Chemistry · JEE

Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change MCQs for JEE

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Master Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change through exam-style multiple-choice questions. This page features 11+ JEE MCQs covering Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change, each with verified answers and clear explanations.

Syllabus context

Part of Redox Reactions and Electrochemistry in JEE Main Chemistry.

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Q1ChemistryUnit 7: Redox Reactions and Electrochemistry

Which of the following changes will cause the free energy of a cell reaction to decrease?

\boldsymbol{Z} \boldsymbol{n} \mid \boldsymbol{Z} \boldsymbol{n} \boldsymbol{S} \boldsymbol{O}_{4}(\boldsymbol{a} \boldsymbol{q})\left(\boldsymbol{x}_{1} \boldsymbol{M}\right) \| \boldsymbol{H} \boldsymbol{C l}(\boldsymbol{a} \boldsymbol{q})\left(\boldsymbol{x}_{2} \boldsymbol{N}\right.

This question has multiple correct options

Q2ChemistryUnit 7: Redox Reactions and Electrochemistry

Assertion In the Daniel cell, if concentration of

C u^{2+}

and

Z n^{2+}

ions are doubled, the emf of the cell will not change. Reason f the concentration of ions in contact with the metals is doubled, the electrode potential is doubled.

Q3ChemistryUnit 7: Redox Reactions and Electrochemistry

For the reaction:

\boldsymbol{F} \boldsymbol{e}^{2+}(\boldsymbol{a} \boldsymbol{q})+\boldsymbol{A} \boldsymbol{g}^{+}(\boldsymbol{a} \boldsymbol{q}) \longrightarrow \boldsymbol{A} \boldsymbol{g}(\boldsymbol{s})+

\boldsymbol{F} \boldsymbol{e}^{+\boldsymbol{3}}(\boldsymbol{a} \boldsymbol{q})

Predict which change will decrease the cell voltage?

Q4ChemistryUnit 7: Redox Reactions and Electrochemistry

Calculate

\boldsymbol{E}_{\text {cell}}

\boldsymbol{P t}(\boldsymbol{s})\left|\boldsymbol{H}_{2}(\boldsymbol{g})_{1 a t m}\right| \boldsymbol{H} \boldsymbol{A}_{\left(\boldsymbol{K}_{a}=10^{-7}\right)} \mathbf{1} \boldsymbol{M} \| \boldsymbol{H} \boldsymbol{B}_{(\boldsymbol{k}}

Q5ChemistryUnit 7: Redox Reactions and Electrochemistry

The standard cell potential for

Z n\left|Z n^{2+}\right|\left|C u^{2+}\right| C u

1.10 V .

When the cell is completely discharged,

\log \left[Z n^{2+}\right] /\left[C u^{2+}\right]

is closest to:

Q6ChemistryUnit 7: Redox Reactions and Electrochemistry

The standard oxidation potential of Zn referred to SHE is

0.76 \mathrm{V}

and that of

\mathrm{Cu}

-0.34 V

25^{\circ} \mathrm{C} .

When excess of Zn is added to

C u S O_{4}, Z n

displaces

C u^{2+}

till equilibrium is reached. What is the ratio of

Z n^{2+}

C u^{2+}

ions at equilibrium? Express the ans in the form

\left[Z n^{2+}\right] /\left[C u^{2+}\right]=k \times 10^{37},

and find

k

Q7ChemistryUnit 7: Redox Reactions and Electrochemistry

The equilibrium constant for the reaction

\boldsymbol{S} \boldsymbol{r}(\boldsymbol{s})+\boldsymbol{M} \boldsymbol{g}^{+2}(\boldsymbol{a} \boldsymbol{q}) \rightleftharpoons \boldsymbol{S} \boldsymbol{r}^{+2}(\boldsymbol{a} \boldsymbol{q})+

M g(s)

4 \times 10^{12}

25^{\circ} C

The

E^{o}

for a cell made up of the

\boldsymbol{S} \boldsymbol{r} \mid \boldsymbol{S} \boldsymbol{r}^{+2}

and

\boldsymbol{M} \boldsymbol{g}^{+2} \mid \boldsymbol{M} \boldsymbol{g}

half cells

(\log

\mathbf{2}=\mathbf{0 . 3})

Q8ChemistryUnit 7: Redox Reactions and Electrochemistry

The

E_{\text {cell}}

for a given cell is 1.2346 and

1.2340 V

300 \mathrm{K}

and

310 \mathrm{K}

respectively. Calculate the change in entropy during the cell reaction if the redox change involves three electrons.

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