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

Oxygen

Hydrogen

Chlorine

Chloride

2. 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

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

Standard reduction potential

Ionization potential

Cell voltage

Standard oxidation potential

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

5.65

1.32

6.1

5.51

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

1.5

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

0 to 5.

0 to –3

2 to 5

1 to 5

7. 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

8. The conductivity of strong electrolyte

Does not change on dilution

Increases on dilution slightly

Decreases on dilution

Depends on density of electrolyte itself.

9. 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

10.8 g

108 g

10. The solubility of a gas in water depends upon

Pressure of the gas

Temperature

Nature of the gas

All of these

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

Drops to zero

Decreases slowly

Decrease rapidly

Does not change

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

Chloroform

Dilute solution of glucose

Pure distilled water

Molten NaCl

13. 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

14. 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

15. Pure water does not conduct electricity because it

Has low boiling point

Is almost unionized

Is neutral

Is readily decomposed

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

NaCl

BaCl₂

MgCl₂

KCl

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

0.5

1.0

1.5

2.0

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

Glass

0.1 N NaCl

0.1 N HCl

Graphite

19. The depression of freezing point is directly proportional to

Mole fraction of the solution

Molarity of the solvent

Molality of the solution

Molarity of the solution

20. Colligative properties are the properties of

Both a and b

Dilute solution which behave as nearly ideal solution

Neither a nor b

Concentration solutions behave as nearly non – ideal solutions

21. Salt bridge transfers

Anion

Electrons

Ions

Current

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

H₃PO₃

H₃PO₂

H₄P₃O₇

H₃PO₄

23. The reference electrode is made by using

ZnCl₂

Hg₂Cl₂

HgCl₂

CuSO₄

24. Corrosion is basically a

Union between two light metals and a heavy metal

Interaction

Electrochemical phenomenon

Altered reaction in presence of H₂O

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

Na and S only

Na, Pt and graphite

Pt and graphite only

Na and Hg

Page 2 of 8

26. 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 less than the total volume of the components

Slightly more than the total volume of the components

None of these

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

750 torr

2.5 atom

760 mm of Hg

Slightly more than 1 atom

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

0.54 g

1.08 g

0.27 g

2.16 g

29. 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

1.12 cm¯¹

0.66 cm¯¹

0.918 cm¯¹

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

0.2

0.1

0.01

0.0196

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

302 S cm² mol¯¹

278 S cm² mol¯¹

176 S cm² mol¯¹

128 S cm² mol¯¹

32. Salt bridge transfers

Electrons

Current

Anions

Solvent particles

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

Produce high purity water

Remove adsorbed oxygen from electrode surfaces

Generate heat

Create potential difference between two electrodes

34. In electrolytic cell, electricity in carried out by

Spontaneous reaction

Non-spontaneous reaction

Neutralization

All

35. 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

0.20

0.60

0.75

36. 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

0.4 N

0.2 N

4 N

2 N

37. Cathode provides electrons to

Neutral atom

-Ve ion

+Ve ion

Does not provide any electron

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

Na₂O₂

Cl₂O

Na₂O

F₂O

39. 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

53.07 kJ

175.4 kJ

40. Voltaic cell can be recharged by

By addition of fresh solution

By removal of solution

By heating it

By replacing external circuit with external source of electricity

41. In a Galvanic cell, the electrons flow from

Anode to cathode through the solution

Anode to cathode through the external circuit

Cathode to anode through the external circuit

Cathode to anode through the solution

42. 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

2.3 g

6.4 g

3.2 g

12.8 g

43. Decrease in oxidation number is called

Redox

Oxidation

Reduction

All of these

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

40.5

45.1

42.7

39.6

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

0.3

0.9

0.2

0.6

46. 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

Lesser

Greater

None

47. The best reducing agent is

I¯

Cl¯

Br¯

F¯

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

Arrhenius law

Raoult’s law

Henry’s law

Ostwald’s law

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

1 M

1 N

1 f

2 M

50. 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)₄Cl₄]

[Pt(NH₃)₄Cl]Cl₃

Page 3 of 8

51. Molton NaCl conducts electricity due to the presence of

Free molecules

Free electrons

Free ions

Atoms of Na and Cl.

52. Strong reducing agents have

Greater positive value of standard reduction potential

None of these

Greater negative value of standard reduction potential

Lesser positive value of standard reduction potential

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

Rust removal

Making leather

Electroplating

Manufacture of bleach

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

0.0196

0.2

0.01

0.1

55. In alkaline battery the anode is made up of

AgO2

Cadmium

MnO2

56. Potential of Zn is called

Reduction

Redox

It has not potential

Oxidation

57. A redox reaction involves

A reaction in a solution

Proton transfer

Ion combination reaction

Electron transfer

58. In a chemical reaction, oxidation process involves

Increase in oxidation number of element

Increase in oxidation number of the elements in reactants

Decrease in oxidation number of element

Oxidation number neither increases nor decreases

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

Ag⁺

I₂

Pb²⁺

60. 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

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

Hg is more inert than Pt

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

61. Secondary cell is

Non rechargeable

Daniel cell

Rechargeable

Electrolytic cell

62. Electrode potential of Zn is

Reduction

Oxidation

Oxidation-reduction

Depends on the nature of the coupled electrode

63. Oxidation number of carbon in NaHCO₃ is

-6

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

Hg₂Cl₂

CuSO₄

HgCl₂

ZnCl₂

65. Specific conductivity of a solution

Increases with dilution

Depends on mass of electrolyte

Decreases with dilution

Remains unchanged with dilution

66. The art of electroplating was given by

Brugan

Edison

Faraday

Thomas Gradam

67. Reduction always occurs

At anode

None of these

Both A and B

At cathode

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

102 sec

12157.48 sec

642 sec

510 sec

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

Electrode

None of these

Cathode

Anode

70. The degree of dissociation of weak electrolyte increases as

None

Dilution increases

Pressure increases

Dilution decreases

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

Galvanic cell

Fuel cell

Daniel cell

Electrolytic cell

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

– 0.35 V

– 1.17 V

+ 0.35

+ 1.17 V

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

Ostwald’s dilution law

Distribution law

Raoult’s law

Henry’s law

74. 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

20 C

120 C

4 C

240 C

75. 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 – α

1 + 2 α

1 – 2 α

Page 4 of 8

76. In alkaline battery anode is made up of

MnO₂

AgO₂

Cadmium

77. 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

78. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.04 M

0.2 M

0.4 M

0.8 M

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

NaCl

CH₃ CooNH₄

NH₄Cl

Na₂SO₄

80. Azeotropic mixture of HCl and water has

22.2% HCl

48% HCl

20.2% HCl

36% HCl

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

82. 96500 C of electricity liberates from CuSO₄ solution

31.75 g of Cu

96500 g of CU

63.5 g of Cu

100 g of Cu

83. 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¯²

S m mol¯¹

S² m² mol

S m² mol¯¹

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

85. Temperature for standard electrode potential is

273 K

310 K

300 K

25 C°

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

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

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⁺

Li is smaller in size as compared to Cu

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

Standard electrode potential

Ionization potential

Electric change

Electroplating

88. 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

0.40

0.25

0.35

0.30

89. 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

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

Heat energy

Chemical energy

None of these

Electrical energy

91. Corrosion reactions are

Spontaneous redox reactions

Spontaneous acid–base reactions

Non-spontaneous redox reactions

None of these

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

Not particular

Higher

Lower

In middle

93. 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

94. Standard hydrogen electrode has an arbitrarily fixed potential

0.10 volt

1.00 volt

None of these

0.00 volt

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

Cathodic protection

Photo electrolysis

Galvanization

Electrolysis

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

∆ G = 0, ∆E = 0

∆ G = -ve

∆ G = +ve, ∆ E = 0

∆ G = -ve, ∆ E = 0

97. Molarity of water is

55.5

98. 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

18 M

18.4 M

8.14 M

99. Oxidation in a chemical reaction involves

Decrease in oxidation number

Increase in oxidation number of all the elements on reactant side

Increase in oxidation number

Both are possible

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

None of these

Cl¯

Both Na⁺ and CI¯

Na⁺

Page 5 of 8

101. 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

2 g

10 g

1 g

102. 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

22400 cm³

224 cm³

1.008 g

103. Vant Hoff’s factor of Ca(NO₃)₂ is

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

5 g

2 g

4 g

1 g

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

2 ampere

1 faraday

1 coulomb

1 ampere

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

20 ml

80 ml

40 ml

10 ml

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

NH₄OH

KOH

Ca(OH)₂

NaOH

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

4 g

40 g

60 g

6 g

109. Stronger the oxidizing agent, greater is the

Oxidation potential

Reduction potential

Redox potential

e.m.f of cell

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

Equal to that of water

Equal to that of ethanol

Less than that of water

More than that of H₂O

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

0.0512

0.80

0.186

0.512

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

Oxidized

Precipitated

Reduced

Hydrolyzed

113. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

1 N

10 N

0.1N

11 N

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

1 molar

All

1 normal

1 molal

115. Alkaline battery has a voltage of

2.5V

1.5V

3.5V

4.5V

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

Both

Oxidation

Reduction

117. Reaction takes place at anode is

Reduction

Hydrolysis

Ionization

Oxidation

118. Maximum freezing point falls in

Naphthalene

Camphor

Benzene

Water

119. Oxidation state of hydrogen in CaH₂ is

-2

-1

120. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

1.0 mole

2.00 mole

0.5 mole

0.25 mole

121. 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

Boiling point of pure water decreases by the addition of ethanol

Vapour pressure of pure benzene decreases by the addition of naphthalene

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

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

Electrochemical equivalent

One gm. atomic weight

One gm. Equivalent weight

None of these

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

1.25 cm¯³

1.81 cm¯³

1.15 cm¯³

2.15 cm¯³

124. Which of the following is a strong electrolyte?

CH₃COOH

Ca(NO₃)₂

NH₄OH

HCN

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

A chemical cell

A galvanic cell

A voltaic cell

An electrolytic cell

Page 6 of 8

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

0.1 M Sucrose

0.1 M BaCl₂

0.1 M NaCl

0.1 M Glucose

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

Surface tension

Viscosity

Refractive index

Osmotic pressure

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

Milligram percent

Parts per million

Gram per million

Microgram percent

129. Density of H₂SO₄ in lead accumulator is

1.2 g/Cm³

1.15 g/Cm³

1.25g/Cm³

120 g Cm³

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

30 s

30,000 s

10,000 s

10 s

131. In a Galvanic cell

Electrical energy is converted into chemical energy

Electrical energy is converted into heat

Chemical energy is converted into electricity

Chemical energy is converted into heat

132. During a redox reaction, an oxidizing agent

Is oxidized

Is hydrolysed

Loses electrons

Gains electrons

133. If liquids A and B form an ideal solution

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

The enthalpy of mixing is zero

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

Loses electrons

Gains electrons

Acts as a catalyst

pH is changed

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

Sulphuric acid

Nitric acid

Boric acid

Phosphorus acid

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

0.0521

1.86

0.0186

0.521

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

Ideal

Saturated

Supersaturated

Unsaturated

138. 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

12.7 gm

31.8 gm

139. Electricity in voltaic cell is produced due to

Neutralization

B + C

Oxidation

Reduction

140. Mole fraction of pure water is

Slightly less than one

None of these

Exactly equal to one

Slightly greater than one

141. 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

0.5 molal

1 molal

1.1 molal

142. 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 10²

4.0 x 10¹²

1.0 x 10¹⁰

2.0 x 10¹¹

143. 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

1.0

0.5

2.0

1.5

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

Strong acid and its salt of weak base

Weak acid and its salt of strong base

Weak acid and its salt of weak base

A strong acid and its salt of a strong base

145. Metals usually conduct electricity because

Metals are decomposed by current

In metals the ions are free to more

They are mobile electrons in the metallic structure

Metals have high resistance

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

0.217

7.20

4.10

3.12

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

Both oxidation and reduction

Reduction

Neither oxidation and reduction

Oxidation

148. In an electrolytic cell current flows

From cathode to anode inside the cell

From anode to cathode inside the cell

From anode to cathode in an outer circuit

From cathode to anode in outer circuit

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

Gold is denser

Gold has higher reduction potential then iron

Iron rusts

Gold has lower reduction potential then iron

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

Conduction

Electroplating

Electrolysis

Induction

Page 7 of 8

151. 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

56 cm³

550 cm³

5.6 cm³

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

Distillation

Vacuum distillation

None of these

Fractional distillation

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

1.21 atm

2.46 atm

12.1 atm

24.6 atm

154. 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

155. Camphor is often used in molecular mass determination because

It is volatile

It has a very high cryoscopic constant

It is readily available

It is solvent for organic substances

156. Pick out the wrong statement. In electrochemical cell

Chemical energy is converted into electrical energy

Electrons are released at anode

Cathode is regarded as negative electrode

Salt bridge maintains the electrical neutrality of the solution

157. 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

2 N

9 N

3 N

158. Chemical used in salt bridge is

KNO3

KBr

KCI

KOH

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

Dry cell

Galvanic cell

Electrolytic cell

Fuel cell

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

760 mm of Hg

780 mm of Hg

750 mm of Hg

800 mm of Hg

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

48250

10000

193000

96500

162. Which of the following statements is FALSE?

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

All electrochemical reactions involve the transfer of electrons

Reduction occurs at cathode

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

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

2.05

0.25

0.5

0.05

164. The Vant Hoff factor (i) accounts for

Degree of solubilization of solute

The degree of decomposition of solution

The extent of dissolution of solute

The extent of dissociation of solute

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

9.09%

13.1%

14.25%

11.2%

166. The unit of specific conductivity is

Ohm¯¹ cm¯¹

Ohm cm¯¹

Ohm¯¹ cm

Ohm cm¯²

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

58.5g NaCl/100ml

5.58g NaCl/100m

10.0g NaCl/100ml

20g NaCl/100ml

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

Electrons flow cathode to anode within the electrolytic solution

None of these

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

Electrons flow from cathode to anode through the external battery

169. Which has maximum oxidation number

170. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.3g/cm3

1.25g/cm3

1.20g/cm3

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

Drops to zero

Increases rapidly

Increases gradually

Does not change

172. Best way to prevent rusting iron is by

None of these

Putting it in saline water

Both of these

Making iron cathode

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

100

0.01

0.001

174. Solution with same osmotic pressures are called

Normal

Hypertonic

Hypotonic

Isotonic

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

Page 8 of 8

176. 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

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

Heat energy

Magnetic energy

Electrical energy

Sound energy

178. What are the ions present in water?

H2O

H and OH

H2 and O

H+ and OH-

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

4 N

2 N

6 N

8 N

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

Electroplating

Both A and B

None of these

Electrorefining

181. 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

1.25

None of these

2.5

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

None

183. Half cells are interconnected through

Electric circuit

Wire

Salt Bridge

No connection exists

184. Units of molarity are

None of these

Kg/lit

Mol/lit

Gm/lit

185. 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

18.6 c°

1.86 c°

186. When common salt is dissolved in water

B.P of water increase

Any possibility

B.P of water decrease

B.P of water remain constant

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

Na⁺ + e– → Na

Na → Na⁺ + e–

Br₂ + 2e – → 2Br –

2Br– → Br₂ + 2e –

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

Ionic concentration

Flow of solvent from a concentrated to a dilute solution

Elevation in boiling point

Diffusion rate of the solute

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

Melting point

Inversion point

Sublimation point

Boiling point

190. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/5

1/51

5.1

191. 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

0.281 V

0.176 V

0.399 V

192. Choose the best reducing agent among the following

F¯¹

Cl¯¹

I¯¹

Br¯¹

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Maan AliLast Updated: April 19, 2025

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