write relationship between standard free energy change and standard cell potential

get write relationship between standard free energy change and standard cell potential from screen.

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.

Suggest Corrections 22

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

स्रोत : byjus.com

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:

Join / Login Class 12 >>Chemistry >>Electrochemistry >>Nernst Equation

>>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

Easy Open in App

Updated on : 2022-09-05

Solution Verified by Toppr

Correct option is C)

For an electrochemical reaction, the free energy change is given as

ΔG=−nFE

Was this answer helpful?

The Gibbs energy change accompanying a given process is -85.77 kJ mol

3 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 (△G

Hard 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 reaction

o ) (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 >

REVISE WITH CONCEPTS

Nernst Equation and Calculation of Emf

Example Definitions Formulaes >

Emf, Gibbs Energy and Equilibrium Constant

Example Definitions Formulaes > LEARN WITH VIDEOS

Nernst Equation 14 mins

Relation between EMF, Gibbs Free Energy, and Reaction Constant

15 mins

Numerical on Nernst Equation

14 mins SHORTCUTS & TIPS

Common Misconceptions

>

Problem solving tips

> Important Diagrams > Memorization tricks > Mindmap > Cheatsheets >

PRACTICE MORE QUESTIONS

Easy Questions 96 Qs > Medium Questions 564 Qs > Hard Questions 324 Qs >

Get the Free Answr app

Click a picture with our app and get instant verified solutions

Scan Me OR

Receive an SMS with download link

+91 Send

स्रोत : www.toppr.com

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.

Home > English > Class 12 > Chemistry > Chapter > Electrochemistry >

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.

Related Videos

644541782 12 300 1:55

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

30709906 10 400 1:23

Write equation for the reaction between free energy change and standard cell potential.

225666495 5 3.9 K 4:22

सेल अभिक्रिया की मानक मुक्त ऊर्जा

(Δ G ∘ ) (ΔG∘)

और सेल के मानक इलेक्ट्रोड विभव में संबंध स्थापित कीजिये।

643259260 0 3.7 K 1:25

Write the relationship between equilibrium constant of the reaction and standard potential of the cell.

646936455 3 1.2 K 4:10

Choose the correct relation between standard free energy change and standard cell potential

645640733 49 5.6 K

What is the relation between standard Gibb.s free energy and standard emf of the cell ?

Show More ADVERTISEMENT Follow Us:

Popular Chapters by Class:

Class 6 Algebra

Basic Geometrical Ideas

Data Handling Decimals Fractions Class 7

Algebraic Expressions

Comparing Quantities

Congruence of Triangles

Data Handling

Exponents and Powers

Class 8

Algebraic Expressions and Identities

Comparing Quantities

Cubes and Cube Roots

Data Handling

Direct and Inverse Proportions

Class 9

Areas of Parallelograms and Triangles

Circles Coordinate Geometry Herons Formula

Introduction to Euclids Geometry

Class 10

Areas Related to Circles

Arithmetic Progressions

Circles Coordinate Geometry

Introduction to Trigonometry

Class 11 Binomial Theorem

Complex Numbers and Quadratic Equations

Conic Sections

Introduction to Three Dimensional Geometry

Limits and Derivatives

Class 12

Application of Derivatives

Application of Integrals

Continuity and Differentiability

Determinants

Differential Equations

Privacy Policy

Terms And Conditions

Disclosure Policy Contact Us

स्रोत : www.doubtnut.com