The standard emf of the cell F e - F e 2- aq Cd 2- aq - Cd is 0-0372 V and temperature coefficient of the cell is -1-25 - 10-4 V K -1- Whichis-are correct about the cell at 300 K -A- - G -7-18 kJ - - H -14-42 kJB- - G -7-18 kJ - - H -57-50 JC- - G -7-18 kJ - - H -14-42 kJD- - S -24-125 JK -1- reaction is spontaneous

The correct options are C ∆G° nbsp;= nbsp; 7.18 nbsp;kJ, nbsp;∆H° nbsp;= nbsp; 14.42 nbsp;kJ D ∆S° nbsp;= nbsp; 24.125 nbsp;JK 1, nbsp;rea ...

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Byju's Answer

Standard XII

Chemistry

Gibb's Energy and Nernst Equation

The standard ...

Question

The standard emf of the cell $F e | F e^{2 +} (a q) | | C d^{2 +} (a q) | C d$ is 0.0372 V and temperature coefficient of the cell is $- 1.25 \times 10^{- 4} V K^{- 1}$ . Which is/are correct about the cell (at 300 K)?

Δ G ° = 7.18 k J, Δ H ° = - 14.42 k J

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Δ G ° = - 7.18 k J, Δ H ° = 57.50 J

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Δ G ° = - 7.18 k J, Δ H ° = - 14.42 k J

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Δ S ° = - 24.125 {JK}^{- 1}, reaction is spontaneous

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Solution

The correct options are
C $Δ G ° = - 7.18 k J, Δ H ° = - 14.42 k J$
D $Δ S ° = - 24.125 {JK}^{- 1}, reaction is spontaneous$
The standard emf of the cell
$F e | F e^{2 +} (a q) | | C d^{2 +} (a q) | C d$
$E ° =$ 0.0372 V
$Δ G ° = - nFE ° = - 7.18 kJ$
$Δ S ° = n \times F \times {(\frac{\partial E_{Cell}}{\partial T})}_{P}$
$Δ S ° = 2 \times 96500 \times (- 1.25 \times 10^{- 4}) = - 24.125 {JK}^{- 1}$
$Δ G ° = Δ H ° - T Δ S °$
$- 7180 = - Δ H ° - 300 \times (- 24.125)$
$Δ H ° = - 14417.5 J$

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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.

At 300K,

Δ H

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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

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Q. If

Δ G = Δ H - T Δ S

and

Δ G = Δ H + T {[\frac{d (Δ G)}{d T}]}_{p}

then variation of EMF of a cell with temperature T is given by

Q. The standard emf of the cell

F e | F e^{2 +} (a q) | | C d^{2 +} (a q) | C d

is 0.0372 V and temperature coefficient of the cell is

- 1.25 \times 10^{- 4} V K^{- 1}

. Which is/are correct about the cell (at 300 K)?

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.

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 {[\frac{δ (Δ G)}{δ T}]}_{P}

where

- Δ H

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E = \frac{- Δ H}{n F} + T {[\frac{δ E}{δ T}]}_{P}

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E^{0} = \frac{2.303 R T l o g k}{n F}

.

The standard emf of the cell,

\begin{matrix} Z n & Z n^{+ 2} & F e^{+ 3} F e^{+ 2} (S) & (a q) & (a q) (a q) \end{matrix}

Pt at

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The standard emf of the cell Fe|Fe2+(aq)||Cd2+(aq)|Cd is 0.0372 V and temperature coefficient of the cell is −1.25×10−4VK−1. Which is/are correct about the cell (at 300 K)?

The standard emf of the cell $F e | F e^{2 +} (a q) | | C d^{2 +} (a q) | C d$ is 0.0372 V and temperature coefficient of the cell is $- 1.25 \times 10^{- 4} V K^{- 1}$ . Which is/are correct about the cell (at 300 K)?