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Gibb's Energy and Nernst Equation

The cell pote...

Question

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

A

△ G = n F log E

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B

△ G = n F E

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C

△ G = - n F E

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D

- △ G = n F log E

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Solution

The correct option is C $△ G = - n F E$
For an electrochemical reaction, the free energy change is given as
$Δ G = - n F E$

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Similar questions

Q. Match the thermodynamic properties (List I) with their relation (List II).

List I	List II
A. Free energy change ( $Δ G^{o}$ )	(i) $R T {log}_{e} K$
B. Entropy change $Δ S^{o}$	(ii) $- n F E$
C. $Δ H^{o}$ enthalpy change of a reaction in standard state	(iii) ${R T}^{2} {(\frac{d ln K}{d T})}_{P}$
D. Standard free energy change $(Δ G^{o})$	(iv) $- {\frac{d Δ G^{o}}{d T}}_{P}$

Q. For the cell:

C r (s) | C r^{3 +} | | F e^{2 +} | F e (s)

△ G^{\circ} = - n F E^{\circ}

n

Q. The equilibrium constant of a

2

electron redox reaction at

298 K

3.8 \times 10^{- 3}

. The cell potential

E^{\circ}

V

) and the free energy change

△ G^{\circ}

k J m o l^{- 1})

for this equilibrium, respectively, are:

Q. The cell potential

(E_{c e l l})

of a reaction is related as

Δ G = n F E_{c e l l}

Δ G

represents maximum useful electrical work.
n = no. of moles of electrons exchanged during the reaction.
For reversible cell reaction

d (Δ G) = (Δ V) d p - (Δ S) d T

d (Δ G) = - (Δ S) d T

Δ G = Δ H - T Δ S

∴ Δ G = Δ H + T {(\frac{d (Δ G)}{Δ T})}_{P}

{(\frac{d E_{c e l l}}{d T})}_{p}

is known as temperature coefficient of the emf of the cell.

The temperature coefficient of the emf the cell,

{(\frac{d E}{d T})}_{p}

Q. For the reaction

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)

Δ H = - 67.37 K c a l

25^{o} C

. The change in entropy in the accompanying process is

- 20.7 c a l d e g^{- 1} m o l^{- 1}

. The change in free energy at

25^{o} C

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