Class 12 Chemistry Ch-3 Electrochemistry MCQs Exam 2027

Unit: Electrochemistry

Topic 1: Faraday’s Laws & Electrolysis

1. 96500 Coulombs of electricity releases how much copper from a $CuSO_4$ solution? [BSEB, 2026]

(A) 63.5g Cu

(B) 31.75g Cu

(C) 96500 g Cu

(D) 100 g Cu

2. The electric charge required for reducing one mole of $Al^{3+}$ to Al is: [BSEB, 2026]

(A) $1 \times 10^5 \text{ C}$

(B) $3.0 \times 10^5 \text{ C}$

(C) $2.89 \times 10^5 \text{ C}$

(D) $9.65 \times 10^4 \text{ C}$

3. The amount of substance deposited by passing one Faraday of electricity is equal to: [BSEB, 2026]

(A) One gram equivalent

(B) One gram mole

(C) Electrochemical equivalent

(D) Half gram equivalent

4. Faraday’s second law of electrolysis is related to: [BSEB, 2026]

(A) Atomic number of the cation

(B) Equivalent weight of the electrolyte

(C) Atomic number of the anion

(D) Velocity of the cation

5. In electrolysis, oxidation occurs at: [BSEB, 2026]

(A) Anode

(B) Cathode

(C) Both Anode and Cathode

(D) Depends on the electrolyte used

6. Which of the following is released at the cathode during the electrolysis of aqueous NaCl solution? [BSEB, 2026]

(A) Chlorine

(B) Sodium

(C) Sodium amalgam

(D) Hydrogen

7. How much electricity is required to release 32 g of Oxygen? [BSEB, 2026]

(A) 1 Faraday

(B) 2 Faraday

(C) 3 Faraday

(D) 4 Faraday

8. What is the value of one Faraday (1 F) of electricity? [BSEB, 2026]

(A) 96,500 Ampere

(B) 96,500 Coulomb

(C) 96,500 Volt

(D) 96,500 Newton

9. Which of the following equations represents Faraday’s first law of electrolysis? [BSEB, 2026]

(A) $mz = c \cdot t$

(B) $m = z \cdot c \cdot t$

(C) $mc = z \cdot t$

(D) $c = m \cdot z \cdot t$

10. The unit of electrochemical equivalent is: [BSEB, 2026]

(A) gram/Coulomb

(B) gram/Ampere

(C) gram/Coulomb/gram

(D) Coulomb/gram

11. During the electrolysis of molten NaCl, what is released at the cathode? [BSEB, 2026]

(A) Chlorine

(B) Sodium

(C) Sodium amalgam

(D) Hydrogen

12. The amount of electricity required to deposit 108 g of silver from a silver nitrate solution is: [BSEB, 2026]

(A) 1 Faraday

(B) 1 Ampere

(C) 1 Coulomb

(D) 2 Faraday

13. The laws of electrolysis were given by: [BSEB, 2026]

(A) Lamarck

(B) Ostwald

(C) Faraday

(D) Arrhenius

14. When one Faraday of electricity is passed, the mass deposited is equal to: [BSEB, 2026]

(A) One gram mole

(B) Electrochemical equivalent

(C) Chemical equivalent

(D) Half gram equivalent

15. The unit of Faraday is: [BSEB, 2026]

(A) Ampere

(B) C

(C) $C \cdot mol^{-1}$

(D) $C \cdot sec^{-1}$

16. The amount of ions deposited in electrolysis does not depend on: [BSEB, 2026]

(A) Resistance

(B) Time

(C) Electrochemical equivalent

(D) Electric current

17. Which gas is released at the anode during the electrolysis of water? [BSEB, 2026]

(A) $H_2$

(B) $SO_2$

(C) $O_2$

(D) $Cl_2$

18. Charge required to convert 1 mole of $Al^{3+}$ to Al is: [BSEB, 2026]

(A) $3F$

(B) $1F$

(C) $2F$

(D) $96500 C$

19. Faraday’s first law is: [BSEB, 2026]

(A) $m = ect$

(B) $m = Zit$

(C) $m = Ze$

(D) $E = mc^2$

20. In an electrolytic cell, electrons enter through: [BSEB, 2026]

(A) Anode

(B) Cathode

(C) Solution

(D) Anywhere

21. Faraday required to deposit 2 moles of Copper from a $Cu^{2+}$ solution is: [BSEB, 2026]

(A) 2

(B) 4

(C) 1

(D) 3

22. Flow of current in an electrolyte solution is due to: [BSEB, 2026]

(A) Electrons

(B) Ions

(C) Atoms

(D) Molecules

23. The accurate value of Faraday constant ($F$) is approximately: [BSEB, 2026]

(A) 96500 C

(B) 96485 C

(C) 96000 C

(D) 97000 C

24. One Coulomb of charge is equal to: [BSEB, 2026]

(A) $6.24 \times 10^{18}$ electrons

(B) $1.6 \times 10^{-19}$ electrons

(C) 1 Ampere

(D) 96500 electrons

25. For the reaction $Zn^{2+} + 2e^- \to Zn$, how many Faradays are required? [BSEB, 2026]

(A) 1 F

(B) 2 F

(C) 0.5 F

(D) 4 F

Topic 2: Conductance & Molar Conductivity

26. The formula for calculating molar conductivity is: [BSEB, 2026]

(A) $\Lambda_m = \frac{\kappa \times 1000}{C}$

(B) $\Lambda_m = \frac{\kappa \times C}{1000}$

(C) $\Lambda_m = \kappa \times C$

(D) $\Lambda_m = \frac{1000}{\kappa \times C}$

27. The unit of cell constant is: [BSEB, 2026]

(A) $ohm^{-1}$

(B) $cm$

(C) $cm^{-1}$

(D) $ohm \cdot cm$

28. The unit of specific conductance is: [BSEB, 2026]

(A) $ohm \cdot cm^{-1}$

(B) $ohm \cdot cm^{-2}$

(C) $ohm^{-1} \cdot cm^{-1}$

(D) $ohm^{-1} \cdot cm^{-2}$

29. The unit of molar conductivity of a solution is: [BSEB, 2026]

(A) $ohm^{-1} \cdot cm^2 \cdot mol^{-1}$

(B) $ohm \cdot cm^2 \cdot mol^{-1}$

(C) $ohm^{-1} \cdot cm \cdot mol^{-1}$

(D) $ohm \cdot cm \cdot mol^{-1}$

30. On increasing dilution, the specific conductance of an electrolyte solution: [BSEB, 2026]

(A) Increases

(B) Decreases

(C) Remains constant

(D) None of these

31. The cell constant of a conductivity cell is: [BSEB, 2026]

(A) $\frac{l}{A}$

(B) $\frac{a}{l}$

(C) $a \times l$

(D) $a + l$

32. The unit of conductivity is: [BSEB, 2026]

(A) $ohm^{-1} \cdot cm^{-1}$

(B) $ohm \cdot cm^{-2}$

(C) $ohm^{-1} \cdot cm$

(D) $ohm^{-1} \cdot cm^{-2}$

33. On increasing the temperature, the conductivity of an electrolyte: [BSEB, 2026]

(A) Increases

(B) Decreases

(C) Remains unchanged

(D) None of these

34. The unit of specific resistance is: [BSEB, 2026]

(A) $ohm^{-1}$

(B) $ohm^{-1} \cdot cm^{-1}$

(C) ohm cm

(D) ohm cm$^{-1}$

35. Kohlrausch’s law is: [BSEB, 2026]

(A) $\lambda_m^\infty = \lambda_+^\infty + \lambda_-^\infty$

(B) $\lambda_m^\infty = \lambda_+^\infty – \lambda_-^\infty$

(C) $\lambda_m^\infty = \lambda_+^\infty \cdot \lambda_-^\infty$

(D) None of these

36. The relation between molar conductivity ($\Lambda_m$) and specific conductivity ($\kappa$) is: [BSEB, 2026]

(A) $\Lambda_m = \kappa \times V$

(B) $\Lambda_m = \frac{\kappa}{V}$

(C) $\Lambda_m = \frac{V}{\kappa}$

(D) $\Lambda_m = \kappa + V$

37. The conductivity of a solution is proportional to: [BSEB, 2026]

(A) Dilution

(B) Number of ions

(C) Volume of solution

(D) Current density

38. When electric current flows through a conductor via electrons, the conductor is called: [BSEB, 2026]

(A) Metallic conductor

(B) Electrolytic conductor

(C) Insulator

(D) None of these

39. Strong electrolytes are those which: [BSEB, 2026]

(A) Dissolve quickly in water

(B) Conduct electricity

(C) Dissociate into ions at high dilution

(D) Dissociate into ions at all dilutions

40. $ohm^{-1}$ is equal to: [BSEB, 2026]

(A) Siemens (S)

(B) Volt

(C) Ampere

(D) Coulomb

41. The reciprocal of specific conductivity is called: [BSEB, 2026]

(A) Conductivity

(B) Specific resistance

(C) Cell constant

(D) Resistance

42. On decreasing the concentration, molar conductivity: [BSEB, 2026]

(A) Increases

(B) Decreases

(C) Remains unchanged

(D) Becomes zero

43. The value of $\kappa$ is maximum for: [BSEB, 2026]

(A) Metals

(B) Insulators

(C) Semiconductors

(D) Solutions

44. What will be the unit of cell constant ($l/A$) in $m$? [BSEB, 2026]

(A) $m$

(B) $m^{-1}$

(C) $m^2$

(D) $m^{-2}$

45. Siemens (S) is the unit of: [BSEB, 2026]

(A) Resistance

(B) Conductance

(C) Specific resistance

(D) Potential

46. Kohlrausch law is useful for weak electrolytes to: [BSEB, 2026]

(A) Determine $\Lambda_m^\infty$

(B) Determine degree of dissociation

(C) Both (A) and (B)

(D) None of these

47. Conductivity of an electrolyte depends on: [BSEB, 2026]

(A) Concentration of ions

(B) Mobility of ions

(C) Nature of solvent

(D) All of the above

48. Molar conductivity of an electrolyte at infinite dilution is: [BSEB, 2026]

(A) Zero

(B) Maximum

(C) Minimum

(D) Constant

49. The SI unit of resistivity is: [BSEB, 2026]

(A) $\Omega \cdot m$

(B) $\Omega/m$

(C) $\Omega$

(D) $S/m$

50. Which of the following equations represents Kohlrausch law? [BSEB, 2026]

(A) $\Lambda_m = \kappa/C$

(B) $\Lambda_m^\infty = \Sigma \nu \lambda^\infty$

(C) $E = E^\circ – 0.059/n \log Q$

(D) $PV = nRT$

Topic 3: Galvanic Cells, EMF & Nernst Equation

51. The cell reaction occurring in a Daniell cell is: [BSEB, 2026]

(A) $Zn + Cu^{2+} \to Zn^{2+} + Cu$

(B) $Zn^{2+} + Cu \to Zn + Cu^{2+}$

(C) $Zn + Cu \to Zn^{2+} + Cu^{2+}$

(D) None of these

52. In a galvanic cell, the anode is: [BSEB, 2026]

(A) Negative electrode

(B) Positive electrode

(C) Neutral electrode

(D) None of these

53. The EMF of the cell $Zn | ZnSO_4 || CuSO_4 | Cu$ is 1.1 V. Its cathode is: [BSEB, 2026]

(A) $Zn$

(B) $Cu$

(C) $ZnSO_4$

(D) $CuSO_4$

54. At equilibrium of a cell reaction, the EMF of the cell is: [BSEB, 2026]

(A) Positive

(B) Zero

(C) Negative

(D) None of these

55. $Zn(s) | Zn^{2+}(aq) || Cu^{2+}(aq) | Cu(s)$ is: [BSEB, 2026]

(A) Weston cell

(B) Daniell cell

(C) Calomel cell

(D) None of these

56. According to Nernst equation, electrode potential depends on: [BSEB, 2026]

(A) Nature of metal

(B) Concentration of ions in solution

(C) Temperature

(D) All of the above

57. If the standard oxidation potential of an electrode is +0.763 V, its standard reduction potential will be: [BSEB, 2026]

(A) +0.763 V

(B) -0.763 V

(C) 0.00 V

(D) None of these

58. A cell in which chemical energy is converted into electrical energy is called: [BSEB, 2026]

(A) Electrolytic cell

(B) Galvanic cell

(C) Conductivity cell

(D) All of the above

59. For the half-cell reactions $Zn^{2+} + 2e^- \to Zn$ ($E^\circ = -0.76 V$) and $Fe^{2+} + 2e^- \to Fe$ ($E^\circ = -0.41 V$), the EMF of the cell will be: [BSEB, 2026]

(A) -0.35 V

(B) +0.35 V

(C) +1.17 V

(D) -1.17 V

60. For the cell reaction $Zn + Cu^{2+} \to Zn^{2+} + Cu$, the value of $\Delta G^\circ$ will be: [BSEB, 2026]

(A) -212.3 kJ

(B) +212.3 kJ

(C) -110 kJ

(D) +110 kJ

61. The electrode used to measure standard electrode potential is: [BSEB, 2026]

(A) Calomel electrode

(B) Standard Hydrogen Electrode (SHE)

(C) Silver chloride electrode

(D) Glass electrode

62. Which is used in a Salt Bridge? [BSEB, 2026]

(A) $NaCl$

(B) $KNO_3$

(C) $ZnSO_4$

(D) $H_2O$

63. What is measured by a Potentiometer? [BSEB, 2026]

(A) Current

(B) Resistance

(C) EMF

(D) Power

64. In a galvanic cell, chemical energy is converted into: [BSEB, 2026]

(A) Light energy

(B) Electrical energy

(C) Potential energy

(D) Atomic energy

65. The potential of a Standard Hydrogen Electrode is: [BSEB, 2026]

(A) 1.1 V

(B) 0.0 V

(C) 1.0 V

(D) -1.0 V

66. The correct relation between $\Delta G^\circ$ and $E^\circ_{\text{cell}}$ is: [BSEB, 2026]

(A) $\Delta G^\circ = -nFE^\circ_{\text{cell}}$

(B) $\Delta G^\circ = nFE^\circ_{\text{cell}}$

(C) $\Delta G^\circ = RT \ln K$

(D) None of these

67. For a spontaneous reaction, $\Delta G$ should be: [BSEB, 2026]

(A) Positive

(B) Negative

(C) Zero

(D) Infinite

68. The relation between equilibrium constant ($K$) and $E^\circ_{\text{cell}}$ is: [BSEB, 2026]

(A) $E^\circ = \frac{0.059}{n} \log K$

(B) $E^\circ = -nFK$

(C) $K = e^{E^\circ}$

(D) $E^\circ = \log K$

69. The reaction occurring at the anode is called: [BSEB, 2026]

(A) Reduction

(B) Oxidation

(C) Neutralization

(D) Condensation

70. The reaction occurring at the cathode is called: [BSEB, 2026]

(A) Reduction

(B) Oxidation

(C) Ionization

(D) Hydrolysis

71. In the cell $Cu | Cu^{2+} || Ag^+ | Ag$, the anode is: [BSEB, 2026]

(A) $Ag$ electrode

(B) $Cu$ electrode

(C) $Ag^+$ solution

(D) Salt bridge

72. The value of cell potential ($E_{\text{cell}}$) does not depend on: [BSEB, 2026]

(A) Temperature

(B) Concentration

(C) Size of electrodes

(D) Nature of metal

73. The main function of a salt bridge is: [BSEB, 2026]

(A) To stop current

(B) To complete the circuit and maintain neutrality

(C) To increase oxidation

(D) To heat the cell

74. $KCl$ is filled in the salt bridge of a Daniell cell because: [BSEB, 2026]

(A) Velocity of $K^+$ is higher

(B) Velocity of $Cl^-$ is higher

(C) Velocities of both ions are nearly equal

(D) It is colored

75. In the formula $E_{\text{cell}} = E_{\text{cathode}} – E_{\text{anode}}$, the potentials should be: [BSEB, 2026]

(A) Oxidation potential

(B) Reduction potential

(C) Both different

(D) Any of these

Topic 4: Electrochemical Series & Redox Power

76. Which of the following is the strongest oxidizing agent? [BSEB, 2026]

(A) $I_2$

(B) $Br_2$

(C) $Cl_2$

(D) $F_2$

77. On moving down the electrochemical series, the reducing power of elements: [BSEB, 2026]

(A) Increases

(B) Decreases

(C) Remains constant

(D) Increases then decreases

78. Which of the following has the highest oxidation potential? [BSEB, 2026]

(A) $Zn$

(B) $Cu$

(C) $Ag$

(D) $Mg$

79. Standard reduction potentials of metals A, B, C, and D are -3.05, -1.66, -0.40, and +0.80 V respectively. Which metal has the highest reducing power? [BSEB, 2026]

(A) A

(B) B

(C) C

(D) D

80. In aqueous solution, which alkali metal has the highest standard reduction potential (most negative)? [BSEB, 2026]

(A) $Li$

(B) $Na$

(C) $K$

(D) $Cs$

81. Which of the following is the strongest reducing agent? [BSEB, 2026]

(A) $F_2$

(B) $Cl_2$

(C) $I_2$

(D) $Br_2$

82. The metal located at the top of the electrochemical series is: [BSEB, 2026]

(A) $Li$

(B) $Au$

(C) $Pt$

(D) $Ag$

83. Which of the following ions is the least powerful reducing agent? [BSEB, 2026]

(A) $F^-$

(B) $Cl^-$

(C) $Br^-$

(D) $I^-$

84. $Cu$ metal does not react with $HCl$ because: [BSEB, 2026]

(A) Its reduction potential is higher than $H$

(B) It is very expensive

(C) It is solid

(D) It is liquid

85. The strongest reducing agent is: [BSEB, 2026]

(A) $Li$

(B) $Na$

(C) $K$

(D) $Al$

86. The correct order of activity for metals $Zn, Fe, Cu, Ag$ is: [BSEB, 2026]

(A) $Zn > Fe > Cu > Ag$

(B) $Ag > Cu > Fe > Zn$

(C) $Fe > Zn > Ag > Cu$

(D) $Cu > Ag > Zn > Fe$

87. $CuSO_4$ solution cannot be kept in an iron vessel because: [BSEB, 2026]

(A) Iron is more reactive than $Cu$

(B) $Cu$ is more reactive than iron

(C) Both are equally reactive

(D) No reaction occurs

88. Which of the following metals can displace $H_2$ from water? [BSEB, 2026]

(A) $Na$

(B) $Ag$

(C) $Au$

(D) $Cu$

89. On increasing the standard reduction potential value, oxidizing power: [BSEB, 2026]

(A) Increases

(B) Decreases

(C) Remains constant

(D) Becomes zero

90. Among $Cl_2, Br_2, I_2, F_2$, the strongest oxidizing agent is: [BSEB, 2026]

(A) $F_2$

(B) $Cl_2$

(C) $Br_2$

(D) $I_2$

91. The electrochemical series is also known as: [BSEB, 2026]

(A) Activity series

(B) Passivity series

(C) Atomic series

(D) Periodic series

92. The standard reduction potential of $Zn$ is -0.76V, it means $Zn$ is: [BSEB, 2026]

(A) Anode

(B) Cathode

(C) More reactive than $H$

(D) Inert

93. Which metal does not give $H_2$ gas with dilute $H_2SO_4$? [BSEB, 2026]

(A) $Cu$

(B) $Mg$

(C) $Zn$

(D) $Al$

94. Who has the most negative electrode potential? [BSEB, 2026]

(A) $Li$

(B) $K$

(C) $Ca$

(D) $Ba$

95. The more positive the value of $E^\circ$, the element will be: [BSEB, 2026]

(A) Strong oxidizing agent

(B) Strong reducing agent

(C) Neutral

(D) Gas

96. The corrosion rate of metals depends on: [BSEB, 2026]

(A) Their position in the activity series

(B) Humidity

(C) Presence of air

(D) All of the above

97. Who is the strongest reducing agent among non-metals? [BSEB, 2026]

(A) $I^-$

(B) $Cl^-$

(C) $Br^-$

(D) $F^-$

98. For which of the following is the electrode potential set to 0.0V? [BSEB, 2026]

(A) $H_2$

(B) $O_2$

(C) $N_2$

(D) $Cl_2$

99. Metals located above $H$ in the electrochemical series: [BSEB, 2026]

(A) Displace $H_2$ from acids

(B) Do not displace $H_2$

(C) Are inert

(D) React only with water

100. Adding $Fe$ to $CuSO_4$ solution makes the blue color fade because: [BSEB, 2026]

(A) $Fe$ gets oxidized

(B) $Cu$ gets reduced

(C) $Fe$ displaces $Cu$

(D) All of the above

Topic 5: Types of Cells, Batteries & Corrosion

101. Which of the following is a secondary cell? [BSEB, 2026]

(A) Leclanché cell

(B) Lead storage battery

(C) Concentration cell

(D) All of the above

102. The best way to prevent the corrosion (rusting) of iron is: [BSEB, 2026]

(A) By making iron cathode

(B) By keeping it in saline water

(C) Both (A) and (B)

(D) None of these

103. Which cell converts the chemical energy of Hydrogen and Oxygen into electrical energy? [BSEB, 2026]

(A) Mercury cell

(B) Daniell cell

(C) Fuel cell

(D) Leclanché cell

104. Which substance is used as an electrolyte in a Mercury cell? [BSEB, 2026]

(A) $NH_4Cl + ZnCl_2$

(B) $KOH + ZnO$

(C) $H_2SO_4$

(D) $NaOH$

105. Rust is: [BSEB, 2026]

(A) Powdered iron

(B) Ferrous oxide

(C) Ferric oxide

(D) Hydrated ferric oxide

106. When a lead storage cell is charged, what happens? [BSEB, 2026]

(A) Lead dioxide dissolves

(B) $H_2SO_4$ is regenerated

(C) Lead sulfate deposits on lead electrode

(D) Concentration of sulfuric acid decreases

107. Which metal coating is most suitable to prevent rusting of iron? [BSEB, 2026]

(A) $Cu$

(B) $Pb$

(C) $Zn$

(D) $Sn$

108. An example of a primary cell is: [BSEB, 2026]

(A) Dry cell

(B) Mercury cell

(C) Both (A) and (B)

(D) Nickel-Cadmium cell

109. The main factor affecting corrosion is: [BSEB, 2026]

(A) Reactivity of metal

(B) Air and moisture

(C) Impurities in metal

(D) All of the above

110. The efficiency of a Fuel Cell is: [BSEB, 2026]

(A) 40%

(B) 100%

(C) 70-75%

(D) 10%

111. In a dry cell, the anode is made of: [BSEB, 2026]

(A) Zinc (Zn)

(B) Carbon (C)

(C) Copper (Cu)

(D) Iron (Fe)

112. In a dry cell, the cathode is made of: [BSEB, 2026]

(A) Zinc

(B) Graphite (Carbon) rod

(C) Nickel

(D) Lead

113. The concentration of acid used in a lead storage battery is: [BSEB, 2026]

(A) 10% $H_2SO_4$

(B) 38% $H_2SO_4$

(C) 100% $H_2SO_4$

(D) 38% $HCl$

114. Nickel-Cadmium cell is a: [BSEB, 2026]

(A) Primary cell

(B) Secondary cell

(C) Fuel cell

(D) Inert cell

115. The cell used in the Apollo mission was: [BSEB, 2026]

(A) Dry cell

(B) Fuel cell ($H_2-O_2$)

(C) Mercury cell

(D) Daniell cell

116. Which cell is also known as a Button Cell? [BSEB, 2026]

(A) Dry cell

(B) Mercury cell

(C) Lead cell

(D) Fuel cell

117. The metal used in Galvanization is: [BSEB, 2026]

(A) $Zn$

(B) $Sn$

(C) $Pb$

(D) $Cu$

118. In the chemical process of rusting, iron acts as: [BSEB, 2026]

(A) Anode

(B) Cathode

(C) Electrolyte

(D) Insulator

119. The pH required for rusting of iron is: [BSEB, 2026]

(A) Acidic medium

(B) Highly alkaline

(C) Neutral

(D) Any of these

120. Corrosion is a type of process: [BSEB, 2026]

(A) Redox

(B) Only oxidation

(C) Only reduction

(D) Thermal

121. Secondary cells are also called: [BSEB, 2026]

(A) Storage cells

(B) Voltaic cells

(C) Primary cells

(D) Mercury cells

122. During discharge in a lead storage cell, what is formed? [BSEB, 2026]

(A) $PbSO_4$

(B) $PbO_2$

(C) $Pb$

(D) $H_2SO_4$

123. Fuel cells are used in spacecraft because: [BSEB, 2026]

(A) They have low weight

(B) They are pollution-free

(C) They provide water

(D) All of the above

124. What is used in sacrificial protection to prevent corrosion of iron? [BSEB, 2026]

(A) $Mg$ or $Zn$

(B) $Cu$ or $Ag$

(C) $Pt$

(D) $Au$

125. Primary cells: [BSEB, 2026]

(A) Can be recharged

(B) Cannot be recharged

(C) Can be recharged by heating

(D) Can be recharged by adding water

Topic 6: Miscellaneous Questions

126. Who gave the theory of ionization? [BSEB, 2026]

(A) Faraday

(B) Arrhenius

(C) Ostwald

(D) Rutherford

127. The movement of colloidal particles under the influence of an electric field is called: [BSEB, 2026]

(A) Dialysis

(B) Tyndall effect

(C) Emulsion

(D) Electrophoresis

128. Products obtained at the anode and cathode on electrolysis of aqueous Sodium Fluoride are: [BSEB, 2026]

(A) $F_2, Na$

(B) $F_2, H_2$

(C) $O_2, Na$

(D) $O_2, H_2$

129. In aqueous solution, Hydrogen ($H_2$) will not reduce: [BSEB, 2026]

(A) $Fe^{3+}$

(B) $Cu^{2+}$

(C) $Au^{2+}$

(D) $Ag^+$

130. The charge on an electron is: [BSEB, 2026]

(A) $4.8 \times 10^{-10} \text{ esu}$

(B) $1.6 \times 10^{-19} \text{ C}$

(C) $4.8 \times 10^{-10} \text{ a.m.u.}$

(D) $1.5 \times 10^{-11} \text{ a.m.u.}$

131. An electrolyte: [BSEB, 2026]

(A) Forms complex ions in solution

(B) Gives ions only when electricity is passed

(C) Keeps ions even in solid state

(D) Gives ions only when dissolved in water

132. Which of the following is an insulator? [BSEB, 2026]

(A) Graphite

(B) Aluminum

(C) Diamond

(D) Silicon

133. Electricity is conducted in a solution by: [BSEB, 2026]

(A) Electrolytes

(B) Non-electrolytes

(C) $H_2O$ molecules

(D) Copper wires

134. Which of the following metals is not obtained by electrolysis? [BSEB, 2026]

(A) $Na$

(B) $Mg$

(C) $Al$

(D) $Fe$

135. For a redox reaction to occur in a cell, the EMF of the cell must be: [BSEB, 2026]

(A) Positive

(B) Negative

(C) Constant

(D) Zero

136. The electrode through which electrons enter the solution in an electrolytic cell is called: [BSEB, 2026]

(A) Cathode

(B) Anode

(C) Either anode or cathode

(D) None of these

137. The conductivity of pure water is: [BSEB, 2026]

(A) Very high

(B) Zero

(C) Very low

(D) Infinite

138. Ohm’s law applies to: [BSEB, 2026]

(A) Metallic conductors

(B) Electrolytes

(C) Both (A) and (B)

(D) Insulators

139. Aqueous solution of $KCl$ is a good conductor because it contains: [BSEB, 2026]

(A) Free electrons

(B) Free ions

(C) Free molecules

(D) Atoms

140. What is the unit of Faraday Constant ($F$)? [BSEB, 2026]

(A) Coulomb

(B) Coulomb/mole

(C) Ampere/second

(D) Joule/Volt