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The standard ...

Question

The standard potential of the following cells is 0.23 V at 15 $^{o}$ C and 0.21 V at 35 $^{o}$ C.

$P t, {H_{2}}_{(g)} | H C l_{(a q)} | | A g C l_{(S)} | A g_{(S)}$

The cell reaction is :

\frac{1}{2} H_{2} + A g C l \to H^{+} + A g + C l^{-}

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\frac{3}{2} H_{2} + 2 A g C l \to H^{+} + 2 A g + C l^{-}

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\frac{1}{2} H_{2} + 3 A g C l \to H^{+} + 3 A g + C l^{-}

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None of these

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Solution

The correct option is C $\frac{1}{2} H_{2} + A g C l \to H^{+} + A g + C l^{-}$
$P t, {H_{2}}_{(g)} | H C l_{(a q)} | A g C l_{(S)} | A g_{(S)}$
(i) Anodic half : $\frac{1}{2} H_{2 (g)} \to H_{(a q)}^{+} + e^{- 1}$

(ii) Cathodic half : $A g C l_{(S)} + e^{- 1} \to A g_{(S)}^{+} + C l_{(a q)}^{-}$
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Net reaction : $\frac{1}{2} H_{2 (g)} + A g C l_{(S)} \to H_{(a q)}^{+} + A g_{(S)} + C l_{(a q)}^{-}$

Suggest Corrections

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