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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. Electrode potential of Zn is

Reduction

Depends on the nature of the coupled electrode

Oxidation-reduction

Oxidation

2. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

1 2

None of these

2.5

1.25

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

Both A and B

Electroplating

Electrorefining

None of these

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

None

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

6 N

4 N

2 N

8 N

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

Sufficient date not given

0.186 c°

18.6 c°

1.86 c°

7. During a redox reaction, an oxidizing agent

Gains electrons

Loses electrons

Is hydrolysed

Is oxidized

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

∆ G = -ve, ∆ E = 0

∆ G = +ve, ∆ E = 0

∆ G = 0, ∆E = 0

∆ G = -ve

9. Standard hydrogen electrode has an arbitrarily fixed potential

0.00 volt

None of these

1.00 volt

0.10 volt

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

Milligram percent

Parts per million

Gram per million

Microgram percent

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

Manufacture of bleach

Making leather

Electroplating

Rust removal

12. Camphor is often used in molecular mass determination because

It is solvent for organic substances

It has a very high cryoscopic constant

It is readily available

It is volatile

13. 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

14. In alkaline battery anode is made up of

Cadmium

AgO₂

MnO₂

15. Maximum freezing point falls in

Camphor

Water

Benzene

Naphthalene

16. Salt bridge transfers

Anions

Current

Electrons

Solvent particles

17. In electrolytic cell, electricity in carried out by

All

Spontaneous reaction

Neutralization

Non-spontaneous reaction

18. 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

2 N

0.4 N

4 N

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

0.5

0.05

2.05

0.25

20. Salt bridge transfers

Electrons

Ions

Anion

Current

21. Azeotropic mixture of HCl and water has

36% HCl

20.2% HCl

22.2% HCl

48% HCl

22. 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

23. The Vant Hoff factor (i) accounts for

The extent of dissolution of solute

Degree of solubilization of solute

The extent of dissociation of solute

The degree of decomposition of solution

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

80 ml

10 ml

40 ml

20 ml

25. Density of H₂SO₄ in lead accumulator is

1.25g/cm3

1.3g/cm3

1.15g/cm3

1.20g/cm3

Page 2 of 8

26. When common salt is dissolved in water

B.P of water decrease

B.P of water increase

B.P of water remain constant

Any possibility

27. Cathode provides electrons to

+Ve ion

Neutral atom

Does not provide any electron

-Ve ion

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

Fuel cell

Galvanic cell

Dry cell

Electrolytic cell

29. The best reducing agent is

F¯

Cl¯

Br¯

I¯

30. 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

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

Electroplating

Conduction

Electrolysis

Induction

32. 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%

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

0.0196

0.1

0.2

0.01

34. 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 benzene decreases by the addition of naphthalene

Boiling point of pure water decreases by the addition of ethanol

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

35. 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

36. 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

33.3

3.33

37. Chemical used in salt bridge is

KCI

KNO3

KBr

KOH

38. The solubility of a gas in water depends upon

Nature of the gas

Temperature

All of these

Pressure of the gas

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

Ionization potential

Cell voltage

Standard oxidation potential

Standard reduction potential

40. What are the ions present in water?

H+ and OH-

H and OH

H2 and O

H2O

41. 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

S² m² mol¯²

S m mol¯¹

S m² mol¯¹

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

1 ampere

1 coulomb

1 faraday

2 ampere

43. Alkaline battery has a voltage of

4.5V

3.5V

2.5V

1.5V

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

Ag⁺

Pb²⁺

I₂

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

Gold has lower reduction potential then iron

Gold is denser

Iron rusts

Gold has higher reduction potential then iron

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

None of these

Electrical energy

Heat energy

Chemical energy

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

Loses electrons

Gains electrons

Acts as a catalyst

pH is changed

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

Decrease rapidly

Does not change

Drops to zero

Decreases slowly

49. In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at cathode while with Hg cathode it forms sodium amalgam

Hg is more inert than Pt

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

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

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

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

Hydrolyzed

Precipitated

Reduced

Oxidized

Page 3 of 8

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

Less than that of water

Equal to that of water

More than that of H₂O

Equal to that of ethanol

52. In a Galvanic cell

Chemical energy is converted into electricity

Chemical energy is converted into heat

Electrical energy is converted into heat

Electrical energy is converted into chemical energy

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

KCl

MgCl₂

NaCl

BaCl₂

54. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

1 N

10 N

0.1N

11 N

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

CuSO₄

Hg₂Cl₂

HgCl₂

ZnCl₂

56. Solution with same osmotic pressures are called

Normal

Hypertonic

Isotonic

Hypotonic

57. 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

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

0.6

0.3

0.2

0.9

59. 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

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

None

Lesser

Greater

Sum of reduction and oxidation potentials

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

0.1 N HCl

0.1 N NaCl

Glass

Graphite

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

2.0

1.5

1.0

0.5

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

2 g

1 g

5 g

4 g

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

53.07 kJ

212.3 kJ

175.4 kJ

106.15 kJ

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

Chlorine

Chloride

Hydrogen

Oxygen

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

Drops to zero

Increases gradually

Does not change

Increases rapidly

67. Temperature for standard electrode potential is

310 K

300 K

25 C°

273 K

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

F₂O

Na₂O₂

Na₂O

Cl₂O

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

Heat energy

Sound energy

Electrical energy

Magnetic energy

70. 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

71. Decrease in oxidation number is called

Oxidation

All of these

Reduction

Redox

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

0.0186

0.0521

1.86

0.521

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

642 sec

510 sec

102 sec

12157.48 sec

74. Pick out the wrong statement. In electrochemical cell

Salt bridge maintains the electrical neutrality of the solution

Chemical energy is converted into electrical energy

Electrons are released at anode

Cathode is regarded as negative electrode

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

10000

48250

193000

96500

Page 4 of 8

76. 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

5.51

1.32

77. Half cells are interconnected through

Electric circuit

Wire

No connection exists

Salt Bridge

78. 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

79. The degree of dissociation of weak electrolyte increases as

Dilution increases

Pressure increases

Dilution decreases

None

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

None of these

Vacuum distillation

Fractional distillation

Distillation

81. Which of the following statements is FALSE?

Reduction occurs at cathode

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

All electrochemical reactions involve the transfer of electrons

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

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

Unsaturated

Ideal

Supersaturated

Saturated

83. 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

1.08 g

21.6 g

10.8 g

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

Oxidation

Both oxidation and reduction

Neither oxidation and reduction

Reduction

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

Galvanic cell

Daniel cell

Fuel cell

Electrolytic cell

86. Pure water does not conduct electricity because it

Is almost unionized

Is readily decomposed

Is neutral

Has low boiling point

87. Stronger the oxidizing agent, greater is the

Oxidation potential

e.m.f of cell

Reduction potential

Redox potential

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

None of these

Electrode

Anode

Cathode

89. Molton NaCl conducts electricity due to the presence of

Free ions

Free electrons

Free molecules

Atoms of Na and Cl.

90. 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

91. Which of the following is a strong electrolyte?

HCN

Ca(NO₃)₂

NH₄OH

CH₃COOH

92. Units of molarity are

Mol/lit

Kg/lit

Gm/lit

None of these

93. 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 and S only

Na and Hg

Na, Pt and graphite

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

0.01

0.0196

0.2

0.1

95. In a chemical reaction, oxidation process involves

Increase in oxidation number of the elements in reactants

Decrease in oxidation number of element

Increase in oxidation number of element

Oxidation number neither increases nor decreases

96. Vant Hoff’s factor of Ca(NO₃)₂ is

97. Electricity in voltaic cell is produced due to

Oxidation

B + C

Reduction

Neutralization

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

Dilute solution of glucose

Pure distilled water

Chloroform

Molten NaCl

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

0.0512

0.186

0.512

0.80

100. Corrosion reactions are

Spontaneous acid–base reactions

Non-spontaneous redox reactions

Spontaneous redox reactions

None of these

Page 5 of 8

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

– 0.35 V

+ 1.17 V

– 1.17 V

+ 0.35

102. The reference electrode is made by using

HgCl₂

CuSO₄

ZnCl₂

Hg₂Cl₂

103. 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 – α

1 – 2 α

1 + α

104. If liquids A and B form an ideal solution

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

The free energy of mixing is zero

105. Reduction always occurs

Both A and B

At anode

At cathode

None of these

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

CH₃ CooNH₄

Na₂SO₄

NH₄Cl

NaCl

107. At room temperature, the mole fraction of a solution in 0.25 and the vapour pressure of the solvent is 0.80 atm. Then the lowering of vapour pressure is

0.80

0.20

0.75

0.60

108. 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

109. Molarity of water is

55.5

110. 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

111. 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

0.15 M

0.2 M

0.1 M

0.05 M

112. The unit of specific conductivity is

Ohm¯¹ cm¯¹

Ohm cm¯²

Ohm¯¹ cm

Ohm cm¯¹

113. 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 oxidation potential of Li/Li⁺ is lower than that of CuCu²⁺

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

Li is smaller in size as compared to Cu

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

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

Ostwald’s law

Arrhenius law

Henry’s law

Raoult’s law

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

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

Electrons flow cathode to anode within the electrolytic solution

117. Secondary cell is

Non rechargeable

Electrolytic cell

Rechargeable

Daniel cell

118. 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

0.1 molal

1 molal

1.1 molal

119. Specific conductivity of a solution

Depends on mass of electrolyte

Remains unchanged with dilution

Decreases with dilution

Increases with dilution

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

1.25 cm¯³

1.15 cm¯³

2.15 cm¯³

1.81 cm¯³

121. 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

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

1 f

1 N

2 M

1 M

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

None of these

Slightly less than the total volume of the components

Equal to the total volume of the components

Slightly more than the total volume of the components

124. In a Galvanic cell, the electrons flow from

Anode to cathode through the solution

Anode to cathode through the external circuit

Cathode to anode through the external circuit

Cathode to anode through the solution

125. How many g of dibasic acid (mol. wt. 200) should be present in 100 ml of the aqueous solution to give 0.1 Normality?

1 g

2 g

20 g

10 g

Page 6 of 8

126. The conductivity of strong electrolyte

Decreases on dilution

Increases on dilution slightly

Depends on density of electrolyte itself.

Does not change on dilution

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

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

Electroplating

Standard electrode potential

Ionization potential

Electric change

129. 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

1.5

1.0

0.5

2.0

130. 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)₄Cl₃]Cl

[Pt(NH₃)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl]Cl₃

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

All

1 normal

1 molal

1 molar

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

Nitric acid

Boric acid

Phosphorus acid

Sulphuric acid

133. Corrosion is basically a

Interaction

Union between two light metals and a heavy metal

Altered reaction in presence of H₂O

Electrochemical phenomenon

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

H₄P₃O₇

H₃PO₂

H₃PO₃

H₃PO₄

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

278 S cm² mol¯¹

302 S cm² mol¯¹

176 S cm² mol¯¹

128 S cm² mol¯¹

136. Oxidation number of carbon in NaHCO₃ is

-6

137. Choose the best reducing agent among the following

I¯¹

Cl¯¹

Br¯¹

F¯¹

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

Sublimation point

Inversion point

Melting point

Boiling point

139. Voltaic cell can be recharged by

By heating it

By replacing external circuit with external source of electricity

By removal of solution

By addition of fresh solution

140. A redox reaction involves

Ion combination reaction

Proton transfer

A reaction in a solution

Electron transfer

141. Oxidation in a chemical reaction involves

Increase in oxidation number of all the elements on reactant side

Increase in oxidation number

Decrease in oxidation number

Both are possible

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

2Br– → Br₂ + 2e –

Br₂ + 2e – → 2Br –

Na⁺ + e– → Na

Na → Na⁺ + e–

143. 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

12.8 g

6.4 g

3.2 g

2.3 g

144. 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

145. Best way to prevent rusting iron is by

Making iron cathode

None of these

Both of these

Putting it in saline water

146. 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 10⁴

1.06 x 10³

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

Reduction

Oxidation

Both

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

Galvanization

Photo electrolysis

Cathodic protection

Electrolysis

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

2.16 g

0.27 g

1.08 g

0.54 g

150. 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

Page 7 of 8

151. 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

152. If the standard electrode potential of CU²⁺/Cu electrode is 0.34 V, what is the electrode potential of 0.01 M concentration of Cu²⁺? (T = 298 K)

0.222 V

0.281 V

0.176 V

0.399 V

153. Potential of Zn is called

Redox

Oxidation

It has not potential

Reduction

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

Strong acid and its salt of weak base

Weak acid and its salt of strong base

A strong acid and its salt of a strong base

Weak acid and its salt of weak base

155. Reaction takes place at anode is

Hydrolysis

Reduction

Ionization

Oxidation

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

0.4 M

0.2 M

0.04 M

0.8 M

157. Strong reducing agents have

Greater negative value of standard reduction potential

Lesser positive value of standard reduction potential

Greater positive value of standard reduction potential

None of these

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

4 g

40 g

6 g

60 g

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

O₂, SO₂

O₂, Na

None of these

O₂,H₂

160. 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

161. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

0.25 mole

0.5 mole

1.0 mole

2.00 mole

162. 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

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

24.6 atm

1.21 atm

2.46 atm

12.1 atm

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

2 to 5

1 to 5

0 to –3

0 to 5.

165. 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

100

0.01

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

Higher

Not particular

Lower

In middle

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

A chemical cell

A voltaic cell

An electrolytic cell

A galvanic cell

168. 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

0.30

0.25

0.40

0.35

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

B > C > A

C > B > A

A > B > C

A > C > B

170. An electrolyte

Gives ions only when electricity is passed

Forms complex ions in solution

Gives ions only when dissolved in water

Possesses ions even in solid state

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

NH₄OH

NaOH

KOH

Ca(OH)₂

172. 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

56 cm³

5.6 cm³

550 cm³

11.2 cm³

173. Metals usually conduct electricity because

In metals the ions are free to more

Metals have high resistance

They are mobile electrons in the metallic structure

Metals are decomposed by current

174. 96500 C of electricity liberates from CuSO₄ solution

96500 g of CU

31.75 g of Cu

63.5 g of Cu

100 g of Cu

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

20g NaCl/100ml

10.0g NaCl/100ml

58.5g NaCl/100ml

5.58g NaCl/100m

Page 8 of 8

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

1.5

177. In alkaline battery the anode is made up of

AgO2

Cadmium

MnO2

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

3.12

7.20

0.217

4.10

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

Na⁺

Cl¯

None of these

Both Na⁺ and CI¯

180. Mole fraction of pure water is

Slightly less than one

None of these

Slightly greater than one

Exactly equal to one

181. The vapour pressure of two liquids ‘P’ and ‘Q’ are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol of Q would be

68 torr

20 torr

72 torr

140 torr

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

183. Density of H₂SO₄ in lead accumulator is

120 g Cm³

1.2 g/Cm³

1.15 g/Cm³

1.25g/Cm³

184. 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

120 C

20 C

185. The art of electroplating was given by

Edison

Brugan

Thomas Gradam

Faraday

186. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/5

5.1

1/51

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

Surface tension

Viscosity

Osmotic pressure

Refractive index

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

Elevation in boiling point

Flow of solvent from a concentrated to a dilute solution

Ionic concentration

Diffusion rate of the solute

189. Oxidation state of hydrogen in CaH₂ is

-1

-2

190. 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 positive value of reduction potential

Very high negative values reduction potential

Very low ionization potential values

191. What is the molarity of H₂SO₄ solution that has density of 1.84 gm/cm³ which was at 35°C and contains 98% by weight?

4.18 M

18.4 M

8.14 M

18 M

192. Which has maximum oxidation number

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Malik TahirLast Updated: May 24, 2025

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