Chemistry · JEE

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

11+ syllabus-aligned questions available

Quick answer

Master Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change by understanding definitions, standard results, and typical JEE question patterns — then practise with syllabus-aligned MCQs on Goodmarks.

Build clear conceptual foundations for Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change before speed practice. This guide covers what JEE expects and how to test yourself with MCQs.

Concept explainer

Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change 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 Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change in the JEE syllabus
Memorise key formulas and standard results linked to Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change
Practise 20–40 syllabus-aligned MCQs with step-by-step solutions

JEE tips

Revise Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change with a one-page formula sheet before attempting mixed tests
After each practice set, log mistakes specific to Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change and reattempt after 48 hours

Common trap

Students often rush Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change 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

Attempt 8 free MCQs for Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change. Unlock 3+ more with Pro.

Unlock full bank

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.

Want unlimited Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change practice?

Pro unlocks the full question bank, topic filters, and attempt history.

Get started free View Pro plans

Frequently asked questions

What concepts in Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change are essential for JEE?

Focus on core ideas across Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change. JEE tests application, not just memorisation.