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Chemistry Electro Chemistry Online Mcqs Test

Malik TahirLast Updated: October 14, 2025

Important Electro Chemistry Question and Answer

Total Questions:	192
Time Allowed:	60 Minutes
Total Marks:	192
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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Electro Chemistry Practice Test Online With Explanation

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Page 1 of 8

Chemistry

1. The molality of 2% NaCl. W/W solution is approximately

0.05

0.25

0.5

2.05

2. The strength of solution an element whose electrode potential is to be measured

2 M

1 M

1 f

1 N

3. Salt bridge transfers

Electrons

Current

Solvent particles

Anions

4. The number of coulombs required for the deposition of 107.870 g of silver is

193000

10000

96500

48250

5. Alkaline battery has a voltage of

4.5V

2.5V

3.5V

1.5V

6. When Cu, Ag, Au and Pt are reacted with acids, these metals do not liberate hydrogen, this is due to the reason that

Reduction potentials are negative

Very low ionization potential values

Very high negative values reduction potential

Very high positive value of reduction potential

7. Maximum freezing point falls in

Water

Benzene

Naphthalene

Camphor

8. Reduction always occurs

At anode

None of these

At cathode

Both A and B

9. Stronger the oxidizing agent, greater is the

e.m.f of cell

Oxidation potential

Redox potential

Reduction potential

10. A dry alkaline cell has porous Zn anode & MnO₂ as cathode the electrolyte used is

KOH

NH₄OH

NaOH

Ca(OH)₂

11. Which of the following is the use of electrolysis?

None of these

Electroplating

Both A and B

Electrorefining

12. In an electrolytic cell current flows

From cathode to anode in outer circuit

From anode to cathode inside the cell

From cathode to anode inside the cell

From anode to cathode in an outer circuit

13. The + 1 oxidation state of P is found in

H₃PO₄

H₃PO₃

H₄P₃O₇

H₃PO₂

14. In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to

Generate heat

Remove adsorbed oxygen from electrode surfaces

Produce high purity water

Create potential difference between two electrodes

15. The specific conductance of a 0.1 N KCl solution at 23°C is 0.012 ohm¯¹ cm¯¹. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be

1.12 cm¯¹

0.142 cm¯¹

0.918 cm¯¹

0.66 cm¯¹

16. Which of the following solution of H₂SO₄ is more concentrated?

All

1 molar

1 normal

1 molal

17. Under the process of rusting of iron, 4Fe + 3O₂ → 2Fe₂O₃, iron is

Reduced

Oxidized

Hydrolyzed

Precipitated

18. A cell constant is generally found by measuring the conductivity of aqueous solution of

NaCl

KCl

MgCl₂

BaCl₂

19. When molten sodium undergoes electrolysis, the ion reduces is

Both Na⁺ and CI¯

Cl¯

None of these

Na⁺

20. Sea water has 5.65 x 10¯³ g of dissolved oxygen calculate the conclusion of oxygen in sea water in ppx

5.65

6.1

1.32

5.51

21. The depression of freezing point is directly proportional to

Mole fraction of the solution

Molarity of the solvent

Molarity of the solution

Molality of the solution

22. Corrosion reactions are

Spontaneous acid–base reactions

None of these

Non-spontaneous redox reactions

Spontaneous redox reactions

23. Vant Hoff’s factor of Ca(NO₃)₂ is

24. 96500 C of electricity liberates from CuSO₄ solution

96500 g of CU

31.75 g of Cu

63.5 g of Cu

100 g of Cu

25. Colligative properties are the properties of

Dilute solution which behave as nearly ideal solution

Neither a nor b

Both a and b

Concentration solutions behave as nearly non – ideal solutions

Page 2 of 8

26. An electric current is passed through silver nitrate solution using silver electrodes. 10.79 g of silver was found to be deposited on the cathode if the same amount of electricity is passed through copper sulphate solution using copper electrodes, the weight of copper deposited on the cathode is

12.8 g

6.4 g

2.3 g

3.2 g

27. A 20% solution of NaCl by weight means that

10.0g NaCl/100ml

20g NaCl/100ml

5.58g NaCl/100m

58.5g NaCl/100ml

28. A certain current liberate 0.5 g of hydrogen in 2 h. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution?

12.7 gm

15.9 gm

63.5 gm

31.8 gm

29. When the solute is present in trace quantities the following expression is used?

Parts per million

Milligram percent

Microgram percent

Gram per million

30. The substance having highest conductivity at room temperature among the following is

0.1 N NaCl

Glass

Graphite

0.1 N HCl

31. After adding a solute freezing point of solvent decreases to -0.186. Calculate ∆ Tb if Kf = 1.86 and Kb = 0.521

0.521

1.86

0.0521

0.0186

32. The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25°C. The equilibrium constant of the reaction would be

1.0 x 10¹⁰

1.0 x 10²

4.0 x 10¹²

2.0 x 10¹¹

33. Molton NaCl conducts electricity due to the presence of

Free electrons

Atoms of Na and Cl.

Free ions

Free molecules

34. The temperature at which the vapour pressure of a liquid becomes equal to external pressure is

Melting point

Inversion point

Boiling point

Sublimation point

35. The molarity of the solution containing x grams (NH₄)SO₄ in 500 cm³ of the solution is 0.6. What is x

42.7

45.1

40.5

39.6

36. A cell in which chemical energy is converted into electrical energy is called

Galvanic cell

Electrolytic cell

Fuel cell

Dry cell

37. It azeotropic mixture showing positive deviation from Rault’s law, the volume of the mixture is

None of these

Slightly more than the total volume of the components

Equal to the total volume of the components

Slightly less than the total volume of the components

38. If the ionic product of a solution is less than the solubility product, the solution is

Saturated

Ideal

Unsaturated

Supersaturated

39. The reference electrode is made by using

CuSO₄

ZnCl₂

HgCl₂

Hg₂Cl₂

40. Pure water does not conduct electricity because it

Is neutral

Is readily decomposed

Is almost unionized

Has low boiling point

41. A redox reaction involves

Ion combination reaction

A reaction in a solution

Proton transfer

Electron transfer

42. If 5.85 g of NaCl are dissolved in 90 g of water, the mole fraction of NaCl is

0.1

0.0196

0.2

0.01

43. Best way to prevent rusting iron is by

Putting it in saline water

Making iron cathode

Both of these

None of these

44. The ionic strength of a solution containing 0.1 mole/kg of KCl and 0.2 mole/kg of CuSO₄ is

0.6

0.2

0.9

0.3

45. Cathode provides electrons to

Neutral atom

Does not provide any electron

+Ve ion

-Ve ion

46. In a Galvanic cell, the electrons flow from

Anode to cathode through the external circuit

Anode to cathode through the solution

Cathode to anode through the solution

Cathode to anode through the external circuit

47. What is the molality of a solution prepared by dissolving 5 g of toluene in 250 g of Benzene.

0.217

4.10

3.12

7.20

48. Oxidation in a chemical reaction involves

Increase in oxidation number of all the elements on reactant side

Both are possible

Increase in oxidation number

Decrease in oxidation number

49. When common salt is dissolved in water

B.P of water remain constant

Any possibility

B.P of water decrease

B.P of water increase

50. Which of the statements given below concerning properties of solution, describe a colligaive effect?

Boiling point of pure benzene increases by the addition of toluene

Vapour pressure of pure water decreases by the addition of nitric acid

Boiling point of pure water decreases by the addition of ethanol

Vapour pressure of pure benzene decreases by the addition of naphthalene

Page 3 of 8

51. Pick out the wrong statement. In electrochemical cell

Salt bridge maintains the electrical neutrality of the solution

Cathode is regarded as negative electrode

Electrons are released at anode

Chemical energy is converted into electrical energy

52. Temperature for standard electrode potential is

300 K

310 K

273 K

25 C°

53. For spontaneity of a cell, which is correct?

∆ G = -ve

∆ G = 0, ∆E = 0

∆ G = +ve, ∆ E = 0

∆ G = -ve, ∆ E = 0

54. The Vant Hoff factor (i) accounts for

The extent of dissolution of solute

Degree of solubilization of solute

The extent of dissociation of solute

The degree of decomposition of solution

55. Which one of the following substance when dissolved in water give acidic solution

NH₄Cl

Na₂SO₄

CH₃ CooNH₄

NaCl

56. The equivalent conductivity of 0.1 M week acid is 100 times less than that at infinite dilution. The degree of dissociation is

0.01

100

0.001

57. The art of electroplating was given by

Brugan

Faraday

Edison

Thomas Gradam

58. Standard hydrogen electrode has an arbitrarily fixed potential

0.10 volt

None of these

1.00 volt

0.00 volt

59. A smuggler could not carry gold by chemically depositing iron on the gold surface since

Gold is denser

Gold has lower reduction potential then iron

Gold has higher reduction potential then iron

Iron rusts

60. At room temperature, the mole fraction of a solution in 0.25 and the vapour pressure of the solvent is 0.80 atm. Then the lowering of vapour pressure is

0.75

0.20

0.60

0.80

61. Cathodic reaction in the electrolysis of dil. H₂SO₄ is always

Both

Oxidation

Reduction

62. Which of the following element act as inert electrode?

None

63. Molarity of water is

55.5

64. Density of H₂SO₄ in lead accumulator is

1.15 g/Cm³

1.2 g/Cm³

1.25g/Cm³

120 g Cm³

65. Decrease in oxidation number is called

Redox

All of these

Oxidation

Reduction

66. Which of the following (IM) conducts more electricity?

Nitric acid

Sulphuric acid

Phosphorus acid

Boric acid

67. Which oxide has +2 oxidation number of oxygen?

F₂O

Na₂O

Cl₂O

Na₂O₂

68. The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is:

Na → Na⁺ + e–

2Br– → Br₂ + 2e –

Na⁺ + e– → Na

Br₂ + 2e – → 2Br –

69. In galvanic cell Zn acts as an anode so its value of standard reduction potential in comparison to coupled electrode would be

Lesser

Greater

Sum of reduction and oxidation potentials

None

70. If the salt bridge is not used between two half cells, then the voltage

Does not change

Decreases slowly

Drops to zero

Decrease rapidly

71. Calculate the amount of charge flowing in 2 minute in a wire of resistance 10 Ω when a potential difference of 20 V is applied

120 C

240 C

4 C

20 C

72. The relative lowering of vapour pressure is equal to mole fraction of the solute. This law is called:

Raoult’s law

Henry’s law

Ostwald’s law

Arrhenius law

73. The weight of pure NaOH required to prepare 250 cm³ of 0.1 N solution is

2 g

5 g

4 g

1 g

74. Time required to deposit one millimole of aluminum metal by the passage of 9.65 amperes through molten electrolyte containing aluminum ion is

10,000 s

30,000 s

30 s

10 s

75. Corrosion is basically a

Interaction

Electrochemical phenomenon

Union between two light metals and a heavy metal

Altered reaction in presence of H₂O

Page 4 of 8

76. Strong reducing agents have

None of these

Greater positive value of standard reduction potential

Lesser positive value of standard reduction potential

Greater negative value of standard reduction potential

77. The standard EMF of Daniel cell is 1.10 volt. The maximum electrical work obtained from the Daniel cell is

106.15 kJ

212.3 kJ

175.4 kJ

53.07 kJ

78. An oxidizing agent in a chemical reaction in the substance which

Acts as a catalyst

pH is changed

Loses electrons

Gains electrons

79. Prevention of corrosion of iron by Zn coating is called

Photo electrolysis

Galvanization

Cathodic protection

Electrolysis

80. Wen quantity of electricity passed is one faraday then the mass deposited at the electrode is equal to

One gm. Equivalent weight

Electrochemical equivalent

None of these

One gm. atomic weight

81. Solution with same osmotic pressures are called

Isotonic

Hypertonic

Hypotonic

Normal

82. A solution of sodium sulphate was electrolyzed using some inert electrodes. The products at the electrodes are

O₂,H₂

None of these

O₂, Na

O₂, SO₂

83. Standard reduction electrode potential of three metals A, B and C are respectively + 0.05 V, - 3.0 and -1.2V. The reducing power of

B > C > A

A > C > B

C > B > A

A > B > C

84. In the electrolysis of molten sodium chloride, what is the yellow green gas formed?

Chloride

Oxygen

Hydrogen

Chlorine

85. The osmotic pressure of 1 m solution at 27°C is

24.6 atm

1.21 atm

12.1 atm

2.46 atm

86. Hydrogen gas is not liberated when the following metal is added to dil. HCI.

87. What will be the density of H₂SO₄ when lead accumulator is recharged?

2.15 cm¯³

1.81 cm¯³

1.25 cm¯³

1.15 cm¯³

88. The EMF of the cell rection Fe²⁺ + zn = Zn²⁺ + feis

+ 1.17 V

– 1.17 V

– 0.35 V

+ 0.35

89. An electric current is passed through silver voltmeter connected to a water voltmeter. The cathode of the silver voltammeter is 0.108 g more at the end of the electrolysis. The volume of oxygen evolved at STP is

550 cm³

5.6 cm³

56 cm³

11.2 cm³

90. Out of Cu, Ag, Fe and Zn the metal which can displace all others from their salt solutions is

91. Which one of the following is a colligative property?

Refractive index

Surface tension

Viscosity

Osmotic pressure

92. Chemical used in salt bridge is

KCI

KNO3

KOH

KBr

93. If the standard electrode potential of CU²⁺/Cu electrode is 0.34 V, what is the electrode potential of 0.01 M concentration of Cu²⁺? (T = 298 K)

0.222 V

0.176 V

0.281 V

0.399 V

94. What are the ions present in water?

H2 and O

H2O

H and OH

H+ and OH-

95. If 5.85 g of NaCl are dissolved in 90g of water, the mole fraction of NaCl is

0.01

0.1

0.2

0.0196

96. The number of moles of a solute in 500 cm³, 3M solution is

1.5

97. The reference calomel electrode is made from which of the following?

Hg₂Cl₂

HgCl₂

CuSO₄

ZnCl₂

98. 1.0 g of pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of HCl solution is given by

4 N

0.2 N

2 N

0.4 N

99. Anode electrode element always have _________ position in electrochemical series

Lower

Not particular

Higher

In middle

100. Azeotropic mixture of HCl and water has

20.2% HCl

22.2% HCl

36% HCl

48% HCl

Page 5 of 8

101. Which has maximum oxidation number

102. A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is monovalent. The atomic mass of the metal is

96.5

103. Oxidation state of hydrogen in CaH₂ is

-2

-1

104. What is the molarity of H₂SO₄ solution that has density of 1.84 gm/cm³ which was at 35°C and contains 98% by weight?

18 M

18.4 M

8.14 M

4.18 M

105. If a salt bridge is removed between the two half cells, the voltage

Drops to zero

Does not change

Increases rapidly

Increases gradually

106. The cathodic reaction in the electrolysis of dil. H₂SO₄ with Pt electrodes is

Oxidation

Neither oxidation and reduction

Reduction

Both oxidation and reduction

107. Mole fraction of pure water is

Exactly equal to one

Slightly less than one

None of these

Slightly greater than one

108. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

1.25

2.5

None of these

1 2

109. By means of fuel cells, chemical energy may be converted into

Electrical energy

Magnetic energy

Heat energy

Sound energy

110. Units of molarity are

Gm/lit

None of these

Mol/lit

Kg/lit

111. The specific conductance of 0.1 M NaCl solution is 1.06 x 10¯² ohm¯¹mol¯¹. Its molar conductance in ohm¯¹ cm² mol¯¹ is

1.06 x 10⁴

1.06 x 10³

1.06 x 10²

112. Equal volumes of ethylene glycol (molar mass = 62) and water (molar mass = 18) are mixed. The depression in freezing point of water is (given Kf of water 1.86 K mol¯¹ kg and specific gravity of ethylene glycol is 1.11)

0.333

33.3

3.33

0.0033

113. How much of NaOH is required to neutralize 1500 cm³ of 0.1 N HCl?

40 g

6 g

60 g

4 g

114. The pressure at which water boils at 101.5 °c is

750 torr

2.5 atom

Slightly more than 1 atom

760 mm of Hg

115. The osmotic pressure of a dilute solution is directly proportional to the

Ionic concentration

Elevation in boiling point

Flow of solvent from a concentrated to a dilute solution

Diffusion rate of the solute

116. Which substances are mixed to form a buffer solution?

Weak acid and its salt of strong base

Weak acid and its salt of weak base

Strong acid and its salt of weak base

A strong acid and its salt of a strong base

117. In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at cathode while with Hg cathode it forms sodium amalgam

More voltage is required to reduce H⁺ at Hg than at Pt

Hg is more inert than Pt

Conc. Of H⁺ ions is when Pt electrode is taken

Na is dissolved in Hg while it does not dissolve in Pt

118. Which of the following statements is FALSE?

Reduction occurs at cathode

All electrochemical reactions involve the transfer of electrons

Oxidation and reduction half-reactions occur at electrodes in electrochemical cells.

All voltaic (galvanic) cells involve the use of electricity to initiate nonspontaneous chemical reactions

119. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

0.1N

1 N

10 N

11 N

120. Which of these is not an application of electrolysis?

Electroplating

Manufacture of bleach

Rust removal

Making leather

121. When during electrolysis of a solution of AgNO₃, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

1.08 g

10.8 g

108 g

21.6 g

122. Which of the following statement is correct for electrolytic cell?

Electrons flow cathode to anode within the electrolytic solution

Migration of ions along with oxidation reaction at anode and reduction reaction at cathode

None of these

Electrons flow from cathode to anode through the external battery

123. The best reducing agent is

I¯

F¯

Br¯

Cl¯

124. The conductivity of strong electrolyte

Depends on density of electrolyte itself.

Does not change on dilution

Decreases on dilution

Increases on dilution slightly

125. Electricity in voltaic cell is produced due to

Neutralization

Reduction

Oxidation

B + C

Page 6 of 8

126. The volume of 0.1 M H₂SO₄ required to neutralize completely 40 ml of 0.2 M NaOH solution is

40 ml

80 ml

20 ml

10 ml

127. Calculate the percentage by weight if NaCl, if 2.0 g of NaCl is dissolved in 20g of water

13.1%

14.25%

9.09%

11.2%

128. Metals usually conduct electricity because

They are mobile electrons in the metallic structure

Metals have high resistance

In metals the ions are free to more

Metals are decomposed by current

129. A solution contains 1.2046 x 10²⁴ hydrochloric acid molecules in one dm³ of the solution. The strength of the solution is

2 N

6 N

4 N

8 N

130. The cryoscopic constant of water is 1.86. The elevation of B.P for a 0.1m solution of a solute in water is

18.6 c°

1.86 c°

0.186 c°

Sufficient date not given

131. The unit of specific conductivity is

Ohm¯¹ cm¯¹

Ohm cm¯¹

Ohm¯¹ cm

Ohm cm¯²

132. Partial pressure of a solution component is directly proportional to its mole fraction. This statement is known as

Raoult’s law

Ostwald’s dilution law

Distribution law

Henry’s law

133. An electrolyte

Gives ions only when dissolved in water

Gives ions only when electricity is passed

Forms complex ions in solution

Possesses ions even in solid state

134. H₂ gas in SHE is filled at a pressure of

800 mm of Hg

780 mm of Hg

760 mm of Hg

750 mm of Hg

135. Electrochemical series is a list of elements arranged into increasing order to either

Standard reduction potential

Cell voltage

Ionization potential

Standard oxidation potential

136. In electrolytic cell, electricity in carried out by

Neutralization

Spontaneous reaction

All

Non-spontaneous reaction

137. In a Galvanic cell

Electrical energy is converted into heat

Electrical energy is converted into chemical energy

Chemical energy is converted into heat

Chemical energy is converted into electricity

138. The limiting molar conductivities ʌ’ for NaCl, KBr and KCl are 126, 152 and 150 S cm² respectively. The ʌ’ for NaBr is

278 S cm² mol¯¹

128 S cm² mol¯¹

176 S cm² mol¯¹

302 S cm² mol¯¹

139. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.2 M

0.4 M

0.8 M

0.04 M

140. The vapour pressure of two liquids ‘P’ and ‘Q’ are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol of Q would be

20 torr

72 torr

68 torr

140 torr

141. A 0.001 molal solution of [Pt(NH₃)₄Cl₄] in water had a freezing point depression of 0.0054°C. If Kf for water is 1.80, the correct formulation for the above molecule is

[Pt(NH₃)₄Cl]Cl₃

[Pt(NH₃)₄Cl₄]

[Pt(NH₃)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl₃]Cl

142. Secondary cell is

Rechargeable

Non rechargeable

Electrolytic cell

Daniel cell

143. Which of the following is the strongest oxidizing agent?

Ag⁺

I₂

Pb²⁺

144. Which of the substances Na, Hg, S Pt and graphite can be used as electrodes in electrolytic cells having aqueous solution?

Na and Hg

Na, Pt and graphite

Pt and graphite only

Na and S only

145. Reaction takes place at anode is

Oxidation

Reduction

Ionization

Hydrolysis

146. 50 mL of 10 N H₂SO₄. 25 mL of 12 N HCl and 40 mL of 5N HNO₃ are mixed and the volume of the mixture is made 1000 mL by adding water. The normality of resulting solution will be

2 N

1 N

3 N

9 N

147. Voltaic cell can be recharged by

By addition of fresh solution

By removal of solution

By replacing external circuit with external source of electricity

By heating it

148. If α is the degree of dissociation of Na₂SO₄ the Vant Hoff’s factor (i) used for calculating the molecular mass is

1 – α

1 – 2 α

1 + α

1 + 2 α

149. Salt bridge transfers

Electrons

Anion

Ions

Current

150. Equal volumes of 0.1 M AgNO₃ and 0.2 M NaCl are mixed. The concentration of NO¯₃ ions in the mixture will be

0.05 M

0.15 M

0.1 M

0.2 M

Page 7 of 8

151. Separation of azeotropic mixture into pure components is carried out by

Vacuum distillation

None of these

Fractional distillation

Distillation

152. When a metal is dipped in 1 molar of its solution at 298k, then potential set up is called

Electroplating

Ionization potential

Standard electrode potential

Electric change

153. The solubility of a gas in water depends upon

Temperature

Nature of the gas

Pressure of the gas

All of these

154. Electrolysis is the process in which a chemical reaction takes place at the expense of

Heat energy

None of these

Electrical energy

Chemical energy

155. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

0.5 mole

2.00 mole

0.25 mole

1.0 mole

156. The degree of dissociation of weak electrolyte increases as

Dilution increases

Dilution decreases

None

Pressure increases

157. When electricity is passed through molten electrolyte consisting of alumina and cryolite, 13.5 g of Al are deposited. The number of faradays of electricity passed must be

0.5

1.0

1.5

2.0

158. When electricity is passed through molten Al₂O₃ + Na₃AIF₆ and 13.5 gms of Al are deposited, the number of faraday must be

1.5

1.0

2.0

0.5

159. An aqueous solution freezes at -0.186°C. (Kf = 1.86, Kb = 0.512). What is the elevation in boiling point?

0.0512

0.512

0.80

0.186

160. In a chemical reaction, oxidation process involves

Oxidation number neither increases nor decreases

Increase in oxidation number of the elements in reactants

Increase in oxidation number of element

Decrease in oxidation number of element

161. Half cells are interconnected through

Salt Bridge

Wire

Electric circuit

No connection exists

162. How many g of dibasic acid (mol. wt. 200) should be present in 100 ml of the aqueous solution to give 0.1 Normality?

20 g

1 g

2 g

10 g

163. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.3g/cm3

1.25g/cm3

1.20g/cm3

164. Potential of Zn is called

Oxidation

Redox

It has not potential

Reduction

165. Which one of the following will be good conductor of electricity?

Molten NaCl

Pure distilled water

Dilute solution of glucose

Chloroform

166. During a redox reaction, an oxidizing agent

Loses electrons

Gains electrons

Is hydrolysed

Is oxidized

167. Li occupies higher position in the electrochemical series of metals as compared to Cu since

The standard oxidation potential of Li/Li⁺ is lower than that of CuCu²⁺

The standard reduction potential of Li⁺/Li is lower than that of Cu²+/Cu

Li is smaller in size as compared to Cu

The standard reduction potential of Cu²+/Cu is lower than that of Li⁺/Li

168. If 18 g of glucose (C₆H₁₂C₆) is present in 1000 g of an aqueous solution of glucose it is said to be

0.1 molal

1 molal

0.5 molal

1.1 molal

169. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/51

1/5

5.1

170. A device which converts electrical energy into chemical energy is called

A galvanic cell

A voltaic cell

A chemical cell

An electrolytic cell

171. Of the following, the metal that cannot be obtained by electrolysis of aqueous solution of their salts are:

172. An aqueous solution of ethanol in water has vapour pressure

More than that of H₂O

Less than that of water

Equal to that of ethanol

Equal to that of water

173. Which of the following is a strong electrolyte?

Ca(NO₃)₂

CH₃COOH

NH₄OH

HCN

174. Electrode potential of Zn is

Reduction

Depends on the nature of the coupled electrode

Oxidation-reduction

Oxidation

175. The amount of electricity that can deposit 108 g of silver from silver nitrate solution is

1 coulomb

2 ampere

1 ampere

1 faraday

Page 8 of 8

176. What will be the weight of deposited silver on passing 965 coulombs of electricity in solution of AgNO₃?

1.08 g

0.27 g

0.54 g

2.16 g

177. In alkaline battery anode is made up of

MnO₂

AgO₂

Cadmium

178. The electrode with more negative value of reduction potential acts as

Electrode

None of these

Anode

Cathode

179. Choose the best reducing agent among the following

Br¯¹

Cl¯¹

I¯¹

F¯¹

180. Conductivity (Unit : siemen’s S) is directly proportionally to the area of the vessel and the concentration of the solution in it and is inversely proportional to the length of vessel, then the unit of constant of proportionality is

S m mol¯¹

S² m² mol¯²

S² m² mol

S m² mol¯¹

181. In a solution of CuSO₄ how much time will be required to precipitate 2g copper by 0.5 ampere current?

642 sec

102 sec

12157.48 sec

510 sec

182. If liquids A and B form an ideal solution

The enthalpy of mixing is zero

The free energy as well as the entropy of mixing are each zero

The entropy of mixing is zero

The free energy of mixing is zero

183. Camphor is often used in molecular mass determination because

It is readily available

It is solvent for organic substances

It is volatile

It has a very high cryoscopic constant

184. Same amount of electric current is passed through solution if AgNO₃ and HCl. If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated as S.T.P. in the second case is:

224 cm³

1.008 g

22400 cm³

112 cm³

185. A solution contains A, B and C components. The mole fraction A and C are 0.25 and 0.35 respectively. The mole fraction B will be

0.30

0.35

0.25

0.40

186. Which of the following will have the highest boiling point at 1 atm pressure?

0.1 M BaCl₂

0.1 M Glucose

0.1 M NaCl

0.1 M Sucrose

187. In alkaline battery the anode is made up of

Cadmium

MnO2

AgO2

188. In the conversion of Br2 to BrO₃¯¹ the oxidation state of bromine changes from

2 to 5

0 to –3

0 to 5.

1 to 5

189. Oxidation number of carbon in NaHCO₃ is

-6

190. Choose the cell among the following list in which conversation of electrical energy into chemical energy takes place

Fuel cell

Electrolytic cell

Galvanic cell

Daniel cell

191. The process of electrical coating of one metal on another to protect, decorate or to have a greater resistance to corrosion is called

Electroplating

Induction

Conduction

Electrolysis

192. Specific conductivity of a solution

Remains unchanged with dilution

Depends on mass of electrolyte

Decreases with dilution

Increases with dilution

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Malik TahirLast Updated: October 14, 2025

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