell}})$ is the difference in electrode potential of the cathode and anode.

  ${\text{E}}^{\text{°}}{}_{\text{cell}}={\text{E}}^{\text{°}}{}_{\text{cathode}}-{\text{E}}^{\text{°}}{}_{\text{anode}}$

The relation between Gibbs free energy and cell potential: The amount of energy in a system that can be converted into useful energy is defined as free energy in thermodynamics. 

Free energy and the cell potential is related by the given equation.

  $\text{ΔG=-nFE}$

Where,

  $\text{ΔG}$ is the change in free energy

  $\text{n}$ is the number of electrons transferred

  $\text{F}$ is the Faraday constant $\text{(F}=\text{96485}{\text{.338Cmol}}^{\text{-1}})$

  $\text{E}$ is the cell potential

(b)

Interpretation Introduction

Interpretation:

For each of the given redox reactions, the half-cell reactions, the completely balanced cell reaction and the direction of spontaneous reactions has to be found.

Concept Introduction:

Redox reactions are the reactions in which both oxidation and reduction takes place simultaneously.  Oxidation is the removal electron from an atom or ion.  Oxidation process increases the oxidation number.  Reduction is the addition of electron to an atom or ion.  Reduction process decreases the oxidation number.  The electrochemical reaction of zinc with copper sulphate is an example of redox reaction.

  ${\text{Zn}}_{\text{(s)}}{\text{+ CuSO}}_{\text{4}}{}_{\text{(aq)}}\to {\text{ZnSO}}_{\text{4}}{\text{+ Cu}}_{\text{(s)}}$

Standard reduction potential is the measure of the tendency of a species to undergo reduction.  It is measured in terms of volts.  The substance which is having high positive value will easily undergo reduction.

The standard electrode potential of a cell${\text{(E}}^{°}{}_{\text{cell}})$ is the difference in electrode potential of the cathode and anode.

  ${\text{E}}^{\text{°}}{}_{\text{cell}}={\text{E}}^{\text{°}}{}_{\text{cathode}}-{\text{E}}^{\text{°}}{}_{\text{anode}}$

The relation between Gibbs free energy and cell potential: The amount of energy in a system that can be converted into useful energy is defined as free energy in thermodynamics. 

Free energy and the cell potential is related by the given equation.

  $\text{ΔG=-nFE}$

Where,

  $\text{ΔG}$ is the change in free energy

  $\text{n}$ is the number of electrons transferred

  $\text{F}$ is the Faraday constant $\text{(F}=\text{96485}{\text{.338Cmol}}^{\text{-1}})$

  $\text{E}$ is the cell potential

(c)

Interpretation Introduction

Interpretation:

For each of the given redox reactions, the half-cell reactions, the completely balanced cell reaction and the direction of spontaneous reactions has to be found.

Concept Introduction:

Redox reactions are the reactions in which both oxidation and reduction takes place simultaneously.  Oxidation is the removal electron from an atom or ion.  Oxidation process increases the oxidation number.  Reduction is the addition of electron to an atom or ion.  Reduction process decreases the oxidation number.  The electrochemical reaction of zinc with copper sulphate is an example of redox reaction.

  ${\text{Zn}}_{\text{(s)}}{\text{+ CuSO}}_{\text{4}}{}_{\text{(aq)}}\to {\text{ZnSO}}_{\text{4}}{\text{+ Cu}}_{\text{(s)}}$

Standard reduction potential is the measure of the tendency of a species to undergo reduction.  It is measured in terms of volts.  The substance which is having high positive value will easily undergo reduction.

The standard electrode potential of a cell${\text{(E}}^{°}{}_{\text{cell}})$ is the difference in electrode potential of the cathode and anode.

  ${\text{E}}^{\text{°}}{}_{\text{cell}}={\text{E}}^{\text{°}}{}_{\text{cathode}}-{\text{E}}^{\text{°}}{}_{\text{anode}}$

The relation between Gibbs free energy and cell potential: The amount of energy in a system that can be converted into useful energy is defined as free energy in thermodynamics. 

Free energy and the cell potential is related by the given equation.

  $\text{ΔG=-nFE}$

Where,

  $\text{ΔG}$ is the change in free energy

  $\text{n}$ is the number of electrons transferred

  $\text{F}$ is the Faraday constant $\text{(F}=\text{96485}{\text{.338Cmol}}^{\text{-1}})$

  $\text{E}$ is the cell potential