Chemistry · Textbook solutions

Electrochemistry

Every solved example, exercise, and miscellaneous question, in the order the textbook teaches them. Plus every board question asked from this chapter. · 43 questions

Worked Examples

10 q

Solved Examples

Worked · 10

Eg 2.1 $\text{Mg}(s) + 2\text{Ag}^{+}(0.0001\,\text{M}) \rightarrow \text{Mg}^{2+}(0.130\,\text{M}) + 2\text{Ag}(s)$
Eg 2.2 $\text{Cu}(s) + 2\text{Ag}^{+}(aq) \rightarrow \text{Cu}^{2+}(aq) + 2\text{Ag}(s)$
Eg 2.3 $1.1\,\text{V}$
Eg 2.4 $0.1\,\text{mol L}^{-1}$
Eg 2.5 $0.05\,\text{mol L}^{-1}$
Eg 2.6 $\text{KCl}$
Eg 2.7 $\Lambda_m^{\circ}$
Eg 2.8 $\Lambda_m^{\circ}$
Eg 2.9 $0.001028\,\text{mol L}^{-1}$
Eg 2.10 $\text{CuSO}_4$

$c/\text{mol L}^{-1}$	$\Lambda_m/\text{S cm}^{2}\,\text{mol}^{-1}$
0.000198	148.61
0.000309	148.29
0.000521	147.81
0.000989	147.09

Intext Questions

15 q

Intext 2.1 $\text{Mg}^{2+}\,|\,\text{Mg}$
Intext 2.2 $Can you store copper sulphate solutions in a zinc pot?$
Intext 2.3 $Consult the table of standard electrode potentials and suggest three substances that can oxidise ferrous ions under suitable conditions.$
Intext 2.4 $Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10.$
Intext 2.5 $\text{Ni}(s) + 2\text{Ag}^{+}(0.002\,\text{M}) \rightarrow \text{Ni}^{2+}(0.160\,\text{M}) + 2\text{Ag}(s)$
Intext 2.6 $2\text{Fe}^{3+}(aq) + 2\text{I}^{-}(aq) \rightarrow 2\text{Fe}^{2+}(aq) + \text{I}_2(s)$
Intext 2.7 $Why does the conductivity of a solution decrease with dilution?$
Intext 2.8 $\Lambda_m^{\circ}$
Intext 2.9 $0.025\,\text{mol L}^{-1}$
Intext 2.10 $If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?$
Intext 2.11 $Suggest a list of metals that are extracted electrolytically.$
Intext 2.12 $\text{Cr}_2\text{O}_7^{2-} + 14\text{H}^{+} + 6e^{-} \rightarrow 2\text{Cr}^{3+} + 7\text{H}_2\text{O}$
Intext 2.13 $Write the chemistry of recharging the lead storage battery, highlighting all the materials that are involved during recharging.$
Intext 2.14 $Suggest two materials other than hydrogen that can be used as fuels in fuel cells.$
Intext 2.15 $Explain how rusting of iron is envisaged as setting up of an electrochemical cell.$

Exercises

18 q

Ex 2.1 $\text{Al}$
Ex 2.2 $\text{K}^{+}/\text{K} = -2.93\,\text{V}$
Ex 2.3 $\text{Zn}(s) + 2\text{Ag}^{+}(aq) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Ag}(s)$
Ex 2.4 $2\text{Cr}(s) + 3\text{Cd}^{2+}(aq) \rightarrow 2\text{Cr}^{3+}(aq) + 3\text{Cd}$
Ex 2.5 $\text{Mg}(s)\,|\,\text{Mg}^{2+}(0.001\,\text{M})\,||\,\text{Cu}^{2+}(0.0001\,\text{M})\,|\,\text{Cu}(s)$
Ex 2.6 $\text{Zn}(s) + \text{Ag}_2\text{O}(s) + \text{H}_2\text{O}(l) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Ag}(s) + 2\text{OH}^{-}(aq)$
Ex 2.7 $Define conductivity and molar conductivity for the solution of an electrolyte. Discuss their variation with concentration.$
Ex 2.8 $\text{KCl}$
Ex 2.9 $\text{KCl}$
Ex 2.10 $10^{2} \times \kappa/\text{S m}^{-1}$
Ex 2.11 $7.896 \times 10^{-5}\,\text{S cm}^{-1}$
Ex 2.12 $\text{Al}^{3+}$
Ex 2.13 $\text{Ca}$
Ex 2.14 $\text{H}_2\text{O}$
Ex 2.15 $\text{Ni(NO}_3)_2$
Ex 2.16 $\text{ZnSO}_4$
Ex 2.17 $\text{Fe}^{3+}(aq)$
Ex 2.18 $\text{AgNO}_3$

Concentration/M	0.001	0.010	0.020	0.050	0.100
$10^{2} \times \kappa/\text{S m}^{-1}$	1.237	11.85	23.15	55.53	106.74

What the board has asked from this chapter

Questions per paper · 26 papers · 2022 to 2026

Bars average the full papers of each year. 54 further questions come from set variants and are listed below.

2026

29 q

1 $\mathrm{Zn_{(s)}} + \mathrm{Ag_2O_{(s)}} + \mathrm{H_2O}(l) \rightarrow \mathrm{Zn^{2+}_{(aq)}} + 2\mathrm{Ag_{(s)}} + 2\mathrm{OH^{-}_{(aq)}}$
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Nernst Equation
5 $\mathrm{Cr_2O_7^{2-}}$
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Electrolytic Cells and Electrolysis
5 $\mathrm{CuCl_2}$
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Electrolytic Cells and Electrolysis
9 $\mathrm{Mg\,(s)\,|\,Mg^{2+}\,(1{\cdot}0\ M)\,||\,Cu^{2+}\,(1{\cdot}0\ M)\,|\,Cu\,(s)}$
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Nernst Equation
9 $How the conductivity varies on decreasing concentration for both weak and strong electrolytes ?$
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Conductance of Electrolytic Solutions
10 $On electrolysis of very dilute aqueous solution of NaCl using platinum electrodes :$
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Electrolytic Cells and Electrolysis
18 $(a) Name any two materials other than hydrogen that can be used as fuel in fuel cells. (b) Define molar conductivity.$
Fuel Cells
18 $(a) Name the cell used in hearing aids and watches. (b) Define conductivity. Why is direct current (DC) not used for the measurement of resistance of an ionic solution ?$
Batteries
18 $(a) Name the cell which was used in the Apollo space programme for providing electrical power. (b) Define limiting molar conductivity.$
Fuel Cells
22 $\mathrm{Cr\,(s)} \mid \mathrm{Cr^{3+}(aq)}\ (0{\cdot}1\ \mathrm{M}) \parallel \mathrm{Fe^{2+}(aq)}\ (0{\cdot}01\ \mathrm{M}) \mid \mathrm{Fe\,(s)}$
Nernst Equation
22 $\mathrm{Al\,(s)} \mid \mathrm{Al^{3+}(aq)}\ (0{\cdot}1\ \mathrm{M}) \parallel \mathrm{Ni^{2+}(aq)}\ (0{\cdot}01\ \mathrm{M}) \mid \mathrm{Ni\,(s)}$
Nernst Equation
22 $\mathrm{Zn\,(s)} \mid \mathrm{Zn^{2+}(aq)}\ (0{\cdot}1\ \mathrm{M}) \parallel \mathrm{Ag^{+}(aq)}\ (0{\cdot}01\ \mathrm{M}) \mid \mathrm{Ag\,(s)}$
Nernst Equation
23 $\mathrm{Sn} \mid \mathrm{Sn^{2+}}\ (0.001\ \mathrm{M}) \parallel \mathrm{H^{+}}\ (0.01\ \mathrm{M}) \mid \mathrm{H_{2(g)}}\ (1\ \mathrm{bar}) \mid \mathrm{Pt_{(s)}}$
Nernst Equation
23 (a) $\mathrm{(K_c)}$
Nernst Equation
23 $\Lambda_m^{o}$
Conductance of Electrolytic Solutions
23 (b) $What type of battery is Mercury cell ? Why it is more advantageous than dry cell ? Write overall reaction taking place in Mercury cell.$
Batteries
24 $\mathrm{AgNO_3}$
Conductance of Electrolytic Solutions
Electrochemistry is the study of the relationship between chemical energy and electrical energy. Many spontaneously occurring chemical reactions liberate electrical energy. In electrolysis, electrical energy is converted directly into chemical energy. The product of an electrolytic reaction depends on the nature of the material being electrolysed and the type of electrode used. Oxidising and reducing species present in the electrolytic cell and their standard electrode potential too, affect the products of electrolysis. Electrolysis plays an important role in most people’s daily lives, whether it is for the manufacturing of aluminium, electroplating of metals, or the synthesis of chemical compounds. Michael Faraday was the first scientist who proposed two laws to explain the quantitative aspects of electrolysis, popularly known as Faraday’s laws of electrolysis. Faraday’s laws of electrolysis provide a basis for mathematical analysis of the mass deposited at electrodes and the amount of charge passed through them. Faraday’s laws are fundamental in various applications, including electroplating, metal extraction, battery technology and chemical synthesis. These laws also help in environmental monitoring and in various chemistry experiments.
30 (a) $\mathrm{CuCl_2}$
Electrolytic Cells and Electrolysis
Electrochemistry is the study of the relationship between chemical energy and electrical energy. Many spontaneously occurring chemical reactions liberate electrical energy. In electrolysis, electrical energy is converted directly into chemical energy. The product of an electrolytic reaction depends on the nature of the material being electrolysed and the type of electrode used. Oxidising and reducing species present in the electrolytic cell and their standard electrode potential too, affect the products of electrolysis. Electrolysis plays an important role in most people’s daily lives, whether it is for the manufacturing of aluminium, electroplating of metals, or the synthesis of chemical compounds. Michael Faraday was the first scientist who proposed two laws to explain the quantitative aspects of electrolysis, popularly known as Faraday’s laws of electrolysis. Faraday’s laws of electrolysis provide a basis for mathematical analysis of the mass deposited at electrodes and the amount of charge passed through them. Faraday’s laws are fundamental in various applications, including electroplating, metal extraction, battery technology and chemical synthesis. These laws also help in environmental monitoring and in various chemistry experiments.
30 (b) $\mathrm{Ag^{+}}$
Electrolytic Cells and Electrolysis
Electrochemistry is the study of the relationship between chemical energy and electrical energy. Many spontaneously occurring chemical reactions liberate electrical energy. In electrolysis, electrical energy is converted directly into chemical energy. The product of an electrolytic reaction depends on the nature of the material being electrolysed and the type of electrode used. Oxidising and reducing species present in the electrolytic cell and their standard electrode potential too, affect the products of electrolysis. Electrolysis plays an important role in most people’s daily lives, whether it is for the manufacturing of aluminium, electroplating of metals, or the synthesis of chemical compounds. Michael Faraday was the first scientist who proposed two laws to explain the quantitative aspects of electrolysis, popularly known as Faraday’s laws of electrolysis. Faraday’s laws of electrolysis provide a basis for mathematical analysis of the mass deposited at electrodes and the amount of charge passed through them. Faraday’s laws are fundamental in various applications, including electroplating, metal extraction, battery technology and chemical synthesis. These laws also help in environmental monitoring and in various chemistry experiments.
30 (b) OR $State Faraday’s second law of electrolysis.$
Electrolytic Cells and Electrolysis
Electrochemistry is the study of the relationship between chemical energy and electrical energy. Many spontaneously occurring chemical reactions liberate electrical energy. In electrolysis, electrical energy is converted directly into chemical energy. The product of an electrolytic reaction depends on the nature of the material being electrolysed and the type of electrode used. Oxidising and reducing species present in the electrolytic cell and their standard electrode potential too, affect the products of electrolysis. Electrolysis plays an important role in most people’s daily lives, whether it is for the manufacturing of aluminium, electroplating of metals, or the synthesis of chemical compounds. Michael Faraday was the first scientist who proposed two laws to explain the quantitative aspects of electrolysis, popularly known as Faraday’s laws of electrolysis. Faraday’s laws of electrolysis provide a basis for mathematical analysis of the mass deposited at electrodes and the amount of charge passed through them. Faraday’s laws are fundamental in various applications, including electroplating, metal extraction, battery technology and chemical synthesis. These laws also help in environmental monitoring and in various chemistry experiments.
30 (c) $\mathrm{Cl^{-}(aq)} \longrightarrow \frac{1}{2}\mathrm{Cl_2(g) + e^{-}}$
Electrolytic Cells and Electrolysis
32 (A) $\mathrm{L^{-1}}$
Conductance of Electrolytic Solutions
32 (B) $\Omega$
Conductance of Electrolytic Solutions
33 (a) $\Delta\mathrm{G}$
Nernst Equation
33 (a) $\mathrm{E^{o}_{cell}}$
Nernst Equation
33 (a) $0{\cdot}01$
Nernst Equation
33 (b) $0{\cdot}001$
Conductance of Electrolytic Solutions
33 (b) $\mathrm{2AgCl(s) + H_2(g)\ (0.4\ atm) \longrightarrow 2Ag(s) + 2H^{+}(0.1\ M) + 2Cl^{-}(0.2\ M)}$
Nernst Equation
33 (b) $0{\cdot}0024$
Conductance of Electrolytic Solutions

2025

41 q

1 $\mathrm{MnO_4^{-}}$
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Electrolytic Cells and Electrolysis
1 $\mathrm{2Cu^{+}\,(aq) + Zn\,(s) \rightarrow 2Cu\,(s) + Zn^{2+}\,(aq)}$
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Nernst Equation
2 $\mathrm{Sn^{4+}/Sn^{2+}}$
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Galvanic Cells
3 $A conductivity cell usually consists of two :$
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Conductance of Electrolytic Solutions
3 $\mathrm{H_2SO_4}$
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Electrolytic Cells and Electrolysis
3 $\Lambda_m = \Lambda_m^{\circ} - \mathrm{A}\sqrt{\mathrm{C}}$
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Conductance of Electrolytic Solutions
9 $\mathrm{2Ag^{+}\,(aq) + Mg\,(s) \rightarrow 2Ag\,(s) + Mg^{2+}\,(aq)}$
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Nernst Equation
9 $We cannot measure the resistance of an ionic solution using DC because :$
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Conductance of Electrolytic Solutions
10 $A galvanic cell can behave like an electrolytic cell when$
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Electrochemical Cells
10 $\mathrm{Fe_2O_3}$
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Electrolytic Cells and Electrolysis
10 $Which of the following cell converts the energy of combustion of fuel into electrical energy ?$
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Fuel Cells
11 $Match the type of cell given in Column I with their use given in Column II. Column I Column II i. Lead storage cell a. Wall clock ii. Mercury cell b. Apollo Space Programme iii. Dry cell c. Wrist watch iv. Fuel cell d. Inverter$
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Batteries
11 $\mathrm{MnO_4^{-}}$
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Electrolytic Cells and Electrolysis
12 $\mathrm{H_2O}$
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Electrolytic Cells and Electrolysis
For Questions number 13 to 16, two statements are given — one labelled as Assertion (A) and the other labelled as Reason (R). Select the correct answer to these questions from the codes (A), (B), (C) and (D) as given below.
13 $Assertion (A) : For measuring resistance of an ionic solution an AC source is used. Reason (R) : Concentration of ionic solution will change if DC source is used.$
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Conductance of Electrolytic Solutions
For Questions number 13 to 16, two statements are given — one labelled as Assertion (A) and the other labelled as Reason (R). Select the correct answer to these questions from the codes (A), (B), (C) and (D) as given below.
13 $\mathrm{H_2}$
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Electrolytic Cells and Electrolysis
19 $Name and define the cell which was used for providing electric power in the Apollo space programme. Also write its one advantage.$
Fuel Cells

Column I	Column II
i. Lead storage cell	a. Wall clock
ii. Mercury cell	b. Apollo Space Programme
iii. Dry cell	c. Wrist watch
iv. Fuel cell	d. Inverter

298{\cdot}15

Concentration of KCl solution in mol / L	Conductivity at $298{\cdot}15$ K in S $\mathrm{cm^{-1}}$	Molar Conductivity at $298{\cdot}15$ K in S $\mathrm{cm^{2}\,mol^{-1}}$
$1{\cdot}000$	$0{\cdot}1113$	$111{\cdot}3$
$0{\cdot}100$	$0{\cdot}0129$	$129{\cdot}0$
$0{\cdot}010$	$0{\cdot}00141$	$141{\cdot}0$

Conductance of Electrolytic Solutions

19 $Define fuel cell. Give two advantages of fuel cell over ordinary cell.$
Fuel Cells
23 $\mathrm{E^{\circ}_{values}}$
Conductance of Electrolytic Solutions
23 $Give reasons : (a) Fuel cells are preferred for production of electrical energy than thermal plants. (b) Iron does not rust even if zinc coating is broken in a galvanized pipe. (c) In the experimental determination of electrolytic conductance, Direct Current (DC) is not used.$
Fuel Cells
23 (a) $Write the name of the cell which is generally used in inverters. Write the reactions taking place at anode and cathode of this cell, when it is in use.$
Batteries
23 $\Delta_r \mathrm{G^{\circ}}$
Nernst Equation
23 $\Delta_r G^{\circ}$
Nernst Equation
23 $\mathrm{cm^2}$
Conductance of Electrolytic Solutions
23 $\Lambda^{\circ}\mathrm{m}$
Conductance of Electrolytic Solutions
24 $25^{\circ}\mathrm{C}$
Nernst Equation
23 (b) $\mathrm{H_2}$
Electrolytic Cells and Electrolysis
23 $25^{\circ}\mathrm{C}$
Nernst Equation
24 $Give reasons for the following : (a) The pH of aqueous NaCl increases when it is electrolysed. (b) Unlike dry cell, mercury cell has a constant cell potential through its lifetime. (c) Conductivity of solution decreases with dilution.$
Electrolytic Cells and Electrolysis
28 $25^{\circ}\mathrm{C}$
Nernst Equation
31 (A) $\mathrm{Sn(s) \mid Sn^{2+}\ (0.004\ M) \parallel H^{+}\ (0.02\ M) \mid H_2(g)\ (1\ Bar) \mid Pt\ (s)}$
Nernst Equation
31 (a) $\mathrm{Cr^{3+}} + 3\mathrm{e^{-}} \rightarrow \mathrm{Cr\,(s)}$
Nernst Equation
31 (a) $\mathrm{E_{cell}}$
Nernst Equation
31 (b) $\Lambda^{\circ}_{\mathrm{m}}\,\mathrm{NH_4Cl}$
Conductance of Electrolytic Solutions
31 (b) $0{\cdot}001$
Conductance of Electrolytic Solutions
31 (B) $\mathrm{K_2Cr_2O_7(aq)}$
Nernst Equation
32 (A) $(\Delta_\mathrm{r}\mathrm{G}^{\circ})$
Nernst Equation
32 (B) $\mathrm{Zn(s)} \mid \mathrm{Zn^{2+}_{(0.1M)}} \parallel \mathrm{Cd^{2+}_{(0.01M)}} \mid \mathrm{Cd(s)}$
Nernst Equation
33 (a) $\mathrm{Zn(s)} \mid \mathrm{Zn^{2+}}\ (0{\cdot}1\ \mathrm{M}) \parallel \mathrm{H^{+}}\ (0{\cdot}01\ \mathrm{M}) \mid \mathrm{H_2(g)}\ (1\ \mathrm{bar}),\ \mathrm{Pt(s)}$
Nernst Equation
33 (b) $0{\cdot}20$
Conductance of Electrolytic Solutions

2024

37 q

1 $\mathrm{Mg^{2+}}$
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Conductance of Electrolytic Solutions
1 $\mathrm{Al^{3+}}$
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Conductance of Electrolytic Solutions
1 $\mathrm{Ca^{2+}}$
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Conductance of Electrolytic Solutions
6 $Which of the following cell is used in hearing aids ?$
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Batteries
7 $Which of the following cell was used in Apollo space programme ?$
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Fuel Cells
9 $The unit of cell constant is :$
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Conductance of Electrolytic Solutions
9 $\mathrm{CuCl_2}$
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Electrolytic Cells and Electrolysis
9 $Dilution affects both molar conductivity as well as conductivity. Effect of dilution on both is$
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Conductance of Electrolytic Solutions
10 $During electrolysis of aqueous solution of NaCl :$
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Electrolytic Cells and Electrolysis
10 $Which of the following cell is used in inverter ?$
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Batteries
11 $Which of the following cells is used in hearing aids ?$
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Batteries
11 $Dilution affects both conductivity as well as molar conductivity. Effect of dilution on both is as follows :$
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Conductance of Electrolytic Solutions
12 $During the electrolysis of aqueous NaCl, the cathodic reaction is :$
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Electrolytic Cells and Electrolysis
12 $Which of the following is a secondary cell ?$
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Batteries
For questions number 13 to 16, two statements are given – one labelled as Assertion (A) and the other labelled as Reason (R). Select the correct answer to these questions from the codes (A), (B), (C) and (D) as given below :
16 $\mathrm{Zn/Zn^{2+}}$
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Galvanic Cells
17 $\mathrm{Fe^{2+}}$
Nernst Equation
17 $Define the following terms : (a) Faraday’s second law of electrolysis (b) Corrosion$
Electrolytic Cells and Electrolysis
17 $State : (a) Kohlrausch law of independent migration of ions. (b) Faraday’s first law of electrolysis.$
Conductance of Electrolytic Solutions
18 $(\Lambda^{\circ}_{\mathrm{m}})$
Conductance of Electrolytic Solutions
21 $0.2\ \mathrm{mol\ L^{-1}}$
Conductance of Electrolytic Solutions
22 $0{\cdot}05$
Conductance of Electrolytic Solutions
23 $25\,^{\circ}\mathrm{C}$
Nernst Equation
23 $0{\cdot}2$
Conductance of Electrolytic Solutions
25 $\mathrm{Ni(s) + 2Ag^+(0.01\ M) \longrightarrow Ni^{2+}(0.1\ M) + 2Ag(s)}$
Nernst Equation
27 $\mathrm{Zn\,(s)} \mid \mathrm{Zn^{2+}}\ (0{\cdot}1\ \mathrm{M}) \parallel \mathrm{Sn^{2+}}\ (0{\cdot}001\ \mathrm{M}) \mid \mathrm{Sn\,(s)}$
Nernst Equation
Batteries and fuel cells are very useful forms of galvanic cell. Any battery or cell that we use as a source of electrical energy is basically a galvanic cell. However, for a battery to be of practical use it should be reasonably light, compact and its voltage should not vary appreciably during its use. There are mainly two types of batteries — primary batteries and secondary batteries. In the primary batteries, the reaction occurs only once and after use over a period of time the battery becomes dead and cannot be reused again, whereas the secondary batteries are rechargeable. Production of electricity by thermal plants is not a very efficient method and is a major source of pollution. To solve this problem, galvanic cells are designed in such a way that energy of combustion of fuels is directly converted into electrical energy, and these are known as fuel cells. One such fuel cell was used in the Apollo space programme.
29 (a) $How do primary batteries differ from secondary batteries ?$
Batteries
Batteries and fuel cells are very useful forms of galvanic cell. Any battery or cell that we use as a source of electrical energy is basically a galvanic cell. However, for a battery to be of practical use it should be reasonably light, compact and its voltage should not vary appreciably during its use. There are mainly two types of batteries — primary batteries and secondary batteries. In the primary batteries, the reaction occurs only once and after use over a period of time the battery becomes dead and cannot be reused again, whereas the secondary batteries are rechargeable. Production of electricity by thermal plants is not a very efficient method and is a major source of pollution. To solve this problem, galvanic cells are designed in such a way that energy of combustion of fuels is directly converted into electrical energy, and these are known as fuel cells. One such fuel cell was used in the Apollo space programme.
29 (b) $1{\cdot}35$
Batteries
Batteries and fuel cells are very useful forms of galvanic cell. Any battery or cell that we use as a source of electrical energy is basically a galvanic cell. However, for a battery to be of practical use it should be reasonably light, compact and its voltage should not vary appreciably during its use. There are mainly two types of batteries — primary batteries and secondary batteries. In the primary batteries, the reaction occurs only once and after use over a period of time the battery becomes dead and cannot be reused again, whereas the secondary batteries are rechargeable. Production of electricity by thermal plants is not a very efficient method and is a major source of pollution. To solve this problem, galvanic cells are designed in such a way that energy of combustion of fuels is directly converted into electrical energy, and these are known as fuel cells. One such fuel cell was used in the Apollo space programme.
29 (c) $Write the reactions involved in the recharging of the lead storage battery.$
Batteries
Batteries and fuel cells are very useful forms of galvanic cell. Any battery or cell that we use as a source of electrical energy is basically a galvanic cell. However, for a battery to be of practical use it should be reasonably light, compact and its voltage should not vary appreciably during its use. There are mainly two types of batteries — primary batteries and secondary batteries. In the primary batteries, the reaction occurs only once and after use over a period of time the battery becomes dead and cannot be reused again, whereas the secondary batteries are rechargeable. Production of electricity by thermal plants is not a very efficient method and is a major source of pollution. To solve this problem, galvanic cells are designed in such a way that energy of combustion of fuels is directly converted into electrical energy, and these are known as fuel cells. One such fuel cell was used in the Apollo space programme.
29 (c) OR $Write two advantages of fuel cells over other galvanic cells.$
Fuel Cells
In a galvanic cell, chemical energy of a redox reaction is converted into electrical energy, whereas in an electrolytic cell the redox reaction occurs on passing electricity. The simplest galvanic cell is in which Zn rod is placed in a solution of $\mathrm{ZnSO_4}$ and Cu rod is placed in a solution of $\mathrm{CuSO_4}$ . The two rods are connected by a metallic wire through a voltmeter. The two solutions are joined by a salt bridge. The difference between the two electrode potentials of the two electrodes is known as electromotive force. In the process of electrolysis, the decomposition of a substance takes place by passing an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis.
30 (a) $What is the function of a salt bridge in a galvanic cell ?$
Galvanic Cells
In a galvanic cell, chemical energy of a redox reaction is converted into electrical energy, whereas in an electrolytic cell the redox reaction occurs on passing electricity. The simplest galvanic cell is in which Zn rod is placed in a solution of $\mathrm{ZnSO_4}$ and Cu rod is placed in a solution of $\mathrm{CuSO_4}$ . The two rods are connected by a metallic wire through a voltmeter. The two solutions are joined by a salt bridge. The difference between the two electrode potentials of the two electrodes is known as electromotive force. In the process of electrolysis, the decomposition of a substance takes place by passing an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis.
30 (b) $When does galvanic cell behave like an electrolytic cell ?$
Galvanic Cells
In a galvanic cell, chemical energy of a redox reaction is converted into electrical energy, whereas in an electrolytic cell the redox reaction occurs on passing electricity. The simplest galvanic cell is in which Zn rod is placed in a solution of $\mathrm{ZnSO_4}$ and Cu rod is placed in a solution of $\mathrm{CuSO_4}$ . The two rods are connected by a metallic wire through a voltmeter. The two solutions are joined by a salt bridge. The difference between the two electrode potentials of the two electrodes is known as electromotive force. In the process of electrolysis, the decomposition of a substance takes place by passing an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis.
30 (c) $\mathrm{E^{\circ}}$
Galvanic Cells
In a galvanic cell, chemical energy of a redox reaction is converted into electrical energy, whereas in an electrolytic cell the redox reaction occurs on passing electricity. The simplest galvanic cell is in which Zn rod is placed in a solution of $\mathrm{ZnSO_4}$ and Cu rod is placed in a solution of $\mathrm{CuSO_4}$ . The two rods are connected by a metallic wire through a voltmeter. The two solutions are joined by a salt bridge. The difference between the two electrode potentials of the two electrodes is known as electromotive force. In the process of electrolysis, the decomposition of a substance takes place by passing an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis.
30 (c) OR $\mathrm{MnO_4^-}$
Electrolytic Cells and Electrolysis
31 (a) $25^{\circ}\mathrm{C}$
Nernst Equation
31 (b) $\Delta_{\mathrm{r}}\mathrm{G^{o}}$
Nernst Equation
33 (a) $0{\cdot}05$
Conductance of Electrolytic Solutions
33 (b) $0{\cdot}0025\ \mathrm{mol\,L^{-1}}$
Conductance of Electrolytic Solutions

2023

45 q

3 $\mathrm{Zn} + 2\mathrm{Ag}^{+} \longrightarrow \mathrm{Zn}^{2+} + 2\mathrm{Ag}$
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Galvanic Cells
3 $\mathrm{Fe^{3+}_{(aq)}} + \mathrm{e}^{-} \rightarrow \mathrm{Fe^{2+}_{(aq)}}$
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Galvanic Cells
3 $\mathrm{Ag^{+}\,(aq)} + \mathrm{e^{-}} \longrightarrow \mathrm{Ag\,(s)}\qquad \mathrm{E}^{\circ} = +\,0{\cdot}80$
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Galvanic Cells
3 $\mathrm{Sn^{2+}_{(aq)}} + 2\mathrm{e}^{-} \rightarrow \mathrm{Sn_{(s)}}$
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Galvanic Cells
3 $\mathrm{Sn^{2+}_{(aq)}} + 2\mathrm{e^{-}} \rightarrow \mathrm{Sn_{(s)}}$
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Galvanic Cells
4 $\Delta \mathrm{G}$
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Nernst Equation
4 $2\mathrm{Cl^{-}} \rightarrow \mathrm{Cl_2} + 2\mathrm{e^{-}}$
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Electrolytic Cells and Electrolysis
6 $The unit of molar conductivity is$
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Conductance of Electrolytic Solutions
8 $\Lambda = \Lambda_{o} - \mathrm{A}\sqrt{\mathrm{C}}$
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Conductance of Electrolytic Solutions
8 $\mathrm{KCl}$
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Conductance of Electrolytic Solutions
8 $Which of the following relations is incorrect ?$
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Conductance of Electrolytic Solutions
9 $\mathrm{MnO_4^{-}}$
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Electrolytic Cells and Electrolysis
9 $The cathode reaction during the charging of a lead storage battery leads to the :$
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Batteries
9 $\mathrm{CuSO_4}$
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Electrolytic Cells and Electrolysis
9 $Corrosion of iron is :$
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Corrosion
12 $Which of the following cell was used in Apollo space programme ?$
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Fuel Cells
For Questions number 15 to 18, two statements are given — one labelled as Assertion (A) and the other labelled as Reason (R). Select the correct answer to these questions from the codes (a), (b), (c) and (d) as given below.
16 $\Lambda_{\mathrm{m}}$
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Conductance of Electrolytic Solutions
For Questions number 15 to 18, two statements are given — one labelled as Assertion (A) and the other labelled as Reason (R). Select the correct answer to these questions from the codes (a), (b), (c) and (d) as given below.
16 $\mathrm{NaCl}$
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Electrolytic Cells and Electrolysis
Given below are two statements labelled as Assertion (A) and Reason (R). Select the most appropriate answer from the options given below :
16 $Assertion (A) : Molar conductivity decreases with increase in concentration. Reason (R) : When concentration approaches zero, the molar conductivity is known as limiting molar conductivity.$
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Conductance of Electrolytic Solutions
Given below are two statements labelled as Assertion (A) and Reason (R). Select the most appropriate answer from the options given below :
16 $Assertion (A) : Conductivity decreases with decrease in concentration of electrolyte. Reason (R) : Number of ions per unit volume that carry the current in a solution decreases on dilution.$
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Conductance of Electrolytic Solutions
For Questions number 15 to 18, two statements are given — one labelled as Assertion (A) and the other labelled as Reason (R). Select the correct answer to these questions from the codes (a), (b), (c) and (d) as given below.
16 $\Lambda_{\mathrm{m}}$
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Conductance of Electrolytic Solutions
For Questions number 15 to 18, two statements are given — one labelled as Assertion (A) and the other labelled as Reason (R). Select the correct answer to these questions from the codes (a), (b), (c) and (d) as given below.
17 $(\Lambda^{\circ}_{\mathrm{m}})$
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Conductance of Electrolytic Solutions
19 (a) $\mathrm{E^{\circ}_{Cell}}$
Galvanic Cells
19 (b) $\mathrm{Fe_{(s)}} \mid \mathrm{Fe^{2+}}\,(0.01\mathrm{M}) \parallel \mathrm{H^{+}_{(1M)}} \mid \mathrm{H_{2(g)}}\,(1\ \mathrm{bar}),\ \mathrm{Pt_{(s)}}$
Nernst Equation
20 (a) $\Lambda_{\mathrm{m}}$
Conductance of Electrolytic Solutions
20 (a) $\Delta_{\mathrm{r}}\mathrm{G}^{\circ}$
Nernst Equation
20 (a) $Give reasons : (i) Mercury cell delivers a constant potential during its life time. (ii) In the experimental determination of electrolytic conductance, Direct Current (DC) is not used.$
Batteries
21 (a) $Define fuel cell and write its two advantages.$
Fuel Cells
20 (b) $0{\cdot}05$
Conductance of Electrolytic Solutions
20 (b) $Define fuel cell with an example. What advantages do the fuel cells have over primary and secondary batteries ?$
Fuel Cells
21 $Name the cell which : (a) was used in Apollo Space programme. (b) is used in automobiles and inverters. (c) is suitable for hearing aids and watches. (d) does not give a steady potential and is used in transistors.$
Batteries
21 (b) $\mathrm{E}^{\circ}$
Corrosion

Rahul set-up an experiment to find resistance of aqueous KCl solution for different concentrations at 298 K using a conductivity cell connected to a Wheatstone bridge. He fed the Wheatstone bridge with a.c. power in the audio frequency range 550 to 5000 cycles per second. Once the resistance was calculated from null point he also calculated the conductivity K and molar conductivity

\Lambda_{\mathrm{m}}

and recorded his readings in tabular form.

S.No.	Conc.(M)	k S $\mathrm{cm^{-1}}$	$\Lambda_{\mathrm{m}}$ S $\mathrm{cm^2\ mol^{-1}}$
1.	1.00	$111.3 \times 10^{-3}$	111.3
2.	0.10	$12.9 \times 10^{-3}$	129.0
3.	0.01	$1.41 \times 10^{-3}$	141.0

32 (a)

Why does conductivity decrease with dilution ?

Conductance of Electrolytic Solutions

\Lambda_{\mathrm{m}}

and recorded his readings in tabular form.

S.No.	Conc.(M)	k S $\mathrm{cm^{-1}}$	$\Lambda_{\mathrm{m}}$ S $\mathrm{cm^2\ mol^{-1}}$
1.	1.00	$111.3 \times 10^{-3}$	111.3
2.	0.10	$12.9 \times 10^{-3}$	129.0
3.	0.01	$1.41 \times 10^{-3}$	141.0

32 (a)

Why does conductivity increase though the conductivity decrease with dilution ?

Conductance of Electrolytic Solutions

\Lambda_{\mathrm{m}}

and recorded his readings in tabular form.

S.No.	Conc.(M)	k S $\mathrm{cm^{-1}}$	$\Lambda_{\mathrm{m}}$ S $\mathrm{cm^2\ mol^{-1}}$
1.	1.00	$111.3 \times 10^{-3}$	111.3
2.	0.10	$12.9 \times 10^{-3}$	129.0
3.	0.01	$1.41 \times 10^{-3}$	141.0

32 (b)

\Lambda_{\mathrm{m}}^{\circ}

Conductance of Electrolytic Solutions

\Lambda_{\mathrm{m}}

and recorded his readings in tabular form.

S.No.	Conc.(M)	k S $\mathrm{cm^{-1}}$	$\Lambda_{\mathrm{m}}$ S $\mathrm{cm^2\ mol^{-1}}$
1.	1.00	$111.3 \times 10^{-3}$	111.3
2.	0.10	$12.9 \times 10^{-3}$	129.0
3.	0.01	$1.41 \times 10^{-3}$	141.0

32 (c) (a)

\Lambda_{\mathrm{m}}

Conductance of Electrolytic Solutions

\Lambda_{\mathrm{m}}

and recorded his readings in tabular form.

S.No.	Conc.(M)	k S $\mathrm{cm^{-1}}$	$\Lambda_{\mathrm{m}}$ S $\mathrm{cm^2\ mol^{-1}}$
1.	1.00	$111.3 \times 10^{-3}$	111.3
2.	0.10	$12.9 \times 10^{-3}$	129.0
3.	0.01	$1.41 \times 10^{-3}$	141.0

32 (c) (b)

\mathrm{CH_3COOH}

Conductance of Electrolytic Solutions

\Lambda_{\mathrm{m}}

and recorded his readings in tabular form.

S.No.	Conc.(M)	k S $\mathrm{cm^{-1}}$	$\Lambda_{\mathrm{m}}$ S $\mathrm{cm^2\ mol^{-1}}$
1.	1.00	$111.3 \times 10^{-3}$	111.3
2.	0.10	$12.9 \times 10^{-3}$	129.0
3.	0.01	$1.41 \times 10^{-3}$	141.0

32 (c) (b)

\mathrm{CH_3COOH}

Conductance of Electrolytic Solutions

33 (a) $\log \mathrm{K_c}$
Nernst Equation
33 (a) $\mathrm{Al\,(s)} \mid \mathrm{Al}^{3+}\,(0{\cdot}001\ \mathrm{M}) \parallel \mathrm{Ni}^{2+}\,(0{\cdot}1\ \mathrm{M}) \mid \mathrm{Ni\,(s)}$
Nernst Equation
33 (b) $\mathrm{Cu}^{2+}$
Nernst Equation
33 (b) $\mathrm{NH_4^{+}}$
Conductance of Electrolytic Solutions
35 (a) $\log \mathrm{K_c}$
Nernst Equation
35 $25^{\circ}\mathrm{C}$
Nernst Equation
35 $2 \times 10^{-3}$
Conductance of Electrolytic Solutions

2022

22 q

2 $Define molar conductivity for the solution of an electrolyte. How does it vary with concentration ?$
Conductance of Electrolytic Solutions
2 $\Lambda_m$
Conductance of Electrolytic Solutions
2 $\mathrm{CH_3COOH}$
Conductance of Electrolytic Solutions
2 $\Lambda_{\mathrm{m}}$
Conductance of Electrolytic Solutions
2 $\Lambda_{\mathrm{m}}$
Conductance of Electrolytic Solutions
2 $0{\cdot}001$
Conductance of Electrolytic Solutions
3 $7.8 \times 10^{-5}\ \mathrm{S\ cm^{-1}}$
Conductance of Electrolytic Solutions
3 $\mathrm{Zn(s)} + \mathrm{Cu^{2+}\,(aq)} \rightarrow \mathrm{Zn^{2+}\,(aq)} + \mathrm{Cu(s)}$
Nernst Equation
3 $Define conductivity for the solution of an electrolyte. Why does the conductivity of a solution decrease with dilution ?$
Conductance of Electrolytic Solutions
3 $\alpha$
Conductance of Electrolytic Solutions
5 (a) $\Delta_r G^\circ$
Nernst Equation
5 $\mathrm{Zn\,(s)} \mid \mathrm{Zn^{2+}}\,(0{\cdot}01\ \mathrm{M}) \parallel (0{\cdot}001\ \mathrm{M})\ \mathrm{Ag^{+}} \mid \mathrm{Ag\,(s)}$
Nernst Equation
5 (b) $\mathrm{Fe(s)\,|\,Fe^{2+}\,(0.001\ M)\,||\,H^{+}\,(0.01M)\,|\,H_2(g)\,(1\ bar)\,|\,Pt(s)}$
Nernst Equation
10 $\mathrm{Zn} \,|\, \mathrm{Zn^{2+}}\,(0{\cdot}1\ \mathrm{M}) \,\|\, \mathrm{Cd^{2+}}\,(0{\cdot}01) \,|\, \mathrm{Cd}$
Nernst Equation
10 $\mathrm{Cr} \,|\, \mathrm{Cr^{3+}}\,(0{\cdot}1\ \mathrm{M}) \,\|\, \mathrm{Fe^{2+}}\,(0{\cdot}01\ \mathrm{M}) \,|\, \mathrm{Fe}$
Nernst Equation
10 $\mathrm{Zn} \,|\, \mathrm{Zn^{2+}}\,(0{\cdot}001\ \mathrm{M}) \,\|\, \mathrm{H^{+}}\,(0{\cdot}01\ \mathrm{M}) \,|\, \mathrm{H_2}\,(\mathrm{g})\,(1\ \mathrm{bar}) \,|\, \mathrm{Pt}\,(\mathrm{s})$
Nernst Equation
11 $(\Delta_{\mathrm{r}}\mathrm{G}^{\circ})$
Nernst Equation
Oxidation-reduction reactions are commonly known as redox reactions. They involve transfer of electrons from one species to another. In a spontaneous reaction, energy is released which can be used to do useful work. The reaction is split into two half reactions. Two different containers are used and a wire is used to drive the electrons from one side to the other and a Voltaic/Galvanic cell is created. It is an electrochemical cell that uses spontaneous redox reactions to generate electricity. A salt bridge also connects to the half cells. The reading of the voltmeter gives the cell voltage or cell potential or electromotive force. If $\mathrm{E^{o}_{cell}}$ is positive the reaction is spontaneous and if it is negative the reaction is non-spontaneous and is referred to as electrolytic cell. Electrolysis refers to the decomposition of a substance by an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis. The conductance of material is the property of materials due to which a material allows the flow of ions through itself and thus conducts electricity. Conductivity is represented by k and it depends upon nature and concentration of electrolyte, temperature etc. A more common term molar conductivity of a solution at a given concentration is conductance of the volume of solution containing one mole of electrolyte kept between two electrodes with the unit area of cross-section and distance of unit length. Limiting molar conductivity of weak electrolytes cannot be obtained graphically.
12 (a) $Is silver plate the anode or cathode?$
Galvanic Cells
Oxidation-reduction reactions are commonly known as redox reactions. They involve transfer of electrons from one species to another. In a spontaneous reaction, energy is released which can be used to do useful work. The reaction is split into two half reactions. Two different containers are used and a wire is used to drive the electrons from one side to the other and a Voltaic/Galvanic cell is created. It is an electrochemical cell that uses spontaneous redox reactions to generate electricity. A salt bridge also connects to the half cells. The reading of the voltmeter gives the cell voltage or cell potential or electromotive force. If $\mathrm{E^{o}_{cell}}$ is positive the reaction is spontaneous and if it is negative the reaction is non-spontaneous and is referred to as electrolytic cell. Electrolysis refers to the decomposition of a substance by an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis. The conductance of material is the property of materials due to which a material allows the flow of ions through itself and thus conducts electricity. Conductivity is represented by k and it depends upon nature and concentration of electrolyte, temperature etc. A more common term molar conductivity of a solution at a given concentration is conductance of the volume of solution containing one mole of electrolyte kept between two electrodes with the unit area of cross-section and distance of unit length. Limiting molar conductivity of weak electrolytes cannot be obtained graphically.
12 (b) $What will happen if the salt bridge is removed?$
Galvanic Cells
Oxidation-reduction reactions are commonly known as redox reactions. They involve transfer of electrons from one species to another. In a spontaneous reaction, energy is released which can be used to do useful work. The reaction is split into two half reactions. Two different containers are used and a wire is used to drive the electrons from one side to the other and a Voltaic/Galvanic cell is created. It is an electrochemical cell that uses spontaneous redox reactions to generate electricity. A salt bridge also connects to the half cells. The reading of the voltmeter gives the cell voltage or cell potential or electromotive force. If $\mathrm{E^{o}_{cell}}$ is positive the reaction is spontaneous and if it is negative the reaction is non-spontaneous and is referred to as electrolytic cell. Electrolysis refers to the decomposition of a substance by an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis. The conductance of material is the property of materials due to which a material allows the flow of ions through itself and thus conducts electricity. Conductivity is represented by k and it depends upon nature and concentration of electrolyte, temperature etc. A more common term molar conductivity of a solution at a given concentration is conductance of the volume of solution containing one mole of electrolyte kept between two electrodes with the unit area of cross-section and distance of unit length. Limiting molar conductivity of weak electrolytes cannot be obtained graphically.
12 (c) $When does electrochemical cell behaves like an electrolytic cell?$
Electrolytic Cells and Electrolysis
Oxidation-reduction reactions are commonly known as redox reactions. They involve transfer of electrons from one species to another. In a spontaneous reaction, energy is released which can be used to do useful work. The reaction is split into two half reactions. Two different containers are used and a wire is used to drive the electrons from one side to the other and a Voltaic/Galvanic cell is created. It is an electrochemical cell that uses spontaneous redox reactions to generate electricity. A salt bridge also connects to the half cells. The reading of the voltmeter gives the cell voltage or cell potential or electromotive force. If $\mathrm{E^{o}_{cell}}$ is positive the reaction is spontaneous and if it is negative the reaction is non-spontaneous and is referred to as electrolytic cell. Electrolysis refers to the decomposition of a substance by an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis. The conductance of material is the property of materials due to which a material allows the flow of ions through itself and thus conducts electricity. Conductivity is represented by k and it depends upon nature and concentration of electrolyte, temperature etc. A more common term molar conductivity of a solution at a given concentration is conductance of the volume of solution containing one mole of electrolyte kept between two electrodes with the unit area of cross-section and distance of unit length. Limiting molar conductivity of weak electrolytes cannot be obtained graphically.
12 (d) $\mathrm{Zn^{2+}}$
Nernst Equation
Oxidation-reduction reactions are commonly known as redox reactions. They involve transfer of electrons from one species to another. In a spontaneous reaction, energy is released which can be used to do useful work. The reaction is split into two half reactions. Two different containers are used and a wire is used to drive the electrons from one side to the other and a Voltaic/Galvanic cell is created. It is an electrochemical cell that uses spontaneous redox reactions to generate electricity. A salt bridge also connects to the half cells. The reading of the voltmeter gives the cell voltage or cell potential or electromotive force. If $\mathrm{E^{o}_{cell}}$ is positive the reaction is spontaneous and if it is negative the reaction is non-spontaneous and is referred to as electrolytic cell. Electrolysis refers to the decomposition of a substance by an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as $\mathrm{Cu^{2+}}$ . This was first formulated by Faraday in the form of laws of electrolysis. The conductance of material is the property of materials due to which a material allows the flow of ions through itself and thus conducts electricity. Conductivity is represented by k and it depends upon nature and concentration of electrolyte, temperature etc. A more common term molar conductivity of a solution at a given concentration is conductance of the volume of solution containing one mole of electrolyte kept between two electrodes with the unit area of cross-section and distance of unit length. Limiting molar conductivity of weak electrolytes cannot be obtained graphically.
12 (d) $\mathrm{cm^2\,mol^{-1}}$
Conductance of Electrolytic Solutions

The 10 board questions to practise first

The questions the board asked again come first, most asked first. Each one says how often and when.

Question 1
Asked 2 times: 2024, 2026
5 $\mathrm{CuCl_2}$
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Question 2
Asked 2 times: 2022, 2026
23 $\Lambda_m^{o}$
Question 3
Asked 2 times: 2024, 2026
23 $\mathrm{Sn} \mid \mathrm{Sn^{2+}}\ (0.001\ \mathrm{M}) \parallel \mathrm{H^{+}}\ (0.01\ \mathrm{M}) \mid \mathrm{H_{2(g)}}\ (1\ \mathrm{bar}) \mid \mathrm{Pt_{(s)}}$
Question 4
Asked 2 times: 2022*, 2026 (* = numbers or wording changed that year)
22 $\mathrm{Cr\,(s)} \mid \mathrm{Cr^{3+}(aq)}\ (0{\cdot}1\ \mathrm{M}) \parallel \mathrm{Fe^{2+}(aq)}\ (0{\cdot}01\ \mathrm{M}) \mid \mathrm{Fe\,(s)}$
Question 5
Asked 2 times: 2025*, 2026 (* = numbers or wording changed that year)
22 $\mathrm{Al\,(s)} \mid \mathrm{Al^{3+}(aq)}\ (0{\cdot}1\ \mathrm{M}) \parallel \mathrm{Ni^{2+}(aq)}\ (0{\cdot}01\ \mathrm{M}) \mid \mathrm{Ni\,(s)}$
Question 6
Asked 2 times: 2022*, 2026 (* = numbers or wording changed that year)
22 $\mathrm{Zn\,(s)} \mid \mathrm{Zn^{2+}(aq)}\ (0{\cdot}1\ \mathrm{M}) \parallel \mathrm{Ag^{+}(aq)}\ (0{\cdot}01\ \mathrm{M}) \mid \mathrm{Ag\,(s)}$
Question 7
Asked 2 times: 2023, 2025
11 $\mathrm{MnO_4^{-}}$
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Question 8
Asked 2 times: 2023, 2025
3 $\Lambda_m = \Lambda_m^{\circ} - \mathrm{A}\sqrt{\mathrm{C}}$
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Question 9
Asked 2 times: 2023, 2025
11 $Match the type of cell given in Column I with their use given in Column II. Column I Column II i. Lead storage cell a. Wall clock ii. Mercury cell b. Apollo Space Programme iii. Dry cell c. Wrist watch iv. Fuel cell d. Inverter$
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Question 10
Asked 2 times: 2023, 2025
19 $Define fuel cell. Give two advantages of fuel cell over ordinary cell.$

Worked Examples

Solved Examples

Intext Questions

Exercises

What the board has asked from this chapter

2026

2025

2024

2023

2022

The 10 board questions to practise first

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

Question 9

Question 10