An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered. Concept introduction: The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes. 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 ) To determine: The potential of the cell at 25 ° C if the copper electrode is placed in a given concentration of solution.

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Answer 1

Question

Chapter 17, Problem 79E

(a)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The potential of the cell at 25 °C if the copper electrode is placed in a given concentration of solution.

(b)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The value of concentration of Cu2+ at the given measured potential.

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Answer 2

Question

Chapter 17, Problem 79E

(a)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The potential of the cell at 25 °C if the copper electrode is placed in a given concentration of solution.

(b)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The value of concentration of Cu2+ at the given measured potential.

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Answer 3

Question

Chapter 17, Problem 79E

(a)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The potential of the cell at 25 °C if the copper electrode is placed in a given concentration of solution.

(b)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The value of concentration of Cu2+ at the given measured potential.

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Answer 4

Question

Chapter 17, Problem 79E

(a)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The potential of the cell at 25 °C if the copper electrode is placed in a given concentration of solution.

(b)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The value of concentration of Cu2+ at the given measured potential.

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Answer 5

Chapter 17, Problem 79E

(a)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The potential of the cell at 25 °C if the copper electrode is placed in a given concentration of solution.

(b)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The value of concentration of Cu2+ at the given measured potential.

Answer 6

Chapter 17, Problem 79E

(a)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The potential of the cell at 25 °C if the copper electrode is placed in a given concentration of solution.

Answer 7

Chapter 17, Problem 79E

(a)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The potential of the cell at 25 °C if the copper electrode is placed in a given concentration of solution.

Answer 8

(b)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The value of concentration of Cu2+ at the given measured potential.

Answer 9

(b)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

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)

To determine: The value of concentration of Cu2+ at the given measured potential.

Answer 10

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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....

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