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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. 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

2. 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)

3.33

0.0033

0.333

33.3

3. Strong reducing agents have

Greater positive value of standard reduction potential

Greater negative value of standard reduction potential

None of these

Lesser positive value of standard reduction potential

4. Salt bridge transfers

Current

Anions

Electrons

Solvent particles

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

1.08 g

0.27 g

0.54 g

2.16 g

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

1.5

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

40 ml

10 ml

80 ml

20 ml

8. 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

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

None

10. Pure water does not conduct electricity because it

Has low boiling point

Is neutral

Is readily decomposed

Is almost unionized

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

KCl

NaCl

BaCl₂

MgCl₂

12. Density of H₂SO₄ in lead accumulator is

1.2 g/Cm³

120 g Cm³

1.25g/Cm³

1.15 g/Cm³

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

Chloroform

Pure distilled water

Molten NaCl

Dilute solution of glucose

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

0.05

0.5

0.25

2.05

15. Solution with same osmotic pressures are called

Normal

Hypotonic

Isotonic

Hypertonic

16. Pick out the wrong statement. In electrochemical cell

Salt bridge maintains the electrical neutrality of the solution

Chemical energy is converted into electrical energy

Cathode is regarded as negative electrode

Electrons are released at anode

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

Hydrogen

Chloride

Chlorine

Oxygen

18. Units of molarity are

Gm/lit

Kg/lit

Mol/lit

None of these

19. Corrosion reactions are

Non-spontaneous redox reactions

Spontaneous acid–base reactions

Spontaneous redox reactions

None of these

20. Decrease in oxidation number is called

All of these

Oxidation

Redox

Reduction

21. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

None of these

1 2

1.25

2.5

22. Electrode potential of Zn is

Depends on the nature of the coupled electrode

Oxidation-reduction

Oxidation

Reduction

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

8 N

6 N

2 N

4 N

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

Diffusion rate of the solute

Elevation in boiling point

Flow of solvent from a concentrated to a dilute solution

Ionic concentration

25. 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⁺

Page 2 of 8

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

More than that of H₂O

Less than that of water

Equal to that of ethanol

Equal to that of water

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

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

0.2

0.1

0.01

0.0196

29. 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

10,000 s

10 s

30,000 s

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

Distribution law

Raoult’s law

Ostwald’s dilution law

Henry’s law

31. In a chemical reaction, oxidation process involves

Oxidation number neither increases nor decreases

Increase in oxidation number of element

Decrease in oxidation number of element

Increase in oxidation number of the elements in reactants

32. 96500 C of electricity liberates from CuSO₄ solution

63.5 g of Cu

96500 g of CU

31.75 g of Cu

100 g of Cu

33. 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

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

1 normal

All

1 molar

1 molal

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

175.4 kJ

212.3 kJ

106.15 kJ

53.07 kJ

36. The art of electroplating was given by

Edison

Thomas Gradam

Faraday

Brugan

37. If liquids A and B form an ideal solution

The enthalpy of mixing is zero

The entropy of mixing is zero

The free energy of mixing is zero

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

38. Density of H₂SO₄ in lead accumulator is

1.20g/cm3

1.25g/cm3

1.3g/cm3

1.15g/cm3

39. What are the ions present in water?

H and OH

H+ and OH-

H2 and O

H2O

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

Gains electrons

pH is changed

Loses electrons

Acts as a catalyst

41. Metals usually conduct electricity because

In metals the ions are free to more

They are mobile electrons in the metallic structure

Metals have high resistance

Metals are decomposed by current

42. 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

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

Cathodic protection

Galvanization

Electrolysis

Photo electrolysis

44. 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

0.176 V

0.281 V

0.222 V

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

Supersaturated

Ideal

Saturated

Unsaturated

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

One gm. atomic weight

One gm. Equivalent weight

Electrochemical equivalent

None of these

47. During a redox reaction, an oxidizing agent

Gains electrons

Is hydrolysed

Is oxidized

Loses electrons

48. 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

Na and S only

Pt and graphite only

49. Vant Hoff’s factor of Ca(NO₃)₂ is

50. Voltaic cell can be recharged by

By replacing external circuit with external source of electricity

By heating it

By removal of solution

By addition of fresh solution

Page 3 of 8

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

0.1 M Sucrose

0.1 M BaCl₂

0.1 M NaCl

0.1 M Glucose

52. 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

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

Distillation

Fractional distillation

None of these

Vacuum distillation

54. Temperature for standard electrode potential is

310 K

300 K

273 K

25 C°

55. Azeotropic mixture of HCl and water has

36% HCl

22.2% HCl

48% HCl

20.2% HCl

56. The depression of freezing point is directly proportional to

Molality of the solution

Molarity of the solution

Molarity of the solvent

Mole fraction of the solution

57. Specific conductivity of a solution

Depends on mass of electrolyte

Increases with dilution

Decreases with dilution

Remains unchanged with dilution

58. 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 cathode to anode within the electrolytic solution

Electrons flow from cathode to anode through the external battery

None of these

59. 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 – α

1 – 2 α

60. Half cells are interconnected through

No connection exists

Salt Bridge

Wire

Electric circuit

61. 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

62. Which has maximum oxidation number

63. Which of the following is a strong electrolyte?

HCN

NH₄OH

Ca(NO₃)₂

CH₃COOH

64. 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

1.08 g

108 g

10.8 g

65. Best way to prevent rusting iron is by

None of these

Making iron cathode

Both of these

Putting it in saline water

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

Electrical energy

Heat energy

Chemical energy

None of these

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

4 g

2 g

5 g

1 g

68. Secondary cell is

Electrolytic cell

Non rechargeable

Rechargeable

Daniel cell

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

Dry cell

Galvanic cell

Fuel cell

Electrolytic cell

70. Mole fraction of pure water is

Slightly less than one

Slightly greater than one

None of these

Exactly equal to one

71. 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

20 g

1 g

10 g

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

Oxidation

Reduction

Both oxidation and reduction

Neither oxidation and reduction

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

1 faraday

1 coulomb

1 ampere

2 ampere

74. Which of the following statements is FALSE?

All electrochemical reactions involve the transfer of electrons

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

Reduction occurs at cathode

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

75. Molton NaCl conducts electricity due to the presence of

Atoms of Na and Cl.

Free molecules

Free ions

Free electrons

Page 4 of 8

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

14.25%

9.09%

13.1%

11.2%

77. Corrosion is basically a

Union between two light metals and a heavy metal

Interaction

Altered reaction in presence of H₂O

Electrochemical phenomenon

78. Colligative properties are the properties of

Both a and b

Neither a nor b

Dilute solution which behave as nearly ideal solution

Concentration solutions behave as nearly non – ideal solutions

79. Reduction always occurs

At cathode

At anode

None of these

Both A and B

80. Salt bridge transfers

Electrons

Anion

Ions

Current

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

1.0

0.5

1.5

2.0

82. The reference electrode is made by using

ZnCl₂

CuSO₄

Hg₂Cl₂

HgCl₂

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

4 g

6 g

40 g

60 g

84. 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

224 cm³

1.008 g

112 cm³

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

1 f

1 M

2 M

1 N

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

+ 0.35

– 1.17 V

+ 1.17 V

– 0.35 V

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

Does not change

Increases rapidly

Drops to zero

Increases gradually

88. The solubility of a gas in water depends upon

Pressure of the gas

Temperature

Nature of the gas

All of these

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

550 cm³

11.2 cm³

5.6 cm³

56 cm³

90. An electrolyte

Gives ions only when dissolved in water

Forms complex ions in solution

Possesses ions even in solid state

Gives ions only when electricity is passed

91. 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

0.60

0.75

0.80

92. 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

93. Conductivity (Unit : siemen’s S) is directly proportionally to the area of the vessel and the concentration of the solution in it and is inversely proportional to the length of vessel, then the unit of constant of proportionality is

S m mol¯¹

S² m² mol

S² m² mol¯²

S m² mol¯¹

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

KOH

NH₄OH

NaOH

Ca(OH)₂

95. Oxidation number of carbon in NaHCO₃ is

-6

96. 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

3 N

1 N

9 N

2 N

97. Oxidation state of hydrogen in CaH₂ is

-1

-2

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

0 to –3

2 to 5

0 to 5.

1 to 5

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

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

Boiling point

Inversion point

Melting point

Sublimation point

Page 5 of 8

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

Lesser

Greater

Sum of reduction and oxidation potentials

None

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

Surface tension

Osmotic pressure

Viscosity

Refractive index

103. Alkaline battery has a voltage of

2.5V

4.5V

1.5V

3.5V

104. 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

2.0

1.0

0.5

1.5

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

0.521

1.86

0.0521

0.0186

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

58.5g NaCl/100ml

10.0g NaCl/100ml

5.58g NaCl/100m

20g NaCl/100ml

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

Decrease rapidly

Does not change

Decreases slowly

Drops to zero

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

Not particular

Lower

In middle

Higher

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

HgCl₂

ZnCl₂

Hg₂Cl₂

CuSO₄

110. 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

0.2 M

0.15 M

0.05 M

0.1 M

111. Electricity in voltaic cell is produced due to

B + C

Neutralization

Oxidation

Reduction

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

Standard electrode potential

Electric change

Ionization potential

Electroplating

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

Gram per million

Microgram percent

Milligram percent

Parts per million

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

Both Na⁺ and CI¯

None of these

Na⁺

Cl¯

115. 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

102 sec

642 sec

116. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.4 M

0.04 M

0.8 M

0.2 M

117. 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

118. The conductivity of strong electrolyte

Increases on dilution slightly

Depends on density of electrolyte itself.

Decreases on dilution

Does not change on dilution

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

2.46 atm

12.1 atm

24.6 atm

1.21 atm

120. 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

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

None of these

Electrorefining

Both A and B

Electroplating

122. The best reducing agent is

Cl¯

I¯

Br¯

F¯

123. Standard hydrogen electrode has an arbitrarily fixed potential

0.10 volt

0.00 volt

1.00 volt

None of these

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

Remove adsorbed oxygen from electrode surfaces

Create potential difference between two electrodes

Produce high purity water

Generate heat

125. Oxidation in a chemical reaction involves

Decrease in oxidation number

Both are possible

Increase in oxidation number of all the elements on reactant side

Increase in oxidation number

Page 6 of 8

126. 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

127. 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°

1.86 c°

18.6 c°

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

None of these

Equal to the total volume of the components

Slightly more than the total volume of the components

Slightly less than the total volume of the components

129. The unit of specific conductivity is

Ohm cm¯¹

Ohm¯¹ cm¯¹

Ohm cm¯²

Ohm¯¹ cm

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

∆ G = -ve, ∆ E = 0

∆ G = 0, ∆E = 0

∆ G = -ve

∆ G = +ve, ∆ E = 0

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

7.20

4.10

3.12

0.217

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

Cathode

None of these

Anode

Electrode

133. 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 10⁴

1.06 x 10²

1.06 x 10³

134. Choose the best reducing agent among the following

I¯¹

Cl¯¹

Br¯¹

F¯¹

135. 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

15.9 gm

12.7 gm

31.8 gm

136. 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

137. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

1.0 mole

0.5 mole

2.00 mole

0.25 mole

138. Reaction takes place at anode is

Hydrolysis

Ionization

Oxidation

Reduction

139. Cathode provides electrons to

Does not provide any electron

Neutral atom

-Ve ion

+Ve ion

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

0.1 N NaCl

Glass

Graphite

0.1 N HCl

141. 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 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

142. Stronger the oxidizing agent, greater is the

Redox potential

Oxidation potential

e.m.f of cell

Reduction potential

143. In a Galvanic cell, the electrons flow from

Cathode to anode through the solution

Anode to cathode through the solution

Anode to cathode through the external circuit

Cathode to anode through the external circuit

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

Rust removal

Manufacture of bleach

Making leather

Electroplating

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

Pb²⁺

I₂

Ag⁺

146. In an electrolytic cell current flows

From anode to cathode inside the cell

From cathode to anode in outer circuit

From cathode to anode inside the cell

From anode to cathode in an outer circuit

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

0.9

0.3

0.6

0.2

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

Na₂SO₄

NH₄Cl

CH₃ CooNH₄

NaCl

149. 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

150. 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

Page 7 of 8

151. 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)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl]Cl₃

[Pt(NH₃)₄Cl₄]

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

Standard reduction potential

Cell voltage

Ionization potential

Standard oxidation potential

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

Na → Na⁺ + e–

Br₂ + 2e – → 2Br –

Na⁺ + e– → Na

2Br– → Br₂ + 2e –

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

42.7

39.6

45.1

40.5

155. In electrolytic cell, electricity in carried out by

Non-spontaneous reaction

Spontaneous reaction

Neutralization

All

156. Maximum freezing point falls in

Naphthalene

Benzene

Water

Camphor

157. Camphor is often used in molecular mass determination because

It is solvent for organic substances

It has a very high cryoscopic constant

It is volatile

It is readily available

158. Molarity of water is

55.5

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

193000

48250

10000

96500

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

Reduction

Both

Oxidation

Reduction

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

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

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

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

Hg is more inert than Pt

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

None of these

O₂, Na

O₂,H₂

O₂, SO₂

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

Induction

Conduction

Electrolysis

164. 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

12.8 g

2.3 g

3.2 g

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

H₃PO₂

H₄P₃O₇

H₃PO₄

H₃PO₃

166. In alkaline battery anode is made up of

Cadmium

MnO₂

AgO₂

167. 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

240 C

4 C

120 C

168. 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

1.0 x 10²

4.0 x 10¹²

2.0 x 10¹¹

169. Potential of Zn is called

Oxidation

It has not potential

Redox

Reduction

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

Heat energy

Magnetic energy

Sound energy

Electrical energy

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

Sulphuric acid

Nitric acid

Boric acid

Phosphorus acid

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

0.1

0.2

0.0196

0.01

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

Cl₂O

Na₂O₂

F₂O

Na₂O

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

Oxidized

Hydrolyzed

Precipitated

Reduced

175. A redox reaction involves

Ion combination reaction

A reaction in a solution

Proton transfer

Electron transfer

Page 8 of 8

176. Standard reduction electrode potential of three metals A, B and C are respectively + 0.05 V, - 3.0 and -1.2V. The reducing power of

A > B > C

C > B > A

A > C > B

B > C > A

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

An electrolytic cell

A galvanic cell

A chemical cell

A voltaic cell

178. In alkaline battery the anode is made up of

AgO2

Cadmium

MnO2

179. The specific conductance of a 0.1 N KCl solution at 23°C is 0.012 ohm¯¹ cm¯¹. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be

0.66 cm¯¹

0.142 cm¯¹

1.12 cm¯¹

0.918 cm¯¹

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

Electrolytic cell

Galvanic cell

Daniel cell

Fuel cell

181. When common salt is dissolved in water

Any possibility

B.P of water decrease

B.P of water increase

B.P of water remain constant

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

183. 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

Reduction potentials are negative

Very low ionization potential values

Very high positive value of reduction potential

184. Chemical used in salt bridge is

KOH

KNO3

KCI

KBr

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

Henry’s law

Raoult’s law

Ostwald’s law

Arrhenius law

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

Gold is denser

Gold has lower reduction potential then iron

Gold has higher reduction potential then iron

Iron rusts

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

1.15 cm¯³

1.81 cm¯³

2.15 cm¯³

1.25 cm¯³

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

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

Weak acid and its salt of strong base

189. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

5.1

1/5

1/51

190. The degree of dissociation of weak electrolyte increases as

Dilution increases

Dilution decreases

Pressure increases

None

191. 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

128 S cm² mol¯¹

302 S cm² mol¯¹

176 S cm² mol¯¹

192. 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

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Malik TahirLast Updated: May 24, 2025

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