(A) The calomel electrode is represented as $Hg | Hg_2Cl_2(s) | Cl^-(aq)$. It consists of mercury in contact with solid mercurous chloride $(Hg_2Cl_2)

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Metal - Insoluble Salt - Anion electrodes

(A) The calomel electrode is represented as $Hg | Hg_2Cl_2(s) | Cl^-(aq)$. It consists of mercury in contact with solid mercurous chloride $(Hg_2Cl_2)$ and a solution of chloride ions $(Cl^-)$. This structure classifies it as a $Metal - Insoluble Salt - Anion$ electrode.

Class 12 Chemistry Electrochemistry Electrochemical cells

Medium

One of the commonly used electrodes is the calomel electrode. Under which of the following categories does the calomel electrode fall?

JEE MAIN 2024 All JEE MAIN

A
Metal - Insoluble Salt - Anion electrodes
B
Oxidation - Reduction electrodes
C
Gas - Ion electrodes
D
Metal ion - Metal electrodes

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Derive the relation between the dissociation constant $K_a$ and the limiting molar conductivity $\Lambda_m^o$ for a solution of a weak electrolyte.

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In a dry cell,the reaction which takes place at the zinc anode is:

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AIPMT 2008

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Standard electrode potentials of $Zn$ and $Fe$ are known to be $(i) -0.76 \ V$ and $(ii) -0.44 \ V$ respectively. How does this explain that galvanization prevents rusting of iron while zinc slowly dissolves away?

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One of the commonly used electrodes is the calomel electrode. Under which of the following categories does the calomel electrode fall?

Similar Questions

Derive the relation between the dissociation constant $K_a$ and the limiting molar conductivity $\Lambda_m^o$ for a solution of a weak electrolyte.

Provide the chemical reaction and the potential of a Daniell cell by drawing a labelled diagram. Also,provide primary information indicating what type of cell it is.

In a dry cell,the reaction which takes place at the zinc anode is:

Standard free energies of formation (in $kJ/mol$) at $298 \ K$ are $-237.2$,$-394.4$,and $-8.2$ for $H_2O_{(l)}$,$CO_{2_{(g)}}$,and pentane$_{(g)}$ respectively. The value of $E^o_{cell}$ for the pentane-oxygen fuel cell is .......... $V$.

Standard electrode potentials of $Zn$ and $Fe$ are known to be $(i) -0.76 \ V$ and $(ii) -0.44 \ V$ respectively. How does this explain that galvanization prevents rusting of iron while zinc slowly dissolves away?

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