Chemistry · JEE

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

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The most important Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions questions for JEE cover conceptual traps, standard results, and numerical patterns from Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions. Goodmarks provides 41+ high-yield MCQs with full solutions.

Focus on what matters most. These important Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions questions cover high-weightage concepts from Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions — the topics JEE repeats every year.

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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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