The cell potential E cell of a reaction is related as - G - nF E cell- where - G represents maximum useful electrical work- n - no- of moles of electrons exchanged during the reaction- For reversible cell reaction d - G - V dp - S d TAt const- P- d - G - S dTAt const- P- - G - H - T - S-1- G - H - T d - G - T P -2 dE cell - dT p is known as temperature coefficient of the emf of the cell-The - S for the cell reaction Zn -2 AgCl - ZnCl 2-2 Ag isA- 100 JK -1 mol -1B- -73-53 JK -1 mol -1C- 83-53 JK -1 mol -1D- 200 JK -1 mol -1

The correct option is B 73.53JK^ 1mol^ 1Δ S=nF ( dE/dT ) 2×96500( 3.81× 10^ 4) = 73.53 j/mole k ...

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Byju's Answer

Standard XII

Chemistry

Properties of Water

The cell pote...

Question

The cell potential $(E_{c e l l})$ of a reaction is related as $Δ G = n F E_{c e l l}$ , where $Δ G$ represents maximum useful electrical work.
n = no. of moles of electrons exchanged during the reaction.
For reversible cell reaction $d (Δ G) = (Δ V) d p - (Δ S) d T$
At const. P, $d (Δ G) = - (Δ S) d T$
At const. P, $Δ G = Δ H - T Δ S$ ..(1)
$∴ Δ G = Δ H + T {(\frac{d (Δ G)}{Δ T})}_{P}$ . (2)
${(\frac{d E_{c e l l}}{d T})}_{p}$ is known as temperature coefficient of the emf of the cell.

The $Δ S$ for the cell reaction $Z n + 2 A g C l \to Z n C l_{2} + 2 A g$ is

- 73.53 J K^{- 1} m o l^{- 1}

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83.53 J K^{- 1} m o l^{- 1}

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100 J K^{- 1} m o l^{- 1}

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200 J K^{- 1} m o l^{- 1}

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Solution

The correct option is A $- 73.53 J K^{- 1} m o l^{- 1}$
$Δ S = n F (\frac{d E}{d T})$
$2 \times 96500 (- 3.81 \times 10^{- 4})$
$= - 73.53 j / m o l e k$

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Similar questions

Q. The cell potential

(E_{c e l l})

of a reaction is related as

Δ G = n F E_{c e l l}

, where

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

At const. P,

d (Δ G) = - (Δ S) d T

At const. P,

Δ G = Δ H - T Δ S

. (1)

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

. (2)

{(\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}

is given by

Q. The cell potential

(E_{c e l l})

of a reaction is related as

Δ G = n F E_{c e l l}

, where

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

At const. P,

d (Δ G) = - (Δ S) d T

At const. P,

Δ G = Δ H - T Δ S

. (1)

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

. (2)

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

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

At 300K,

Δ H

for the reaction

Z n + 2 A g C l \to Z n C l_{2} + 2 A g i s - 218

kJ/mole while emf of the cell was

1.015 V . {(\frac{d E}{d T})}_{p}

of the cell is

d (Δ G) = - (Δ S_{reaction}) . d T

Δ G = Δ H - T Δ S

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

Calculate

Δ S

for the given cell reaction in the previous question.

d (Δ G) = - (Δ S_{reaction}) . d T

Δ G = Δ H - T Δ S

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

Calculate

Δ S

for the given cell reaction in the previous question.

d (Δ G) = - (Δ S_{reaction}) . d T

Δ G = Δ H - T Δ S

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

300 K, Δ H

for the reaction,

Z n_{(S)} + 2 A g C l_{(S)} \to Z n C l_{2_{(a q)}} + 2 A g_{(S)}

- 218 kJ/mol

while the e.m.f of the cell is

1.015 V

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

of the cell is:

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The correct option is A −73.53JK−1mol−1ΔS=nF(dEdT) 2×96500(−3.81×10−4) =−73.53j/mole k

The correct option is A $- 73.53 J K^{- 1} m o l^{- 1}$
$Δ S = n F (\frac{d E}{d T})$
$2 \times 96500 (- 3.81 \times 10^{- 4})$
$= - 73.53 j / m o l e k$