NCERT Solutions for Class 12 Chemistry Chemistry I Chapter 3 Electrochemistry

Electrochemistry Here is the CBSE Chemistry Chapter 3 for Class 12 students. Summary and detailed explanation of the lesson, including the definitions of difficult words. All of the exercises and questions and answers from the lesson's back end have been completed. NCERT Solutions for Class 12 Chemistry Electrochemistry Chapter 3 NCERT Solutions for Class 12 Chemistry Electrochemistry Chapter 3 The following is a summary in Hindi and English for the academic year 2025-26. You can save these solutions to your computer or use the Class 12 Chemistry.

Question 1

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How would you determine the standard electrode potential of the system Mg²⁺/Mg?

Solution

Answer:

Use standard hydrogen electrode as anode and Mg²⁺ | Mg as a cathode we can measure the standard electrodepotential of systemMg²⁺ | Mg. Standard hydrogen electrode, represented by Pt(s), H₂(g) (1 atm) | H⁺ (aq) and dip the electrode of Magnesium wire in a 1M MgSO₄ solution .The standard hydrogen electrode is always zero.

Use formula

E^o_cell = E^o_right – E^o_left

The standard hydrogen electrode is always zero.

So that the value of

E^o_left=0

Hence

E^o_cell = E^o_Mg|Mg2+

E^o_Mg|Mg2+= E^o_cell

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NCERT Solutions for Class 12 Chemistry Chemistry I Chapter 3 Electrochemistry

How would you determine the standard electrode potential of the system Mg²⁺/Mg?

Can you store copper sulphate solutions in a Zinc pot?

Consult the table of standard electrode potentials and suggest three substance that can oxidize ferrous ions under suitable conditions.

Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10.

Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag⁺ (0.002 M) $\to$ Ni²⁺ (0.160 M) + 2Ag(s)
Given that ${E^{o}}_{Cell} = 1.05 V$

The cell in which the following reaction occurs:
2Fe³⁺ (aq) + 2I^–(aq) $\to$ 2Fe²⁺ (aq) + I₂(s) has E⁰_cell = 0.236 V at 298 K. Calculate the standerd Gibbs energy and the equilibrium constance of the cell reaction.

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

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For Daily Free Study Material Join wiredfaculty

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NCERT Solutions for Class 12 Chemistry Chemistry I Chapter 3 Electrochemistry

How would you determine the standard electrode potential of the system Mg2+/Mg?

Can you store copper sulphate solutions in a Zinc pot?

Consult the table of standard electrode potentials and suggest three substance that can oxidize ferrous ions under suitable conditions.

Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10.

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 EoCell = 1.05 V

The cell in which the following reaction occurs:2Fe3+ (aq) + 2I–(aq) → 2Fe2+ (aq) + I2(s) has E0cell = 0.236 V at 298 K. Calculate the standerd Gibbs energy and the equilibrium constance of the cell reaction.

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°m value of water.

The molar conductivity of 0.025 mol L–1 methanoic acid is 46.1 S cm2 mol–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H+) = 349.6 S cm2 mol–1 and λ° (HCOO– ) = 54.6 s cm2 mol–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

How would you determine the standard electrode potential of the system Mg²⁺/Mg?

Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag⁺ (0.002 M) $\to$ Ni²⁺ (0.160 M) + 2Ag(s)
Given that ${E^{o}}_{Cell} = 1.05 V$

The cell in which the following reaction occurs:
2Fe³⁺ (aq) + 2I^–(aq) $\to$ 2Fe²⁺ (aq) + I₂(s) has E⁰_cell = 0.236 V at 298 K. Calculate the standerd Gibbs energy and the equilibrium constance of the cell reaction.

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.