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

0.5 mole

2.00 mole

1.0 mole

0.25 mole

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

Fuel cell

Electrolytic cell

Galvanic cell

Dry cell

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

Oxidation

Reduction

Neither oxidation and reduction

Both oxidation and reduction

4. 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

1.12 cm¯¹

0.66 cm¯¹

0.142 cm¯¹

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

Osmotic pressure

Surface tension

Refractive index

Viscosity

6. Density of H₂SO₄ in lead accumulator is

120 g Cm³

1.15 g/Cm³

1.2 g/Cm³

1.25g/Cm³

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

0 to –3

1 to 5

2 to 5

0 to 5.

8. Molarity of water is

55.5

9. What are the ions present in water?

H2 and O

H and OH

H+ and OH-

H2O

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

0.6

0.9

0.3

0.2

11. Stronger the oxidizing agent, greater is the

e.m.f of cell

Reduction potential

Redox potential

Oxidation potential

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

0.2 N

2 N

13. 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

14. 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

3.2 g

2.3 g

12.8 g

6.4 g

15. Electricity in voltaic cell is produced due to

Oxidation

Reduction

B + C

Neutralization

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

An electrolytic cell

A galvanic cell

A voltaic cell

A chemical cell

17. 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

18. 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

Na and Hg

Pt and graphite only

19. Molton NaCl conducts electricity due to the presence of

Free ions

Free electrons

Free molecules

Atoms of Na and Cl.

20. 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

21. Secondary cell is

Electrolytic cell

Daniel cell

Rechargeable

Non rechargeable

22. In a Galvanic cell, the electrons flow from

Anode to cathode through the solution

Cathode to anode through the external circuit

Cathode to anode through the solution

Anode to cathode through the external circuit

23. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/51

5.1

1/5

24. Which has maximum oxidation number

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

Electrolytic cell

Fuel cell

Daniel cell

Galvanic cell

Page 2 of 8

26. If liquids A and B form an ideal solution

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

The enthalpy of mixing is zero

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

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

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

28. Pick out the wrong statement. In electrochemical cell

Electrons are released at anode

Chemical energy is converted into electrical energy

Cathode is regarded as negative electrode

Salt bridge maintains the electrical neutrality of the solution

29. 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

30. Oxidation number of carbon in NaHCO₃ is

-6

31. 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

32. 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

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

80 ml

20 ml

40 ml

10 ml

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

Nitric acid

Boric acid

Phosphorus acid

Sulphuric acid

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

1.5

36. 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

1.08 g

10.8 g

108 g

21.6 g

37. 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

38. Solution with same osmotic pressures are called

Hypertonic

Isotonic

Hypotonic

Normal

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

∆ G = 0, ∆E = 0

∆ G = +ve, ∆ E = 0

∆ G = -ve

∆ G = -ve, ∆ E = 0

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

1.81 cm¯³

1.25 cm¯³

2.15 cm¯³

1.15 cm¯³

41. Specific conductivity of a solution

Depends on mass of electrolyte

Increases with dilution

Decreases with dilution

Remains unchanged with dilution

42. When common salt is dissolved in water

B.P of water remain constant

B.P of water decrease

Any possibility

B.P of water increase

43. Density of H₂SO₄ in lead accumulator is

1.25g/cm3

1.3g/cm3

1.20g/cm3

1.15g/cm3

44. In alkaline battery anode is made up of

Cadmium

MnO₂

AgO₂

45. Electrode potential of Zn is

Depends on the nature of the coupled electrode

Oxidation

Reduction

Oxidation-reduction

46. 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 > C > B

B > C > A

A > B > C

47. Oxidation state of hydrogen in CaH₂ is

-1

-2

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

Anode

Cathode

None of these

Electrode

49. 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

50. Maximum freezing point falls in

Water

Benzene

Naphthalene

Camphor

Page 3 of 8

51. Alkaline battery has a voltage of

3.5V

1.5V

2.5V

4.5V

52. Vant Hoff’s factor of Ca(NO₃)₂ is

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

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

None of these

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

Strong acid and its salt of weak base

A strong acid and its salt of a strong base

Weak acid and its salt of strong base

Weak acid and its salt of weak base

55. 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

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

Na → Na⁺ + e–

Br₂ + 2e – → 2Br –

2Br– → Br₂ + 2e –

Na⁺ + e– → Na

57. In an electrolytic cell current flows

From cathode to anode inside the cell

From anode to cathode in an outer circuit

From cathode to anode in outer circuit

From anode to cathode inside the cell

58. Oxidation in a chemical reaction involves

Both are possible

Increase in oxidation number of all the elements on reactant side

Decrease in oxidation number

Increase in oxidation number

59. The reference electrode is made by using

ZnCl₂

CuSO₄

Hg₂Cl₂

HgCl₂

60. 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

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

40.5

45.1

42.7

39.6

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

F₂O

Na₂O

Cl₂O

Na₂O₂

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

Does not change

Drops to zero

Decrease rapidly

Decreases slowly

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

– 1.17 V

+ 1.17 V

+ 0.35

– 0.35 V

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

1.86 c°

0.186 c°

18.6 c°

Sufficient date not given

66. The art of electroplating was given by

Edison

Brugan

Faraday

Thomas Gradam

67. 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

68. A redox reaction involves

Electron transfer

Ion combination reaction

Proton transfer

A reaction in a solution

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

0.1

0.2

0.01

0.0196

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

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

Not particular

Higher

In middle

Lower

72. In electrolytic cell, electricity in carried out by

Spontaneous reaction

Neutralization

Non-spontaneous reaction

All

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

Very low ionization potential values

Very high positive value of reduction potential

Reduction potentials are negative

Very high negative values reduction potential

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

None of these

Electrons flow cathode to anode within the electrolytic solution

Electrons flow from cathode to anode through the external battery

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

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

2.0

1.0

0.5

1.5

Page 4 of 8

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

Magnetic energy

Sound energy

Heat energy

Electrical energy

77. Pure water does not conduct electricity because it

Is almost unionized

Has low boiling point

Is neutral

Is readily decomposed

78. The Vant Hoff factor (i) accounts for

The degree of decomposition of solution

Degree of solubilization of solute

The extent of dissolution of solute

The extent of dissociation of solute

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

NH₄Cl

CH₃ CooNH₄

Na₂SO₄

NaCl

80. 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

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

Raoult’s law

Arrhenius law

Ostwald’s law

Henry’s law

82. Camphor is often used in molecular mass determination because

It has a very high cryoscopic constant

It is readily available

It is solvent for organic substances

It is volatile

83. Voltaic cell can be recharged by

By removal of solution

By heating it

By replacing external circuit with external source of electricity

By addition of fresh solution

84. Li occupies higher position in the electrochemical series of metals as compared to Cu since

Li is smaller in size as compared to Cu

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

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

Elevation in boiling point

Ionic concentration

Diffusion rate of the solute

Flow of solvent from a concentrated to a dilute solution

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

87. Decrease in oxidation number is called

All of these

Reduction

Redox

Oxidation

88. 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

1.0

2.0

0.5

1.5

89. 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 m mol¯¹

S² m² mol

S m² mol¯¹

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

3.12

7.20

4.10

0.217

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

0.80

0.75

92. The depression of freezing point is directly proportional to

Mole fraction of the solution

Molality of the solution

Molarity of the solution

Molarity of the solvent

93. 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 – 2 α

1 – α

1 + α

94. Azeotropic mixture of HCl and water has

48% HCl

20.2% HCl

36% HCl

22.2% HCl

95. Corrosion is basically a

Electrochemical phenomenon

Interaction

Altered reaction in presence of H₂O

Union between two light metals and a heavy metal

96. 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 M

4.18 M

8.14 M

18.4 M

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

Reduction

Both

Oxidation

98. Standard hydrogen electrode has an arbitrarily fixed potential

0.00 volt

1.00 volt

0.10 volt

None of these

99. Chemical used in salt bridge is

KCI

KOH

KNO3

KBr

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

6 g

40 g

60 g

4 g

Page 5 of 8

101. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.8 M

0.4 M

0.2 M

0.04 M

102. The solubility of a gas in water depends upon

All of these

Pressure of the gas

Temperature

Nature of the gas

103. 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

104. 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)₄Cl]Cl₃

[Pt(NH₃)₄Cl₃]Cl

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

1 M

2 M

1 N

1 f

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

Unsaturated

Ideal

Supersaturated

Saturated

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

33.3

3.33

0.333

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

None of these

Both Na⁺ and CI¯

Cl¯

Na⁺

109. 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

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

1 normal

All

1 molar

1 molal

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

0.0186

0.0521

1.86

0.521

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

One gm. Equivalent weight

Electrochemical equivalent

None of these

One gm. atomic weight

113. Corrosion reactions are

Spontaneous redox reactions

Spontaneous acid–base reactions

Non-spontaneous redox reactions

None of these

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

O₂,H₂

O₂, Na

None of these

O₂, SO₂

115. 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

9 N

3 N

116. 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

4 C

120 C

240 C

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

Melting point

Boiling point

Sublimation point

Inversion point

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

Milligram percent

Gram per million

Parts per million

Microgram percent

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

750 mm of Hg

800 mm of Hg

780 mm of Hg

760 mm of Hg

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

0.27 g

0.54 g

2.16 g

1.08 g

121. Choose the best reducing agent among the following

Br¯¹

Cl¯¹

I¯¹

F¯¹

122. 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

123. 2.5 faradays of electricity is passed through solution of CuSO₄. The number of gram equivalents of copper deposited on the cathode would be

2.5

1.25

1 2

None of these

124. 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

0.0512

0.512

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

Acts as a catalyst

Gains electrons

pH is changed

Loses electrons

Page 6 of 8

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

Reduced

Hydrolyzed

Oxidized

Precipitated

127. Reaction takes place at anode is

Reduction

Ionization

Oxidation

Hydrolysis

128. Strong reducing agents have

None of these

Greater positive value of standard reduction potential

Lesser positive value of standard reduction potential

Greater negative value of standard reduction potential

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

750 torr

Slightly more than 1 atom

2.5 atom

760 mm of Hg

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

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

Chloroform

Molten NaCl

Dilute solution of glucose

Pure distilled water

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

1 g

2 g

20 g

10 g

133. Potential of Zn is called

It has not potential

Reduction

Redox

Oxidation

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

Drops to zero

Increases rapidly

Does not change

Increases gradually

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

HgCl₂

ZnCl₂

CuSO₄

Hg₂Cl₂

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

H₃PO₂

H₃PO₃

H₃PO₄

H₄P₃O₇

137. 0.5 M of H₂SO₄ is diluted from 1 liter to 10 liter, normality of resulting solution is

0.1N

10 N

1 N

11 N

138. The best reducing agent is

I¯

Br¯

F¯

Cl¯

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

9.09%

11.2%

13.1%

14.25%

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

MgCl₂

KCl

NaCl

BaCl₂

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

Distillation

None of these

Fractional distillation

Vacuum distillation

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

NaOH

NH₄OH

KOH

Ca(OH)₂

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

None

144. Cathode provides electrons to

Neutral atom

Does not provide any electron

+Ve ion

-Ve ion

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

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

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

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

None of these

Electroplating

Electrorefining

Both A and B

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

0.01

0.2

0.1

0.0196

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

0.05

2.05

0.5

0.25

149. 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?

15.9 gm

63.5 gm

12.7 gm

31.8 gm

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

5 g

2 g

1 g

4 g

Page 7 of 8

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

Manufacture of bleach

Rust removal

Making leather

Electroplating

152. 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

153. Mole fraction of pure water is

None of these

Exactly equal to one

Slightly greater than one

Slightly less than one

154. 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

None

Greater

Lesser

155. Metals usually conduct electricity because

Metals are decomposed by current

In metals the ions are free to more

They are mobile electrons in the metallic structure

Metals have high resistance

156. 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

157. 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

11.2 cm³

56 cm³

550 cm³

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

Graphite

0.1 N HCl

0.1 N NaCl

Glass

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

5.58g NaCl/100m

10.0g NaCl/100ml

58.5g NaCl/100ml

20g NaCl/100ml

160. In a Galvanic cell

Chemical energy is converted into electricity

Electrical energy is converted into heat

Chemical energy is converted into heat

Electrical energy is converted into chemical energy

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

Standard electrode potential

Electroplating

Ionization potential

Electric change

162. 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

163. The conductivity of strong electrolyte

Decreases on dilution

Depends on density of electrolyte itself.

Increases on dilution slightly

Does not change on dilution

164. Which of the following statements is FALSE?

Reduction occurs at cathode

All electrochemical reactions involve the transfer of electrons

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

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

Standard reduction potential

Cell voltage

Standard oxidation potential

Ionization potential

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

0.222 V

0.399 V

0.281 V

0.176 V

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

1 coulomb

1 ampere

1 faraday

2 ampere

168. Reduction always occurs

At cathode

None of these

At anode

Both A and B

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

193000

48250

96500

10000

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

Photo electrolysis

Electrolysis

Galvanization

Cathodic protection

171. In alkaline battery the anode is made up of

MnO2

Cadmium

AgO2

172. During a redox reaction, an oxidizing agent

Is hydrolysed

Gains electrons

Is oxidized

Loses electrons

173. 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

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

12.1 atm

24.6 atm

1.21 atm

2.46 atm

175. Salt bridge transfers

Current

Solvent particles

Anions

Electrons

Page 8 of 8

176. Salt bridge transfers

Current

Ions

Anion

Electrons

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

Generate heat

Remove adsorbed oxygen from electrode surfaces

Create potential difference between two electrodes

Produce high purity water

178. The unit of specific conductivity is

Ohm cm¯²

Ohm¯¹ cm

Ohm¯¹ cm¯¹

Ohm cm¯¹

179. 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

180. The degree of dissociation of weak electrolyte increases as

Dilution increases

None

Pressure increases

Dilution decreases

181. Temperature for standard electrode potential is

273 K

310 K

25 C°

300 K

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

Pb²⁺

I₂

Ag⁺

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

68 torr

140 torr

20 torr

72 torr

184. Best way to prevent rusting iron is by

None of these

Putting it in saline water

Making iron cathode

Both of these

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

Electrical energy

Chemical energy

Heat energy

None of these

186. Units of molarity are

None of these

Gm/lit

Mol/lit

Kg/lit

187. Half cells are interconnected through

No connection exists

Electric circuit

Salt Bridge

Wire

188. Which of the following is a strong electrolyte?

NH₄OH

Ca(NO₃)₂

HCN

CH₃COOH

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

Chloride

Hydrogen

Oxygen

Chlorine

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

8 N

2 N

6 N

4 N

191. The equivalent conductivity of 0.1 M week acid is 100 times less than that at infinite dilution. The degree of dissociation is

100

0.01

0.001

192. An electrolyte

Possesses ions even in solid state

Gives ions only when dissolved in water

Forms complex ions in solution

Gives ions only when electricity is passed

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