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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. Mole fraction of pure water is

None of these

Exactly equal to one

Slightly less than one

Slightly greater than one

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

1.5

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

40 g

60 g

4 g

6 g

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

Acts as a catalyst

Gains electrons

pH is changed

Loses electrons

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

Conduction

Induction

Electroplating

Electrolysis

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

∆ G = -ve, ∆ E = 0

∆ G = +ve, ∆ E = 0

∆ G = 0, ∆E = 0

∆ G = -ve

7. An electrolyte

Gives ions only when electricity is passed

Possesses ions even in solid state

Gives ions only when dissolved in water

Forms complex ions in solution

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

9. 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

10. Density of H₂SO₄ in lead accumulator is

120 g Cm³

1.25g/Cm³

1.15 g/Cm³

1.2 g/Cm³

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

Henry’s law

Raoult’s law

Ostwald’s dilution law

Distribution law

12. 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

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

Henry’s law

Arrhenius law

Ostwald’s law

Raoult’s law

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

1 ampere

1 coulomb

1 faraday

2 ampere

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

1.21 atm

12.1 atm

2.46 atm

24.6 atm

16. During a redox reaction, an oxidizing agent

Loses electrons

Gains electrons

Is oxidized

Is hydrolysed

17. 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 water decreases by the addition of nitric acid

Vapour pressure of pure benzene decreases by the addition of naphthalene

18. Secondary cell is

Rechargeable

Electrolytic cell

Daniel cell

Non rechargeable

19. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.25g/cm3

1.20g/cm3

1.3g/cm3

20. Potential of Zn is called

Oxidation

Reduction

It has not potential

Redox

21. Vant Hoff’s factor of Ca(NO₃)₂ is

22. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.4 M

0.04 M

0.2 M

0.8 M

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

Heat energy

Electrical energy

Sound energy

Magnetic energy

24. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/5

5.1

1/51

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

Vacuum distillation

Distillation

Fractional distillation

None of these

Page 2 of 8

26. Which has maximum oxidation number

27. In alkaline battery the anode is made up of

Cadmium

MnO2

AgO2

28. Pick out the wrong statement. In electrochemical cell

Electrons are released at anode

Salt bridge maintains the electrical neutrality of the solution

Chemical energy is converted into electrical energy

Cathode is regarded as negative electrode

29. Which of the following statements is FALSE?

All electrochemical reactions involve the transfer of electrons

Reduction occurs at cathode

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

30. Salt bridge transfers

Anions

Solvent particles

Current

Electrons

31. If liquids A and B form an ideal solution

The free energy of mixing is zero

The enthalpy of mixing is zero

The entropy of mixing is zero

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

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

1.81 cm¯³

1.25 cm¯³

1.15 cm¯³

2.15 cm¯³

33. 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

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

Cl¯

None of these

Both Na⁺ and CI¯

Na⁺

35. Standard hydrogen electrode has an arbitrarily fixed potential

0.00 volt

1.00 volt

None of these

0.10 volt

36. 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

37. The art of electroplating was given by

Thomas Gradam

Brugan

Faraday

Edison

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

Saturated

Unsaturated

Ideal

Supersaturated

39. The Vant Hoff factor (i) accounts for

Degree of solubilization of solute

The extent of dissociation of solute

The degree of decomposition of solution

The extent of dissolution of solute

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

Chemical energy

Heat energy

Electrical energy

None of these

41. Units of molarity are

Mol/lit

Kg/lit

Gm/lit

None of these

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

1 M

1 f

1 N

2 M

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

Gold has higher reduction potential then iron

Gold is denser

Iron rusts

Gold has lower reduction potential then iron

44. 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

0.1 M

0.15 M

0.2 M

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

4 g

5 g

1 g

2 g

46. Metals usually conduct electricity because

Metals have high resistance

Metals are decomposed by current

In metals the ions are free to more

They are mobile electrons in the metallic structure

47. 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

4 C

20 C

120 C

240 C

48. 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

63.5 gm

15.9 gm

31.8 gm

49. 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

5.6 cm³

11.2 cm³

56 cm³

550 cm³

50. 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

Page 3 of 8

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

212.3 kJ

175.4 kJ

53.07 kJ

106.15 kJ

52. Best way to prevent rusting iron is by

Making iron cathode

Putting it in saline water

Both of these

None of these

53. Half cells are interconnected through

No connection exists

Salt Bridge

Electric circuit

Wire

54. 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

C > B > A

A > C > B

B > C > A

A > B > C

55. Oxidation state of hydrogen in CaH₂ is

-2

-1

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

H₃PO₄

H₃PO₃

H₄P₃O₇

H₃PO₂

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

45.1

40.5

39.6

42.7

58. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

11 N

10 N

1 N

0.1N

59. 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

1.0 x 10¹⁰

4.0 x 10¹²

2.0 x 10¹¹

60. Specific conductivity of a solution

Decreases with dilution

Remains unchanged with dilution

Depends on mass of electrolyte

Increases with dilution

61. 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

10,000 s

30 s

30,000 s

62. Electrode potential of Zn is

Oxidation

Depends on the nature of the coupled electrode

Oxidation-reduction

Reduction

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

Dilute solution of glucose

Chloroform

Molten NaCl

Pure distilled water

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

2.16 g

0.27 g

0.54 g

1.08 g

65. Reaction takes place at anode is

Oxidation

Reduction

Hydrolysis

Ionization

66. 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

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

58.5g NaCl/100ml

20g NaCl/100ml

10.0g NaCl/100ml

5.58g NaCl/100m

68. 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

1.5

1.0

2.0

69. 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

0.30

0.25

0.35

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

71. 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

0.60

0.80

0.20

72. In an electrolytic cell current flows

From cathode to anode inside the cell

From cathode to anode in outer circuit

From anode to cathode inside the cell

From anode to cathode in an outer circuit

73. 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

74. 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

278 S cm² mol¯¹

302 S cm² mol¯¹

128 S cm² mol¯¹

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

Greater

Lesser

Sum of reduction and oxidation potentials

None

Page 4 of 8

76. 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

9 N

2 N

3 N

77. Maximum freezing point falls in

Camphor

Benzene

Naphthalene

Water

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

Precipitated

Hydrolyzed

Reduced

Oxidized

79. Temperature for standard electrode potential is

25 C°

300 K

273 K

310 K

80. Strong reducing agents have

Greater positive value of standard reduction potential

None of these

Lesser positive value of standard reduction potential

Greater negative value of standard reduction potential

81. What are the ions present in water?

H and OH

H2O

H2 and O

H+ and OH-

82. Colligative properties are the properties of

Concentration solutions behave as nearly non – ideal solutions

Both a and b

Neither a nor b

Dilute solution which behave as nearly ideal solution

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

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

Strong acid and its salt of weak base

84. Stronger the oxidizing agent, greater is the

Oxidation potential

Reduction potential

Redox potential

e.m.f of cell

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

0.25

0.5

0.05

2.05

86. Choose the best reducing agent among the following

I¯¹

F¯¹

Cl¯¹

Br¯¹

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

510 sec

642 sec

102 sec

12157.48 sec

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

0.0196

0.01

0.1

0.2

89. Alkaline battery has a voltage of

4.5V

2.5V

3.5V

1.5V

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

Ionization potential

Standard oxidation potential

Standard reduction potential

Cell voltage

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

None

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

Nitric acid

Boric acid

Sulphuric acid

Phosphorus acid

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

I₂

Pb²⁺

Ag⁺

94. Voltaic cell can be recharged by

By removal of solution

By heating it

By addition of fresh solution

By replacing external circuit with external source of electricity

95. Molarity of water is

55.5

96. 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

97. 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

98. Solution with same osmotic pressures are called

Hypotonic

Hypertonic

Normal

Isotonic

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

Increases rapidly

Drops to zero

Increases gradually

Does not change

100. 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)

0.399 V

0.176 V

0.281 V

0.222 V

Page 5 of 8

101. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

2.5

None of these

1 2

1.25

102. The best reducing agent is

Br¯

Cl¯

F¯

I¯

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

0.217

7.20

3.12

4.10

104. In a Galvanic cell, the electrons flow from

Anode to cathode through the solution

Cathode to anode through the solution

Cathode to anode through the external circuit

Anode to cathode through the external circuit

105. 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

0.918 cm¯¹

0.66 cm¯¹

1.12 cm¯¹

0.142 cm¯¹

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

Lower

Not particular

Higher

In middle

107. 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

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

Both A and B

Electrorefining

None of these

Electroplating

109. 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 10³

1.06 x 10²

1.06 x 10⁴

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

Galvanization

Electrolysis

Cathodic protection

Photo electrolysis

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

0.1 M Sucrose

0.1 M Glucose

0.1 M BaCl₂

0.1 M NaCl

112. 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

0.512

0.186

113. 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

Hg is more inert than Pt

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

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

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

0.0196

0.1

0.01

0.2

115. Camphor is often used in molecular mass determination because

It is solvent for organic substances

It is volatile

It is readily available

It has a very high cryoscopic constant

116. The solubility of a gas in water depends upon

Temperature

Nature of the gas

Pressure of the gas

All of these

117. Reduction always occurs

Both A and B

At cathode

None of these

At anode

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

Galvanic cell

Electrolytic cell

Fuel cell

Dry cell

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

Ionization potential

Electroplating

Electric change

Standard electrode potential

120. 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

2 N

4 N

0.4 N

0.2 N

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

All

1 normal

1 molal

1 molar

122. 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

4 N

6 N

123. A redox reaction involves

A reaction in a solution

Proton transfer

Electron transfer

Ion combination reaction

124. 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

6.4 g

12.8 g

3.2 g

2.3 g

125. The degree of dissociation of weak electrolyte increases as

Pressure increases

None

Dilution decreases

Dilution increases

Page 6 of 8

126. Oxidation number of carbon in NaHCO₃ is

-6

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

2.5 atom

Slightly more than 1 atom

750 torr

760 mm of Hg

128. In a Galvanic cell

Electrical energy is converted into heat

Electrical energy is converted into chemical energy

Chemical energy is converted into electricity

Chemical energy is converted into heat

129. 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

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

O₂, Na

O₂,H₂

O₂, SO₂

None of these

131. 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°

132. 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)

33.3

3.33

0.0033

0.333

133. Corrosion is basically a

Altered reaction in presence of H₂O

Interaction

Union between two light metals and a heavy metal

Electrochemical phenomenon

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

+ 1.17 V

+ 0.35

– 0.35 V

– 1.17 V

135. 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

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

HgCl₂

Hg₂Cl₂

CuSO₄

ZnCl₂

137. In alkaline battery anode is made up of

Cadmium

MnO₂

AgO₂

138. Cathode provides electrons to

-Ve ion

+Ve ion

Does not provide any electron

Neutral atom

139. Oxidation in a chemical reaction involves

Increase in oxidation number

Increase in oxidation number of all the elements on reactant side

Decrease in oxidation number

Both are possible

140. In a chemical reaction, oxidation process involves

Increase in oxidation number of element

Decrease in oxidation number of element

Oxidation number neither increases nor decreases

Increase in oxidation number of the elements in reactants

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

0.5 molal

1.1 molal

0.1 molal

1 molal

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

F₂O

Cl₂O

Na₂O₂

Na₂O

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

Ca(OH)₂

NaOH

KOH

NH₄OH

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

Na₂SO₄

CH₃ CooNH₄

NH₄Cl

NaCl

145. Chemical used in salt bridge is

KOH

KNO3

KCI

KBr

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

Electrons flow cathode to anode within the electrolytic solution

Electrons flow from cathode to anode through the external battery

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

None of these

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

Boiling point

Inversion point

Melting point

Sublimation point

148. Which of the following is a strong electrolyte?

HCN

NH₄OH

Ca(NO₃)₂

CH₃COOH

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

Na → Na⁺ + e–

Br₂ + 2e – → 2Br –

2Br– → Br₂ + 2e –

Na⁺ + e– → Na

150. 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 and Hg

Na, Pt and graphite

Pt and graphite only

Page 7 of 8

151. 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

152. In electrolytic cell, electricity in carried out by

Spontaneous reaction

Non-spontaneous reaction

Neutralization

All

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

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

Surface tension

Osmotic pressure

Refractive index

Viscosity

155. Molton NaCl conducts electricity due to the presence of

Atoms of Na and Cl.

Free molecules

Free ions

Free electrons

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

Generate heat

Remove adsorbed oxygen from electrode surfaces

Create potential difference between two electrodes

Produce high purity water

157. 96500 C of electricity liberates from CuSO₄ solution

100 g of Cu

31.75 g of Cu

96500 g of CU

63.5 g of Cu

158. Decrease in oxidation number is called

All of these

Oxidation

Reduction

Redox

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

0.9

0.6

0.2

0.3

160. Azeotropic mixture of HCl and water has

22.2% HCl

36% HCl

20.2% HCl

48% HCl

161. Corrosion reactions are

Spontaneous redox reactions

Spontaneous acid–base reactions

None of these

Non-spontaneous redox reactions

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

2 to 5

0 to 5.

0 to –3

1 to 5

163. Pure water does not conduct electricity because it

Is almost unionized

Has low boiling point

Is neutral

Is readily decomposed

164. The conductivity of strong electrolyte

Decreases on dilution

Does not change on dilution

Depends on density of electrolyte itself.

Increases on dilution slightly

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

Hydrogen

Oxygen

Chloride

Chlorine

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

Gram per million

Microgram percent

Milligram percent

Parts per million

167. When common salt is dissolved in water

B.P of water increase

B.P of water decrease

B.P of water remain constant

Any possibility

168. 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

224 cm³

1.008 g

112 cm³

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

5.51

6.1

1.32

5.65

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

Elevation in boiling point

Diffusion rate of the solute

Ionic concentration

Flow of solvent from a concentrated to a dilute solution

171. 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

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

Equal to that of water

Less than that of water

Equal to that of ethanol

More than that of H₂O

173. Salt bridge transfers

Electrons

Anion

Ions

Current

174. The unit of specific conductivity is

Ohm¯¹ cm

Ohm cm¯¹

Ohm¯¹ cm¯¹

Ohm cm¯²

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

193000

10000

48250

96500

Page 8 of 8

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

Reduction

Oxidation

Both

Reduction

177. Electricity in voltaic cell is produced due to

Reduction

B + C

Neutralization

Oxidation

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

An electrolytic cell

A galvanic cell

A chemical cell

A voltaic cell

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

KCl

MgCl₂

NaCl

BaCl₂

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

Rust removal

Making leather

Manufacture of bleach

Electroplating

181. 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 m² mol¯¹

S² m² mol¯²

S m mol¯¹

182. 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

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

0.1 N NaCl

Graphite

Glass

0.1 N HCl

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

14.25%

13.1%

9.09%

11.2%

185. The reference electrode is made by using

Hg₂Cl₂

CuSO₄

ZnCl₂

HgCl₂

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

Decrease rapidly

Does not change

Decreases slowly

Drops to zero

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

Both oxidation and reduction

Oxidation

Neither oxidation and reduction

Reduction

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

800 mm of Hg

780 mm of Hg

750 mm of Hg

760 mm of Hg

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

10 ml

80 ml

40 ml

20 ml

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

Cathode

None of these

Electrode

Anode

191. 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 negative values reduction potential

Reduction potentials are negative

Very high positive value of reduction potential

Very low ionization potential values

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

None of these

Electrochemical equivalent

One gm. Equivalent weight

One gm. atomic weight

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Maan AliLast Updated: April 19, 2025

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