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

1.5

2. 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

0.142 cm¯¹

1.12 cm¯¹

3. In electrolytic cell, electricity in carried out by

All

Spontaneous reaction

Non-spontaneous reaction

Neutralization

4. 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

0.20

0.60

0.75

0.80

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

Reduced

Oxidized

Precipitated

Hydrolyzed

6. 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

20 g

2 g

1 g

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

Chloride

Chlorine

Hydrogen

Oxygen

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

4 g

1 g

5 g

2 g

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

None

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

39.6

45.1

42.7

40.5

11. Pick out the wrong statement. In electrochemical cell

Electrons are released at anode

Chemical energy is converted into electrical energy

Cathode is regarded as negative electrode

Salt bridge maintains the electrical neutrality of the solution

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

9.09%

14.25%

11.2%

13.1%

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

1.21 atm

12.1 atm

24.6 atm

2.46 atm

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

15. The art of electroplating was given by

Brugan

Faraday

Edison

Thomas Gradam

16. The degree of dissociation of weak electrolyte increases as

Pressure increases

None

Dilution increases

Dilution decreases

17. Specific conductivity of a solution

Remains unchanged with dilution

Decreases with dilution

Increases with dilution

Depends on mass of electrolyte

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

Reduction

Both

Oxidation

19. Pure water does not conduct electricity because it

Is readily decomposed

Is neutral

Has low boiling point

Is almost unionized

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

Greater

None

Lesser

Sum of reduction and oxidation potentials

21. In alkaline battery the anode is made up of

Cadmium

AgO2

MnO2

22. 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

176 S cm² mol¯¹

128 S cm² mol¯¹

278 S cm² mol¯¹

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

1 coulomb

1 faraday

2 ampere

1 ampere

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

I₂

Pb²⁺

Ag⁺

25. 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

Page 2 of 8

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

Electrolytic cell

Fuel cell

Galvanic cell

Dry cell

27. In a Galvanic cell

Chemical energy is converted into electricity

Chemical energy is converted into heat

Electrical energy is converted into chemical energy

Electrical energy is converted into heat

28. 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

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

0.01

0.1

0.0196

0.2

30. 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

C > B > A

B > C > A

A > C > B

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

KOH

NH₄OH

Ca(OH)₂

NaOH

32. Cathode provides electrons to

Neutral atom

-Ve ion

Does not provide any electron

+Ve ion

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

Lower

Not particular

Higher

In middle

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

48250

10000

193000

96500

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

Henry’s law

Raoult’s law

Arrhenius law

Ostwald’s law

36. The unit of specific conductivity is

Ohm¯¹ cm

Ohm¯¹ cm¯¹

Ohm cm¯²

Ohm cm¯¹

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

Gold has lower reduction potential then iron

Iron rusts

Gold has higher reduction potential then iron

Gold is denser

38. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.20g/cm3

1.3g/cm3

1.25g/cm3

39. 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

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

H₃PO₃

H₃PO₂

H₃PO₄

H₄P₃O₇

41. Alkaline battery has a voltage of

3.5V

1.5V

4.5V

2.5V

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

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

Ostwald’s dilution law

Distribution law

Henry’s law

Raoult’s law

44. Azeotropic mixture of HCl and water has

22.2% HCl

20.2% HCl

36% HCl

48% HCl

45. Salt bridge transfers

Anion

Ions

Electrons

Current

46. 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)₄Cl]Cl₃

[Pt(NH₃)₄Cl₄]

[Pt(NH₃)₄Cl₃]Cl

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

Both A and B

None of these

Electroplating

Electrorefining

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

Less than that of water

Equal to that of ethanol

More than that of H₂O

Equal to that of water

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

212.3 kJ

106.15 kJ

175.4 kJ

53.07 kJ

50. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

1.0 mole

0.5 mole

0.25 mole

2.00 mole

Page 3 of 8

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

Unsaturated

Supersaturated

Saturated

Ideal

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

Melting point

Sublimation point

Boiling point

Inversion point

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

Standard oxidation potential

Standard reduction potential

Ionization potential

Cell voltage

54. 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

5.6 cm³

550 cm³

55. 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

S m² mol¯¹

S² m² mol¯²

S² m² mol

56. 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

1.0

1.5

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

Chemical energy

Electrical energy

Heat energy

None of these

58. A redox reaction involves

Proton transfer

A reaction in a solution

Electron transfer

Ion combination reaction

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

1.15 cm¯³

2.15 cm¯³

1.25 cm¯³

1.81 cm¯³

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

800 mm of Hg

780 mm of Hg

760 mm of Hg

750 mm of Hg

61. Salt bridge transfers

Solvent particles

Electrons

Anions

Current

62. Vant Hoff’s factor of Ca(NO₃)₂ is

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

Sulphuric acid

Phosphorus acid

Boric acid

Nitric acid

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

MgCl₂

KCl

BaCl₂

NaCl

65. An electric current is passed through silver nitrate solution using silver electrodes. 10.79 g of silver was found to be deposited on the cathode if the same amount of electricity is passed through copper sulphate solution using copper electrodes, the weight of copper deposited on the cathode is

3.2 g

12.8 g

6.4 g

2.3 g

66. An electrolyte

Possesses ions even in solid state

Forms complex ions in solution

Gives ions only when dissolved in water

Gives ions only when electricity is passed

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

Electrolytic cell

Fuel cell

Galvanic cell

Daniel cell

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

Osmotic pressure

Viscosity

Surface tension

Refractive index

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

Electrolysis

Induction

Electroplating

Conduction

70. Stronger the oxidizing agent, greater is the

Oxidation potential

e.m.f of cell

Redox potential

Reduction potential

71. 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

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

Boiling point of pure water decreases by the addition of ethanol

Boiling point of pure benzene increases by the addition of toluene

72. Voltaic cell can be recharged by

By removal of solution

By addition of fresh solution

By heating it

By replacing external circuit with external source of electricity

73. Decrease in oxidation number is called

Reduction

All of these

Oxidation

Redox

74. The solubility of a gas in water depends upon

Pressure of the gas

Temperature

All of these

Nature of the gas

75. 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

Page 4 of 8

76. Same amount of electric current is passed through solution if AgNO₃ and HCl. If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated as S.T.P. in the second case is:

112 cm³

1.008 g

22400 cm³

224 cm³

77. Chemical used in salt bridge is

KBr

KCI

KOH

KNO3

78. Temperature for standard electrode potential is

25 C°

300 K

310 K

273 K

79. Reaction takes place at anode is

Hydrolysis

Reduction

Oxidation

Ionization

80. Metals usually conduct electricity because

They are mobile electrons in the metallic structure

Metals have high resistance

Metals are decomposed by current

In metals the ions are free to more

81. 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

0.281 V

0.222 V

0.176 V

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

1 molal

1 normal

All

1 molar

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

Microgram percent

Parts per million

Milligram percent

Gram per million

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

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

None of these

Electrons flow cathode to anode within the electrolytic solution

Electrons flow from cathode to anode through the external battery

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

86. 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

87. 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

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

Drops to zero

Decrease rapidly

Does not change

Decreases slowly

89. Maximum freezing point falls in

Benzene

Naphthalene

Water

Camphor

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

Electroplating

Rust removal

Manufacture of bleach

Making leather

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

3.12

4.10

7.20

0.217

92. The conductivity of strong electrolyte

Decreases on dilution

Does not change on dilution

Depends on density of electrolyte itself.

Increases on dilution slightly

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

6.1

5.65

1.32

5.51

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

Acts as a catalyst

pH is changed

Gains electrons

Loses electrons

95. If liquids A and B form an ideal solution

The free energy of mixing is zero

The enthalpy of mixing is zero

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

The entropy of mixing is zero

96. In alkaline battery anode is made up of

MnO₂

Cadmium

AgO₂

97. 96500 C of electricity liberates from CuSO₄ solution

63.5 g of Cu

96500 g of CU

100 g of Cu

31.75 g of Cu

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

0.0186

1.86

0.0521

0.521

99. Oxidation number of carbon in NaHCO₃ is

-6

100. The best reducing agent is

Br¯

I¯

F¯

Cl¯

Page 5 of 8

101. 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

1.0 x 10²

4.0 x 10¹²

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

Cl₂O

Na₂O₂

Na₂O

F₂O

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

102 sec

510 sec

642 sec

12157.48 sec

104. 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

18.4 M

4.18 M

18 M

105. Density of H₂SO₄ in lead accumulator is

1.25g/Cm³

120 g Cm³

1.15 g/Cm³

1.2 g/Cm³

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

1.08 g

2.16 g

0.54 g

0.27 g

107. In a chemical reaction, oxidation process involves

Decrease in oxidation number of element

Increase in oxidation number of the elements in reactants

Oxidation number neither increases nor decreases

Increase in oxidation number of element

108. In an electrolytic cell current flows

From anode to cathode inside the cell

From cathode to anode inside the cell

From cathode to anode in outer circuit

From anode to cathode in an outer circuit

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

Increases gradually

Does not change

Drops to zero

Increases rapidly

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

NaCl

CH₃ CooNH₄

Na₂SO₄

NH₄Cl

111. 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

112. Colligative properties are the properties of

Dilute solution which behave as nearly ideal solution

Both a and b

Neither a nor b

Concentration solutions behave as nearly non – ideal solutions

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

750 torr

2.5 atom

Slightly more than 1 atom

760 mm of Hg

114. Potential of Zn is called

Oxidation

Redox

It has not potential

Reduction

115. In a Galvanic cell, the electrons flow from

Cathode to anode through the solution

Anode to cathode through the external circuit

Anode to cathode through the solution

Cathode to anode through the external circuit

116. 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

117. The reference electrode is made by using

HgCl₂

CuSO₄

ZnCl₂

Hg₂Cl₂

118. 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 –

119. Half cells are interconnected through

Electric circuit

Salt Bridge

Wire

No connection exists

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

Electrolysis

Galvanization

Cathodic protection

Photo electrolysis

121. 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

0.35

0.30

0.25

0.40

122. Units of molarity are

None of these

Gm/lit

Kg/lit

Mol/lit

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

CuSO₄

HgCl₂

ZnCl₂

Hg₂Cl₂

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

0.25

2.05

0.5

0.05

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

0.1 M Glucose

0.1 M Sucrose

0.1 M NaCl

0.1 M BaCl₂

Page 6 of 8

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

Diffusion rate of the solute

Flow of solvent from a concentrated to a dilute solution

Ionic concentration

Elevation in boiling point

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

80 ml

40 ml

20 ml

10 ml

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

None of these

Cl¯

Na⁺

Both Na⁺ and CI¯

129. Molton NaCl conducts electricity due to the presence of

Atoms of Na and Cl.

Free electrons

Free ions

Free molecules

130. During a redox reaction, an oxidizing agent

Is oxidized

Is hydrolysed

Gains electrons

Loses electrons

131. Which of the following statements is FALSE?

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

All electrochemical reactions involve the transfer of electrons

132. Camphor is often used in molecular mass determination because

It is solvent for organic substances

It has a very high cryoscopic constant

It is volatile

It is readily available

133. Solution with same osmotic pressures are called

Normal

Hypertonic

Isotonic

Hypotonic

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

1 M

2 M

1 N

1 f

135. Reduction always occurs

Both A and B

At cathode

None of these

At anode

136. Oxidation in a chemical reaction involves

Both are possible

Increase in oxidation number

Decrease in oxidation number

Increase in oxidation number of all the elements on reactant side

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

None of these

Distillation

Fractional distillation

Vacuum distillation

138. Choose the best reducing agent among the following

I¯¹

Br¯¹

F¯¹

Cl¯¹

139. 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 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⁺

Li is smaller in size as compared to Cu

140. The depression of freezing point is directly proportional to

Mole fraction of the solution

Molarity of the solvent

Molarity of the solution

Molality of the solution

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

None of these

One gm. atomic weight

One gm. Equivalent weight

Electrochemical equivalent

142. Molarity of water is

55.5

143. 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

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

6 N

8 N

2 N

4 N

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

Generate heat

Remove adsorbed oxygen from electrode surfaces

Produce high purity water

Create potential difference between two electrodes

146. 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 high negative values reduction potential

Very high positive value of reduction potential

Very low ionization potential values

147. Calculate the amount of charge flowing in 2 minute in a wire of resistance 10 Ω when a potential difference of 20 V is applied

240 C

4 C

20 C

120 C

148. 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

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

60 g

4 g

40 g

6 g

150. 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

Page 7 of 8

151. 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

72 torr

140 torr

20 torr

152. 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

31.8 gm

63.5 gm

15.9 gm

153. Which has maximum oxidation number

154. 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

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

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

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

0 to –3

0 to 5.

2 to 5

1 to 5

156. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.8 M

0.4 M

0.2 M

0.04 M

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

An electrolytic cell

A chemical cell

A voltaic cell

A galvanic cell

158. 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°

18.6 c°

Sufficient date not given

1.86 c°

159. The Vant Hoff factor (i) accounts for

The extent of dissolution of solute

The degree of decomposition of solution

Degree of solubilization of solute

The extent of dissociation of solute

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

None of these

Equal to the total volume of the components

Slightly more than the total volume of the components

Slightly less than the total volume of the components

161. Electrode potential of Zn is

Oxidation-reduction

Reduction

Oxidation

Depends on the nature of the coupled electrode

162. What are the ions present in water?

H2O

H+ and OH-

H2 and O

H and OH

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

Oxidation

Both oxidation and reduction

Reduction

Neither oxidation and reduction

164. Electricity in voltaic cell is produced due to

Reduction

Oxidation

Neutralization

B + C

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

58.5g NaCl/100ml

10.0g NaCl/100ml

5.58g NaCl/100m

20g NaCl/100ml

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

Strong acid and its salt of weak base

A strong acid and its salt of a strong base

Weak acid and its salt of weak base

Weak acid and its salt of strong base

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

– 0.35 V

+ 1.17 V

+ 0.35

– 1.17 V

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

∆ G = 0, ∆E = 0

∆ G = +ve, ∆ E = 0

∆ G = -ve

∆ G = -ve, ∆ E = 0

169. 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

33.3

0.0033

0.333

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

1 molal

0.5 molal

0.1 molal

1.1 molal

171. Corrosion is basically a

Altered reaction in presence of H₂O

Interaction

Union between two light metals and a heavy metal

Electrochemical phenomenon

172. Secondary cell is

Daniel cell

Rechargeable

Electrolytic cell

Non rechargeable

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

Electrical energy

Sound energy

Magnetic energy

Heat energy

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

Molten NaCl

Pure distilled water

Chloroform

Dilute solution of glucose

175. Mole fraction of pure water is

Exactly equal to one

None of these

Slightly greater than one

Slightly less than one

Page 8 of 8

176. 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

108 g

10.8 g

1.08 g

21.6 g

177. 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

178. 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

179. Best way to prevent rusting iron is by

Both of these

Making iron cathode

None of these

Putting it in saline water

180. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/51

5.1

1/5

181. Oxidation state of hydrogen in CaH₂ is

-1

-2

182. Standard hydrogen electrode has an arbitrarily fixed potential

None of these

0.00 volt

1.00 volt

0.10 volt

183. Strong reducing agents have

Lesser positive value of standard reduction potential

Greater positive value of standard reduction potential

Greater negative value of standard reduction potential

None of these

184. 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

185. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

10 N

11 N

0.1N

1 N

186. Which of the following is a strong electrolyte?

NH₄OH

Ca(NO₃)₂

CH₃COOH

HCN

187. 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

10 s

30 s

30,000 s

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

Electrode

None of these

Anode

Cathode

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

0.512

0.0512

0.186

0.80

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

0.1 N NaCl

0.1 N HCl

Graphite

Glass

191. 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

192. Corrosion reactions are

Spontaneous redox reactions

None of these

Non-spontaneous redox reactions

Spontaneous acid–base reactions

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Maan AliLast Updated: April 19, 2025

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