# write relationship between standard free energy change and standard cell potential

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## What is the relation between electrochemical cell and Gibbs free energy of the cell reaction?

What is the relation between electrochemical cell and Gibbs free energy of the cell reaction?

Byju's Answer Standard XII Chemistry

Redox Reactions and Couple

What is the r... Question

What is the relation between electrochemical cell and Gibbs free energy of the cell reaction?

Open in App Solution

The change in Gibbs free energy for an electrochemical cell can be related to the cell potential. Relation between Electrochemical Cell Potential and Gibbs free Energy change is given by; Δ G = -nFE where Delta G is Gibbs Free energy change , n is the number of electrons involved in the reaction and F is Faraday and E is the Cell potential.

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SIMILAR QUESTIONS

**Q.**

Gibbs free energy change for a cell reaction is positive what does it indicates?

**Q.**Electrical energy produced by a reversible electrochemical cell is given by the free energy decrease

( – Δ G )

of the reaction occurring in the cell. According to Gibbs- Helmholtz equation, decrease in free energy is given by

– Δ G = – Δ H – T [ δ ( Δ G ) δ T ] P where – Δ H

is the decrease in enthalpy of the cell reaction at constant pressure. EMF of the cell,

E = − Δ H n F + T [ δ E δ T ] P

. By measuring the emf of the cell and its temperature co-efficient, thermodynamic quantities like

Δ H , Δ G and Δ S

can be determined. Standard emf of the cell is related to equilibrium constant of the cell reaction as

E 0 = 2.303 R T l o g k n F . EMF of the cell, A A 2 + B + B ( S ) ( a q ) ( a q ) ( s ) 1 M 0.1 M

is found to be 1.475 Volt. The equilibrium constant of the cell reaction at

25 ∘

C is (approximately)

**Q.**Electrical energy produced by a reversible electrochemical cell is given by the free energy decrease

( – Δ G )

of the reaction occurring in the cell. According to Gibbs- Helmholtz equation, decrease in free energy is given by

– Δ G = – Δ H – T [ δ ( Δ G ) δ T ] P where – Δ H

is the decrease in enthalpy of the cell reaction at constant pressure. EMF of the cell,

E = − Δ H n F + T [ δ E δ T ] P

. By measuring the emf of the cell and its temperature co-efficient, thermodynamic quantities like

Δ H , Δ G and Δ S

can be determined. Standard emf of the cell is related to equilibrium constant of the cell reaction as

E 0 = 2.303 R T l o g k n F .

From the following values of electrode potentials,

(i) ( f u m a r a t e ) 2 − + 2 H + + 2 e − → ( s u c c i n a t e ) − 2 , E 0 1 = 0.03 V and (ii) ( p y r u v a t e ) − + 2 H + + 2 e − → ( l a c t a t e ) − , E 0 2 = – 0.18 V . C a l c u l a t e Δ G ∘ for the reaction, ( f u m a r a t e ) 2 − + ( l a c t a t e ) − → ( s u c c i n a t e ) − 2 + ( p y r u v a t e ) −

**Q.**Electrical energy produced by a reversible electrochemical cell is given by the free energy decrease

( – Δ G )

of the reaction occurring in the cell. According to Gibbs- Helmholtz equation, decrease in free energy is given by

– Δ G = – Δ H – T [ δ ( Δ G ) δ T ] P where – Δ H

is the decrease in enthalpy of the cell reaction at constant pressure. EMF of the cell,

E = − Δ H n F + T [ δ E δ T ] P

. By measuring the emf of the cell and its temperature co-efficient, thermodynamic quantities like

Δ

## The cell potential (E) and the free energy change (G) accompanying an electrochemical reaction are related by:

Click here👆to get an answer to your question ✍️ The cell potential (E) and the free energy change (G) accompanying an electrochemical reaction are related by:

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>>The cell potential (E) and the free ener

Question

## The cell potential (E) and the free energy change (△G) accompanying an electrochemical reaction are related by:

**A**

## △G=nF logE

**B**

## △G=nFE

**C**

## △G=−nFE

**D**

## −△G=nF logE

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Updated on : 2022-09-05

Solution Verified by Toppr

Correct option is C)

For an electrochemical reaction, the free energy change is given asΔG=−nFE

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The Gibbs energy change accompanying a given process is -85.77 kJ mol3 1 SIMILAR QUESTIONS −1 at 25 o C and -83.68 kJ mol −1 at 35 o

C. The heat of reaction of process at 30

o C is: Hard View solution >

### The free energy change is x kJ. −100x is :

The standard Gibbs free energy change (△GHard View solution > ∘ in kJ mol −1

), in a Daniel cell (E

cell ∘

=1.1V), when 2 moles of Zn(s) is oxidized at 298 K, is closest to:

Match the thermodynamic properties (List I) with their relation (List II).Hard View solution > List I List II

A. Free energy change (ΔG

o ) (i) RTlog e K

B. Entropy change ΔS

o (ii) −nFE C. ΔH o

enthalpy change of a

reaction in standard state (iii) RT

2 ( dT dlnK ) P

D. Standard free energy change (ΔG

for the cell reactiono ) (iv) −{ dT dΔG o } P Medium View solution > Cu 2+ (C 1 aq)+Zn(s)=Zn 2+ (C 2 aq)+Cu(s)

of an electrochemical cell, the change in free energy at a given temperature is a function of

Hard View solution > MORE FROM CHAPTER Electrochemistry View chapter >

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## Nernst Equation and Calculation of Emf

Example Definitions Formulaes >

## Emf, Gibbs Energy and Equilibrium Constant

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## Write the equation showing the relationship between standard free energy and standard cell potential.

DeltaG^(@)=-nFE(cell)^(@)Write the equation showing the relationship between standard free energy and standard cell potential.

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Write the equation showing the...

Write the equation showing the relationship between standard free energy and standard cell potential.

Updated On: 27-06-2022

( 00 : 20 ) ADVERTISEMENT Text Solution Open Answer in App Solution Δ G ∘ =−nF E ∘ cell ΔG∘=-nFEcell∘

Answer

Step by step solution by experts to help you in doubt clearance & scoring excellent marks in exams.

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Guys, does anyone know the answer?