Chemistry · JEE

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

11+ syllabus-aligned questions available

Quick answer

Goodmarks provides free online JEE practice for Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change with 11+ MCQs, instant answer checking, and full solutions. Sign up to unlock the complete question bank and topic-wise filters.

Sharpen your chemistry preparation with interactive online practice for Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change. Goodmarks offers 11+ JEE-style MCQs mapped to the official syllabus, each with detailed explanations so you learn from every attempt.

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

How do I practice Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change online for JEE?

Open this page, attempt the free sample MCQs, then sign up on Goodmarks to access the full Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change question bank with topic filters and detailed explanations.

How many Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change questions are available?

Goodmarks currently has 11+ JEE-aligned MCQs for Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change, with more added regularly.

Is this aligned with the JEE Main syllabus?

Yes. All Chemistry questions on Goodmarks are organised by official JEE Main units and subtopics, including Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change.

Do I get solutions after each question?

Every question includes the correct answer and a step-by-step explanation. Free users can practise a random mix; Pro unlocks full subject and topic filters.