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

2.15 cm¯³

1.81 cm¯³

1.25 cm¯³

1.15 cm¯³

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

Gains electrons

Loses electrons

Acts as a catalyst

pH is changed

3. 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

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

1.21 atm

24.6 atm

2.46 atm

12.1 atm

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

5.65

5.51

6.1

1.32

6. In a Galvanic cell, the electrons flow from

Cathode to anode through the solution

Cathode to anode through the external circuit

Anode to cathode through the external circuit

Anode to cathode through the solution

7. 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

8. The solubility of a gas in water depends upon

Pressure of the gas

Nature of the gas

Temperature

All of these

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

Raoult’s law

Ostwald’s dilution law

Henry’s law

Distribution law

10. 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 > C > B

A > B > C

C > B > A

B > C > A

11. 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

4 N

0.4 N

2 N

12. 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

30 s

10 s

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

Gram per million

Parts per million

Milligram percent

Microgram percent

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

Arrhenius law

Henry’s law

Ostwald’s law

Raoult’s law

15. Corrosion is basically a

Altered reaction in presence of H₂O

Union between two light metals and a heavy metal

Interaction

Electrochemical phenomenon

16. 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

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

None

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

2Br– → Br₂ + 2e –

Na⁺ + e– → Na

Br₂ + 2e – → 2Br –

Na → Na⁺ + e–

19. Reduction always occurs

None of these

At anode

At cathode

Both A and B

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

Cl¯

None of these

Both Na⁺ and CI¯

Na⁺

21. The reference electrode is made by using

ZnCl₂

Hg₂Cl₂

CuSO₄

HgCl₂

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

1 to 5

0 to 5.

0 to –3

2 to 5

23. 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

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

∆ G = -ve

∆ G = +ve, ∆ E = 0

∆ G = 0, ∆E = 0

∆ G = -ve, ∆ E = 0

25. Metals usually conduct electricity because

In metals the ions are free to more

Metals are decomposed by current

Metals have high resistance

They are mobile electrons in the metallic structure

Page 2 of 8

26. 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

0.60

0.20

0.75

0.80

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

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

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

Hg is more inert than Pt

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

28. If liquids A and B form an ideal solution

The entropy of mixing is zero

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

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

1 molar

1 normal

All

1 molal

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

Nitric acid

Boric acid

Sulphuric acid

Phosphorus acid

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

Electrode

Anode

None of these

Cathode

32. Stronger the oxidizing agent, greater is the

Reduction potential

Oxidation potential

e.m.f of cell

Redox potential

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

Electrorefining

None of these

Both A and B

Electroplating

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

11.2%

13.1%

9.09%

14.25%

35. Maximum freezing point falls in

Camphor

Benzene

Water

Naphthalene

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

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

Strong acid and its salt of weak base

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

Neither oxidation and reduction

Reduction

Oxidation

Both oxidation and reduction

38. Electrode potential of Zn is

Oxidation-reduction

Oxidation

Depends on the nature of the coupled electrode

Reduction

39. 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

40. 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

Li is smaller in size as compared to Cu

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

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

Chloroform

Molten NaCl

Dilute solution of glucose

Pure distilled water

42. Reaction takes place at anode is

Hydrolysis

Oxidation

Ionization

Reduction

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

Melting point

Inversion point

Sublimation point

Boiling point

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

Drops to zero

Increases rapidly

Does not change

Increases gradually

45. In alkaline battery anode is made up of

MnO₂

AgO₂

Cadmium

46. Secondary cell is

Electrolytic cell

Rechargeable

Daniel cell

Non rechargeable

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

0.3

0.9

0.6

0.2

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

H₄P₃O₇

H₃PO₃

H₃PO₄

H₃PO₂

49. Mole fraction of pure water is

None of these

Exactly equal to one

Slightly less than one

Slightly greater than one

50. 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

Page 3 of 8

51. Pick out the wrong statement. In electrochemical cell

Cathode is regarded as negative electrode

Salt bridge maintains the electrical neutrality of the solution

Chemical energy is converted into electrical energy

Electrons are released at anode

52. 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

53. 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

54. 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

0.222 V

0.176 V

0.281 V

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

Flow of solvent from a concentrated to a dilute solution

Diffusion rate of the solute

Elevation in boiling point

Ionic concentration

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

Decrease rapidly

Drops to zero

Decreases slowly

Does not change

57. The degree of dissociation of weak electrolyte increases as

Dilution decreases

Dilution increases

None

Pressure increases

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

Na and S only

Na, Pt and graphite

Pt and graphite only

Na and Hg

59. Oxidation in a chemical reaction involves

Decrease in oxidation number

Increase in oxidation number of all the elements on reactant side

Both are possible

Increase in oxidation number

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

– 1.17 V

– 0.35 V

+ 0.35

+ 1.17 V

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

760 mm of Hg

780 mm of Hg

800 mm of Hg

750 mm of Hg

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

HgCl₂

ZnCl₂

CuSO₄

Hg₂Cl₂

63. Vant Hoff’s factor of Ca(NO₃)₂ is

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

0.01

0.1

0.0196

0.2

65. During a redox reaction, an oxidizing agent

Is hydrolysed

Loses electrons

Is oxidized

Gains electrons

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

10.0g NaCl/100ml

5.58g NaCl/100m

20g NaCl/100ml

58.5g NaCl/100ml

67. The Vant Hoff factor (i) accounts for

The extent of dissolution of solute

Degree of solubilization of solute

The degree of decomposition of solution

The extent of dissociation of solute

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

NaCl

BaCl₂

KCl

MgCl₂

69. Camphor is often used in molecular mass determination because

It is volatile

It is readily available

It is solvent for organic substances

It has a very high cryoscopic constant

70. Solution with same osmotic pressures are called

Normal

Hypotonic

Isotonic

Hypertonic

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

2 M

1 f

1 M

1 N

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

Produce high purity water

Create potential difference between two electrodes

Generate heat

Remove adsorbed oxygen from electrode surfaces

73. Molton NaCl conducts electricity due to the presence of

Free electrons

Free ions

Atoms of Na and Cl.

Free molecules

74. What are the ions present in water?

H+ and OH-

H2O

H2 and O

H and OH

75. 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

224 cm³

1.008 g

22400 cm³

Page 4 of 8

76. Best way to prevent rusting iron is by

Putting it in saline water

Both of these

None of these

Making iron cathode

77. A redox reaction involves

Proton transfer

Ion combination reaction

A reaction in a solution

Electron transfer

78. Oxidation state of hydrogen in CaH₂ is

-1

-2

79. The art of electroplating was given by

Faraday

Brugan

Edison

Thomas Gradam

80. Pure water does not conduct electricity because it

Is neutral

Is readily decomposed

Is almost unionized

Has low boiling point

81. Which of the following is a strong electrolyte?

HCN

CH₃COOH

NH₄OH

Ca(NO₃)₂

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

Fuel cell

Galvanic cell

Dry cell

Electrolytic cell

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

Induction

Conduction

Electroplating

Electrolysis

84. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.25g/cm3

1.3g/cm3

1.20g/cm3

85. Salt bridge transfers

Electrons

Anion

Ions

Current

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

Chemical energy

Heat energy

None of these

Electrical energy

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

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

Electrons flow from cathode to anode through the external battery

None of these

Electrons flow cathode to anode within the electrolytic solution

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

Oxidation

Both

Reduction

89. A solution contains A, B and C components. The mole fraction A and C are 0.25 and 0.35 respectively. The mole fraction B will be

0.40

0.35

0.25

0.30

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

Osmotic pressure

Surface tension

Viscosity

Refractive index

91. Chemical used in salt bridge is

KBr

KOH

KNO3

KCI

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

96500

48250

10000

193000

93. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

1.0 mole

0.25 mole

0.5 mole

2.00 mole

94. Standard hydrogen electrode has an arbitrarily fixed potential

0.00 volt

1.00 volt

0.10 volt

None of these

95. Half cells are interconnected through

Salt Bridge

Electric circuit

No connection exists

Wire

96. Potential of Zn is called

Reduction

It has not potential

Redox

Oxidation

97. When common salt is dissolved in water

Any possibility

B.P of water increase

B.P of water remain constant

B.P of water decrease

98. 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

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

5 g

1 g

2 g

4 g

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

NH₄OH

Ca(OH)₂

KOH

NaOH

Page 5 of 8

101. 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

0.1 M

0.05 M

0.2 M

0.15 M

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

0.1

0.01

0.2

0.0196

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

0.54 g

0.27 g

1.08 g

2.16 g

104. Specific conductivity of a solution

Remains unchanged with dilution

Depends on mass of electrolyte

Increases with dilution

Decreases with dilution

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

Chlorine

Hydrogen

Chloride

Oxygen

106. Density of H₂SO₄ in lead accumulator is

1.25g/Cm³

1.2 g/Cm³

120 g Cm³

1.15 g/Cm³

107. 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

2.0 x 10¹¹

1.0 x 10¹⁰

1.0 x 10²

4.0 x 10¹²

108. Cathode provides electrons to

+Ve ion

-Ve ion

Neutral atom

Does not provide any electron

109. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

1.25

1 2

None of these

2.5

110. 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

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

Ideal

Unsaturated

Saturated

Supersaturated

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

Higher

Lower

Not particular

In middle

113. Choose the best reducing agent among the following

F¯¹

Br¯¹

I¯¹

Cl¯¹

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

2.05

0.5

0.05

0.25

115. 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

116. 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?

63.5 gm

12.7 gm

15.9 gm

31.8 gm

117. 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

0.142 cm¯¹

1.12 cm¯¹

0.66 cm¯¹

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

760 mm of Hg

750 torr

2.5 atom

Slightly more than 1 atom

119. An electrolyte

Gives ions only when dissolved in water

Gives ions only when electricity is passed

Forms complex ions in solution

Possesses ions even in solid state

120. 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. atomic weight

One gm. Equivalent weight

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

2 N

8 N

6 N

4 N

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

Making leather

Rust removal

Manufacture of bleach

Electroplating

123. Corrosion reactions are

Spontaneous acid–base reactions

None of these

Spontaneous redox reactions

Non-spontaneous redox reactions

124. In a Galvanic cell

Chemical energy is converted into electricity

Electrical energy is converted into chemical energy

Chemical energy is converted into heat

Electrical energy is converted into heat

125. The unit of specific conductivity is

Ohm cm¯¹

Ohm cm¯²

Ohm¯¹ cm¯¹

Ohm¯¹ cm

Page 6 of 8

126. 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

0.0186

1.86

127. 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

140 torr

20 torr

68 torr

128. Decrease in oxidation number is called

All of these

Redox

Oxidation

Reduction

129. 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

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

Precipitated

Oxidized

Hydrolyzed

Reduced

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

Electrolysis

Photo electrolysis

Cathodic protection

Galvanization

132. Temperature for standard electrode potential is

310 K

300 K

273 K

25 C°

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

80 ml

20 ml

10 ml

40 ml

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

1.5

135. 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

1.86 c°

18.6 c°

0.186 c°

136. In alkaline battery the anode is made up of

MnO2

Cadmium

AgO2

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

F₂O

Cl₂O

Na₂O₂

Na₂O

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

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

A galvanic cell

An electrolytic cell

A voltaic cell

A chemical cell

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

I₂

Ag⁺

Pb²⁺

141. In electrolytic cell, electricity in carried out by

Neutralization

Spontaneous reaction

Non-spontaneous reaction

All

142. Oxidation number of carbon in NaHCO₃ is

-6

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

Electrolytic cell

Galvanic cell

Fuel cell

Daniel cell

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

0.1 N HCl

Glass

0.1 N NaCl

Graphite

145. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

0.1N

11 N

10 N

1 N

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

Gold has lower reduction potential then iron

Gold has higher reduction potential then iron

Iron rusts

Gold is denser

147. The conductivity of strong electrolyte

Increases on dilution slightly

Decreases on dilution

Depends on density of electrolyte itself.

Does not change on dilution

148. 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

1 g

2 g

10 g

149. 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

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

Equal to that of ethanol

More than that of H₂O

Less than that of water

Equal to that of water

Page 7 of 8

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

CH₃ CooNH₄

NH₄Cl

NaCl

Na₂SO₄

152. 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

18.4 M

18 M

153. Azeotropic mixture of HCl and water has

20.2% HCl

22.2% HCl

48% HCl

36% HCl

154. Voltaic cell can be recharged by

By replacing external circuit with external source of electricity

By removal of solution

By heating it

By addition of fresh solution

155. 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

156. Electricity in voltaic cell is produced due to

Oxidation

Reduction

Neutralization

B + C

157. 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

2 N

1 N

3 N

9 N

158. In an electrolytic cell current flows

From anode to cathode inside the cell

From cathode to anode in outer circuit

From anode to cathode in an outer circuit

From cathode to anode inside the cell

159. Alkaline battery has a voltage of

4.5V

2.5V

3.5V

1.5V

160. 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

Boiling point of pure benzene increases by the addition of toluene

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

Boiling point of pure water decreases by the addition of ethanol

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

4.10

7.20

0.217

3.12

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

1.1 molal

0.5 molal

0.1 molal

1 molal

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)

33.3

0.333

3.33

0.0033

164. Salt bridge transfers

Electrons

Anions

Solvent particles

Current

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

Magnetic energy

Electrical energy

Heat energy

Sound energy

166. 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

3.2 g

12.8 g

2.3 g

167. Molarity of water is

55.5

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

169. Units of molarity are

Mol/lit

Kg/lit

Gm/lit

None of these

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

Ionization potential

Cell voltage

Standard oxidation potential

Standard reduction potential

171. 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

120 C

20 C

4 C

240 C

172. 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

173. In a chemical reaction, oxidation process involves

Increase in oxidation number of element

Oxidation number neither increases nor decreases

Increase in oxidation number of the elements in reactants

Decrease in oxidation number of element

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

128 S cm² mol¯¹

278 S cm² mol¯¹

302 S cm² mol¯¹

176 S cm² mol¯¹

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

0.1 M BaCl₂

0.1 M Glucose

0.1 M NaCl

0.1 M Sucrose

Page 8 of 8

176. The best reducing agent is

Br¯

F¯

Cl¯

I¯

177. 96500 C of electricity liberates from CuSO₄ solution

100 g of Cu

63.5 g of Cu

96500 g of CU

31.75 g of Cu

178. An electric current is passed through silver voltmeter connected to a water voltmeter. The cathode of the silver voltammeter is 0.108 g more at the end of the electrolysis. The volume of oxygen evolved at STP is

5.6 cm³

56 cm³

550 cm³

11.2 cm³

179. 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

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

0.5

1.0

1.5

2.0

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

1.06 x 10³

1.06 x 10²

1.06 x 10⁴

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

212.3 kJ

175.4 kJ

53.07 kJ

106.15 kJ

183. When during electrolysis of a solution of AgNO₃, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

10.8 g

108 g

21.6 g

1.08 g

184. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/51

1/5

5.1

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

Vacuum distillation

Fractional distillation

Distillation

None of these

186. Which has maximum oxidation number

187. Strong reducing agents have

Greater positive value of standard reduction potential

Greater negative value of standard reduction potential

Lesser positive value of standard reduction potential

None of these

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

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

60 g

6 g

4 g

40 g

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

0.0512

0.512

0.186

0.80

191. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.4 M

0.8 M

0.04 M

0.2 M

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

1 ampere

1 coulomb

2 ampere

1 faraday

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Malik TahirLast Updated: May 24, 2025

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