Chemistry · JEE

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

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Short tricks for Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions work only with strong fundamentals. Apply the tips below in timed sets and review every explanation.

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Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions focus drill
Solve 15 mixed MCQs for Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions, review every explanation, and note formulas you hesitated on.
NCERT line recall
For Inorganic, exact NCERT phrasing often matches the correct option — highlight one-liners during revision.
Balance then compare
In Physical Chemistry numericals, write the balanced relation first, then substitute values with units.

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Part of Redox Reactions and Electrochemistry in JEE Main Chemistry.

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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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Short tricks for speed

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Are short tricks enough for Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions in JEE?

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