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Development of Endosperm

11. Cell Hg|H...

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11. Cell Hg|Hg2Cl2|Cl-(0.1M)||Cl-(0.01M)|PtCl2 ke liye E^° =1.10V what is the E 1)1.1591V 2)1.1591V 3)1.0409V 4)1.0409V

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The electrical work done during the reaction at 298 K:
$2 H g_{(l)} + C l_{2 (g)} \to H g_{2} C l_{2 (s)}, i s G i v e n t h a t E_{\frac{C l_{2}}{C l^{-}}}^{\circ} = 1.36 V; E_{\frac{H g_{2} C l_{2}}{H g, C l^{-}}}^{\circ} = 0.27 V; P_{C l_{2}} = 1 a t m,$

Q. The cell reaction for the given cell is spontaneous if :

P t C l_{2} P_{1} | C l^{-} 1 M | | C l^{-} 1 M | P t C l_{2} P_{2}

Q. For the cell,

P t | C l_{2} (g, 0.4 b a r) | C l^{-} (a q, 0.1 M) | | C l^{-} (a q, 0.01 M) | C l_{2} (g, 0.2 b a r) | P t

. The cell potential at

298 K

E_{r e d}^{o}

of the half-cell

H g_{2} C l_{2} (s) + 2 e^{-} \to 2 H g (s) + 2 C l^{-} (a q)

0.27 V

p K_{s p}

corresponding to solubility product for

H g_{2} C l_{2} (s)

is 17 then find the

E_{r e d}^{\circ}

for the half cell

H g_{2}^{2 +} (a q) + 2 e \to 2 H g (s) .

\frac{2.303 R T}{F} = 0.06)

Q. Construct galvanic cells from the following pairs of half cells and calculate their emf at

25^{o} C .

C d^{2 +} (a q, 1 M) ∣ C d (s); E_{C d^{2 +} / C d}^{0} = - 0.40 V

H g_{2} C l_{2} (s) ∣ H g (l) ∣ C l^{-} (a q, 0.1 M); E_{C l^{-} / H g_{2} C l_{2} / H g}^{0} = 0.28 V

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