This Class 12 Electrochemistry numerical helps students learn how to apply the Nernst equation to calculate the e.m.f. of a galvanic cell at 298 K. The given cell, Mg(s) | Mg²⁺ (0.130 M) || Ag⁺ (1.0×10⁻⁴ M) | Ag(s), uses standard electrode potentials E°(Ag⁺/Ag) = 0.80 V and E°(Mg²⁺/Mg) = –2.36 V. This numerical strengthens understanding of cell reactions, electrode potential, concentration effects and electrochemical concepts. Perfect for CBSE Class 12 board exam preparation, it helps students improve numerical solving skills and revise Electrochemistry with clarity. Ideal for notes, assignments and competitive exam practice.

Write the nernst equation and Calculate the e.m.f of the cell of 298 K.

Download Electrochemistry Class 12 Important Questions PDF

OR

Download Electrochemistry Numericals  & PYQs - Class 12 Chemistry

Boost your Class 12 Chemistry exam preparation with this detailed electrochemistry solution. Learn how to write the cell reaction and calculate the EMF of the galvanic cell Mg(s) / Mg²⁺ (0.001 M) || Cu²⁺ (0.0001 M) / Cu(s) at 298 K. Using standard electrode potentials E°(Mg²⁺/Mg) = –2.37 V and E°(Cu²⁺/Cu) = 0.34 V, this post explains step-by-step how to determine the standard cell potential, Nernst equation application, and final EMF value. Perfect for CBSE Class 12 students and competitive exam aspirants.

Welcome to Electrochemistry Class XII Chemistry Hub — your one-stop destination for mastering one of the most important chapters in Class 12 Chemistry across all education boards (CBSE, ICSE, ISC, and State Boards).

Here, you’ll find comprehensive notes, concept explanations, important questions, and previous year questions (PYQs) carefully organized to help you score high in board exams. Our resources cover every key topic — from galvanic and electrolytic cells to electrode potentials, Nernst equation, and electrochemical series — with clear, step-by-step solutions.

Whether you’re preparing for school exams, board exams, or competitive tests (JEE, NEET), this website provides exam-oriented study material, practice questions, and PYQ analysis to strengthen your understanding and boost your confidence.

✨ Key Features:

• Detailed Electrochemistry notes for Class XII Chemistry (All Boards)
• Important and Most Expected Board Questions
• Chapter-wise Previous Year Questions (PYQs)
• Concept-based MCQs and Numerical Practice
• Easy-to-understand explanations for quick revision

Start your preparation today and make Electrochemistry your strongest chapter!

Questions:-

1.  Write the balanced half-reactions occurring at the anode and cathode of the galvanic cell:
Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

2. Represent the cell in which the following reaction takes place

Mg(s)+2Ag+ (0.0001M)||Mg²+ (0.130M) + 2Ag(s)

Calculate its E (cell) if  E⁰ (cell) = 3.17V .

3.Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag+ (0.002 M) → Ni²+ (0.160 M) + 2Ag(s)
Given that E⁰cell = 1.05 V

4. A copper-silver cell is set up in which the concentration of copper ion is 0.10 M and the concentration of silver ion is not known. The cell potential when measured was found to be 0.422 V. Calculate the concentration of silver ions in the cell. The given cell reaction is:

Cu +2Ag+ → Cu²+ + 2Ag

(Given E°(Ag+/Ag) = +0.80V, E°(Cu²+/Cu) = +0.34 V), use antilog (1.29) = 19.5

5. Depict the galvanic cell in which the reaction
Zn(s) +2Ag+ (aq)  →  Zn²+ (aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode

6.Write the Nernst equation and emf of the following cells at 298 K:

Mg(s) |Mg²+ (0.001M)||Cu²+ (0.0001 M)|Cu(s)

7.Write the Nernst equation and emf of the following cells at 298 K:
(ii) Fe(s)|Fe²+ (0.001M)||H+(1M)| H2(g)(1bar)| Pt(s)

8.Write the Nernst equation and emf of the following cells at 298 K:

Sn(s)|Sn²+ (0.050M)||H+(0.020M)| H2(g)(1bar)| Pt(s)

9. Write the Nernst equation and emf of the following cells at 298 K:

Pt(s) | Br-(0.010M)|Br2(l)||H+(0.030M)| H2(g)(1bar)/ Pt(s).

10.Calculate the standard cell potentials of galvanic cell in which the following reactions take place:

                   2Cr(s)+3Cd²+ (aq)    →  2Cr³+ (aq) + 3Cd
Calculate the ΔG°  and equilibrium constant of the reactions.

11. Calculate the standard cell potentials of galvanic cell in which the following reactions take place:

                  Fe²+ (aq) + Ag+(aq)   →  Fe³+ (aq)+Ag(s)

Calculate the ΔG°  and equilibrium constant of the reactions.

12. What is the amount of electricity required to deposite one mole of aluminium from a solution   of AlCl3 ?

13.  A solution of Ni(NO3)2 is electrolysed between platinum electrode using a current of 5A for 30mint. What is the mass of Ni deposited at the cathode. The atomic mass of Ni=58.5g(amu). 

14.What is amount of electricity required to deposit one mole of calcium from molten  CaCl2 ?

15. What is amount of electricity required to deposit one mole of Zinc from ZnSO4?

16. Consider the reaction Cr2O7²- + 14H+  + 6e- → 2Cr2+   +  7H2O.  What is the quantity of electricity            in coulombs needed to reduce 1 mole of Cr2O72-  ? 

17.Calculate the mass of silver deposited from silver nitrate solution by a current of 2 ampere                 flowing for 30 minutes. (Equivalent mass of silver is 108).

18. How many hours does it take to reduce 3 mol of Fe3+ to Fe2+ with 2.00 A current? (1 Faraday = 96,500 C mol-¹, R = 8.314JK-1 mol-1 ) 

19. What mass of zinc can be produced by electrolysis of zinc sulphate solution when current of 1.5 Ampere is passed for 15 minutes ?The atomic Mass of Zinc = 65.4 amu. 

20. If a current of 0.5 ampere flows through a metallic wire for 2 hours, then howmany electrons would flow through the wire?

21. The molar conductance of infinite dilution for sodium acetate ( CH3COONa) Hydrochloric acid (HCI) and sodium chloride (NaCl) are 92.5, 426.9 and 120.4 S cm²mol-¹ respectively at 298 K. calculate the molar conductance of Acetic Acid (CH3COOH) at infinite dilution.

22.Calculate the molar conductance of a solution of MgCl2 at infinite dilution, given that molar ionic Conductance of ∧⁰ (Mg²+) = 126.1Scm²mol-¹ and ∧⁰(Cl) = 56.3 Scm²mol-¹

23. Calculte molar conductance at infinite dilution for acetic acid, given ∧⁰HCI=425ohm−¹cm²mol−¹,∧⁰ NaCI=188ohm−¹cm²mol−¹,∧⁰  CH3COONa=96ohm−¹cm²mol−¹ 

24.  Given molar conductivities at infinite dilution ∧⁰m for Ba(OH)2 = 517.6 Ω−¹cm²mol−¹ ∧⁰m for BaCl2 = 240.6 Ω−¹cm²mol−¹, ∧⁰m for NH4Cl =  129.8Ω−¹cm²mol−¹ . Calculate ∧⁰m for NH4OH

25. The resistance of 0.25 M molar solution of an electrolyte was found to be 75 Ω.Calculate molar conductivity of the solution, if the electrodes in the cell are 1.8 cm apart and have an area of cross section 3.6 cm². 

26. The Resistance of 0.5 M solution of an electrolyte was found to be 30 Ω. Calculate the molar conductivity of the solution if the electrodes in the cell are 1.5 cm apart and having area of cross section 2.0 cm². 

27. The electrical Resistance of a column of 0.05 M NaOH solution of diameter 1cm and length 50 cm is 5.55 × 10³ Ω. Calculate its Molar conductivity.

28. The Resistance of a 0.5 N solution of an electrolyte in a conductivity cell was found to be 25 Ω. Calculate the equivalent conductivity if the electrodes in the cell are 1.6 cm apart and having an area cross section 3.2 cm². 

29. Write equation and calculate e.m.f of cell at 298 K.

Mg(s) / Mg²+ (0.001M)|| Cu²+ (0.0001M)/Cu(s)

Given E⁰Mg²+/Mg(s) = - 2.37 V, E⁰cu²+/Cu(s) = 0.34 V

30. Calculate ΔG, ΔG° and Ecell for cell.

Al/Al³+ (0.01M)||Fe²+ (0.02M) / Fe
Given that E⁰ (Fe²+/ Fe ) = -0.44V, E⁰ (Al³+/Al ) =-1.66V
F = 96500 C,  R = 8.314JK-¹ mol-¹

31. Calculate Ecell and ΔG for cell,

Cu (s)/ Cu²+ (0.130M) || Ag+ / Ag(s) (1.0×10-⁴M)
E⁰Cu+/Cu = 0.34 V, E⁰Ag+/Ag = 0.80 V
Given, F = 96500 C, R = 8.314 JK-1 mol-1 

32. Write the Nernst equation and calculate the e.m.f. of the following cell at 298 K:

Mg (s) |Mg²+ (0.001M)||Cu²+ (0.0001M)|Cu (s)
Given E⁰ Mg²+ / Mg =-2.37V, E⁰ Cu²+ /Cu =0.34 V 

33. Write the Nernst equation and calculate e.m.f of the following cell of 298 K.

Ni|Ni²+ (0.01M)||Cu²+ | Cu(0.01M)
Given E⁰(Cu²+/Cu) = 0.34V, E⁰ (Ni²+ /Ni) =-0.22V 

34. Write the nernst equation and Calculate the e.m.f of the cell of 298 K.

Mg(s)|Mg²+ (0.130M)| |Ag+(1.0×10-⁴M)|Ag(s)
Given, E⁰ Ag+ /Ag =0.80 V, E (Mg²+ / Mg ) =-2.36 V 

35. Calculate the e.m.f. of the following cell.

Cr | Cr³+ (0.1M) || Fe²+ (0.01M) | Fe
Given,  E⁰(Cr³+/Cr) = -0.75V,   E⁰(Fe²+ /Fe) = -0.45V

What is amount of electricity required to deposit one mole of calcium from molten CaCl2 ?

Answer:- 

Class 12 Chemistry – Electrochemistry Numerical (SEO Blogger Post)

This post covers an important Class 12 Chemistry Electrochemistry numerical based on Faraday’s laws of electrolysis. In this question, a solution of Ni(NO₃)₂ is electrolysed using platinum electrodes with a current of 5 ampere for 30 minutes. Students are asked to calculate the mass of nickel deposited at the cathode, given the atomic mass of Ni = 58.5 g. Such numericals are very important for CBSE board exams and competitive exams. This problem helps students understand the relationship between current, time, charge, and mass deposited during electrolysis. 

A solution of Ni(NO3)2 is electrolysed between platinum electrode using a current of 5A for 30mint. What is the mass of Ni deposited at the cathode. The atomic mass of Ni=58.5g(amu).

A solution of Ni(NO3)2 is electrolysed between platinum electrode using a current of 5A for 30mint. What is the mass of Ni deposited at the cathode. The atomic mass of Ni=58.5g(amu).

Welcome to Electrochemistry Class XII Chemistry Hub — your one-stop destination for mastering one of the most important chapters in Class 12 Chemistry across all education boards (CBSE, ICSE, ISC, and State Boards).

Here, you’ll find comprehensive notes, concept explanations, important questions, and previous year questions (PYQs) carefully organized to help you score high in board exams. Our resources cover every key topic — from galvanic and electrolytic cells to electrode potentials, Nernst equation, and electrochemical series — with clear, step-by-step solutions.

Whether you’re preparing for school exams, board exams, or competitive tests (JEE, NEET), this website provides exam-oriented study material, practice questions, and PYQ analysis to strengthen your understanding and boost your confidence.

✨ Key Features:

• Detailed Electrochemistry notes for Class XII Chemistry (All Boards)
• Important and Most Expected Board Questions
• Chapter-wise Previous Year Questions (PYQs)
• Concept-based MCQs and Numerical Practice
• Easy-to-understand explanations for quick revision

Start your preparation today and make Electrochemistry your strongest chapter!

Questions:-

2. Represent the cell in which the following reaction takes place

Mg(s)+2Ag+ (0.0001M)||Mg²+ (0.130M) + 2Ag(s)

Calculate its E (cell) if  E⁰ (cell) = 3.17V .

3.Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag+ (0.002 M) → Ni²+ (0.160 M) + 2Ag(s)
Given that E⁰cell = 1.05 V

4. A copper-silver cell is set up in which the concentration of copper ion is 0.10 M and the concentration of silver ion is not known. The cell potential when measured was found to be 0.422 V. Calculate the concentration of silver ions in the cell. The given cell reaction is:

Cu +2Ag+ → Cu²+ + 2Ag

(Given E°(Ag+/Ag) = +0.80V, E°(Cu²+/Cu) = +0.34 V), use antilog (1.29) = 19.5

6.Write the Nernst equation and emf of the following cells at 298 K:

7.Write the Nernst equation and emf of the following cells at 298 K:
(ii) Fe(s)|Fe²+ (0.001M)||H+(1M)| H2(g)(1bar)| Pt(s)

8.Write the Nernst equation and emf of the following cells at 298 K:

9. Write the Nernst equation and emf of the following cells at 298 K:

10.Calculate the standard cell potentials of galvanic cell in which the following reactions take place:

11. Calculate the standard cell potentials of galvanic cell in which the following reactions take place:

12. What is the amount of electricity required to deposite one mole of aluminium from a solution   of AlCl3 ?

13.  A solution of Ni(NO3)2 is electrolysed between platinum electrode using a current of 5A for 30mint. What is the mass of Ni deposited at the cathode. The atomic mass of Ni=58.5g(amu). 

14.What is amount of electricity required to deposit one mole of calcium from molten  CaCl2 ?

15. What is amount of electricity required to deposit one mole of Zinc from ZnSO4?

16. Consider the reaction Cr2O7²- + 14H+  + 6e- → 2Cr2+   +  7H2O.  What is the quantity of electricity            in coulombs needed to reduce 1 mole of Cr2O72-  ? 

17.Calculate the mass of silver deposited from silver nitrate solution by a current of 2 ampere                 flowing for 30 minutes. (Equivalent mass of silver is 108).

18. How many hours does it take to reduce 3 mol of Fe3+ to Fe2+ with 2.00 A current? (1 Faraday = 96,500 C mol-¹, R = 8.314JK-1 mol-1 ) 

19. What mass of zinc can be produced by electrolysis of zinc sulphate solution when current of 1.5 Ampere is passed for 15 minutes ?The atomic Mass of Zinc = 65.4 amu. 

20. If a current of 0.5 ampere flows through a metallic wire for 2 hours, then howmany electrons would flow through the wire?

21. The molar conductance of infinite dilution for sodium acetate ( CH3COONa) Hydrochloric acid (HCI) and sodium chloride (NaCl) are 92.5, 426.9 and 120.4 S cm²mol-¹ respectively at 298 K. calculate the molar conductance of Acetic Acid (CH3COOH) at infinite dilution.

22.Calculate the molar conductance of a solution of MgCl2 at infinite dilution, given that molar ionic Conductance of ∧⁰ (Mg²+) = 126.1Scm²mol-¹ and ∧⁰(Cl) = 56.3 Scm²mol-¹

23. Calculte molar conductance at infinite dilution for acetic acid, given ∧⁰HCI=425ohm−¹cm²mol−¹,∧⁰ NaCI=188ohm−¹cm²mol−¹,∧⁰  CH3COONa=96ohm−¹cm²mol−¹ 

24.  Given molar conductivities at infinite dilution ∧⁰m for Ba(OH)2 = 517.6 Ω−¹cm²mol−¹ ∧⁰m for BaCl2 = 240.6 Ω−¹cm²mol−¹, ∧⁰m for NH4Cl =  129.8Ω−¹cm²mol−¹ . Calculate ∧⁰m for NH4OH

25. The resistance of 0.25 M molar solution of an electrolyte was found to be 75 Ω.Calculate molar conductivity of the solution, if the electrodes in the cell are 1.8 cm apart and have an area of cross section 3.6 cm². 

26. The Resistance of 0.5 M solution of an electrolyte was found to be 30 Ω. Calculate the molar conductivity of the solution if the electrodes in the cell are 1.5 cm apart and having area of cross section 2.0 cm². 

27. The electrical Resistance of a column of 0.05 M NaOH solution of diameter 1cm and length 50 cm is 5.55 × 10³ Ω. Calculate its Molar conductivity.

28. The Resistance of a 0.5 N solution of an electrolyte in a conductivity cell was found to be 25 Ω. Calculate the equivalent conductivity if the electrodes in the cell are 1.6 cm apart and having an area cross section 3.2 cm². 

29. Write equation and calculate e.m.f of cell at 298 K.

Mg(s) / Mg²+ (0.001M)|| Cu²+ (0.0001M)/Cu(s)

Mg (s) |Mg²+ (0.001M)||Cu²+ (0.0001M)|Cu (s)
Given E⁰ Mg²+ / Mg =-2.37V, E⁰ Cu²+ /Cu =0.34 V 

33. Write the Nernst equation and calculate e.m.f of the following cell of 298 K.

This post explains an important Class 12 Chemistry Electrochemistry numerical based on Faraday’s laws of electrolysis. The question asks: What is the amount of electricity required to deposit one mole of aluminium from a solution of AlCl₃? Such problems are frequently asked in CBSE board exams and help students understand the concept of charge required for metal deposition. Aluminium is deposited by the gain of electrons, and the calculation involves the valency of aluminium and Faraday constant. This numerical strengthens concepts related to electrolysis, oxidation-reduction reactions, and electrochemical

What is the amount of electricity required to deposite one mole of aluminium from a solution   of AlCl3 ?

Video solution:-

Text solution:-