Dry cell and lead acid battery mcqs electrochemistry is an important topic in Class 12 electrochemistry because it connects theoretical concepts with practical devices we use every day. When aspirants prepare for dry cell and lead acid battery mcqs electrochemistry, they must clearly understand the construction, working, reactions, and differences between primary and secondary cells. A strong conceptual base makes solving dry cell and lead acid battery mcqs electrochemistry much easier and more accurate.

In the context of dry cell and lead acid battery mcqs electrochemistry, the dry cell is classified as a primary cell. It is commonly used in flashlights, remotes, and clocks. The anode of the dry cell is zinc, which undergoes oxidation. The cathode is a carbon rod surrounded by manganese dioxide, which acts as a depolarizer. Understanding these electrode materials is crucial when attempting dry cell and lead acid battery mcqs electrochemistry because questions often test electrode identification and half-reactions.

Another essential point in dry cell and lead acid battery mcqs electrochemistry is the electrolyte used in the dry cell. It consists of a paste containing ammonium chloride and zinc chloride. During operation, zinc is oxidized to Zn²⁺, and reduction occurs at the cathode involving manganese dioxide. These reaction mechanisms frequently appear in dry cell and lead acid battery mcqs electrochemistry to test redox understanding.

When shifting focus to the secondary cell, dry cell and lead acid battery mcqs electrochemistry emphasizes the lead-acid battery, which is rechargeable. The lead-acid battery consists of a lead (Pb) anode and lead dioxide (PbO₂) cathode immersed in sulfuric acid. During discharge, both electrodes form lead sulfate (PbSO₄). Recognizing this change is critical in solving dry cell and lead acid battery mcqs electrochemistry accurately.

In dry cell and lead acid battery mcqs electrochemistry, aspirants must also understand the difference between charging and discharging processes. During discharge, chemical energy converts into electrical energy. During charging, electrical energy is supplied externally to reverse the reaction. This reversible nature distinguishes the lead-acid battery from the dry cell and is frequently tested in dry cell and lead acid battery mcqs electrochemistry.

Another core concept in dry cell and lead acid battery mcqs electrochemistry is the standard emf values. The dry cell typically has an emf of about 1.5 V, while the lead-acid battery provides approximately 2.0 V per cell. Numerical and conceptual comparisons involving emf are common in dry cell and lead acid battery mcqs electrochemistry.

In preparation for dry cell and lead acid battery mcqs electrochemistry, aspirants should focus on oxidation at the anode and reduction at the cathode. In the dry cell, zinc undergoes oxidation. In the lead-acid battery, lead is oxidized during discharge. These oxidation-reduction principles form the backbone of dry cell and lead acid battery mcqs electrochemistry.

A frequently tested area in dry cell and lead acid battery mcqs electrochemistry is the change in electrolyte concentration. In a lead-acid battery, the concentration of sulfuric acid decreases during discharge and increases during charging. The specific gravity of sulfuric acid helps determine the state of charge, a practical application often highlighted in dry cell and lead acid battery mcqs electrochemistry.

The advantages and limitations of both cells are also important in dry cell and lead acid battery mcqs electrochemistry. The dry cell is portable and inexpensive but non-rechargeable. The lead-acid battery is rechargeable and provides high current but is heavier and requires maintenance. These comparison-based points frequently appear in dry cell and lead acid battery mcqs electrochemistry.

Dry Cell and Lead Acid Battery MCQs Electrochemistry:

1. Match the entries from Column I and Column II and choose the correct order

Column I
A – Leclanche cell
B – Fuel cell
C – Ni-Cd Cell

Column II
i – Converts energy of combustion into electrical energy
ii – Rechargeable cell
iii – At anode, Zn → Zn²⁺ + 2e⁻

Options:

Option A
A – iii
B – ii
C – i

Option B
A – i
B – ii
C – iii

Option C
A – iii
B – i
C – ii

Option D
A – ii
B – i
C – iii

Correct Answer: C

2. The hydrogen ion concentration in a standard hydrogen electrode is
A. 1 mol/L
B. 1 g/L
C. 1 mol/mL
D. 1 kg/L
Correct Answer: A

3. In a galvanic cell, electrons flow from
A. anode to cathode through the external circuit
B. cathode to anode through the external circuit
C. anode to cathode through the electrolyte
D. cathode to anode through the electrolyte
Correct Answer: A

4. Which is not true regarding hydrogen as fuel?
A. High calorific value
B. Energy can be directly converted in fuel cell
C. Combustion product is ecofriendly
D. Hydrogen gas can be easily liquefied and stored
Correct Answer: D

5. Fuel cell with 0.001 M HCl electrolyte — which is true?
A. Boiling point decreases with duration
B. Boiling point increases with duration
C. Open circuit voltage remains constant
D. Open circuit voltage increases
Correct Answer: A

6. Oxidising agent in H₂–O₂ fuel cell is
A. H₂
B. C
C. O₂
D. KOH
Correct Answer: C

7. Electrolyte used in Ni-Cd cell
A. KOH
B. H₂SO₄
C. LiOH
D. Al₂O₃
Correct Answer: A

8. Correct statement for fuel cell
A. Hydrogen oxidized to H₂O at cathode
B. Oxygen reduced at anode
C. Hydrogen oxidized at anode
D. Hydrogen oxidized to H⁺ at anode
Correct Answer: C

9. When lead storage battery is discharged
A. SO₂ evolved
B. Lead sulphate consumed
C. Lead formed
D. Sulphuric acid consumed
Correct Answer: D

10. Fuel cell with 1 mol H₂ and 96.5 mA current delivers power for
A. 1 × 10⁵ s
B. 2 × 10⁵ s
C. 1 × 10⁶ s
D. 2 × 10⁶ s
Correct Answer: D

11. Car battery correct statement
A. Cathode PbO₂, anode Cu
B. Cathode Cu, anode PbO₂
C. Cathode Cu, anode Pb
D. Cathode PbO₂, anode Pb
Correct Answer: D

12. Space in dry cell is filled with
A. Paste of KOH and ZnO
B. MnO₂, ZnCl₂ and filter
C. MnO₂, ZnCl₂, NH₄Cl and filter
D. MnCl₂, ZnCl₂, NH₄Cl and filter
Correct Answer: C

13. Incorrect in galvanic cell
A. Oxidation at anode
B. Reduction at cathode
C. Cathode gains electrons
D. Cathode loses electrons
Correct Answer: D

14. A secondary cell
A. Can be recharged
B. Recharged in same direction
C. Recharged in opposite direction
D. Cannot be recharged
Correct Answer: C

15. Negative electrode in dry cell
A. Zinc
B. Graphite
C. Ammonium chloride
D. Manganese dioxide
Correct Answer: A

16. Zinc coats iron because
A. Lighter
B. Lower melting point
C. Lower negative potential
D. Higher negative potential
Correct Answer: D

17. Cell in 0.4% NaCl solution
A. No change
B. Dissolve
C. Swell
D. Shrink
Correct Answer: C

18. Standard emf of Zn-Cu cell
A. 2.1 V
B. 2.8 V
C. 1.2 V
D. 1.1 V
Correct Answer: D

19. Standard Gibbs energy for Daniell cell
A. −212.3 kJ/mol
B. −21.23 kJ/mol
C. 106.15 kJ/mol
D. −106.15 kJ/mol
Correct Answer: A

20. Cathode reaction in dry cell
A. Zn → Zn²⁺ + 2e⁻
B. MnO₂ + NH₄⁺ + e⁻ → MnO(OH) + NH₃
C. Zn(Hg) + 2OH⁻ → ZnO + H₂O + 2e⁻
D. MnO(OH) + NH₃ → MnO₂ + NH₄⁺
Correct Answer: B

21. Lead-acid battery during charging — cathode reaction
A. PbO₂ formation
B. PbSO₄ formation
C. Pb²⁺ reduced to Pb
D. Pb decomposition
Correct Answer: C

22. Cathode reaction in H₂-O₂ fuel cell
A. 2H₂ + O₂ → 2H₂O
B. O₂ + 2H₂O + 4e⁻ → 4OH⁻
C. H⁺ + e⁻ → ½H₂
D. H⁺ + OH⁻ → H₂O
Correct Answer: B

23. While charging lead battery
A. PbSO₄ on anode reduced to Pb
B. PbSO₄ on cathode reduced
C. PbSO₄ oxidized at cathode
D. PbSO₄ reduced to PbO₂
Correct Answer: A

24. Device converting combustion energy directly to electrical energy
A. Dynamo
B. Ni-Cd cell
C. Fuel cell
D. Electrolytic cell
Correct Answer: C

25. Cell converting H₂ and O₂ directly to electrical energy
A. Mercury cell
B. Daniell cell
C. Fuel cell
D. Lead storage cell
Correct Answer: C

26. Electrochemical cell stops because
A. Potential zero
B. Potentials become equal
C. Electrode eaten
D. Reaction reversed
Correct Answer: B

27. Charge of lead accumulator determined by
A. PbSO₄ amount
B. PbO₂ amount
C. Specific gravity of H₂SO₄
D. Pb amount
Correct Answer: C

28. Reaction feasible when
A. ΔG negative, E positive
B. ΔG positive, E negative
C. ΔG zero, E positive
D. ΔG zero, E zero
Correct Answer: A

29. Metal protected by its own oxide layer
A. Al
B. Ag
C. Tl
D. Au
Correct Answer: A

30. During charging of lead battery, cathode reaction is
A. Pb²⁺ + 2e⁻ → Pb
B. Pb → Pb²⁺ + 2e⁻
C. PbSO₄ + 2H₂O → 2PbO₂ + 4H⁺ + SO₄²⁻ + 2e⁻
D. Pb²⁺ + SO₄²⁻ → PbSO₄
Correct Answer: C

Conclusion on Dry Cell and Lead Acid Battery MCQs electrochemistry:

Finally, mastering dry cell and lead acid battery mcqs electrochemistry requires clear understanding of electrode reactions, electrolyte role, emf values, charging mechanisms, and practical applications. When aspirants repeatedly revise these fundamentals, dry cell and lead acid battery mcqs electrochemistry.