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Gibb's Energy and Nernst Equation

Emf of the ce...

Question

Emf of the cell $P t . H_{2} (1 a t m) | H^{+} (a q .) | | A g C l | A g$ is $0.27 V$ and $0.26 V$ at $25^{\circ} C$ and $35^{\circ} C$ . Heat of reaction occuring inside the cell at $25^{\circ} C$ is:

A

- 54.8 k J

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B

26.05 k J

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C

- 26.05 k J

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D

+ 54.8 k J

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Solution

The correct option is C $- 26.05 k J$
The heat of reaction is given by
$Δ G = - n F E_{c e l l}$
$Δ G = - 1 * 96500 * 0.27$ $= - 26.05 K j$

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Similar questions

Q. The EMF of the cell :

P t,

H_{2} (1 a t m) | H^{\oplus} (a q) ∥ A g C l | A g

is 0.27 and 0.26 V at

25^{\circ} C

35^{\circ} C

, respectively. The posituve value of heat of the reaction occurring inside the cell at

25^{\circ} C

i n k J K^{- 1}

) is: ( write your answer to nearest integer)

Q. The EMF of the cell,

C d (s) | C d C l_{2} (a q, 0.1 M) | | A g C l (s) | A g (s)

in which the cell reaction is

C d (s) + 2 A g C l (s) \to 2 A g (s) + C d^{2 +} (a q) + 2 C l^{-} (a q)

0.6915 V

0.6753 V

Δ S

Δ H

of the reaction at 25°C is:
Take,

F = 96485 C m o l^{- 1}

Q. The standard potential of the following cell is

0.23 V

15^{\circ} C

0.21 V

25^{\circ} C

P t H_{2} (g) | H C l (a q .) | | A g C l (s) | A g (s)

(i) Write cell reaction.
(ii) Calculate

△ H^{\circ}

△ S^{\circ}

for the cell reaction by assuming that these quantities remain unchanged in the range

15^{\circ} C

35^{\circ} C

.
(iii) Calculate the solubility of

A g C l

25^{\circ} C

. Given the standard reduction potential of the

A g^{+} / A g

0.80 v o l t

25^{\circ} C

C d (s) | C d C l_{2} (0.10 M) | A g C l (s) | A g (s)

The EMF of the above cell is 0.6315 V at

0^{\circ} C

and 0.6753 V at

25^{\circ} C

Δ H

of reaction in kJ at

25^{\circ} C

The standard potential of the following cells is 0.23 V at 15

^{o}

C and 0.21 V at 35

^{o}

C.

P t | H_{2} (g) | H C l (a q) | A g C l (s) | A g (s)

The solubility of

A g C l

^{o}

[Note : The standard reduction potential of the

A g^{+} (a q) / A g (s)

couple is 0.80 V at 25

^{o}

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