The EMF of given voltaic cell should be calculated by using standard free energy changes of reactants and products. Concept introduction: Free energy change: In thermodynamics the cell potential is known as maximum work of the cell and it is equal to free energy change of the cell and it is given by, ΔG = -nFE cell Where, ΔG is free energy change n is number of electron transferred F is faraday constant E cell is cell potential Free energy change: The free energy change of a reaction is given by the subtraction of free energy changes of reactants from free energy changes of reactants. ΔG = ∑ nΔG f ° (products)- ∑ mΔG f ° (reactants)

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Answer 1

Question

Chapter 19, Problem 19.140QP

(a)

Interpretation Introduction

Interpretation:

The EMF of given voltaic cell should be calculated by using standard free energy changes of reactants and products.

Concept introduction:

Free energy change:

In thermodynamics the cell potential is known as maximum work of the cell and it is equal to free energy change of the cell and it is given by,

$ΔG = -nFEcell$

Where,

$ΔG is free energy changen is number of electron transferredF is faraday constantEcell is cell potential$

Free energy change:

The free energy change of a reaction is given by the subtraction of free energy changes of reactants from free energy changes of reactants.

$ΔG =∑nΔGf° (products)-∑mΔGf° (reactants)$

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant of given reaction should be calculated.

Concept introduction:

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

(c)

Interpretation Introduction

Interpretation:

The effect of concentration of $Fe(aq)2+$ ion on equilibrium constant should be explained.

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

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Answer 2

Question

Chapter 19, Problem 19.140QP

(a)

Interpretation Introduction

Interpretation:

The EMF of given voltaic cell should be calculated by using standard free energy changes of reactants and products.

Concept introduction:

Free energy change:

In thermodynamics the cell potential is known as maximum work of the cell and it is equal to free energy change of the cell and it is given by,

$ΔG = -nFEcell$

Where,

$ΔG is free energy changen is number of electron transferredF is faraday constantEcell is cell potential$

Free energy change:

The free energy change of a reaction is given by the subtraction of free energy changes of reactants from free energy changes of reactants.

$ΔG =∑nΔGf° (products)-∑mΔGf° (reactants)$

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant of given reaction should be calculated.

Concept introduction:

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

(c)

Interpretation Introduction

Interpretation:

The effect of concentration of $Fe(aq)2+$ ion on equilibrium constant should be explained.

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

Expert Solution & Answer

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Answer 3

Question

Chapter 19, Problem 19.140QP

(a)

Interpretation Introduction

Interpretation:

The EMF of given voltaic cell should be calculated by using standard free energy changes of reactants and products.

Concept introduction:

Free energy change:

In thermodynamics the cell potential is known as maximum work of the cell and it is equal to free energy change of the cell and it is given by,

$ΔG = -nFEcell$

Where,

$ΔG is free energy changen is number of electron transferredF is faraday constantEcell is cell potential$

Free energy change:

The free energy change of a reaction is given by the subtraction of free energy changes of reactants from free energy changes of reactants.

$ΔG =∑nΔGf° (products)-∑mΔGf° (reactants)$

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant of given reaction should be calculated.

Concept introduction:

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

(c)

Interpretation Introduction

Interpretation:

The effect of concentration of $Fe(aq)2+$ ion on equilibrium constant should be explained.

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

Expert Solution & Answer

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Answer 4

Question

Chapter 19, Problem 19.140QP

(a)

Interpretation Introduction

Interpretation:

The EMF of given voltaic cell should be calculated by using standard free energy changes of reactants and products.

Concept introduction:

Free energy change:

In thermodynamics the cell potential is known as maximum work of the cell and it is equal to free energy change of the cell and it is given by,

$ΔG = -nFEcell$

Where,

$ΔG is free energy changen is number of electron transferredF is faraday constantEcell is cell potential$

Free energy change:

The free energy change of a reaction is given by the subtraction of free energy changes of reactants from free energy changes of reactants.

$ΔG =∑nΔGf° (products)-∑mΔGf° (reactants)$

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant of given reaction should be calculated.

Concept introduction:

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

(c)

Interpretation Introduction

Interpretation:

The effect of concentration of $Fe(aq)2+$ ion on equilibrium constant should be explained.

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

Expert Solution & Answer

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Answer 5

Chapter 19, Problem 19.140QP

(a)

Interpretation Introduction

Interpretation:

The EMF of given voltaic cell should be calculated by using standard free energy changes of reactants and products.

Concept introduction:

Free energy change:

In thermodynamics the cell potential is known as maximum work of the cell and it is equal to free energy change of the cell and it is given by,

$ΔG = -nFEcell$

Where,

$ΔG is free energy changen is number of electron transferredF is faraday constantEcell is cell potential$

Free energy change:

The free energy change of a reaction is given by the subtraction of free energy changes of reactants from free energy changes of reactants.

$ΔG =∑nΔGf° (products)-∑mΔGf° (reactants)$

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant of given reaction should be calculated.

Concept introduction:

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

(c)

Interpretation Introduction

Interpretation:

The effect of concentration of $Fe(aq)2+$ ion on equilibrium constant should be explained.

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

Answer 6

Chapter 19, Problem 19.140QP

(a)

Interpretation Introduction

Interpretation:

The EMF of given voltaic cell should be calculated by using standard free energy changes of reactants and products.

Concept introduction:

Free energy change:

In thermodynamics the cell potential is known as maximum work of the cell and it is equal to free energy change of the cell and it is given by,

$ΔG = -nFEcell$

Where,

$ΔG is free energy changen is number of electron transferredF is faraday constantEcell is cell potential$

Free energy change:

The free energy change of a reaction is given by the subtraction of free energy changes of reactants from free energy changes of reactants.

$ΔG =∑nΔGf° (products)-∑mΔGf° (reactants)$

Answer 7

Chapter 19, Problem 19.140QP

(a)

Interpretation Introduction

Interpretation:

The EMF of given voltaic cell should be calculated by using standard free energy changes of reactants and products.

Concept introduction:

Free energy change:

In thermodynamics the cell potential is known as maximum work of the cell and it is equal to free energy change of the cell and it is given by,

$ΔG = -nFEcell$

Where,

$ΔG is free energy changen is number of electron transferredF is faraday constantEcell is cell potential$

Free energy change:

The free energy change of a reaction is given by the subtraction of free energy changes of reactants from free energy changes of reactants.

$ΔG =∑nΔGf° (products)-∑mΔGf° (reactants)$

Answer 8

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant of given reaction should be calculated.

Concept introduction:

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

Answer 9

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant of given reaction should be calculated.

Concept introduction:

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

Answer 10

(c)

Interpretation Introduction

Interpretation:

The effect of concentration of $Fe(aq)2+$ ion on equilibrium constant should be explained.

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

Answer 11

(c)

Interpretation Introduction

Interpretation:

The effect of concentration of $Fe(aq)2+$ ion on equilibrium constant should be explained.

Equilibrium constant $Kc$ :

The relationship between equilibrium constant and cell potential (EMF) is given by below equation

$Ecell= 0.0592nFlog Kc$

Where,

$Kc is equilibrium constantn is number of electron transferredF is faraday constantEcell is cell potential$

Answer 12

Expert Solution & Answer

Answer 13

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Answer 14

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Answer 15

Ch. 19.1 - Iodic acid, HIO3, can be prepared by reading...Ch. 19.1 - Balance the following equation using the...Ch. 19.2 - A voltaic cell consists of a silversilver ion...Ch. 19.2 - If you were to construct a wet cell and decided to...Ch. 19.3 - Prob. 19.4E Ch. 19.3 - Prob. 19.5E Ch. 19.4 - What is the maximum electrical work, that can be...Ch. 19.5 - Prob. 19.7E Ch. 19.5 - Prob. 19.8E Ch. 19.5 - Prob. 19.9E

Solution Summary: The author explains that the EMF of a given voltaic cell should be calculated by using standard free energy changes of reactants and products.

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