CBSE Class 12 Chemistry Electrochemistry Question Bank Set 02

Practice Worksheets for Class 12 Chemistry: Unit 2 Electrochemistry

Explore reliable practice materials for Unit 2 Electrochemistry tailored for Class 12 learners. Utilizing these Chemistry worksheets ensures thorough preparation and strengthens problem-solving speed for upcoming school assessments.

Practice Unit 2 Electrochemistry Worksheets for Class 12 Chemistry

Access the complete worksheet PDF for Unit 2 Electrochemistry below. Regular practice with these targeted questions builds familiarity with standard exam patterns and helps secure higher marks in final Chemistry evaluations.

ELECTROCHEMISTRY
 
1. The products formed when an aqueous solution of NaBr is electrolysed in a cell having inert electrodes are:
(a) Na and Br2
(b) Na and O2
(c) H2 ,Br2 and NaOH
(d) H2 and O2
 
2. Time required to deposit one millimole of aluminium metal by the passage of 9.65 amperes through aqueous solution of aluminium ion is
(a) 30 s    (b) 10 s    (c) 30,000 s    (d) 10,000 s
 
3. The cell constant of a given cell is 0.47 cm–1.The resistance of a solution placed in this cell is measured to be 31.6 ohm. The conductivity of the solution in S cm–1 is
(a) 0.15   (b) 1.5     (c) 0.015        (d) 150
 
4. Assertion –Reason type questions:
 
In the following questions a statement of assertion followed by a statement of reason is given.Choose the correct answer from the following choices.
 
(a) Both assertion and reason are correct statements and the reason is a correct explanation for assertion.
 
(b) Both assertion and reason are correct but reason is not a correct explanation for assertion.
 
(c) Assertion is correct but reason is incorrect.
 
(d) Assertion is wrong but reason is correct.
 
(i) Assertion: Electrical conductivity of copper decreases with increase in temperature
Reason: The electrical conductivity of metals is due to motion of electrons.
 
(ii) Assertion:Mercury cell doesnotgivesteady potential
Reason:In the cell reaction,ions are not involved in the solution.
 
5. Read the given passage and answer the questions that follow:
 
A Lead storage battery is the most important type of secondary cell having a lead anode and a grid of lead packed with PbO2 as cathode. A 38% solution of sulphuric acid is used as electrolyte.
(Density=1.294 g mL-1) The battery holds 3.5 L of the acid. During the discharge of the battery, the density of H2SO4 falls to 1.139 g mL-1. (20% H2SO4 by mass)
(i) Write the reaction taking place at the cathode when the battery is in use.
(ii) How much electricity in terms of Faraday is required to carry out the reduction of one mole of PbO2?
(iii)What is the molarity of sulphuric acid before discharge?
(iv)Lead storage battery is considered a secondary cell. Why?
(v) Write the products of electrolysis when dilute sulphuric acid is electrolysed using Platinum electrodes.
 
6. What is meant by limiting molar conductivity?
 
7. The E 0 values of Cu and Zn are 0.34V and –0.76V respectively. Which of the two is a stronger reducing agent?
 
8. Calculate the potential of hydrogen electrode in contact with a solution having pH value 10.
 
9. How many Faradays are required to produce 2.4g of Mg?
 
10. How much charge is needed to oxidize one mole of FeO to Fe2O3?
 
11. Write Nerst equation and calculate the emf of following cell at 298 K:
 
Mg(s)|Mg2+ (0.001 M)||Cu2+ (0.0001 M)|Cu(s) .Given E0 cell= 2.71 V.
 
12. Define and express the relationship between conductivity and molar conductivity for the solution of an electrolyte.
 
13. Electrolytic specific conductance of 0.25M solution of KCl at 250C is 2.56 x 10-2S/cm, calculate the molar conductance.
 
14. Describe the reactions which occur at the electrodes in a fuel cell that causes H2 and O2 to produce electricity.
 
15. How many hours does it take to reduce 3 moles of Fe3+ to Fe2+ with a current of 2amperes?
 
16. Account for the following:
a) Alkaline medium inhibits the rusting of iron.
b) Iron does not rust even if the zinc coating is broken in a galvanized iron pipe.
 
17. Calculate the time to deposit 1.5 g of silver at cathode when a current of 1.5 A was passed through the solution of AgNO3. (Molar mass of Ag = 108 g mol-1, 1 F = 96500 C mol-1)
 
18. Three electrolytic cells A, B, C containing solutions of ZnSO4, AgNO3 and CuSO4,respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?
 
19. Conductivity of 0.00241 M acetic acid is 7.896 × 10–5 S cm–1. Calculate its molar conductivity and if Λ0 m for acetic acid is 390.5Scm2mol–1, what is its dissociation constant?
 
20. Calculate the equilibrium constant and ΔG0 for the following reaction at 250C.
Ni(s)+ 2Ag+(aq) → Ni2+(aq) + 2Ag (s),
Given that the std electrode potential at 250C is 1.05V. (1F = 96500 C mol-1)
 
21. What type of a battery is the lead storage battery? Write the anode and cathode reactions and the overall reaction occurring in a lead storage battery when the cell is in use.
 
22. A conductivity cell with cell constant 3cm-1 is filled with 0.1M acetic acid solution. The resistance is found to be 4000 ohms. Find
a] molar conductance of 0.1M acetic acid
b] Degree of dissociation of acetic acid given that Λ0 (CH3COOH) = 400 S cm2 mol-1.
 

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Exam Preparation Worksheet for Class 12 Chemistry Unit 2 Electrochemistry

Download Practice Sheet: Unit 2 Electrochemistry (Class 12 Chemistry)

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Concept Clarification for Unit 2 Electrochemistry

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Are these Chemistry Class 12 worksheets based on the 2026-27 competency-based pattern?

Yes, our CBSE Class 12 Chemistry Electrochemistry Question Bank Set 02 includes a variety of questions like Case-based studies, Assertion-Reasoning, and MCQs as per the 50% competency-based weightage in the latest curriculum for Class 12.

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