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ECAT Chemistry Electrochemistry Online Test

Maan AliLast Updated: April 19, 2025

Chemistry Electrochemistry MCQS Online Test

ECAT Chemistry Electrochemistry Chapter Online Test

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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ECAT Chemistry Electrochemistry Test

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Page 1 of 8

Chemistry

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

Acts as a catalyst

Loses electrons

pH is changed

Gains electrons

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

Hg₂Cl₂

ZnCl₂

HgCl₂

CuSO₄

3. 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 positive value of reduction potential

Very high negative values reduction potential

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

None of these

Cathode

Electrode

Anode

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

None

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

1.5

7. Salt bridge transfers

Current

Electrons

Anions

Solvent particles

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

9. Specific conductivity of a solution

Depends on mass of electrolyte

Remains unchanged with dilution

Decreases with dilution

Increases with dilution

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

F₂O

Na₂O

Na₂O₂

Cl₂O

11. Stronger the oxidizing agent, greater is the

Oxidation potential

e.m.f of cell

Redox potential

Reduction potential

12. Mole fraction of pure water is

Exactly equal to one

Slightly greater than one

None of these

Slightly less than one

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

0.186 c°

Sufficient date not given

1.86 c°

18.6 c°

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

Electric change

Standard electrode potential

Electroplating

Ionization potential

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

1 molal

0.1 molal

1.1 molal

0.5 molal

16. Units of molarity are

Kg/lit

Mol/lit

Gm/lit

None of these

17. During a redox reaction, an oxidizing agent

Is oxidized

Loses electrons

Gains electrons

Is hydrolysed

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

Flow of solvent from a concentrated to a dilute solution

Elevation in boiling point

Ionic concentration

Diffusion rate of the solute

19. If liquids A and B form an ideal solution

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

The free energy of mixing is zero

The enthalpy of mixing is zero

The entropy of mixing is zero

20. 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:

112 cm³

1.008 g

22400 cm³

224 cm³

21. The reference electrode is made by using

Hg₂Cl₂

CuSO₄

ZnCl₂

HgCl₂

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

Na₂SO₄

NaCl

NH₄Cl

CH₃ CooNH₄

23. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

0.1N

1 N

11 N

10 N

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

Raoult’s law

Henry’s law

Distribution law

Ostwald’s dilution law

25. In a Galvanic cell

Electrical energy is converted into heat

Chemical energy is converted into heat

Electrical energy is converted into chemical energy

Chemical energy is converted into electricity

Page 2 of 8

26. Decrease in oxidation number is called

Oxidation

All of these

Redox

Reduction

27. Which of the following statements is FALSE?

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

All electrochemical reactions involve the transfer of electrons

Reduction occurs at cathode

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

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

Both A and B

None of these

Electrorefining

Electroplating

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

Precipitated

Reduced

Hydrolyzed

Oxidized

30. In an electrolytic cell current flows

From anode to cathode inside the cell

From anode to cathode in an outer circuit

From cathode to anode in outer circuit

From cathode to anode inside the cell

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

Surface tension

Viscosity

Refractive index

Osmotic pressure

32. Voltaic cell can be recharged by

By replacing external circuit with external source of electricity

By removal of solution

By addition of fresh solution

By heating it

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

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

Electrons flow from cathode to anode through the external battery

Electrons flow cathode to anode within the electrolytic solution

None of these

34. The degree of dissociation of weak electrolyte increases as

Dilution decreases

Dilution increases

None

Pressure increases

35. 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

S² m² mol

S m mol¯¹

S m² mol¯¹

S² m² mol¯²

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

Chloride

Oxygen

Hydrogen

Chlorine

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

2Br– → Br₂ + 2e –

Br₂ + 2e – → 2Br –

Na⁺ + e– → Na

Na → Na⁺ + e–

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

0.1 M Glucose

0.1 M NaCl

0.1 M Sucrose

0.1 M BaCl₂

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

0.01

0.0196

0.2

0.1

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

Molten NaCl

Chloroform

Pure distilled water

Dilute solution of glucose

41. The Vant Hoff factor (i) accounts for

The extent of dissociation of solute

The extent of dissolution of solute

The degree of decomposition of solution

Degree of solubilization of solute

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

Graphite

0.1 N NaCl

Glass

0.1 N HCl

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

Cl¯

None of these

Na⁺

Both Na⁺ and CI¯

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

1.25 cm¯³

1.81 cm¯³

2.15 cm¯³

1.15 cm¯³

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

13.1%

14.25%

11.2%

9.09%

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

0.3

0.2

0.6

0.9

47. Which has maximum oxidation number

48. Choose the best reducing agent among the following

Br¯¹

Cl¯¹

I¯¹

F¯¹

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

Pt and graphite only

Na and Hg

Na, Pt and graphite

Na and S only

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

40 ml

10 ml

80 ml

20 ml

Page 3 of 8

51. Electrode potential of Zn is

Reduction

Oxidation

Oxidation-reduction

Depends on the nature of the coupled electrode

52. 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

240 C

4 C

120 C

20 C

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

Slightly more than 1 atom

750 torr

760 mm of Hg

2.5 atom

54. Vant Hoff’s factor of Ca(NO₃)₂ is

55. The unit of specific conductivity is

Ohm cm¯¹

Ohm¯¹ cm¯¹

Ohm cm¯²

Ohm¯¹ cm

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

Ca(OH)₂

NaOH

KOH

NH₄OH

57. 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

0.2 M

0.15 M

0.1 M

0.05 M

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

Heat energy

None of these

Chemical energy

Electrical energy

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

58.5g NaCl/100ml

5.58g NaCl/100m

10.0g NaCl/100ml

20g NaCl/100ml

60. Potential of Zn is called

It has not potential

Oxidation

Reduction

Redox

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

Sum of reduction and oxidation potentials

Greater

None

Lesser

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

Gold has lower reduction potential then iron

Gold has higher reduction potential then iron

Gold is denser

Iron rusts

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

MgCl₂

NaCl

KCl

BaCl₂

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

Supersaturated

Ideal

Saturated

Unsaturated

65. What are the ions present in water?

H2O

H2 and O

H and OH

H+ and OH-

66. Chemical used in salt bridge is

KNO3

KCI

KBr

KOH

67. In alkaline battery the anode is made up of

MnO2

AgO2

Cadmium

68. In a Galvanic cell, the electrons flow from

Anode to cathode through the solution

Cathode to anode through the external circuit

Anode to cathode through the external circuit

Cathode to anode through the solution

69. 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 2

2.5

1.25

None of these

70. Camphor is often used in molecular mass determination because

It has a very high cryoscopic constant

It is volatile

It is readily available

It is solvent for organic substances

71. 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⁺

Li is smaller in size as compared to Cu

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

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

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

0.217

3.12

7.20

4.10

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

45.1

42.7

39.6

40.5

74. Azeotropic mixture of HCl and water has

36% HCl

20.2% HCl

48% HCl

22.2% HCl

75. Oxidation number of carbon in NaHCO₃ is

-6

Page 4 of 8

76. 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

2.0 x 10¹¹

4.0 x 10¹²

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

Electrolysis

Cathodic protection

Photo electrolysis

Galvanization

78. 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?

15.9 gm

63.5 gm

31.8 gm

12.7 gm

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

Melting point

Boiling point

Sublimation point

Inversion point

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

– 1.17 V

– 0.35 V

+ 1.17 V

+ 0.35

81. Oxidation state of hydrogen in CaH₂ is

-1

-2

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

Galvanic cell

Dry cell

Electrolytic cell

Fuel cell

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

Fractional distillation

Distillation

Vacuum distillation

None of these

84. Maximum freezing point falls in

Water

Benzene

Camphor

Naphthalene

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

Sound energy

Magnetic energy

Heat energy

Electrical energy

86. 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

3.2 g

12.8 g

6.4 g

2.3 g

87. 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

0.25

0.30

0.40

0.35

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

2 to 5

1 to 5

0 to 5.

0 to –3

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

176 S cm² mol¯¹

128 S cm² mol¯¹

278 S cm² mol¯¹

302 S cm² mol¯¹

90. The art of electroplating was given by

Brugan

Thomas Gradam

Edison

Faraday

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

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

Boiling point of pure water decreases by the addition of ethanol

Boiling point of pure benzene increases by the addition of toluene

Vapour pressure of pure benzene decreases by the addition of naphthalene

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

A voltaic cell

A galvanic cell

An electrolytic cell

A chemical cell

93. Strong reducing agents have

Greater negative value of standard reduction potential

Lesser positive value of standard reduction potential

Greater positive value of standard reduction potential

None of these

94. Best way to prevent rusting iron is by

Making iron cathode

None of these

Both of these

Putting it in saline water

95. The depression of freezing point is directly proportional to

Molarity of the solvent

Molality of the solution

Mole fraction of the solution

Molarity of the solution

96. 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)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl₄]

[Pt(NH₃)₄Cl]Cl₃

[Pt(NH₃)₄Cl₃]Cl

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

0.25

2.05

0.05

0.5

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

0.2 N

0.4 N

4 N

2 N

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

1.5

0.5

1.0

2.0

100. Reaction takes place at anode is

Ionization

Reduction

Oxidation

Hydrolysis

Page 5 of 8

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

Higher

Lower

Not particular

In middle

102. 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

A > C > B

C > B > A

B > C > A

A > B > C

103. 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

0.399 V

0.281 V

0.176 V

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

Ag⁺

I₂

Pb²⁺

105. Cathode provides electrons to

-Ve ion

Does not provide any electron

Neutral atom

+Ve ion

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

0.27 g

1.08 g

2.16 g

0.54 g

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

10 s

30 s

30,000 s

10,000 s

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

12.1 atm

24.6 atm

1.21 atm

2.46 atm

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

A strong acid and its salt of a strong base

Weak acid and its salt of strong base

Weak acid and its salt of weak base

Strong acid and its salt of weak base

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

175.4 kJ

53.07 kJ

212.3 kJ

106.15 kJ

111. An electrolyte

Gives ions only when electricity is passed

Possesses ions even in solid state

Forms complex ions in solution

Gives ions only when dissolved in water

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

0.1

0.2

0.01

0.0196

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

2 g

1 g

5 g

4 g

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

Equal to the total volume of the components

Slightly more than the total volume of the components

None of these

Slightly less than the total volume of the components

115. Reduction always occurs

At cathode

Both A and B

At anode

None of these

116. 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

1.5

2.0

1.0

0.5

117. Standard hydrogen electrode has an arbitrarily fixed potential

None of these

0.00 volt

1.00 volt

0.10 volt

118. 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

0.142 cm¯¹

0.66 cm¯¹

1.12 cm¯¹

0.918 cm¯¹

119. Density of H₂SO₄ in lead accumulator is

1.2 g/Cm³

120 g Cm³

1.25g/Cm³

1.15 g/Cm³

120. Electricity in voltaic cell is produced due to

B + C

Neutralization

Oxidation

Reduction

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

5.51

1.32

5.65

6.1

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

Phosphorus acid

Boric acid

Sulphuric acid

Nitric acid

123. Temperature for standard electrode potential is

25 C°

273 K

300 K

310 K

124. 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

140 torr

68 torr

72 torr

20 torr

125. Metals usually conduct electricity because

Metals are decomposed by current

Metals have high resistance

They are mobile electrons in the metallic structure

In metals the ions are free to more

Page 6 of 8

126. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.04 M

0.8 M

0.2 M

0.4 M

127. 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

1 N

3 N

2 N

9 N

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

1 coulomb

2 ampere

1 faraday

1 ampere

129. 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

130. 96500 C of electricity liberates from CuSO₄ solution

63.5 g of Cu

96500 g of CU

31.75 g of Cu

100 g of Cu

131. In a chemical reaction, oxidation process involves

Increase in oxidation number of the elements in reactants

Oxidation number neither increases nor decreases

Decrease in oxidation number of element

Increase in oxidation number of element

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

Generate heat

Produce high purity water

Create potential difference between two electrodes

Remove adsorbed oxygen from electrode surfaces

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

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

Electrochemical equivalent

One gm. Equivalent weight

None of these

One gm. atomic weight

135. Which of the following is a strong electrolyte?

CH₃COOH

NH₄OH

HCN

Ca(NO₃)₂

136. 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

56 cm³

5.6 cm³

11.2 cm³

550 cm³

137. Solution with same osmotic pressures are called

Hypotonic

Normal

Isotonic

Hypertonic

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

1 N

2 M

1 f

1 M

139. 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 10²

1.06 x 10³

1.06 x 10⁴

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

Does not change

Drops to zero

Decrease rapidly

Decreases slowly

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

Induction

Electroplating

Electrolysis

Conduction

142. The conductivity of strong electrolyte

Depends on density of electrolyte itself.

Decreases on dilution

Does not change on dilution

Increases on dilution slightly

143. 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

10.8 g

108 g

21.6 g

1.08 g

144. Pure water does not conduct electricity because it

Has low boiling point

Is almost unionized

Is readily decomposed

Is neutral

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

642 sec

102 sec

510 sec

12157.48 sec

146. In alkaline battery anode is made up of

MnO₂

Cadmium

AgO₂

147. 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?

18.4 M

4.18 M

8.14 M

18 M

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

0.0186

0.521

1.86

0.0521

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

Less than that of water

Equal to that of water

Equal to that of ethanol

More than that of H₂O

150. Secondary cell is

Non rechargeable

Rechargeable

Electrolytic cell

Daniel cell

Page 7 of 8

151. When common salt is dissolved in water

Any possibility

B.P of water decrease

B.P of water remain constant

B.P of water increase

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

800 mm of Hg

750 mm of Hg

760 mm of Hg

780 mm of Hg

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

H₃PO₄

H₃PO₂

H₃PO₃

H₄P₃O₇

154. The solubility of a gas in water depends upon

Nature of the gas

Temperature

All of these

Pressure of the gas

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

Daniel cell

Galvanic cell

Electrolytic cell

Fuel cell

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

Standard oxidation potential

Ionization potential

Standard reduction potential

Cell voltage

157. Pick out the wrong statement. In electrochemical cell

Salt bridge maintains the electrical neutrality of the solution

Electrons are released at anode

Chemical energy is converted into electrical energy

Cathode is regarded as negative electrode

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

Does not change

Increases rapidly

Drops to zero

Increases gradually

159. 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 + 2 α

1 – α

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

10000

48250

96500

193000

161. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

5.1

1/5

1/51

162. Molarity of water is

55.5

163. Salt bridge transfers

Ions

Electrons

Anion

Current

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

Reduction

Oxidation

Both

165. Half cells are interconnected through

Salt Bridge

No connection exists

Electric circuit

Wire

166. Colligative properties are the properties of

Concentration solutions behave as nearly non – ideal solutions

Dilute solution which behave as nearly ideal solution

Both a and b

Neither a nor b

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

168. Corrosion reactions are

Spontaneous redox reactions

None of these

Non-spontaneous redox reactions

Spontaneous acid–base reactions

169. Oxidation in a chemical reaction involves

Decrease in oxidation number

Increase in oxidation number

Both are possible

Increase in oxidation number of all the elements on reactant side

170. Molton NaCl conducts electricity due to the presence of

Free electrons

Free ions

Atoms of Na and Cl.

Free molecules

171. A redox reaction involves

A reaction in a solution

Ion combination reaction

Electron transfer

Proton transfer

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

Gram per million

Parts per million

Microgram percent

Milligram percent

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

6 g

60 g

4 g

40 g

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

10 g

1 g

20 g

2 g

175. 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

0.001

100

Page 8 of 8

176. In electrolytic cell, electricity in carried out by

Spontaneous reaction

All

Non-spontaneous reaction

Neutralization

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

Henry’s law

Ostwald’s law

Raoult’s law

Arrhenius law

178. 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

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

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

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

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

Hg is more inert than Pt

180. Density of H₂SO₄ in lead accumulator is

1.3g/cm3

1.15g/cm3

1.20g/cm3

1.25g/cm3

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

1 molal

1 molar

1 normal

All

182. Alkaline battery has a voltage of

2.5V

1.5V

4.5V

3.5V

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

Neither oxidation and reduction

Oxidation

Both oxidation and reduction

Reduction

184. 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

0.60

0.75

0.80

0.20

185. The best reducing agent is

F¯

Cl¯

I¯

Br¯

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

∆ G = +ve, ∆ E = 0

∆ G = -ve, ∆ E = 0

∆ G = -ve

∆ G = 0, ∆E = 0

187. Corrosion is basically a

Interaction

Union between two light metals and a heavy metal

Altered reaction in presence of H₂O

Electrochemical phenomenon

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

Electroplating

Rust removal

Making leather

Manufacture of bleach

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

8 N

4 N

6 N

2 N

190. 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

0.0033

3.33

33.3

191. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

0.25 mole

0.5 mole

2.00 mole

1.0 mole

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

None of these

O₂, SO₂

O₂,H₂

O₂, Na

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Maan AliLast Updated: April 19, 2025

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