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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. 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 – 2 α

1 – α

2. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

1.0 mole

2.00 mole

0.5 mole

0.25 mole

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

Less than that of water

Equal to that of ethanol

Equal to that of water

More than that of H₂O

4. 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

5. Oxidation state of hydrogen in CaH₂ is

-2

-1

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

Graphite

0.1 N HCl

Glass

0.1 N NaCl

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

Galvanic cell

Electrolytic cell

Fuel cell

Daniel cell

8. Density of H₂SO₄ in lead accumulator is

1.25g/cm3

1.15g/cm3

1.20g/cm3

1.3g/cm3

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

6.4 g

12.8 g

10. Potential of Zn is called

It has not potential

Redox

Reduction

Oxidation

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

10.0g NaCl/100ml

20g NaCl/100ml

5.58g NaCl/100m

58.5g NaCl/100ml

12. Chemical used in salt bridge is

KNO3

KOH

KCI

KBr

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

Electrical energy

Sound energy

Heat energy

Magnetic energy

14. Voltaic cell can be recharged by

By addition of fresh solution

By replacing external circuit with external source of electricity

By heating it

By removal of solution

15. 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

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

Decreases slowly

Decrease rapidly

Does not change

Drops to zero

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

750 torr

760 mm of Hg

Slightly more than 1 atom

2.5 atom

18. A redox reaction involves

A reaction in a solution

Proton transfer

Ion combination reaction

Electron transfer

19. Pure water does not conduct electricity because it

Is almost unionized

Has low boiling point

Is readily decomposed

Is neutral

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

0.80

0.186

0.512

0.0512

21. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

1 N

0.1N

10 N

11 N

22. Decrease in oxidation number is called

Oxidation

All of these

Redox

Reduction

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

24. 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

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

None of these

25. Oxidation number of carbon in NaHCO₃ is

-6

Page 2 of 8

26. Electrode potential of Zn is

Oxidation

Reduction

Depends on the nature of the coupled electrode

Oxidation-reduction

27. 96500 C of electricity liberates from CuSO₄ solution

100 g of Cu

63.5 g of Cu

31.75 g of Cu

96500 g of CU

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

Microgram percent

Parts per million

Gram per million

Milligram percent

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

Sublimation point

Boiling point

Melting point

Inversion point

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

Pb²⁺

Ag⁺

I₂

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

20 ml

40 ml

80 ml

10 ml

32. In electrolytic cell, electricity in carried out by

Neutralization

All

Non-spontaneous reaction

Spontaneous reaction

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

48250

96500

193000

10000

34. 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

35. Reduction always occurs

Both A and B

At anode

At cathode

None of these

36. Stronger the oxidizing agent, greater is the

Reduction potential

e.m.f of cell

Redox potential

Oxidation potential

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

Ostwald’s law

Arrhenius law

Raoult’s law

Henry’s law

38. The conductivity of strong electrolyte

Depends on density of electrolyte itself.

Decreases on dilution

Does not change on dilution

Increases on dilution slightly

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

– 0.35 V

+ 1.17 V

+ 0.35

– 1.17 V

40. 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

0.176 V

0.399 V

0.222 V

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

Reduced

Precipitated

Oxidized

Hydrolyzed

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

60 g

40 g

6 g

4 g

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

Osmotic pressure

Surface tension

Refractive index

Viscosity

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

∆ G = 0, ∆E = 0

∆ G = -ve

∆ G = +ve, ∆ E = 0

∆ G = -ve, ∆ E = 0

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

2 g

10 g

1 g

20 g

46. 1.0 g of pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of HCl solution is given by

2 N

0.2 N

0.4 N

4 N

47. When electricity is passed through molten electrolyte consisting of alumina and cryolite, 13.5 g of Al are deposited. The number of faradays of electricity passed must be

0.5

1.5

2.0

1.0

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

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

1 molal

All

1 molar

1 normal

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

Photo electrolysis

Electrolysis

Cathodic protection

Galvanization

Page 3 of 8

51. An electrolyte

Forms complex ions in solution

Gives ions only when dissolved in water

Gives ions only when electricity is passed

Possesses ions even in solid state

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

None of these

Cl¯

Na⁺

Both Na⁺ and CI¯

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

1 g

5 g

4 g

2 g

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

4 N

2 N

6 N

8 N

55. Corrosion reactions are

Spontaneous acid–base reactions

Non-spontaneous redox reactions

None of these

Spontaneous redox reactions

56. Salt bridge transfers

Solvent particles

Electrons

Current

Anions

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

Fuel cell

Dry cell

Electrolytic cell

Galvanic cell

58. Mole fraction of pure water is

None of these

Slightly greater than one

Slightly less than one

Exactly equal to one

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

Chloroform

Dilute solution of glucose

Molten NaCl

Pure distilled water

60. Pick out the wrong statement. In electrochemical cell

Electrons are released at anode

Cathode is regarded as negative electrode

Chemical energy is converted into electrical energy

Salt bridge maintains the electrical neutrality of the solution

61. Vant Hoff’s factor of Ca(NO₃)₂ is

62. 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

68 torr

72 torr

140 torr

63. Choose the best reducing agent among the following

Br¯¹

Cl¯¹

I¯¹

F¯¹

64. 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

65. During a redox reaction, an oxidizing agent

Loses electrons

Is oxidized

Gains electrons

Is hydrolysed

66. What are the ions present in water?

H and OH

H+ and OH-

H2O

H2 and O

67. 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

20 C

120 C

240 C

68. Best way to prevent rusting iron is by

None of these

Making iron cathode

Putting it in saline water

Both of these

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

0.9

0.2

0.6

0.3

70. In an electrolytic cell current flows

From anode to cathode in an outer circuit

From cathode to anode in outer circuit

From cathode to anode inside the cell

From anode to cathode inside the cell

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

Drops to zero

Does not change

Increases rapidly

Increases gradually

72. The solubility of a gas in water depends upon

Pressure of the gas

All of these

Nature of the gas

Temperature

73. 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)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl₃]Cl

[Pt(NH₃)₄Cl]Cl₃

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

Oxygen

Hydrogen

Chloride

Chlorine

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

Acts as a catalyst

pH is changed

Gains electrons

Loses electrons

Page 4 of 8

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

None of these

Electrorefining

Both A and B

Electroplating

77. In a chemical reaction, oxidation process involves

Decrease in oxidation number of element

Increase in oxidation number of the elements in reactants

Oxidation number neither increases nor decreases

Increase in oxidation number of element

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

Neither oxidation and reduction

Reduction

Oxidation

Both oxidation and reduction

79. 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

0.142 cm¯¹

0.918 cm¯¹

0.66 cm¯¹

1.12 cm¯¹

80. Electricity in voltaic cell is produced due to

Neutralization

Oxidation

B + C

Reduction

81. Units of molarity are

Mol/lit

Gm/lit

None of these

Kg/lit

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

One gm. Equivalent weight

Electrochemical equivalent

One gm. atomic weight

None of these

83. Cathode provides electrons to

+Ve ion

Neutral atom

Does not provide any electron

-Ve ion

84. 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

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

11.2 cm³

5.6 cm³

550 cm³

56 cm³

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

Sum of reduction and oxidation potentials

Lesser

None

Greater

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

Heat energy

None of these

Chemical energy

Electrical energy

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

30 s

30,000 s

10,000 s

10 s

89. Strong reducing agents have

None of these

Lesser positive value of standard reduction potential

Greater positive value of standard reduction potential

Greater negative value of standard reduction potential

90. 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

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

1.5

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

Electrode

Anode

None of these

Cathode

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

1.25 cm¯³

1.81 cm¯³

1.15 cm¯³

2.15 cm¯³

94. 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?

31.8 gm

63.5 gm

15.9 gm

12.7 gm

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

Electrolysis

Conduction

Electroplating

Induction

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

0.1

0.0196

0.01

0.2

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

176 S cm² mol¯¹

278 S cm² mol¯¹

302 S cm² mol¯¹

128 S cm² mol¯¹

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

Cell voltage

Ionization potential

Standard reduction potential

Standard oxidation potential

99. 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

9 N

3 N

1 N

2 N

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

Hg₂Cl₂

HgCl₂

CuSO₄

ZnCl₂

Page 5 of 8

101. Standard hydrogen electrode has an arbitrarily fixed potential

0.10 volt

1.00 volt

None of these

0.00 volt

102. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.04 M

0.4 M

0.8 M

0.2 M

103. Molton NaCl conducts electricity due to the presence of

Free ions

Free molecules

Atoms of Na and Cl.

Free electrons

104. 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

0.80

0.75

0.20

105. Alkaline battery has a voltage of

4.5V

3.5V

1.5V

2.5V

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

Na₂SO₄

CH₃ CooNH₄

NH₄Cl

NaCl

107. 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

3.33

33.3

0.333

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

108 g

10.8 g

21.6 g

1.08 g

109. Temperature for standard electrode potential is

300 K

310 K

273 K

25 C°

110. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/51

1/5

5.1

111. 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

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

1.5

0.5

1.0

2.0

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

0.186 c°

1.86 c°

18.6 c°

Sufficient date not given

114. Metals usually conduct electricity because

In metals the ions are free to more

Metals are decomposed by current

They are mobile electrons in the metallic structure

Metals have high resistance

115. In alkaline battery the anode is made up of

Cadmium

MnO2

AgO2

116. Maximum freezing point falls in

Benzene

Water

Camphor

Naphthalene

117. If liquids A and B form an ideal solution

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

The free energy of mixing is zero

The enthalpy of mixing is zero

The entropy of mixing is zero

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

0.05

0.25

2.05

0.5

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

NaOH

KOH

Ca(OH)₂

NH₄OH

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

H₄P₃O₇

H₃PO₄

H₃PO₃

H₃PO₂

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

12.1 atm

24.6 atm

2.46 atm

1.21 atm

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

Gold has higher reduction potential then iron

Gold is denser

Gold has lower reduction potential then iron

Iron rusts

123. Specific conductivity of a solution

Increases with dilution

Depends on mass of electrolyte

Remains unchanged with dilution

Decreases with dilution

124. 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 BaCl₂

0.1 M NaCl

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

In middle

Higher

Not particular

Lower

Page 6 of 8

126. Corrosion is basically a

Interaction

Altered reaction in presence of H₂O

Electrochemical phenomenon

Union between two light metals and a heavy metal

127. Density of H₂SO₄ in lead accumulator is

1.25g/Cm³

120 g Cm³

1.15 g/Cm³

1.2 g/Cm³

128. 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

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

1 ampere

1 coulomb

2 ampere

1 faraday

130. 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

1.25

2.5

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

KCl

NaCl

MgCl₂

BaCl₂

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

None of these

O₂,H₂

O₂, SO₂

O₂, Na

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

1 M

1 f

2 M

1 N

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

45.1

42.7

40.5

39.6

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

136. Colligative properties are the properties of

Dilute solution which behave as nearly ideal solution

Both a and b

Concentration solutions behave as nearly non – ideal solutions

Neither a nor b

137. 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

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 benzene increases by the addition of toluene

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

Weak acid and its salt of strong base

Weak acid and its salt of weak base

A strong acid and its salt of a strong base

Strong acid and its salt of weak base

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

11.2%

9.09%

13.1%

14.25%

140. Oxidation in a chemical reaction involves

Increase in oxidation number of all the elements on reactant side

Increase in oxidation number

Both are possible

Decrease in oxidation number

141. The degree of dissociation of weak electrolyte increases as

None

Pressure increases

Dilution decreases

Dilution increases

142. Solution with same osmotic pressures are called

Isotonic

Normal

Hypotonic

Hypertonic

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

8.14 M

18.4 M

4.18 M

18 M

144. The reference electrode is made by using

CuSO₄

ZnCl₂

Hg₂Cl₂

HgCl₂

145. Salt bridge transfers

Ions

Electrons

Current

Anion

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

Supersaturated

Saturated

Ideal

Unsaturated

147. Which of the following is a strong electrolyte?

Ca(NO₃)₂

CH₃COOH

HCN

NH₄OH

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

Na⁺ + e– → Na

Br₂ + 2e – → 2Br –

2Br– → Br₂ + 2e –

Na → Na⁺ + e–

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

Vacuum distillation

Fractional distillation

None of these

Distillation

150. Reaction takes place at anode is

Hydrolysis

Reduction

Oxidation

Ionization

Page 7 of 8

151. The unit of specific conductivity is

Ohm cm¯²

Ohm cm¯¹

Ohm¯¹ cm¯¹

Ohm¯¹ cm

152. Camphor is often used in molecular mass determination because

It is volatile

It has a very high cryoscopic constant

It is readily available

It is solvent for organic substances

153. 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

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

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

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

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

A voltaic cell

A galvanic cell

An electrolytic cell

A chemical cell

155. 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

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

None

157. 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 high positive value of reduction potential

Reduction potentials are negative

Very low ionization potential values

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

Distribution law

Henry’s law

Ostwald’s dilution law

Raoult’s law

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

Flow of solvent from a concentrated to a dilute solution

Elevation in boiling point

Ionic concentration

Diffusion rate of the solute

160. 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

1 molal

1.1 molal

0.1 molal

161. 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

162. 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

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

Reduction

Both

Oxidation

164. In alkaline battery anode is made up of

MnO₂

AgO₂

Cadmium

165. 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

166. Secondary cell is

Daniel cell

Rechargeable

Non rechargeable

Electrolytic cell

167. 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

0.15 M

0.1 M

0.2 M

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

0.1

0.01

0.2

0.0196

169. The best reducing agent is

F¯

I¯

Br¯

Cl¯

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

0 to –3

0 to 5.

2 to 5

1 to 5

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

Boric acid

Phosphorus acid

Sulphuric acid

Nitric acid

172. The Vant Hoff factor (i) accounts for

Degree of solubilization of solute

The extent of dissociation of solute

The extent of dissolution of solute

The degree of decomposition of solution

173. The art of electroplating was given by

Faraday

Thomas Gradam

Brugan

Edison

174. Azeotropic mixture of HCl and water has

22.2% HCl

36% HCl

48% HCl

20.2% HCl

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

3.12

0.217

7.20

4.10

Page 8 of 8

176. 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

Li is smaller in size as compared to Cu

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

177. 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 10²

2.0 x 10¹¹

4.0 x 10¹²

1.0 x 10¹⁰

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

Na₂O₂

Na₂O

Cl₂O

F₂O

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

Rust removal

Electroplating

Making leather

Manufacture of bleach

180. The depression of freezing point is directly proportional to

Molality of the solution

Molarity of the solvent

Molarity of the solution

Mole fraction of the solution

181. 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

182. 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, Pt and graphite

Pt and graphite only

Na and S only

183. Which of the following statements is FALSE?

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

Reduction occurs at cathode

All electrochemical reactions involve the transfer of electrons

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

184. 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

185. 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

0.25

0.40

0.35

0.30

186. 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

187. Molarity of water is

55.5

188. When common salt is dissolved in water

B.P of water increase

B.P of water remain constant

B.P of water decrease

Any possibility

189. 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 solution

Anode to cathode through the external circuit

190. Which has maximum oxidation number

191. 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

192. Half cells are interconnected through

No connection exists

Electric circuit

Salt Bridge

Wire

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Malik TahirLast Updated: May 24, 2025

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