(a) Interpretation: The sketch of the cell should be drawn that shows the anode and cathode, the sign of the electrodes and the direction of electrons and ion flow for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal. Concept introduction: In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as: E cell ° = E cathode ° - E anode ° E cell ° = E reduction ° - E oxidation ° The potential of cell can be calculated with the help of Nernst equation that can be shown as: E° = E° cell - 0 .0592 V n log Q n = number of electrons Q = reaction quotient

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Answer 1

Question

Chapter 19, Problem 19.132SP

Interpretation Introduction

(a)

Interpretation:

The sketch of the cell should be drawn that shows the anode and cathode, the sign of the electrodes and the direction of electrons and ion flow for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Interpretation Introduction

(b)

Interpretation:

The balance equation for anode, cathode and overall cell reaction for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal should be determined.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

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Answer 2

Question

Chapter 19, Problem 19.132SP

Interpretation Introduction

(a)

Interpretation:

The sketch of the cell should be drawn that shows the anode and cathode, the sign of the electrodes and the direction of electrons and ion flow for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Interpretation Introduction

(b)

Interpretation:

The balance equation for anode, cathode and overall cell reaction for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal should be determined.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

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Answer 3

Question

Chapter 19, Problem 19.132SP

Interpretation Introduction

(a)

Interpretation:

The sketch of the cell should be drawn that shows the anode and cathode, the sign of the electrodes and the direction of electrons and ion flow for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Interpretation Introduction

(b)

Interpretation:

The balance equation for anode, cathode and overall cell reaction for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal should be determined.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

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Answer 4

Question

Chapter 19, Problem 19.132SP

Interpretation Introduction

(a)

Interpretation:

The sketch of the cell should be drawn that shows the anode and cathode, the sign of the electrodes and the direction of electrons and ion flow for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Interpretation Introduction

(b)

Interpretation:

The balance equation for anode, cathode and overall cell reaction for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal should be determined.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

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Answer 5

Chapter 19, Problem 19.132SP

Interpretation Introduction

(a)

Interpretation:

The sketch of the cell should be drawn that shows the anode and cathode, the sign of the electrodes and the direction of electrons and ion flow for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Interpretation Introduction

(b)

Interpretation:

The balance equation for anode, cathode and overall cell reaction for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal should be determined.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Answer 6

Chapter 19, Problem 19.132SP

Interpretation Introduction

(a)

Interpretation:

The sketch of the cell should be drawn that shows the anode and cathode, the sign of the electrodes and the direction of electrons and ion flow for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Answer 7

Chapter 19, Problem 19.132SP

Interpretation Introduction

(a)

Interpretation:

The sketch of the cell should be drawn that shows the anode and cathode, the sign of the electrodes and the direction of electrons and ion flow for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Answer 8

Interpretation Introduction

(b)

Interpretation:

The balance equation for anode, cathode and overall cell reaction for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal should be determined.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Answer 9

Interpretation Introduction

(b)

Interpretation:

The balance equation for anode, cathode and overall cell reaction for the electrolysis of molten magnesium chloride using inter electrode to produce magnesium metal should be determined.

Concept introduction:

In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and combination of both half-reaction gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:

$Ecell° = Ecathode° - Eanode°Ecell° = Ereduction° - Eoxidation°$

The potential of cell can be calculated with the help of Nernst equation that can be shown as:

$E° = E°cell - 0.0592 Vn log Q n = number of electronsQ = reaction quotient$

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 19 - Balance the following net ionic equation by the...Ch. 19 - Balance the following net ionic equation by the...Ch. 19 - Prob. 19.3P Ch. 19 - Balance the following net ionic equation by the...Ch. 19 - Prob. 19.5P Ch. 19 - Prob. 19.6A Ch. 19 - PRACTICE 18.7 Write a balanced equation for the...Ch. 19 - Consider the following galvanic cell with...Ch. 19 - The standard cell potential at 25oC is 1.20 V for...Ch. 19 - The standard free-energy change is 59.8kJ for the...

Solution Summary: The author explains that the sketch of the electrochemical cell should be drawn that shows the anode and cathodes, the sign of electrodes, and the direction of electrons and ion flow.

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