A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered. Concept introduction: The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation. The value of E cell is calculated using Nernst formula, E = E ° − ( R T n F ) ln ( Q ) At room temperature the above equation is specifies as, E = E ° − ( 0.0591 n ) log ( Q ) This relation is further used to determine the relation between Δ G ° and K , Δ G ° and E ° cell . The value of equilibrium constant helps to predict the extent of the reaction. To determine: The concentration of Ag + at the anode.

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Answer 1

Question

Chapter 17, Problem 84E

(a)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The concentration of Ag+ at the anode.

(b)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The value of equilibrium constant for the formation of Ag(S2O3)23− .

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Answer 2

Question

Chapter 17, Problem 84E

(a)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The concentration of Ag+ at the anode.

(b)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The value of equilibrium constant for the formation of Ag(S2O3)23− .

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 17, Problem 84E

(a)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The concentration of Ag+ at the anode.

(b)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The value of equilibrium constant for the formation of Ag(S2O3)23− .

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 17, Problem 84E

(a)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The concentration of Ag+ at the anode.

(b)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The value of equilibrium constant for the formation of Ag(S2O3)23− .

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 17, Problem 84E

(a)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The concentration of Ag+ at the anode.

(b)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The value of equilibrium constant for the formation of Ag(S2O3)23− .

Answer 6

Chapter 17, Problem 84E

(a)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The concentration of Ag+ at the anode.

Answer 7

Chapter 17, Problem 84E

(a)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The concentration of Ag+ at the anode.

Answer 8

(b)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The value of equilibrium constant for the formation of Ag(S2O3)23− .

Answer 9

(b)

Interpretation Introduction

Interpretation:

A concentration cell with silver electrode as cathode and anode with different concentrations of different ions is given. Various questions based on the given concentrations and cell potential are to be answered.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell . The value of equilibrium constant helps to predict the extent of the reaction.

To determine: The value of equilibrium constant for the formation of Ag(S2O3)23− .

Answer 10

Expert Solution & Answer

Answer 11

Expert Solution & Answer

Answer 12

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Answer 13

Ch. 17 - What is a half-reaction? Why must the number of...Ch. 17 - Galvanic cells harness spontaneous...Ch. 17 - Table 17-1 lists common half-reactions along with...Ch. 17 - Prob. 4RQ Ch. 17 - The Nernst equation allows determination of the...Ch. 17 - Prob. 6RQ Ch. 17 - Prob. 7RQ Ch. 17 - Prob. 8RQ Ch. 17 - What characterizes an electrolytic cell? What is...Ch. 17 - Sketch a galvanic cell, and explain how it works....

Solution Summary: The author explains how the Nernst equation calculates the cell potential and the standard reduction potential value. The equilibrium constant helps to predict the extent of the reaction.

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