(a) Interpretation: The value of E cell for the reaction should be calculated. Concept introduction: The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows: [ H + ] × [ OH − ] = 1.0 × 10 − 14 In an electrochemical cell, there are two electrodes that can be observed. If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized. If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced. The electrode potential of cell can be calculated as follows: E 0 cell = E 0 cathode − E 0 anode Nernst equation for a cell can be represented as follows: E c e l l = E 0 c e l l − 0.0592 V z log Q Here, z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

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Answer 1

Question

Chapter 19, Problem 43E

Interpretation Introduction

(a)

Interpretation:

The value of Ecell for the reaction should be calculated.

Concept introduction:

The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows:

[H+]× [OH−] = 1.0 ×10−14

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Interpretation Introduction

(b)

Interpretation:

The Ecell value from the previous subpart should be compared with the E⁰ for the reduction of water to H₂(g) in basic solution, and the relationships between them should be explained.

Concept introduction:

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

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Answer 2

Question

Chapter 19, Problem 43E

Interpretation Introduction

(a)

Interpretation:

The value of Ecell for the reaction should be calculated.

Concept introduction:

The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows:

[H+]× [OH−] = 1.0 ×10−14

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Interpretation Introduction

(b)

Interpretation:

The Ecell value from the previous subpart should be compared with the E⁰ for the reduction of water to H₂(g) in basic solution, and the relationships between them should be explained.

Concept introduction:

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

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Answer 3

Question

Chapter 19, Problem 43E

Interpretation Introduction

(a)

Interpretation:

The value of Ecell for the reaction should be calculated.

Concept introduction:

The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows:

[H+]× [OH−] = 1.0 ×10−14

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Interpretation Introduction

(b)

Interpretation:

The Ecell value from the previous subpart should be compared with the E⁰ for the reduction of water to H₂(g) in basic solution, and the relationships between them should be explained.

Concept introduction:

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

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Answer 4

Question

Chapter 19, Problem 43E

Interpretation Introduction

(a)

Interpretation:

The value of Ecell for the reaction should be calculated.

Concept introduction:

The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows:

[H+]× [OH−] = 1.0 ×10−14

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Interpretation Introduction

(b)

Interpretation:

The Ecell value from the previous subpart should be compared with the E⁰ for the reduction of water to H₂(g) in basic solution, and the relationships between them should be explained.

Concept introduction:

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

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Answer 5

Chapter 19, Problem 43E

Interpretation Introduction

(a)

Interpretation:

The value of Ecell for the reaction should be calculated.

Concept introduction:

The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows:

[H+]× [OH−] = 1.0 ×10−14

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Interpretation Introduction

(b)

Interpretation:

The Ecell value from the previous subpart should be compared with the E⁰ for the reduction of water to H₂(g) in basic solution, and the relationships between them should be explained.

Concept introduction:

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Answer 6

Chapter 19, Problem 43E

Interpretation Introduction

(a)

Interpretation:

The value of Ecell for the reaction should be calculated.

Concept introduction:

The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows:

[H+]× [OH−] = 1.0 ×10−14

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Answer 7

Chapter 19, Problem 43E

Interpretation Introduction

(a)

Interpretation:

The value of Ecell for the reaction should be calculated.

Concept introduction:

The relation between hydrogen ion concentration and hydroxide ion concentration is represented as follows:

[H+]× [OH−] = 1.0 ×10−14

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Answer 8

Interpretation Introduction

(b)

Interpretation:

The Ecell value from the previous subpart should be compared with the E⁰ for the reduction of water to H₂(g) in basic solution, and the relationships between them should be explained.

Concept introduction:

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Answer 9

Interpretation Introduction

(b)

Interpretation:

The Ecell value from the previous subpart should be compared with the E⁰ for the reduction of water to H₂(g) in basic solution, and the relationships between them should be explained.

Concept introduction:

In an electrochemical cell, there are two electrodes that can be observed.

If oxidation takes place on an electrode, that electrode is called anode. The species in that electrode remove electrons and itself gets oxidized.

If reduction takes place on an electrode, that electrode is called cathode. The species in that electrode absorbs electrons and itself gets reduced.

The electrode potential of cell can be calculated as follows:

E0cell= E0cathode − E0anode

Nernst equation for a cell can be represented as follows:

Ecell=E0cell−0.0592 Vz log Q

Here,

z = number of moles of electrons transferred in the cell and Q is ratio of concentration of products to reactant in a cell.

Answer 10

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Answer 11

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Answer 12

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Answer 13

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Solution Summary: The author explains how the value of E_cell for the reaction should be calculated.

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