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

1.15 cm¯³

1.25 cm¯³

1.81 cm¯³

2.15 cm¯³

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

750 mm of Hg

780 mm of Hg

800 mm of Hg

760 mm of Hg

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

0.0196

0.2

0.1

0.01

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

Electrorefining

None of these

Electroplating

Both A and B

5. 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)₄Cl₃]Cl

[Pt(NH₃)₄Cl]Cl₃

[Pt(NH₃)₄Cl₄]

6. The solubility of a gas in water depends upon

All of these

Nature of the gas

Pressure of the gas

Temperature

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

1 faraday

2 ampere

1 ampere

1 coulomb

8. 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

20 C

120 C

4 C

9. 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

10. 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

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

Phosphorus acid

Sulphuric acid

Nitric acid

Boric acid

12. 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

Electrolysis

Conduction

13. 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

21.6 g

108 g

1.08 g

10.8 g

14. Stronger the oxidizing agent, greater is the

Reduction potential

Oxidation potential

e.m.f of cell

Redox potential

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

16. 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

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

Refractive index

Viscosity

Surface tension

Osmotic pressure

18. 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

Very high negative values reduction potential

Very low ionization potential values

Reduction potentials are negative

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

1.06 x 10⁴

1.06 x 10³

1.06 x 10²

20. Molarity of water is

55.5

21. 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

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

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

Decreases slowly

Decrease rapidly

Drops to zero

Does not change

24. Choose the best reducing agent among the following

I¯¹

Br¯¹

F¯¹

Cl¯¹

25. 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

Page 2 of 8

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

8 N

2 N

4 N

6 N

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

Create potential difference between two electrodes

Generate heat

Remove adsorbed oxygen from electrode surfaces

Produce high purity water

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

I₂

Ag⁺

Pb²⁺

29. 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?

8.14 M

4.18 M

18 M

18.4 M

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

Pure distilled water

Chloroform

Molten NaCl

Dilute solution of glucose

31. 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

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

1 M

1 N

1 f

2 M

33. 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 > B > C

A > C > B

C > B > A

B > C > A

34. 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

35. Salt bridge transfers

Current

Ions

Electrons

Anion

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

A galvanic cell

A chemical cell

An electrolytic cell

A voltaic cell

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

∆ G = -ve, ∆ E = 0

∆ G = 0, ∆E = 0

∆ G = +ve, ∆ E = 0

∆ G = -ve

38. Alkaline battery has a voltage of

1.5V

4.5V

3.5V

2.5V

39. 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

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

Electrical energy

Sound energy

Heat energy

Magnetic energy

41. Mole fraction of pure water is

None of these

Exactly equal to one

Slightly greater than one

Slightly less than one

42. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/5

1/51

5.1

43. 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

44. Chemical used in salt bridge is

KNO3

KOH

KCI

KBr

45. In electrolytic cell, electricity in carried out by

All

Spontaneous reaction

Non-spontaneous reaction

Neutralization

46. Which has maximum oxidation number

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

0.25

0.5

0.05

2.05

48. The art of electroplating was given by

Faraday

Edison

Brugan

Thomas Gradam

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

Glass

0.1 N HCl

0.1 N NaCl

Graphite

50. 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

106.15 kJ

53.07 kJ

Page 3 of 8

51. 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

Li is smaller in size as compared to Cu

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

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

52. 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°

1.86 c°

Sufficient date not given

18.6 c°

53. Specific conductivity of a solution

Decreases with dilution

Increases with dilution

Remains unchanged with dilution

Depends on mass of electrolyte

54. The depression of freezing point is directly proportional to

Molarity of the solvent

Mole fraction of the solution

Molarity of the solution

Molality of the solution

55. Salt bridge transfers

Solvent particles

Electrons

Current

Anions

56. 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

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

NaOH

NH₄OH

KOH

Ca(OH)₂

58. Standard hydrogen electrode has an arbitrarily fixed potential

1.00 volt

None of these

0.10 volt

0.00 volt

59. Pick out the wrong statement. In electrochemical cell

Chemical energy is converted into electrical energy

Cathode is regarded as negative electrode

Salt bridge maintains the electrical neutrality of the solution

Electrons are released at anode

60. 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

61. An electrolyte

Gives ions only when electricity is passed

Forms complex ions in solution

Possesses ions even in solid state

Gives ions only when dissolved in water

62. Oxidation in a chemical reaction involves

Both are possible

Decrease in oxidation number

Increase in oxidation number

Increase in oxidation number of all the elements on reactant side

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

Electrons flow from cathode to anode through the external battery

None of these

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

Electrons flow cathode to anode within the electrolytic solution

64. 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

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

Precipitated

Reduced

Oxidized

Hydrolyzed

66. Oxidation state of hydrogen in CaH₂ is

-1

-2

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

12157.48 sec

510 sec

642 sec

102 sec

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

42.7

45.1

40.5

39.6

69. 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

70. 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

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

71. The best reducing agent is

F¯

I¯

Br¯

Cl¯

72. 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

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

Chemical energy

Heat energy

Electrical energy

None of these

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

5.65

6.1

1.32

5.51

75. Electricity in voltaic cell is produced due to

Neutralization

Reduction

Oxidation

B + C

Page 4 of 8

76. Reduction always occurs

None of these

At anode

At cathode

Both A and B

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

F₂O

Cl₂O

Na₂O

Na₂O₂

78. Electrode potential of Zn is

Depends on the nature of the coupled electrode

Oxidation-reduction

Oxidation

Reduction

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

Fuel cell

Daniel cell

Electrolytic cell

Galvanic cell

80. Azeotropic mixture of HCl and water has

20.2% HCl

22.2% HCl

36% HCl

48% HCl

81. Secondary cell is

Electrolytic cell

Daniel cell

Rechargeable

Non rechargeable

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

pH is changed

Acts as a catalyst

Gains electrons

Loses electrons

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

NH₄Cl

NaCl

CH₃ CooNH₄

Na₂SO₄

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

0.1 M NaCl

0.1 M Glucose

0.1 M Sucrose

0.1 M BaCl₂

85. Density of H₂SO₄ in lead accumulator is

1.15 g/Cm³

1.25g/Cm³

120 g Cm³

1.2 g/Cm³

86. Reaction takes place at anode is

Oxidation

Reduction

Ionization

Hydrolysis

87. 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

72 torr

68 torr

20 torr

140 torr

88. The Vant Hoff factor (i) accounts for

The degree of decomposition of solution

Degree of solubilization of solute

The extent of dissociation of solute

The extent of dissolution of solute

89. Colligative properties are the properties of

Neither a nor b

Both a and b

Dilute solution which behave as nearly ideal solution

Concentration solutions behave as nearly non – ideal solutions

90. 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 molal

1.1 molal

0.1 molal

91. Cathode provides electrons to

Neutral atom

+Ve ion

Does not provide any electron

-Ve ion

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

All

1 molal

1 normal

1 molar

93. 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

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

In middle

Higher

Lower

Not particular

95. Voltaic cell can be recharged by

By heating it

By removal of solution

By replacing external circuit with external source of electricity

By addition of fresh solution

96. Corrosion is basically a

Electrochemical phenomenon

Altered reaction in presence of H₂O

Union between two light metals and a heavy metal

Interaction

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

None of these

Cl¯

Na⁺

Both Na⁺ and CI¯

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

Chlorine

Oxygen

Hydrogen

Chloride

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

Greater

Sum of reduction and oxidation potentials

Lesser

None

100. Best way to prevent rusting iron is by

None of these

Both of these

Making iron cathode

Putting it in saline water

Page 5 of 8

101. 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

9 N

2 N

1 N

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

1.21 atm

12.1 atm

2.46 atm

24.6 atm

103. 96500 C of electricity liberates from CuSO₄ solution

96500 g of CU

100 g of Cu

31.75 g of Cu

63.5 g of Cu

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

760 mm of Hg

750 torr

Slightly more than 1 atom

2.5 atom

105. 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

0.15 M

0.1 M

106. In a Galvanic cell, the electrons flow from

Anode to cathode through the external circuit

Anode to cathode through the solution

Cathode to anode through the solution

Cathode to anode through the external circuit

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

CuSO₄

HgCl₂

Hg₂Cl₂

ZnCl₂

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

None

109. In a Galvanic cell

Chemical energy is converted into heat

Electrical energy is converted into chemical energy

Chemical energy is converted into electricity

Electrical energy is converted into heat

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

Ostwald’s law

Raoult’s law

Henry’s law

Arrhenius law

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

Photo electrolysis

Electrolysis

Galvanization

Cathodic protection

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

0.9

0.2

0.6

0.3

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

Oxidation

Reduction

Both

114. 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

224 cm³

112 cm³

115. 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

2.0 x 10¹¹

4.0 x 10¹²

1.0 x 10²

116. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.20g/cm3

1.25g/cm3

1.3g/cm3

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

Supersaturated

Unsaturated

Saturated

Ideal

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

Making leather

Manufacture of bleach

Rust removal

Electroplating

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

0.5

2.0

1.0

1.5

120. 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

5.6 cm³

550 cm³

56 cm³

121. The reference electrode is made by using

Hg₂Cl₂

ZnCl₂

CuSO₄

HgCl₂

122. 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

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

58.5g NaCl/100ml

5.58g NaCl/100m

20g NaCl/100ml

10.0g NaCl/100ml

124. 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

125. In a chemical reaction, oxidation process involves

Increase in oxidation number of the elements in reactants

Increase in oxidation number of element

Oxidation number neither increases nor decreases

Decrease in oxidation number of element

Page 6 of 8

126. Decrease in oxidation number is called

Oxidation

Redox

All of these

Reduction

127. 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, Pt and graphite

Na and Hg

Na and S only

128. In alkaline battery anode is made up of

AgO₂

Cadmium

MnO₂

129. 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 m² mol¯¹

S² m² mol

S m mol¯¹

S² m² mol¯²

130. In alkaline battery the anode is made up of

MnO2

AgO2

Cadmium

131. Corrosion reactions are

Non-spontaneous redox reactions

Spontaneous redox reactions

None of these

Spontaneous acid–base reactions

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

Gold is denser

Gold has lower reduction potential then iron

Iron rusts

Gold has higher reduction potential then iron

133. Maximum freezing point falls in

Camphor

Benzene

Naphthalene

Water

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

Cell voltage

Standard oxidation potential

Ionization potential

Standard reduction potential

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

1.5

136. 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

1.25

1 2

2.5

137. What are the ions present in water?

H and OH

H2O

H2 and O

H+ and OH-

138. 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

Vapour pressure of pure benzene decreases by the addition of naphthalene

Boiling point of pure benzene increases by the addition of toluene

Boiling point of pure water decreases by the addition of ethanol

139. Oxidation number of carbon in NaHCO₃ is

-6

140. Which of the following is a strong electrolyte?

NH₄OH

CH₃COOH

Ca(NO₃)₂

HCN

141. Solution with same osmotic pressures are called

Hypotonic

Hypertonic

Isotonic

Normal

142. 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%

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

144. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

0.5 mole

2.00 mole

1.0 mole

0.25 mole

145. A redox reaction involves

A reaction in a solution

Electron transfer

Proton transfer

Ion combination reaction

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

One gm. Equivalent weight

None of these

Electrochemical equivalent

One gm. atomic weight

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

48250

96500

193000

10000

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

Does not change

Increases rapidly

Increases gradually

Drops to zero

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

MgCl₂

BaCl₂

KCl

NaCl

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

+ 1.17 V

– 0.35 V

– 1.17 V

+ 0.35

Page 7 of 8

151. Half cells are interconnected through

Salt Bridge

Wire

Electric circuit

No connection exists

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

Gram per million

Milligram percent

Microgram percent

Parts per million

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

None of these

Distillation

Fractional distillation

Vacuum distillation

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

1 g

5 g

2 g

4 g

155. Units of molarity are

Gm/lit

Mol/lit

None of these

Kg/lit

156. In an electrolytic cell current flows

From cathode to anode inside the cell

From anode to cathode inside the cell

From cathode to anode in outer circuit

From anode to cathode in an outer circuit

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

Henry’s law

Ostwald’s dilution law

Raoult’s law

Distribution law

158. 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

159. During a redox reaction, an oxidizing agent

Loses electrons

Gains electrons

Is oxidized

Is hydrolysed

160. The unit of specific conductivity is

Ohm cm¯²

Ohm¯¹ cm

Ohm cm¯¹

Ohm¯¹ cm¯¹

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

2 to 5

0 to –3

0 to 5.

1 to 5

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

0.0196

0.1

0.01

0.2

163. 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)

3.33

0.0033

33.3

0.333

164. Metals usually conduct electricity because

They are mobile electrons in the metallic structure

In metals the ions are free to more

Metals are decomposed by current

Metals have high resistance

165. The conductivity of strong electrolyte

Increases on dilution slightly

Decreases on dilution

Depends on density of electrolyte itself.

Does not change on dilution

166. Strong reducing agents have

Lesser positive value of standard reduction potential

None of these

Greater positive value of standard reduction potential

Greater negative value of standard reduction potential

167. Potential of Zn is called

Oxidation

Redox

Reduction

It has not potential

168. 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

0.2 N

4 N

0.4 N

169. The degree of dissociation of weak electrolyte increases as

Dilution decreases

Pressure increases

Dilution increases

None

170. 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

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

Ionic concentration

Elevation in boiling point

Flow of solvent from a concentrated to a dilute solution

Diffusion rate of the solute

172. 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

302 S cm² mol¯¹

278 S cm² mol¯¹

128 S cm² mol¯¹

173. Which of the following statements is FALSE?

Reduction occurs at cathode

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

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

All electrochemical reactions involve the transfer of electrons

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

H₃PO₂

H₃PO₄

H₃PO₃

H₄P₃O₇

175. 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

10 g

2 g

1 g

Page 8 of 8

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

Oxidation

Reduction

Neither oxidation and reduction

Both oxidation and reduction

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

O₂,H₂

O₂, SO₂

None of these

O₂, Na

178. 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

0.80

0.60

0.20

179. 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

2.0

1.5

1.0

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

6 g

4 g

60 g

40 g

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

12.7 gm

15.9 gm

31.8 gm

63.5 gm

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

10,000 s

30,000 s

10 s

30 s

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

7.20

0.217

3.12

4.10

184. Molton NaCl conducts electricity due to the presence of

Atoms of Na and Cl.

Free electrons

Free molecules

Free ions

185. 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)

0.176 V

0.399 V

0.222 V

0.281 V

186. Pure water does not conduct electricity because it

Is readily decomposed

Is neutral

Is almost unionized

Has low boiling point

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. Temperature for standard electrode potential is

25 C°

300 K

273 K

310 K

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

Galvanic cell

Dry cell

Electrolytic cell

Fuel cell

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

None of these

Electrode

Cathode

Anode

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

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

Melting point

Inversion point

Sublimation point

Boiling point

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Maan AliLast Updated: April 19, 2025

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