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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. 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

2. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

2.00 mole

0.25 mole

0.5 mole

1.0 mole

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

40.5

39.6

42.7

45.1

4. Solution with same osmotic pressures are called

Normal

Hypotonic

Hypertonic

Isotonic

5. Vant Hoff’s factor of Ca(NO₃)₂ is

6. 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

7. In a chemical reaction, oxidation process involves

Increase in oxidation number of the elements in reactants

Oxidation number neither increases nor decreases

Increase in oxidation number of element

Decrease in oxidation number of element

8. If liquids A and B form an ideal solution

The enthalpy of mixing is zero

The entropy of mixing is zero

The free energy of mixing is zero

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

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

Saturated

Unsaturated

Ideal

Supersaturated

10. Which of the following is a strong electrolyte?

CH₃COOH

Ca(NO₃)₂

HCN

NH₄OH

11. The reference electrode is made by using

HgCl₂

ZnCl₂

CuSO₄

Hg₂Cl₂

12. Electrode potential of Zn is

Reduction

Oxidation

Depends on the nature of the coupled electrode

Oxidation-reduction

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

1.86

0.0186

0.0521

0.521

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

None

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

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

Drops to zero

Increases rapidly

Does not change

Increases gradually

17. Reaction takes place at anode is

Hydrolysis

Oxidation

Reduction

Ionization

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

Slightly more than 1 atom

750 torr

2.5 atom

760 mm of Hg

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

Cell voltage

Ionization potential

Standard oxidation potential

Standard reduction potential

20. Oxidation number of carbon in NaHCO₃ is

-6

21. Voltaic cell can be recharged by

By addition of fresh solution

By replacing external circuit with external source of electricity

By heating it

By removal of solution

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

0.0196

0.1

0.2

0.01

23. What are the ions present in water?

H2 and O

H and OH

H+ and OH-

H2O

24. 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

2 N

0.4 N

4 N

25. 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

Page 2 of 8

26. The art of electroplating was given by

Brugan

Faraday

Thomas Gradam

Edison

27. 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

0.05 M

0.1 M

0.15 M

28. The depression of freezing point is directly proportional to

Molarity of the solution

Molality of the solution

Mole fraction of the solution

Molarity of the solvent

29. Alkaline battery has a voltage of

3.5V

2.5V

4.5V

1.5V

30. Potential of Zn is called

Redox

Reduction

Oxidation

It has not potential

31. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.20g/cm3

1.3g/cm3

1.25g/cm3

32. Molton NaCl conducts electricity due to the presence of

Free ions

Free electrons

Atoms of Na and Cl.

Free molecules

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

1 molal

1 molar

1 normal

All

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

HgCl₂

ZnCl₂

CuSO₄

Hg₂Cl₂

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

Fuel cell

Dry cell

Electrolytic cell

Galvanic cell

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

37. 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

3.2 g

2.3 g

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

H₃PO₂

H₃PO₃

H₄P₃O₇

H₃PO₄

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

4 g

1 g

2 g

5 g

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

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

Hg is more inert than Pt

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

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

41. Specific conductivity of a solution

Remains unchanged with dilution

Depends on mass of electrolyte

Decreases with dilution

Increases with dilution

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

Raoult’s law

Henry’s law

Arrhenius law

Ostwald’s law

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

0.0196

0.01

0.1

0.2

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

Nitric acid

Sulphuric acid

Phosphorus acid

Boric acid

45. Molarity of water is

55.5

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

Gold is denser

Iron rusts

Gold has lower reduction potential then iron

Gold has higher reduction potential then iron

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

Reduction

Neither oxidation and reduction

Oxidation

Both oxidation and reduction

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

Chemical energy

Electrical energy

None of these

Heat energy

49. In electrolytic cell, electricity in carried out by

Neutralization

Spontaneous reaction

Non-spontaneous reaction

All

50. In alkaline battery anode is made up of

Cadmium

MnO₂

AgO₂

Page 3 of 8

51. Standard hydrogen electrode has an arbitrarily fixed potential

0.10 volt

0.00 volt

None of these

1.00 volt

52. 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 > B > C

C > B > A

A > C > B

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

Electrolysis

Photo electrolysis

Cathodic protection

Galvanization

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

Strong acid and its salt of weak base

Weak acid and its salt of weak base

Weak acid and its salt of strong base

A strong acid and its salt of a strong base

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

Both Na⁺ and CI¯

Cl¯

Na⁺

None of these

56. 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

57. 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

10 g

2 g

58. 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

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

pH is changed

Acts as a catalyst

Gains electrons

Loses electrons

60. 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

S m² mol¯¹

S² m² mol

61. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.2 M

0.8 M

0.04 M

0.4 M

62. Metals usually conduct electricity because

Metals are decomposed by current

They are mobile electrons in the metallic structure

Metals have high resistance

In metals the ions are free to more

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

None

Sum of reduction and oxidation potentials

Lesser

Greater

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

Electrode

None of these

Anode

Cathode

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

O₂, SO₂

O₂,H₂

None of these

O₂, Na

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

Electrolytic cell

Daniel cell

Galvanic cell

Fuel cell

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

Very high positive value of reduction potential

Reduction potentials are negative

Very low ionization potential values

Very high negative values reduction potential

68. Units of molarity are

Kg/lit

Gm/lit

None of these

Mol/lit

69. Salt bridge transfers

Electrons

Anion

Ions

Current

70. Pick out the wrong statement. In electrochemical cell

Chemical energy is converted into electrical energy

Salt bridge maintains the electrical neutrality of the solution

Electrons are released at anode

Cathode is regarded as negative electrode

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

Distribution law

Henry’s law

Ostwald’s dilution law

Raoult’s law

72. 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

3 N

2 N

1 N

9 N

73. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

10 N

1 N

0.1N

11 N

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

Sublimation point

Boiling point

Melting point

Inversion point

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

Na → Na⁺ + e–

Na⁺ + e– → Na

Br₂ + 2e – → 2Br –

2Br– → Br₂ + 2e –

Page 4 of 8

76. Electricity in voltaic cell is produced due to

Neutralization

B + C

Reduction

Oxidation

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

2.46 atm

1.21 atm

12.1 atm

24.6 atm

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

2 M

1 f

1 M

1 N

79. An electrolyte

Forms complex ions in solution

Gives ions only when electricity is passed

Possesses ions even in solid state

Gives ions only when dissolved in water

80. Stronger the oxidizing agent, greater is the

Reduction potential

Redox potential

e.m.f of cell

Oxidation potential

81. 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

0.918 cm¯¹

1.12 cm¯¹

0.66 cm¯¹

82. Secondary cell is

Electrolytic cell

Non rechargeable

Rechargeable

Daniel cell

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

Oxygen

Chloride

Chlorine

Hydrogen

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

Not particular

In middle

Lower

Higher

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

NH₄Cl

Na₂SO₄

NaCl

CH₃ CooNH₄

86. Which of the following statements is FALSE?

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

Reduction occurs at cathode

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

All electrochemical reactions involve the transfer of electrons

87. Choose the best reducing agent among the following

Cl¯¹

Br¯¹

F¯¹

I¯¹

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

13.1%

9.09%

11.2%

14.25%

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

Does not change

Decrease rapidly

Decreases slowly

Drops to zero

90. 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:

22400 cm³

1.008 g

112 cm³

224 cm³

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

0.001

0.01

100

92. Camphor is often used in molecular mass determination because

It is readily available

It has a very high cryoscopic constant

It is volatile

It is solvent for organic substances

93. A redox reaction involves

A reaction in a solution

Proton transfer

Ion combination reaction

Electron transfer

94. 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

0.9

0.6

95. Oxidation in a chemical reaction involves

Both are possible

Decrease in oxidation number

Increase in oxidation number of all the elements on reactant side

Increase in oxidation number

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)₄Cl₃]Cl

[Pt(NH₃)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl]Cl₃

[Pt(NH₃)₄Cl₄]

97. 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

68 torr

20 torr

72 torr

140 torr

98. 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

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

0.512

0.80

0.186

0.0512

100. Decrease in oxidation number is called

Redox

Reduction

Oxidation

All of these

Page 5 of 8

101. Density of H₂SO₄ in lead accumulator is

120 g Cm³

1.2 g/Cm³

1.15 g/Cm³

1.25g/Cm³

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

Glass

0.1 N HCl

Graphite

0.1 N NaCl

103. 96500 C of electricity liberates from CuSO₄ solution

31.75 g of Cu

100 g of Cu

63.5 g of Cu

96500 g of CU

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

Pb²⁺

Ag⁺

I₂

105. 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?

31.8 gm

63.5 gm

12.7 gm

15.9 gm

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

2 N

8 N

6 N

4 N

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

40 g

6 g

60 g

4 g

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

Both A and B

None of these

Electrorefining

Electroplating

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

Vapour pressure of pure benzene decreases by the addition of naphthalene

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 water decreases by the addition of nitric acid

110. Half cells are interconnected through

Electric circuit

No connection exists

Salt Bridge

Wire

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

48250

10000

193000

96500

112. 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

113. 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

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

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

1 to 5

2 to 5

0 to 5.

0 to –3

116. The conductivity of strong electrolyte

Increases on dilution slightly

Decreases on dilution

Depends on density of electrolyte itself.

Does not change on dilution

117. 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

11.2 cm³

550 cm³

5.6 cm³

56 cm³

118. Corrosion reactions are

Spontaneous acid–base reactions

None of these

Non-spontaneous redox reactions

Spontaneous redox reactions

119. During a redox reaction, an oxidizing agent

Loses electrons

Is oxidized

Is hydrolysed

Gains electrons

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

Dilute solution of glucose

Pure distilled water

Chloroform

Molten NaCl

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

NH₄OH

Ca(OH)₂

NaOH

KOH

122. The solubility of a gas in water depends upon

Pressure of the gas

Temperature

All of these

Nature of the gas

123. Which has maximum oxidation number

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

1.86 c°

0.186 c°

Sufficient date not given

18.6 c°

125. Colligative properties are the properties of

Concentration solutions behave as nearly non – ideal solutions

Neither a nor b

Dilute solution which behave as nearly ideal solution

Both a and b

Page 6 of 8

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

780 mm of Hg

750 mm of Hg

760 mm of Hg

800 mm of Hg

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

Remove adsorbed oxygen from electrode surfaces

Create potential difference between two electrodes

Generate heat

Produce high purity water

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

6.1

5.51

5.65

1.32

129. Chemical used in salt bridge is

KCI

KOH

KBr

KNO3

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

Electroplating

Rust removal

Making leather

Manufacture of bleach

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

MgCl₂

KCl

BaCl₂

NaCl

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

Vacuum distillation

Distillation

None of these

Fractional distillation

133. 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 10⁴

1.06 x 10³

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

2.05

0.5

0.25

0.05

135. In alkaline battery the anode is made up of

AgO2

Cadmium

MnO2

136. 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

0.80

0.60

0.75

0.20

137. The Vant Hoff factor (i) accounts for

Degree of solubilization of solute

The extent of dissolution of solute

The extent of dissociation of solute

The degree of decomposition of solution

138. Pure water does not conduct electricity because it

Is almost unionized

Is readily decomposed

Is neutral

Has low boiling point

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

Microgram percent

Milligram percent

Gram per million

Parts per million

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

Electric change

Electroplating

Standard electrode potential

Ionization potential

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

0.217

3.12

4.10

7.20

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

20g NaCl/100ml

5.58g NaCl/100m

10.0g NaCl/100ml

58.5g NaCl/100ml

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

Electrochemical equivalent

One gm. Equivalent weight

One gm. atomic weight

None of these

144. Strong reducing agents have

Lesser positive value of standard reduction potential

Greater negative value of standard reduction potential

Greater positive value of standard reduction potential

None of these

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

1 + 2 α

1 – 2 α

1 + α

1 – α

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

20 ml

40 ml

10 ml

80 ml

147. Salt bridge transfers

Current

Anions

Electrons

Solvent particles

148. When common salt is dissolved in water

Any possibility

B.P of water remain constant

B.P of water decrease

B.P of water increase

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

Equal to the total volume of the components

None of these

Slightly more than the total volume of the components

Slightly less than the total volume of the components

150. Cathode provides electrons to

Does not provide any electron

-Ve ion

Neutral atom

+Ve ion

Page 7 of 8

151. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

None of these

2.5

1.25

1 2

152. Maximum freezing point falls in

Naphthalene

Water

Camphor

Benzene

153. Corrosion is basically a

Altered reaction in presence of H₂O

Electrochemical phenomenon

Interaction

Union between two light metals and a heavy metal

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

1.0

0.5

1.5

2.0

155. 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

2.0 x 10¹¹

1.0 x 10²

1.0 x 10¹⁰

4.0 x 10¹²

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

Equal to that of ethanol

More than that of H₂O

Equal to that of water

Less than that of water

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

Osmotic pressure

Refractive index

Surface tension

Viscosity

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

Electrons flow cathode to anode within the electrolytic solution

None of these

Electrons flow from cathode to anode through the external battery

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

159. 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

0.40

0.25

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

Hydrolyzed

Reduced

Oxidized

Precipitated

161. Azeotropic mixture of HCl and water has

22.2% HCl

36% HCl

48% HCl

20.2% HCl

162. Mole fraction of pure water is

Slightly greater than one

Slightly less than one

Exactly equal to one

None of these

163. The best reducing agent is

Cl¯

Br¯

F¯

I¯

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

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

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

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

Li is smaller in size as compared to Cu

165. 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

302 S cm² mol¯¹

128 S cm² mol¯¹

176 S cm² mol¯¹

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

Heat energy

Magnetic energy

Electrical energy

Sound energy

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

2.16 g

1.08 g

0.54 g

0.27 g

168. Temperature for standard electrode potential is

310 K

300 K

25 C°

273 K

169. Best way to prevent rusting iron is by

None of these

Making iron cathode

Both of these

Putting it in saline water

170. In a Galvanic cell

Electrical energy is converted into chemical energy

Electrical energy is converted into heat

Chemical energy is converted into heat

Chemical energy is converted into electricity

171. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/5

5.1

1/51

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

Diffusion rate of the solute

Ionic concentration

Flow of solvent from a concentrated to a dilute solution

Elevation in boiling point

173. 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)

0.281 V

0.176 V

0.222 V

0.399 V

174. In a Galvanic cell, the electrons flow from

Cathode to anode through the solution

Anode to cathode through the solution

Cathode to anode through the external circuit

Anode to cathode through the external circuit

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

Na₂O

F₂O

Na₂O₂

Cl₂O

Page 8 of 8

176. Reduction always occurs

At anode

Both A and B

At cathode

None of these

177. Oxidation state of hydrogen in CaH₂ is

-1

-2

178. 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

21.6 g

108 g

10.8 g

179. 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 S only

Na, Pt and graphite

Na and Hg

180. 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

181. 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?

4.18 M

8.14 M

18.4 M

18 M

182. The unit of specific conductivity is

Ohm cm¯²

Ohm¯¹ cm¯¹

Ohm¯¹ cm

Ohm cm¯¹

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

∆ G = -ve, ∆ E = 0

∆ G = +ve, ∆ E = 0

∆ G = -ve

∆ G = 0, ∆E = 0

184. 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

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

– 1.17 V

– 0.35 V

+ 0.35

+ 1.17 V

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

1.5

187. 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

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

1 ampere

1 faraday

1 coulomb

2 ampere

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

An electrolytic cell

A chemical cell

A voltaic cell

A galvanic cell

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

Oxidation

Both

Reduction

191. The degree of dissociation of weak electrolyte increases as

Pressure increases

Dilution increases

None

Dilution decreases

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

0.1 M BaCl₂

0.1 M Sucrose

0.1 M Glucose

0.1 M NaCl

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Maan AliLast Updated: April 19, 2025

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