The standard E-M-F of the cell written as CdHg - CdSO4- 8-3 H2O s - CdSO4 sat- - Hg2SO4 s - Hg in which the cell reaction is CdHg - Hg2SO4 s - 8-3H2O l - CdSO4-8-3H2Os - 2Hgl is 1-0185 V at 25oC- Calculate - So for the cell reaction if - Eo- TP for the cell is 5-00 - 10-5 V K-1Take- F - 96485 C mol-1

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Arrhenius Equation

The standard ...

Question

The standard E.M.F of the cell written as
$C d (H g) | C d S O_{4} . \frac{8}{3} H_{2} O (s) | | C d S O_{4} (s a t .) | H g_{2} S O_{4} (s) | H g$ in which the cell reaction is
$C d (H g) + H g_{2} S O_{4} (s) + \frac{8}{3} H_{2} O (l) ⇌ C d S O_{4} . \frac{8}{3} H_{2} O (s) + 2 H g (l)$ is $1.0185 V$ at $25^{o} C$ . Calculate $Δ S^{o}$ for the cell reaction if ${(\frac{\partial E^{o}}{\partial T})}_{P}$ for the cell is $5.00 \times 10^{- 5} V K^{- 1}$
Take, $F = 96485 C m o l^{- 1}$

12.5 k J K^{- 1}

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32.6 J K^{- 1}

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9.65 J K^{- 1}

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8 k J K^{- 1}

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P b (s) + H g_{2} S O_{4} ⇌ P b S O_{4} (s) + 2 H g (l)

E_{P b / P b^{2 +}}^{o}

E_{H g / H g_{2}^{2 +}}^{o}

_{s p}

_{4}

_{2}

_{4}

2.43 \times 10^{- 8}

1.46 \times 10^{- 6}

P b (s) + H g_{2} S O_{4} (s) ⇌ P b S O_{4} (s) + 2 H g (l);

E_{c e l l}^{o} = 0.92 V

K_{s p} (P b S O_{4}) = 2 \times 10^{- 8}, K_{s p} (H g_{2} S O_{4}) = 1 \times 10^{- 6}

E_{c e l l}

\sqrt{2} = 1.4, l o g 0.14 = - 0.85

2 {Fe}^{3 +} (aq) + 2 I^{-} (aq) \to 2 {Fe}^{2 +} (aq) + I_{2} (aq) E °_{cell} = 0.24 V at 298 K

△ G^{o}

1.1

Z n (s) | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u (s)

= 96487

2 F e^{3 +} (a q) + 2 I^{-} (a q) \to 2 F e^{2 +} (a q) + I_{2} (s)

E_{c e l l}^{\circ} = 0.236 V

298 K

1 F = 96, 500 C m o l^{- 1})

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