For given ΔG o value at 25 ∘ C the standard cell potential for the given reaction has to be calculated under given conditions. Concept Introduction: Free energy change ΔG 0 : Change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant K ΔG 0 = − RT ( ln K ) here , T= Temperature R= Gas constant K = Equilibrium constant The Standard Gibb’s free energy change and the standard cell potential are related as followed: Δ ° G = -nFE ° cell n − N u m b e r o f e l e c t r o n s i n v o l v e d p e r e q u i v a l e n t o f t h e n e t r e d o x r e a c t i o n i n t h e c e l l F − F a r a d a y ’ s C o n s tan t ( 96500 C ) E ∘ c e l l − S tan d a r d c e l l p o t e n t i a l .

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Answer 1

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Chapter 21.4, Problem 21.6BFP

Interpretation Introduction

Interpretation:

For given ΔGo value at 25 ∘C the standard cell potential for the given reaction has to be calculated under given conditions.

Concept Introduction:

Free energy changeΔG0: Change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant K

ΔG0 = −RT(ln K)here, T= TemperatureR= Gas constantK = Equilibrium constant

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G = -nFE°cell

n − Number of electrons involved per equivalent of the net redox reaction in the cellF − Faraday’s Constant (96500 C) E∘cell− Standard cell potential.

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Answer 2

Question

Chapter 21.4, Problem 21.6BFP

Interpretation Introduction

Interpretation:

For given ΔGo value at 25 ∘C the standard cell potential for the given reaction has to be calculated under given conditions.

Concept Introduction:

Free energy changeΔG0: Change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant K

ΔG0 = −RT(ln K)here, T= TemperatureR= Gas constantK = Equilibrium constant

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G = -nFE°cell

n − Number of electrons involved per equivalent of the net redox reaction in the cellF − Faraday’s Constant (96500 C) E∘cell− Standard cell potential.

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Answer 3

Question

Chapter 21.4, Problem 21.6BFP

Interpretation Introduction

Interpretation:

For given ΔGo value at 25 ∘C the standard cell potential for the given reaction has to be calculated under given conditions.

Concept Introduction:

Free energy changeΔG0: Change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant K

ΔG0 = −RT(ln K)here, T= TemperatureR= Gas constantK = Equilibrium constant

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G = -nFE°cell

n − Number of electrons involved per equivalent of the net redox reaction in the cellF − Faraday’s Constant (96500 C) E∘cell− Standard cell potential.

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Answer 4

Question

Chapter 21.4, Problem 21.6BFP

Interpretation Introduction

Interpretation:

For given ΔGo value at 25 ∘C the standard cell potential for the given reaction has to be calculated under given conditions.

Concept Introduction:

Free energy changeΔG0: Change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant K

ΔG0 = −RT(ln K)here, T= TemperatureR= Gas constantK = Equilibrium constant

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G = -nFE°cell

n − Number of electrons involved per equivalent of the net redox reaction in the cellF − Faraday’s Constant (96500 C) E∘cell− Standard cell potential.

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Answer 5

Chapter 21.4, Problem 21.6BFP

Interpretation Introduction

Interpretation:

For given ΔGo value at 25 ∘C the standard cell potential for the given reaction has to be calculated under given conditions.

Concept Introduction:

Free energy changeΔG0: Change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant K

ΔG0 = −RT(ln K)here, T= TemperatureR= Gas constantK = Equilibrium constant

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G = -nFE°cell

n − Number of electrons involved per equivalent of the net redox reaction in the cellF − Faraday’s Constant (96500 C) E∘cell− Standard cell potential.

Answer 6

Chapter 21.4, Problem 21.6BFP

Interpretation Introduction

Interpretation:

For given ΔGo value at 25 ∘C the standard cell potential for the given reaction has to be calculated under given conditions.

Concept Introduction:

Free energy changeΔG0: Change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant K

ΔG0 = −RT(ln K)here, T= TemperatureR= Gas constantK = Equilibrium constant

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G = -nFE°cell

n − Number of electrons involved per equivalent of the net redox reaction in the cellF − Faraday’s Constant (96500 C) E∘cell− Standard cell potential.

Answer 7

Chapter 21.4, Problem 21.6BFP

Interpretation Introduction

Interpretation:

For given ΔGo value at 25 ∘C the standard cell potential for the given reaction has to be calculated under given conditions.

Concept Introduction:

Free energy changeΔG0: Change in the free energy takes place while reactant converts to product where both are in standard state. It depends on the equilibrium constant K

ΔG0 = −RT(ln K)here, T= TemperatureR= Gas constantK = Equilibrium constant

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G = -nFE°cell

n − Number of electrons involved per equivalent of the net redox reaction in the cellF − Faraday’s Constant (96500 C) E∘cell− Standard cell potential.

Answer 8

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Answer 10

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Answer 11

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