Mention the reactions occurring at (i) anode (ii) cathode, during working of a mercury cell. Why does the voltage of a mercury cell remain constant during operation ?

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The cell reaction are as follows:
$\begin{matrix} Anode & Z n (H g) + 2 O H^{-} \to Z n O (s) + H_{2} O (l) + 2 e^{-} Cathode & H g O (s) + H_{2} O (l) + 2 e^{-} \to H g (l) + 2 O H^{-} Net reaction & Z n (H g) + H g O (s) \to Z n O (s) + H g (l) \end{matrix}$
Voltage of the mercury cell remains constant because ions are not involved in the net reaction.

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Updated on:21/07/2023

Class 12 CHEMISTRY ELECTROCHEMISTRY

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