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

Ostwald’s law

Raoult’s law

Henry’s law

Arrhenius law

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

1.25

None of these

2.5

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

Na → Na⁺ + e–

2Br– → Br₂ + 2e –

Br₂ + 2e – → 2Br –

Na⁺ + e– → Na

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

In middle

Higher

Not particular

Lower

5. Density of H₂SO₄ in lead accumulator is

1.15 g/Cm³

1.2 g/Cm³

1.25g/Cm³

120 g Cm³

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

Manufacture of bleach

Making leather

Rust removal

Electroplating

7. 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

0.60

0.80

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

Iron rusts

Gold is denser

Gold has lower reduction potential then iron

Gold has higher reduction potential then iron

9. 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

0.15 M

0.2 M

10. Choose the best reducing agent among the following

I¯¹

Cl¯¹

Br¯¹

F¯¹

11. In a chemical reaction, oxidation process involves

Decrease in oxidation number of element

Oxidation number neither increases nor decreases

Increase in oxidation number of the elements in reactants

Increase in oxidation number of element

12. 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

4 N

0.4 N

2 N

0.2 N

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

Standard oxidation potential

Cell voltage

Standard reduction potential

Ionization potential

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

13.1%

9.09%

14.25%

11.2%

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

0.2

0.9

0.6

0.3

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

Anode

None of these

Cathode

Electrode

17. In an electrolytic cell current flows

From cathode to anode inside the cell

From anode to cathode inside the cell

From anode to cathode in an outer circuit

From cathode to anode in outer circuit

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

Less than that of water

More than that of H₂O

Equal to that of ethanol

Equal to that of water

19. 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

1 g

2 g

20 g

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

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

2 M

1 M

1 N

1 f

22. Mole fraction of pure water is

Slightly less than one

Exactly equal to one

None of these

Slightly greater than one

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

A voltaic cell

A chemical cell

A galvanic cell

An electrolytic cell

24. Standard hydrogen electrode has an arbitrarily fixed potential

None of these

1.00 volt

0.00 volt

0.10 volt

25. The best reducing agent is

Cl¯

Br¯

I¯

F¯

Page 2 of 8

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

0.2

0.1

0.01

0.0196

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

30,000 s

10 s

30 s

10,000 s

28. Which of the following statements is FALSE?

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

Reduction occurs at cathode

All electrochemical reactions involve the transfer of electrons

29. Corrosion reactions are

None of these

Spontaneous redox reactions

Non-spontaneous redox reactions

Spontaneous acid–base reactions

30. 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

11.2 cm³

550 cm³

31. Potential of Zn is called

Reduction

It has not potential

Oxidation

Redox

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

96500

193000

10000

48250

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

Henry’s law

Ostwald’s dilution law

Raoult’s law

Distribution law

34. The art of electroplating was given by

Faraday

Thomas Gradam

Brugan

Edison

35. The conductivity of strong electrolyte

Does not change on dilution

Increases on dilution slightly

Decreases on dilution

Depends on density of electrolyte itself.

36. 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

4.0 x 10¹²

1.0 x 10²

1.0 x 10¹⁰

37. 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

38. 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

39. 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

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

21.6 g

10.8 g

108 g

1.08 g

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

0.1 N HCl

Graphite

0.1 N NaCl

Glass

42. 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

128 S cm² mol¯¹

176 S cm² mol¯¹

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

Viscosity

Surface tension

Osmotic pressure

Refractive index

44. The Vant Hoff factor (i) accounts for

The extent of dissociation of solute

The extent of dissolution of solute

The degree of decomposition of solution

Degree of solubilization of solute

45. Stronger the oxidizing agent, greater is the

Oxidation potential

Reduction potential

Redox potential

e.m.f of cell

46. When common salt is dissolved in water

B.P of water remain constant

Any possibility

B.P of water decrease

B.P of water increase

47. During a redox reaction, an oxidizing agent

Loses electrons

Is oxidized

Is hydrolysed

Gains electrons

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

1.5

1.0

0.5

2.0

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

Galvanic cell

Electrolytic cell

Fuel cell

Dry cell

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

NaOH

Ca(OH)₂

KOH

NH₄OH

Page 3 of 8

51. Salt bridge transfers

Current

Anions

Electrons

Solvent particles

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

Cathodic protection

Electrolysis

Galvanization

Photo electrolysis

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

Boric acid

Nitric acid

Sulphuric acid

Phosphorus acid

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

0.1 molal

0.5 molal

1 molal

1.1 molal

55. Reaction takes place at anode is

Ionization

Reduction

Hydrolysis

Oxidation

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

None of these

Electrical energy

Chemical energy

Heat energy

57. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

0.25 mole

1.0 mole

0.5 mole

2.00 mole

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

Oxidation

Reduction

Both

Reduction

59. Molarity of water is

55.5

60. 96500 C of electricity liberates from CuSO₄ solution

100 g of Cu

96500 g of CU

31.75 g of Cu

63.5 g of Cu

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

Cl₂O

F₂O

Na₂O

Na₂O₂

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

Decrease rapidly

Drops to zero

Does not change

Decreases slowly

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

Electrical energy

Sound energy

Magnetic energy

Heat energy

64. Maximum freezing point falls in

Water

Benzene

Camphor

Naphthalene

65. Molton NaCl conducts electricity due to the presence of

Free ions

Free electrons

Atoms of Na and Cl.

Free molecules

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

800 mm of Hg

760 mm of Hg

750 mm of Hg

780 mm of Hg

67. 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

20 torr

140 torr

68 torr

72 torr

68. Vant Hoff’s factor of Ca(NO₃)₂ is

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

KCl

BaCl₂

NaCl

MgCl₂

70. Oxidation state of hydrogen in CaH₂ is

-2

-1

71. 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

C > B > A

A > B > C

B > C > A

A > C > B

72. Electrode potential of Zn is

Depends on the nature of the coupled electrode

Oxidation

Reduction

Oxidation-reduction

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

74. In a Galvanic cell

Chemical energy is converted into heat

Electrical energy is converted into chemical energy

Chemical energy is converted into electricity

Electrical energy is converted into heat

75. Oxidation in a chemical reaction involves

Increase in oxidation number of all the elements on reactant side

Decrease in oxidation number

Increase in oxidation number

Both are possible

Page 4 of 8

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

Electrons flow from cathode to anode through the external battery

Electrons flow cathode to anode within the electrolytic solution

None of these

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

77. Decrease in oxidation number is called

Reduction

All of these

Redox

Oxidation

78. Which of the following is a strong electrolyte?

Ca(NO₃)₂

CH₃COOH

NH₄OH

HCN

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

1 g

5 g

2 g

4 g

80. Corrosion is basically a

Altered reaction in presence of H₂O

Union between two light metals and a heavy metal

Interaction

Electrochemical phenomenon

81. 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

82. A redox reaction involves

A reaction in a solution

Proton transfer

Electron transfer

Ion combination reaction

83. Metals usually conduct electricity because

In metals the ions are free to more

They are mobile electrons in the metallic structure

Metals are decomposed by current

Metals have high resistance

84. Solution with same osmotic pressures are called

Normal

Isotonic

Hypotonic

Hypertonic

85. In alkaline battery anode is made up of

AgO₂

MnO₂

Cadmium

86. Specific conductivity of a solution

Increases with dilution

Depends on mass of electrolyte

Decreases with dilution

Remains unchanged with dilution

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

∆ G = +ve, ∆ E = 0

∆ G = -ve

∆ G = 0, ∆E = 0

∆ G = -ve, ∆ E = 0

88. 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

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

5.51

5.65

6.1

1.32

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

Supersaturated

Ideal

Unsaturated

Saturated

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

Electroplating

Electric change

Standard electrode potential

Ionization potential

92. The solubility of a gas in water depends upon

Pressure of the gas

Temperature

Nature of the gas

All of these

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

Gains electrons

Loses electrons

Acts as a catalyst

pH is changed

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

None of these

Both Na⁺ and CI¯

Cl¯

Na⁺

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

Lesser

Sum of reduction and oxidation potentials

Greater

None

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

Strong acid and its salt of weak base

Weak 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

97. 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

98. The unit of specific conductivity is

Ohm¯¹ cm

Ohm¯¹ cm¯¹

Ohm cm¯²

Ohm cm¯¹

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

4.10

7.20

3.12

0.217

100. 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

Page 5 of 8

101. 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

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

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

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

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

None

103. 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)

0.0033

0.333

3.33

33.3

104. 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

105. 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

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

1 molal

1 normal

1 molar

All

107. Reduction always occurs

At anode

None of these

At cathode

Both A and B

108. Salt bridge transfers

Electrons

Current

Anion

Ions

109. An electrolyte

Forms complex ions in solution

Gives ions only when electricity is passed

Possesses ions even in solid state

Gives ions only when dissolved in water

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

12157.48 sec

642 sec

510 sec

102 sec

111. What are the ions present in water?

H2 and O

H and OH

H2O

H+ and OH-

112. Cathode provides electrons to

Does not provide any electron

+Ve ion

-Ve ion

Neutral atom

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

22400 cm³

112 cm³

1.008 g

224 cm³

114. 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

20 C

120 C

4 C

240 C

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

4 g

60 g

6 g

40 g

116. Colligative properties are the properties of

Dilute solution which behave as nearly ideal solution

Concentration solutions behave as nearly non – ideal solutions

Both a and b

Neither a nor b

117. When Cu, Ag, Au and Pt are reacted with acids, these metals do not liberate hydrogen, this is due to the reason that

Very high positive value of reduction potential

Reduction potentials are negative

Very high negative values reduction potential

Very low ionization potential values

118. 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

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

I₂

Ag⁺

Pb²⁺

120. 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

2.0

0.5

1.0

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

O₂, Na

None of these

O₂, SO₂

O₂,H₂

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

1.5

123. 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¯²

S m² mol¯¹

S m mol¯¹

S² m² mol

124. Chemical used in salt bridge is

KBr

KCI

KNO3

KOH

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

Electrorefining

Both A and B

Electroplating

None of these

Page 6 of 8

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

Drops to zero

Increases rapidly

Does not change

Increases gradually

127. Best way to prevent rusting iron is by

Both of these

None of these

Putting it in saline water

Making iron cathode

128. In alkaline battery the anode is made up of

MnO2

Cadmium

AgO2

129. 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

130. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.4 M

0.8 M

0.2 M

0.04 M

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

Milligram percent

Parts per million

Gram per million

Microgram percent

132. Secondary cell is

Rechargeable

Non rechargeable

Electrolytic cell

Daniel cell

133. The reference electrode is made by using

CuSO₄

HgCl₂

ZnCl₂

Hg₂Cl₂

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

0.25

2.05

0.5

0.05

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

0.80

0.0512

0.512

0.186

136. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

5.1

1/5

1/51

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

Generate heat

Produce high purity water

Remove adsorbed oxygen from electrode surfaces

Create potential difference between two electrodes

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

1.08 g

0.54 g

0.27 g

2.16 g

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

140. Half cells are interconnected through

Electric circuit

Salt Bridge

Wire

No connection exists

141. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

1 N

11 N

10 N

0.1N

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

Na and Hg

Na and S only

Pt and graphite only

Na, Pt and graphite

143. Oxidation number of carbon in NaHCO₃ is

-6

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

Reduction

Oxidation

Both oxidation and reduction

Neither oxidation and reduction

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

Melting point

Sublimation point

Boiling point

Inversion point

146. 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

8 N

2 N

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

10 ml

40 ml

20 ml

80 ml

148. Camphor is often used in molecular mass determination because

It is readily available

It has a very high cryoscopic constant

It is solvent for organic substances

It is volatile

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

0 to 5.

1 to 5

2 to 5

0 to –3

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

760 mm of Hg

2.5 atom

Slightly more than 1 atom

750 torr

Page 7 of 8

151. In a Galvanic cell, the electrons flow from

Anode to cathode through the external circuit

Cathode to anode through the solution

Cathode to anode through the external circuit

Anode to cathode through the solution

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

0.1

0.0196

0.01

0.2

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

0.1 M BaCl₂

0.1 M Sucrose

0.1 M Glucose

0.1 M NaCl

154. If liquids A and B form an ideal solution

The enthalpy of mixing is zero

The free energy of mixing is zero

The entropy of mixing is zero

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

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

Fuel cell

Daniel cell

Electrolytic cell

Galvanic cell

156. The depression of freezing point is directly proportional to

Molarity of the solvent

Mole fraction of the solution

Molarity of the solution

Molality of the solution

157. In electrolytic cell, electricity in carried out by

Spontaneous reaction

Non-spontaneous reaction

Neutralization

All

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

Vacuum distillation

Distillation

None of these

Fractional distillation

159. 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?

18.4 M

18 M

8.14 M

4.18 M

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

1.81 cm¯³

2.15 cm¯³

1.15 cm¯³

1.25 cm¯³

161. Units of molarity are

None of these

Kg/lit

Gm/lit

Mol/lit

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

1.21 atm

24.6 atm

12.1 atm

2.46 atm

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

Electroplating

Electrolysis

Induction

Conduction

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

CH₃ CooNH₄

Na₂SO₄

NH₄Cl

NaCl

165. The degree of dissociation of weak electrolyte increases as

Dilution increases

Dilution decreases

Pressure increases

None

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

HgCl₂

Hg₂Cl₂

CuSO₄

ZnCl₂

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

18.6 c°

Sufficient date not given

1.86 c°

0.186 c°

168. Azeotropic mixture of HCl and water has

20.2% HCl

22.2% HCl

36% HCl

48% HCl

169. 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

53.07 kJ

175.4 kJ

170. 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

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

Precipitated

Oxidized

Hydrolyzed

Reduced

172. Pure water does not conduct electricity because it

Is almost unionized

Is neutral

Is readily decomposed

Has low boiling point

173. Which has maximum oxidation number

174. 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)₄Cl₃]Cl

[Pt(NH₃)₄Cl₄]

[Pt(NH₃)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl]Cl₃

175. Pick out the wrong statement. In electrochemical cell

Electrons are released at anode

Cathode is regarded as negative electrode

Salt bridge maintains the electrical neutrality of the solution

Chemical energy is converted into electrical energy

Page 8 of 8

176. Temperature for standard electrode potential is

273 K

310 K

300 K

25 C°

177. 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

31.8 gm

15.9 gm

178. 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

9 N

1 N

3 N

179. 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

Slightly more than the total volume of the components

Equal to the total volume of the components

180. Electricity in voltaic cell is produced due to

B + C

Oxidation

Reduction

Neutralization

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

Chloroform

Dilute solution of glucose

Pure distilled water

Molten NaCl

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

20g NaCl/100ml

5.58g NaCl/100m

10.0g NaCl/100ml

58.5g NaCl/100ml

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

H₃PO₃

H₄P₃O₇

H₃PO₂

H₃PO₄

184. Which of the statements given below concerning properties of solution, describe a colligaive effect?

Boiling point of pure water decreases by the addition of ethanol

Boiling point of pure benzene increases by the addition of toluene

Vapour pressure of pure benzene decreases by the addition of naphthalene

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

185. Alkaline battery has a voltage of

4.5V

3.5V

2.5V

1.5V

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

+ 0.35

– 0.35 V

+ 1.17 V

– 1.17 V

187. Strong reducing agents have

None of these

Greater negative value of standard reduction potential

Lesser positive value of standard reduction potential

Greater positive value of standard reduction potential

188. Density of H₂SO₄ in lead accumulator is

1.15g/cm3

1.20g/cm3

1.3g/cm3

1.25g/cm3

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

Oxygen

Hydrogen

Chlorine

Chloride

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

2 ampere

1 ampere

1 coulomb

1 faraday

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

45.1

40.5

39.6

42.7

192. 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)

0.281 V

0.222 V

0.176 V

0.399 V

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