Are these practice questions for Electrochemistry based on the CBSE pattern?

Yes. Every practice question is modeled on the CBSE Class 12 - Science Chemistry exam pattern — including MCQs, assertion-reason questions, and short-answer formats that frequently appear in CBSE papers.

Are the practice questions for Electrochemistry free?

Yes. Every chapter includes free practice questions for Class 12 - Science students to get you started.

What types of questions are included?

The practice set for Electrochemistry mainly includes MCQs and CBSE-style short-answer questions, with instant feedback on each answer. For full-length textbook practice, use the NCERT Solutions page.

Are the practice questions suitable for board exam preparation?

Yes. The questions test the same concepts and depth that CBSE asks in board exams. After finishing, also solve the NCERT and NCERT Exemplar exercises for Electrochemistry for full coverage.

How many practice questions are there for Electrochemistry?

The number scales with chapter length and concept density. Each chapter typically has 15-50 practice questions across MCQ and short-answer formats.

Electrochemistry Class 12 Chemistry Practice Questions with Answers

easy

Define a galvanic cell and state its primary function.

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easy

List the two main types of batteries and give one example of each.

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easy

Formulate the general relationship between the standard Gibbs free energy change (

\Delta_r G^\circ

) and the equilibrium constant (

K_c

) for a cell reaction.

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easy

Justify why alternating current (AC) is used instead of direct current (DC) for measuring the resistance of an electrolytic solution.

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easy

Recall the value of the standard electrode potential assigned to the Standard Hydrogen Electrode (SHE) at all temperatures.

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easy

Critique the design of a primary battery. What is its fundamental limitation that secondary batteries overcome?

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easy

State Faraday's first law of electrolysis.

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medium

Evaluate the effect of doubling the concentration of both

\text{Zn}^{2+}

and

\text{Cu}^{2+}

ions on the EMF of a Daniell cell. Justify your answer using the Nernst equation.

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medium

A student proposes using a zinc pot to store a copper sulphate solution. Critique this proposal from an electrochemical standpoint. Justify your conclusion using standard electrode potentials (

E^\circ_{\text{Zn}^{2+}/\text{Zn}} = -0.76 \text{ V}

,

E^\circ_{\text{Cu}^{2+}/\text{Cu}} = +0.34 \text{ V}

).

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medium

Propose an electrochemical method to prevent the rusting of an underground iron pipeline. Justify your method by explaining the underlying electrochemical principles.

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medium

Design a galvanic cell using magnesium and silver electrodes. Formulate the cell notation, write the half-cell and overall cell reactions, and justify why this combination would produce a high cell potential by referencing the standard electrode potential table.

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medium

Critique the statement: "The conductivity of an electrolytic solution always increases upon dilution." Justify your reasoning by differentiating between conductivity (

\kappa

) and molar conductivity (

\Lambda_m

).

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medium

Summarize the key differences between a galvanic cell and an electrolytic cell.

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medium

Explain the function and importance of a salt bridge in a galvanic cell.

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medium

Identify the relationship between the standard Gibbs energy change (

\Delta_r G^{\circ}

) and the standard cell potential (

E_{\text{cell}}^{\circ}

).

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medium

Recall the Nernst equation for a general electrode reaction

\text{M}^{n+}(\text{aq}) + ne^- \rightarrow \text{M}(\text{s})

and explain each term in the equation.

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medium

Explain the difference between metallic conductance and electrolytic conductance.

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medium

Evaluate the feasibility of a reaction between ferrous ions (

\text{Fe}^{2+}

) and bromine (

\text{Br}_2

) under standard conditions. Justify your prediction by calculating the standard cell potential (

E^\circ_{\text{cell}}

) and the standard Gibbs free energy change (

\Delta_r G^\circ

). (Given:

E^\circ_{\text{Fe}^{3+}/\text{Fe}^{2+}} = +0.77 \text{ V}

,

E^\circ_{\text{Br}_2/\text{Br}^-} = +1.09 \text{ V}

).

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medium

State Kohlrausch's law of independent migration of ions and write the mathematical expression for it.

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medium

Describe the construction of a Daniell cell and write its cell representation according to IUPAC convention.

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medium

Explain corrosion of iron as an electrochemical process, identifying the reactions at the anode and cathode.

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medium

Name the cathode, anode, and electrolyte used in a mercury cell.

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medium

You are tasked with designing an industrial process for the electro-refining of impure copper. Create a schematic of the electrolytic cell, specifying the materials for the anode, cathode, and electrolyte. Formulate the electrode reactions and justify why this process results in high-purity copper at the cathode.

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hard

Define resistivity (

\rho

), conductivity (

\kappa

), and molar conductivity (

\Lambda_m

). Explain how conductivity and molar conductivity of an electrolytic solution change with a decrease in concentration.

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hard

Create a hypothetical fuel cell that uses the combustion of methanol (

\text{CH}_3\text{OH}

) in an acidic medium. Formulate the half-cell reactions at the anode and cathode, and the overall cell reaction. Evaluate its potential advantages and disadvantages compared to the hydrogen-oxygen fuel cell.

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hard

Propose a method to determine the standard electrode potential of a

\text{Mg}^{2+}|\text{Mg}

half-cell. Create a diagram of the experimental setup, formulate the cell representation, and explain how the final value would be calculated and interpreted.

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hard

Describe the construction and working of a hydrogen-oxygen fuel cell. List the reactions at the anode and cathode.

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hard

Design an experiment to determine the molar conductivity at infinite dilution (

\Lambda_m^\circ

) for a weak electrolyte like acetic acid (

\text{CH}_3\text{COOH}

). Justify your choice of strong electrolytes and formulate the necessary calculations based on Kohlrausch's law.

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hard

A galvanic cell is constructed with the following reaction:

\text{Mg(s)} + 2\text{Ag}^+(0.001 \text{ M}) \rightarrow \text{Mg}^{2+}(0.10 \text{ M}) + 2\text{Ag(s)}

. Given

E^\circ_{\text{cell}} = 3.17 \text{ V}

. Evaluate whether the cell potential (

E_{\text{cell}}

) will be greater or less than the standard cell potential (

E^\circ_{\text{cell}}

). Justify your prediction qualitatively using Le Chatelier's principle and quantitatively by calculating the actual

E_{\text{cell}}

at

298 \text{ K}

using the Nernst equation.

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hard

Propose a modification to the standard hydrogen electrode (SHE) that would make it more practical for routine laboratory use, while still maintaining its function as a reference electrode. Justify your proposed changes.

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ElectrochemistryClass 12 Chemistry Practice Questions