(a) Interpretation: Whether the given reaction completes or not needs to be determined. 2Cu + (aq) + Sn 4+ ( aq) → 2 Cu 2+ ( aq) + Sn 2+ ( aq) Concept introduction: The E° c e l l value for a redox reaction gives by following equation. E ° c e l l = E ° R e d u c t i o n − E ° O x i d a t i o n When the reactants and products are in their standard states, Δ r G ∘ = − z F E c e l l ∘ Where, z = Electron number F = Faraday constant = 96 , 485 C mol − 1 E c e l l ∘ = Standard Electron cell potential The electron number, z, for a reaction depends on how the reaction is written. Also, Δ r G ∘ = − RT ln K − RT ln K = − z F E c e l l ∘ ∴ ln K = − z F E c e l l ∘ − R T ln K = 11604 C J -1 z E c e l l ∘ T K = e 11604 C J -1 z E c e l l ∘ T

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Answer 1

Question

Chapter 19, Problem 29E

Interpretation Introduction

(a)

Interpretation:

Whether the given reaction completes or not needs to be determined. 2Cu+(aq)+Sn4+(aq)→2Cu2+(aq)+Sn2+(aq)

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Interpretation Introduction

(b)

Interpretation:

The direction in which the reaction completes needs to be determined.

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

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Answer 2

Question

Chapter 19, Problem 29E

Interpretation Introduction

(a)

Interpretation:

Whether the given reaction completes or not needs to be determined. 2Cu+(aq)+Sn4+(aq)→2Cu2+(aq)+Sn2+(aq)

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Interpretation Introduction

(b)

Interpretation:

The direction in which the reaction completes needs to be determined.

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

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Answer 3

Question

Chapter 19, Problem 29E

Interpretation Introduction

(a)

Interpretation:

Whether the given reaction completes or not needs to be determined. 2Cu+(aq)+Sn4+(aq)→2Cu2+(aq)+Sn2+(aq)

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Interpretation Introduction

(b)

Interpretation:

The direction in which the reaction completes needs to be determined.

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

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Answer 4

Question

Chapter 19, Problem 29E

Interpretation Introduction

(a)

Interpretation:

Whether the given reaction completes or not needs to be determined. 2Cu+(aq)+Sn4+(aq)→2Cu2+(aq)+Sn2+(aq)

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Interpretation Introduction

(b)

Interpretation:

The direction in which the reaction completes needs to be determined.

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

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See solution

Answer 5

Chapter 19, Problem 29E

Interpretation Introduction

(a)

Interpretation:

Whether the given reaction completes or not needs to be determined. 2Cu+(aq)+Sn4+(aq)→2Cu2+(aq)+Sn2+(aq)

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Interpretation Introduction

(b)

Interpretation:

The direction in which the reaction completes needs to be determined.

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Answer 6

Chapter 19, Problem 29E

Interpretation Introduction

(a)

Interpretation:

Whether the given reaction completes or not needs to be determined. 2Cu+(aq)+Sn4+(aq)→2Cu2+(aq)+Sn2+(aq)

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Answer 7

Chapter 19, Problem 29E

Interpretation Introduction

(a)

Interpretation:

Whether the given reaction completes or not needs to be determined. 2Cu+(aq)+Sn4+(aq)→2Cu2+(aq)+Sn2+(aq)

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Answer 8

Interpretation Introduction

(b)

Interpretation:

The direction in which the reaction completes needs to be determined.

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Answer 9

Interpretation Introduction

(b)

Interpretation:

The direction in which the reaction completes needs to be determined.

Concept introduction:

The E°_c_e_l_l value for a redox reaction gives by following equation.

E°cell=E°Reduction−E°Oxidation

When the reactants and products are in their standard states,

ΔrG∘=−zFEcell∘Where,z= Electron numberF=Faraday constant=96,485 C mol−1Ecell∘=Standard Electron cell potential

The electron number, z, for a reaction depends on how the reaction is written.

Also,

ΔrG∘=−RTlnK−RTlnK=−zFEcell∘∴lnK=−zFE cell∘−RTlnK=11604 C J-1zE cell∘TK=e11604 C J -1 z E cell ∘ T

Answer 10

Expert Solution & Answer

Answer 11

Expert Solution & Answer

Answer 12

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Answer 13

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Solution Summary: The author explains that the E° c e l value for a redox reaction depends on how the reaction is written.

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