The standard emf of the cell Cds-CdCl2aq0-1M-AgCls-Ags in which the cell-reaction is Cds-2AgCls- 2Ags-Cd2-aq-2Cl-aqis 0-6915V at 273K and 0-6573V at 298K- Calculate enthalpy change of the reaction at 298K is-

The correct option is C +48.179 kJGiven, E_1=0.6915V, T_1=273 K, #160; #160; #160; #160; #160; #160; E_2=0.6573 V, T_ ...

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Vant Hoff's Equation and Effect of Temperature on Equilibrium Constant

The standard ...

Question

The standard 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 $C d (s) + 2 A g C l (s) \to 2 A g (s) + C d^{2 +} (a q) + 2 C l^{-} (a q)$ is $0.6915$ V at $273$ K and $0.6573$ V at $298$ K. Calculate enthalpy change of the reaction at $298$ K is?

- 176.86

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- 245.6

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+ 48.179

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+ 223.5

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

C d_{(s)} + 2 A g C l_{(s)} \Rightarrow 2 A g_{(s)} + C d_{(a q)}^{2 +} + 2 C l_{(a q)}^{-}

0.6915 V

0^{o} C

0.6573

V

25^{o} C

25^{o} C

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

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

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

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

0^{\circ} C

25^{\circ} C

Δ H

25^{\circ} C

K J m o l^{- 1} a t 298 K

Z n (s) + C u^{2 +} (a q) \to Z n^{2 +} (a q) + C u (s), E^{\circ} = 2 V a t 298 K

(F a r a d a y^{'} s c o n s t a n t, F = 96000 C m o l^{- 1})

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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