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MDCAT Chemistry Electrochemistry Test Online

Malik TahirLast Updated: May 24, 2025

Chemistry Electrochemistry MCQS Online Test

MDCAT 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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MDCAT Chemistry Electrochemistry Test

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Page 1 of 8

Chemistry

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

Electrorefining

None of these

Both A and B

Electroplating

2. 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

Very low ionization potential values

Very high positive value of reduction potential

Reduction potentials are negative

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

Electrolysis

Galvanization

Photo electrolysis

Cathodic protection

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

A voltaic cell

A chemical cell

An electrolytic cell

A galvanic cell

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

Gold is denser

Iron rusts

Gold has higher reduction potential then iron

Gold has lower reduction potential then iron

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

Anode

Cathode

None of these

Electrode

7. Oxidation number of carbon in NaHCO₃ is

-6

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

Electrolysis

Electroplating

Induction

Conduction

9. 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

3.2 g

12.8 g

6.4 g

10. In an electrolytic cell current flows

From anode to cathode in an outer circuit

From cathode to anode in outer circuit

From anode to cathode inside the cell

From cathode to anode inside the cell

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

1 ampere

1 coulomb

2 ampere

1 faraday

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

1.5

2.0

0.5

1.0

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

Dry cell

Fuel cell

Electrolytic cell

Galvanic cell

14. 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

0.001

100

15. Which of the following statements is FALSE?

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

Reduction occurs at cathode

16. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

0.1N

1 N

10 N

11 N

17. Molton NaCl conducts electricity due to the presence of

Free molecules

Free ions

Atoms of Na and Cl.

Free electrons

18. The unit of specific conductivity is

Ohm¯¹ cm

Ohm¯¹ cm¯¹

Ohm cm¯¹

Ohm cm¯²

19. What are the ions present in water?

H+ and OH-

H2O

H2 and O

H and OH

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

510 sec

12157.48 sec

102 sec

642 sec

21. 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

22. Oxidation in a chemical reaction involves

Increase in oxidation number of all the elements on reactant side

Both are possible

Decrease in oxidation number

Increase in oxidation number

23. Molarity of water is

55.5

24. 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

1.5

2.0

25. Oxidation state of hydrogen in CaH₂ is

-2

-1

Page 2 of 8

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

Fuel cell

Electrolytic cell

Daniel cell

Galvanic cell

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

10 s

30,000 s

30 s

10,000 s

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

11.2%

13.1%

14.25%

9.09%

29. The depression of freezing point is directly proportional to

Molarity of the solvent

Molality of the solution

Molarity of the solution

Mole fraction of the solution

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

Distillation

Vacuum distillation

None of these

Fractional distillation

31. 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

32. The solubility of a gas in water depends upon

Temperature

Pressure of the gas

Nature of the gas

All of these

33. 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

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

Manufacture of bleach

Making leather

Rust removal

Electroplating

35. Units of molarity are

Kg/lit

Mol/lit

Gm/lit

None of these

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

0.6

0.9

0.2

0.3

37. Colligative properties are the properties of

Neither a nor b

Dilute solution which behave as nearly ideal solution

Concentration solutions behave as nearly non – ideal solutions

Both a and b

38. Choose the best reducing agent among the following

F¯¹

Cl¯¹

Br¯¹

I¯¹

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

1.86 c°

18.6 c°

Sufficient date not given

0.186 c°

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

7.20

3.12

4.10

0.217

41. Electricity in voltaic cell is produced due to

Reduction

Neutralization

Oxidation

B + C

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

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

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

Li is smaller in size as compared to Cu

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

43. 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

20 torr

68 torr

72 torr

44. Specific conductivity of a solution

Decreases with dilution

Increases with dilution

Depends on mass of electrolyte

Remains unchanged with dilution

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

Both

Oxidation

Reduction

46. Potential of Zn is called

Redox

It has not potential

Reduction

Oxidation

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

Slightly more than 1 atom

2.5 atom

750 torr

760 mm of Hg

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

Diffusion rate of the solute

Ionic concentration

Elevation in boiling point

Flow of solvent from a concentrated to a dilute solution

49. Which of the following is a strong electrolyte?

CH₃COOH

HCN

NH₄OH

Ca(NO₃)₂

50. During a redox reaction, an oxidizing agent

Loses electrons

Is oxidized

Gains electrons

Is hydrolysed

Page 3 of 8

51. Mole fraction of pure water is

Slightly greater than one

Exactly equal to one

Slightly less than one

None of these

52. 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

53. In alkaline battery anode is made up of

MnO₂

Cadmium

AgO₂

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

Pure distilled water

Chloroform

Dilute solution of glucose

Molten NaCl

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

Chlorine

Hydrogen

Oxygen

Chloride

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

10000

48250

96500

193000

57. 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

58. Chemical used in salt bridge is

KOH

KCI

KBr

KNO3

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

Na, Pt and graphite

Pt and graphite only

Na and S only

Na and Hg

60. The reference electrode is made by using

Hg₂Cl₂

ZnCl₂

CuSO₄

HgCl₂

61. 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

5.51

6.1

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

BaCl₂

MgCl₂

KCl

NaCl

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

2.05

0.5

0.05

0.25

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

Saturated

Supersaturated

Unsaturated

Ideal

65. 1.0 g of pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of HCl solution is given by

0.2 N

0.4 N

2 N

4 N

66. 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¯²

S² m² mol

S m mol¯¹

67. Solution with same osmotic pressures are called

Hypertonic

Isotonic

Normal

Hypotonic

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

0.1 N HCl

Graphite

Glass

0.1 N NaCl

69. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.2 M

0.04 M

0.4 M

0.8 M

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

1 to 5

0 to –3

0 to 5.

2 to 5

71. 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

550 cm³

56 cm³

11.2 cm³

5.6 cm³

72. Maximum freezing point falls in

Naphthalene

Camphor

Water

Benzene

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

∆ G = 0, ∆E = 0

∆ G = -ve, ∆ E = 0

∆ G = +ve, ∆ E = 0

∆ G = -ve

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

Loses electrons

Acts as a catalyst

pH is changed

Gains electrons

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

1 M

1 N

2 M

1 f

Page 4 of 8

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

Melting point

Boiling point

Inversion point

Sublimation point

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

2 N

4 N

6 N

8 N

78. 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

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

Sound energy

Heat energy

Electrical energy

Magnetic energy

80. Salt bridge transfers

Solvent particles

Electrons

Current

Anions

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

None

Sum of reduction and oxidation potentials

Lesser

Greater

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

Ca(OH)₂

NaOH

NH₄OH

KOH

83. 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)₄Cl₄]

[Pt(NH₃)₄Cl]Cl₃

[Pt(NH₃)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl₃]Cl

84. Standard hydrogen electrode has an arbitrarily fixed potential

0.00 volt

1.00 volt

None of these

0.10 volt

85. In a Galvanic cell

Electrical energy is converted into chemical energy

Chemical energy is converted into electricity

Chemical energy is converted into heat

Electrical energy is converted into heat

86. Strong reducing agents have

None of these

Greater positive value of standard reduction potential

Lesser positive value of standard reduction potential

Greater negative value of standard reduction potential

87. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/51

5.1

1/5

88. 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 solution

Cathode to anode through the external circuit

89. Electrode potential of Zn is

Oxidation

Depends on the nature of the coupled electrode

Oxidation-reduction

Reduction

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

1 molal

1 molar

All

1 normal

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

Microgram percent

Parts per million

Milligram percent

Gram per million

92. 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

93. Pick out the wrong statement. In electrochemical cell

Chemical energy is converted into electrical energy

Salt bridge maintains the electrical neutrality of the solution

Cathode is regarded as negative electrode

Electrons are released at anode

94. 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

95. 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

Strong acid and its salt of weak base

Weak acid and its salt of weak base

96. Azeotropic mixture of HCl and water has

36% HCl

20.2% HCl

48% HCl

22.2% HCl

97. 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

98. Decrease in oxidation number is called

Redox

Reduction

Oxidation

All of these

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

1 molal

1.1 molal

0.5 molal

0.1 molal

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

Page 5 of 8

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

Electrochemical equivalent

None of these

One gm. Equivalent weight

One gm. atomic weight

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:

1.008 g

224 cm³

112 cm³

22400 cm³

103. 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?

18 M

4.18 M

18.4 M

8.14 M

104. Half cells are interconnected through

Electric circuit

No connection exists

Salt Bridge

Wire

105. Reaction takes place at anode is

Ionization

Oxidation

Reduction

Hydrolysis

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

Reduction

Oxidation

Both oxidation and reduction

Neither oxidation and reduction

107. Camphor is often used in molecular mass determination because

It is solvent for organic substances

It is readily available

It is volatile

It has a very high cryoscopic constant

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

Hydrolyzed

Oxidized

Precipitated

Reduced

109. 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

0.222 V

0.399 V

0.281 V

110. Corrosion reactions are

None of these

Non-spontaneous redox reactions

Spontaneous acid–base reactions

Spontaneous redox reactions

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

2Br– → Br₂ + 2e –

Na → Na⁺ + e–

Na⁺ + e– → Na

Br₂ + 2e – → 2Br –

112. 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

0.66 cm¯¹

0.918 cm¯¹

1.12 cm¯¹

0.142 cm¯¹

113. 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

240 C

120 C

20 C

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

Decreases slowly

Decrease rapidly

Does not change

Drops to zero

115. 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 2

2.5

1.25

116. 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

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

More than that of H₂O

Less than that of water

Equal to that of water

Equal to that of ethanol

118. Cathode provides electrons to

Neutral atom

-Ve ion

Does not provide any electron

+Ve ion

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

Surface tension

Refractive index

Osmotic pressure

Viscosity

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

I₂

Pb²⁺

Ag⁺

121. 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

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

H₃PO₃

H₄P₃O₇

H₃PO₂

H₃PO₄

123. Reduction always occurs

At cathode

None of these

At anode

Both A and B

124. In a chemical reaction, oxidation process involves

Increase in oxidation number of the elements in reactants

Oxidation number neither increases nor decreases

Decrease in oxidation number of element

Increase in oxidation number of element

125. Metals usually conduct electricity because

Metals are decomposed by current

Metals have high resistance

They are mobile electrons in the metallic structure

In metals the ions are free to more

Page 6 of 8

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

60 g

4 g

6 g

40 g

127. 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

128. Density of H₂SO₄ in lead accumulator is

1.25g/cm3

1.20g/cm3

1.3g/cm3

1.15g/cm3

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

None

130. 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

0.40

0.25

0.30

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

Increases gradually

Drops to zero

Does not change

Increases rapidly

132. 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

39.6

40.5

133. The degree of dissociation of weak electrolyte increases as

Dilution increases

Pressure increases

Dilution decreases

None

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

0.186

0.80

0.0512

0.512

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

0.0521

0.521

1.86

0.0186

136. 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

137. Stronger the oxidizing agent, greater is the

Redox potential

Oxidation potential

Reduction potential

e.m.f of cell

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

Cl¯

Na⁺

Both Na⁺ and CI¯

None of these

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

175.4 kJ

212.3 kJ

106.15 kJ

53.07 kJ

140. The Vant Hoff factor (i) accounts for

The degree of decomposition of solution

Degree of solubilization of solute

The extent of dissolution of solute

The extent of dissociation of solute

141. Salt bridge transfers

Ions

Anion

Current

Electrons

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

+ 0.35

– 0.35 V

+ 1.17 V

– 1.17 V

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

Electrons flow cathode to anode within the electrolytic solution

None of these

Electrons flow from cathode to anode through the external battery

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

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

Higher

Lower

Not particular

In middle

145. 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 10⁴

1.06 x 10²

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

Standard oxidation potential

Ionization potential

Cell voltage

Standard reduction potential

147. 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

3 N

9 N

2 N

148. Corrosion is basically a

Altered reaction in presence of H₂O

Electrochemical phenomenon

Interaction

Union between two light metals and a heavy metal

149. 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

128 S cm² mol¯¹

278 S cm² mol¯¹

176 S cm² mol¯¹

150. When common salt is dissolved in water

B.P of water decrease

Any possibility

B.P of water remain constant

B.P of water increase

Page 7 of 8

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

Na₂O₂

F₂O

Cl₂O

Na₂O

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

0.1

0.01

0.0196

0.2

153. 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

154. Secondary cell is

Non rechargeable

Electrolytic cell

Rechargeable

Daniel cell

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

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

Nitric acid

Phosphorus acid

Boric acid

Sulphuric acid

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

Henry’s law

Ostwald’s law

Raoult’s law

Arrhenius law

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

CuSO₄

ZnCl₂

Hg₂Cl₂

HgCl₂

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

4 g

5 g

1 g

2 g

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

1.08 g

0.54 g

2.16 g

0.27 g

161. 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

10.8 g

108 g

21.6 g

162. The best reducing agent is

F¯

I¯

Br¯

Cl¯

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

1.5

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

Equal to the total volume of the components

None of these

Slightly more than the total volume of the components

Slightly less than the total volume of the components

165. In electrolytic cell, electricity in carried out by

Spontaneous reaction

Neutralization

Non-spontaneous reaction

All

166. 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

4.0 x 10¹²

2.0 x 10¹¹

1.0 x 10¹⁰

1.0 x 10²

167. Density of H₂SO₄ in lead accumulator is

1.15 g/Cm³

1.25g/Cm³

120 g Cm³

1.2 g/Cm³

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

Ostwald’s dilution law

Raoult’s law

Henry’s law

Distribution law

169. 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

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

12.1 atm

2.46 atm

1.21 atm

24.6 atm

171. Alkaline battery has a voltage of

1.5V

2.5V

3.5V

4.5V

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

O₂,H₂

O₂, SO₂

O₂, Na

None of these

173. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

2.00 mole

0.25 mole

1.0 mole

0.5 mole

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

20g NaCl/100ml

5.58g NaCl/100m

58.5g NaCl/100ml

10.0g NaCl/100ml

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. An electrolyte

Gives ions only when dissolved in water

Gives ions only when electricity is passed

Possesses ions even in solid state

Forms complex ions in solution

177. 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

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 water decreases by the addition of ethanol

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

0.2

0.1

0.0196

0.01

179. 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

0.75

0.80

0.60

180. In alkaline battery the anode is made up of

Cadmium

MnO2

AgO2

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

Na₂SO₄

NH₄Cl

NaCl

CH₃ CooNH₄

182. A redox reaction involves

A reaction in a solution

Ion combination reaction

Electron transfer

Proton transfer

183. Temperature for standard electrode potential is

300 K

25 C°

310 K

273 K

184. The conductivity of strong electrolyte

Depends on density of electrolyte itself.

Increases on dilution slightly

Decreases on dilution

Does not change on dilution

185. Pure water does not conduct electricity because it

Is neutral

Is readily decomposed

Has low boiling point

Is almost unionized

186. Best way to prevent rusting iron is by

Putting it in saline water

None of these

Making iron cathode

Both of these

187. Which has maximum oxidation number

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

Standard electrode potential

Electric change

Electroplating

Ionization potential

189. 96500 C of electricity liberates from CuSO₄ solution

63.5 g of Cu

31.75 g of Cu

96500 g of CU

100 g of Cu

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

191. The art of electroplating was given by

Faraday

Brugan

Edison

Thomas Gradam

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

Heat energy

Electrical energy

None of these

Chemical energy

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Malik TahirLast Updated: May 24, 2025

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