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 ?

Text Solution

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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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Question 1 - Select One
The reaction occuring at the anode during the working of alkaline dry cell -
A $Z n + H_{2} O \to Z n O + 2 O H^{-} + 2 e^{-}$
B $Z n + 2 O H^{-} \to Z n O + H_{2} O + 2 e^{-}$
C $Z n \to Z n^{2 +} + 2 e^{-}$
D $Z n^{2 +} + 2 e^{-} \to Z n$
Question 1 - Select One
Which of the following reaction occurs at the cathode during the working of alkaline dry cell ?
AZn is converted into ZnO
B $M n O_{2}$ is converted into $M n_{2} O_{3}$
C $Z n$ is converted into $Z n^{2 +}$
D $M n_{2} O_{3}$ is converted into $M n O_{2}$

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