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Gibb's Free Energy

What is cell ...

Question

What is cell entropy change of the following cell?
$P t (x) | H_{2} (g) | C H_{3} C O O H, H C l | | K C l (a q) | H g_{2} C l_{2} (s) | H g$
P = 1 atm 0.1 M 0.1 M
Emf of the cell is found to be 0.045 V at 298 K and temperature coefficient is $3.4 \times 10^{- 4} V K^{- 1}$
[Given : $K_{a (C H_{3} C O O H)} = 10^{- 5} M$ ]

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65.62

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69.2

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63.5

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Solution

The correct option is A 65.62
Considering the cell reaction
$H_{2} + 2 e \to 2 H^{+} (a q)$
$H g_{2}^{2 +} + 2 e \to 2 H g (l)$
$Δ S = n F \times {(\frac{\partial E}{\partial T})}_{P} = 2 \times 96500 \times 3.4 \times 10^{- 4} = 65.62 J / (K . m o l)$

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Similar questions

P t (s) | H_{2} (g, 1 a t m) | C H_{3} C O O H, H C l | | K C l (a q) | H g_{2} C l_{2} (s) | H g

0.0045 V

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

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

K_{a (C H_{3} C O O H)} = 10^{- 5} M)

P t (s) ∣ ∣ ∣ \begin{matrix} H_{2} (g) p = 1 a t m \end{matrix} ∣ ∣ ∣ \begin{matrix} C H_{3} C O O H, H C l 0.1 M \end{matrix} ∣ ∣ ∣ ∣ ∣ ∣ \begin{matrix} K C l (a q) 0.1 M \end{matrix} ∣ ∣ ∣ \begin{matrix} H g_{2} C l_{2} (s) \end{matrix} ∣ ∣ ∣ H g

A g | A g C l | | K C l (a q .) | H_{2} C l_{2} | H g

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

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

1.5 \times 10^{- 4} J K^{- 1}

P b (s) + H g C l_{2} (a q) \to P b C l_{2} (a q) + H g (l)

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

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

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