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What is cell entropy change (in J/K) of the following cell?
$P t (s) | \underset{P = 1 a t m}{H_{2} (g)} | \underset{0.1 M}{C H_{3} C O O H}, H C l | \underset{0.1 M}{| K C l} (a q) | H g_{2} C l_{2} (s) | H g$
Emf of the cell is found to be 0.045V at 298K and temperature coefficient is $3.4 \times 10^{- 4} V K^{- 1}$ (No. of electrons transferred in reaction, n=2).
Given $K_{a (C H_{3} C O O H)} = 10^{- 5} M, [1 F = 96500 C / m o l]$

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69.50

65.62

63.5

answer is B.

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Detailed Solution

$Δ G = Δ H - T Δ S, - n F E_{c e l l} = Δ H - T Δ S, Δ S = n F \frac{d E c e l l}{d T}$

$Δ S = n F \frac{d E c e l l}{d T} = 2 \times 96500 \times 3.4 \times 10^{- 4} = 65.6 J / K$

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