Chemistry · JEE

Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions Concepts for JEE

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Quick answer

Master Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions by understanding definitions, standard results, and typical JEE question patterns — then practise with syllabus-aligned MCQs on Goodmarks.

Build clear conceptual foundations for Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions before speed practice. This guide covers what JEE expects and how to test yourself with MCQs.

Concept explainer

Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions is a core JEE Main Chemistry subtopic under Redox Reactions and Electrochemistry. Master the definitions, standard results, and typical MCQ patterns tested in JEE Main and Advanced.

Key points

Understand the definition and scope of Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions in the JEE syllabus
Memorise key formulas and standard results linked to Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions
Practise 20–40 syllabus-aligned MCQs with step-by-step solutions

JEE tips

Revise Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions with a one-page formula sheet before attempting mixed tests
After each practice set, log mistakes specific to Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions and reattempt after 48 hours

Common trap

Students often rush Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions questions without checking units, sign conventions, or boundary conditions — always verify assumptions before calculating.

Syllabus context

Part of Redox Reactions and Electrochemistry in JEE Main Chemistry.

Free sample questions

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Q1ChemistryUnit 7: Redox Reactions and Electrochemistry

Which of the following statement (s) differentiate between electrochemical cell and electrolytic cell? This question has multiple correct options

Q2ChemistryUnit 7: Redox Reactions and Electrochemistry

A half cell reaction is one which:

Q3ChemistryUnit 7: Redox Reactions and Electrochemistry

The reduction potential of an electrode can be increased by:

Q4ChemistryUnit 7: Redox Reactions and Electrochemistry

The e.m.f. of the cell \begin{tabular}{l|c||c|c}

\boldsymbol{P t} \boldsymbol{H}_{2}

\boldsymbol{H O C N}

\boldsymbol{A} \boldsymbol{g}^{+}

\boldsymbol{1} \boldsymbol{a} \boldsymbol{t m}

\boldsymbol{1} . \boldsymbol{3} \times \mathbf{1 0}^{-\boldsymbol{3}} \boldsymbol{M}

\boldsymbol{0 . 8} \boldsymbol{M}

\end{tabular} \mid

\boldsymbol{A} \boldsymbol{g}(s)

0.982 \mathrm{V} .

The

\mathrm{K}_{a}

for HOCN is :

\boldsymbol{A} \boldsymbol{g}^{+}+\boldsymbol{e} \rightarrow \boldsymbol{A} \boldsymbol{g}(\boldsymbol{s}) ; \boldsymbol{E}^{o}=\mathbf{0 . 8 0} \boldsymbol{V}

Q5ChemistryUnit 7: Redox Reactions and Electrochemistry

Cathodic standard reduction potential minus anodic standard reduction potential is equal to:

Q6ChemistryUnit 7: Redox Reactions and Electrochemistry

Assertion In electrochemical cell, we can not use KCl in the salt bridge if anodic or cathodic compartment consists of

\mathrm{Ag}^{+}

P b^{2+}

ion. Reason Salt bridge is employed to maintain the electrical neutrality and to minimize the liquid-liquid junction potential.

Q7ChemistryUnit 7: Redox Reactions and Electrochemistry

The oxidation potential of a hydrogen electrode at

p H=10

and

P_{H_{2}}=1

is:

Q8ChemistryUnit 7: Redox Reactions and Electrochemistry

The

E_{c e l l}^{o}

for

C u\left|C u^{2+}\right|\left|A g^{+}\right| A g

in volt is

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Frequently asked questions

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