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

1.25

1 2

2.5

None of these

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

11.2%

14.25%

13.1%

9.09%

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

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

None of these

Electrons flow from cathode to anode through the external battery

Electrons flow cathode to anode within the electrolytic solution

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

Milligram percent

Microgram percent

Gram per million

Parts per million

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

780 mm of Hg

760 mm of Hg

750 mm of Hg

800 mm of Hg

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

Higher

In middle

Lower

Not particular

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

Conduction

Electrolysis

Induction

Electroplating

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

4 N

6 N

8 N

2 N

9. Best way to prevent rusting iron is by

Putting it in saline water

Making iron cathode

Both of these

None of these

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

None of these

Vacuum distillation

Fractional distillation

Distillation

11. 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

12. Reaction takes place at anode is

Reduction

Oxidation

Hydrolysis

Ionization

13. Half cells are interconnected through

No connection exists

Electric circuit

Wire

Salt Bridge

14. 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

Reduction potentials are negative

Very high positive value of reduction potential

Very high negative values reduction potential

15. 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

31.8 gm

12.7 gm

63.5 gm

16. The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25°C. The equilibrium constant of the reaction would be

2.0 x 10¹¹

1.0 x 10¹⁰

1.0 x 10²

4.0 x 10¹²

17. In a chemical reaction, oxidation process involves

Decrease in oxidation number of element

Increase in oxidation number of the elements in reactants

Increase in oxidation number of element

Oxidation number neither increases nor decreases

18. Decrease in oxidation number is called

Oxidation

Redox

All of these

Reduction

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

I₂

Ag⁺

Pb²⁺

20. A redox reaction involves

A reaction in a solution

Ion combination reaction

Electron transfer

Proton transfer

21. Pick out the wrong statement. In electrochemical cell

Chemical energy is converted into electrical energy

Electrons are released at anode

Salt bridge maintains the electrical neutrality of the solution

Cathode is regarded as negative electrode

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

+ 1.17 V

– 0.35 V

+ 0.35

– 1.17 V

23. Density of H₂SO₄ in lead accumulator is

120 g Cm³

1.25g/Cm³

1.2 g/Cm³

1.15 g/Cm³

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

7.20

4.10

0.217

3.12

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

H₄P₃O₇

H₃PO₃

H₃PO₂

H₃PO₄

Page 2 of 8

26. An electrolyte

Possesses ions even in solid state

Forms complex ions in solution

Gives ions only when dissolved in water

Gives ions only when electricity is passed

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

Boric acid

Phosphorus acid

Sulphuric acid

Nitric acid

28. 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

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

Refractive index

Viscosity

Osmotic pressure

Surface tension

30. Secondary cell is

Daniel cell

Electrolytic cell

Rechargeable

Non rechargeable

31. Corrosion reactions are

None of these

Spontaneous redox reactions

Spontaneous acid–base reactions

Non-spontaneous redox reactions

32. If liquids A and B form an ideal solution

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

The free energy of mixing is zero

33. Specific conductivity of a solution

Decreases with dilution

Increases with dilution

Remains unchanged with dilution

Depends on mass of electrolyte

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

1 faraday

1 coulomb

2 ampere

1 ampere

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

Unsaturated

Saturated

Supersaturated

Ideal

36. Density of H₂SO₄ in lead accumulator is

1.20g/cm3

1.3g/cm3

1.15g/cm3

1.25g/cm3

37. 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

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

Hg is more inert than Pt

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

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

760 mm of Hg

2.5 atom

750 torr

Slightly more than 1 atom

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

Raoult’s law

Ostwald’s dilution law

Henry’s law

Distribution law

40. 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

41. 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

B > C > A

C > B > A

A > C > B

A > B > C

42. 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

12.8 g

2.3 g

6.4 g

43. 96500 C electricity is passed through CuSO₄. The amount of copper precipitated is

0.5 mole

2.00 mole

0.25 mole

1.0 mole

44. 18g of glucose is dissolved in 90g of water. The relative lowering of vapour pressure is equal to

1/5

5.1

1/51

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

Magnetic energy

Sound energy

Electrical energy

Heat energy

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

Both

Oxidation

Reduction

47. 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

2.0

1.0

48. 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

0.15 M

0.05 M

0.2 M

49. 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

20 torr

140 torr

72 torr

50. Molton NaCl conducts electricity due to the presence of

Free molecules

Free ions

Atoms of Na and Cl.

Free electrons

Page 3 of 8

51. 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

0.35

0.25

0.40

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

6 g

40 g

60 g

4 g

53. 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

54. Choose the best reducing agent among the following

Br¯¹

F¯¹

I¯¹

Cl¯¹

55. Oxidation state of hydrogen in CaH₂ is

-1

-2

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

0.3

0.2

0.6

0.9

57. Azeotropic mixture of HCl and water has

22.2% HCl

20.2% HCl

36% HCl

48% HCl

58. Units of molarity are

Kg/lit

None of these

Mol/lit

Gm/lit

59. The reference electrode is made by using

Hg₂Cl₂

CuSO₄

HgCl₂

ZnCl₂

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

1.15 cm¯³

1.25 cm¯³

1.81 cm¯³

2.15 cm¯³

61. The degree of dissociation of weak electrolyte increases as

Dilution increases

None

Pressure increases

Dilution decreases

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

2 to 5

1 to 5

0 to –3

0 to 5.

63. 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

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

0.1

0.0196

0.2

0.01

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

0.1 M Sucrose

0.1 M Glucose

0.1 M BaCl₂

0.1 M NaCl

66. The art of electroplating was given by

Edison

Thomas Gradam

Faraday

Brugan

67. Electricity in voltaic cell is produced due to

Reduction

Neutralization

Oxidation

B + C

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

Na₂O

Cl₂O

Na₂O₂

F₂O

69. The conductivity of strong electrolyte

Does not change on dilution

Decreases on dilution

Depends on density of electrolyte itself.

Increases on dilution slightly

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

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

The standard reduction potential of Cu²+/Cu is lower than that of Li⁺/Li

The standard reduction potential of Li⁺/Li is lower than that of Cu²+/Cu

Li is smaller in size as compared to Cu

71. Mole fraction of pure water is

Slightly greater than one

Slightly less than one

None of these

Exactly equal to one

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

Electrolytic cell

Galvanic cell

Fuel cell

Daniel cell

73. Solution with same osmotic pressures are called

Isotonic

Hypertonic

Hypotonic

Normal

74. Temperature for standard electrode potential is

273 K

300 K

25 C°

310 K

75. Cathode provides electrons to

Neutral atom

Does not provide any electron

+Ve ion

-Ve ion

Page 4 of 8

76. Maximum freezing point falls in

Camphor

Benzene

Naphthalene

Water

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

ZnCl₂

CuSO₄

Hg₂Cl₂

HgCl₂

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

0.01

0.1

0.2

0.0196

79. 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

20 g

10 g

2 g

80. 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

81. Chemical used in salt bridge is

KCI

KBr

KNO3

KOH

82. Reduction always occurs

Both A and B

At cathode

At anode

None of these

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

84. The solubility of a gas in water depends upon

All of these

Pressure of the gas

Nature of the gas

Temperature

85. Electrode potential of Zn is

Depends on the nature of the coupled electrode

Oxidation

Reduction

Oxidation-reduction

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

NH₄OH

KOH

Ca(OH)₂

NaOH

87. 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

21.6 g

1.08 g

10.8 g

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

Decrease rapidly

Does not change

Drops to zero

Decreases slowly

89. 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

90. 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

1.1 molal

0.5 molal

1 molal

91. Salt bridge transfers

Anions

Electrons

Solvent particles

Current

92. Camphor is often used in molecular mass determination because

It is solvent for organic substances

It is readily available

It has a very high cryoscopic constant

It is volatile

93. 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

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

0.918 cm¯¹

0.142 cm¯¹

1.12 cm¯¹

0.66 cm¯¹

95. In alkaline battery the anode is made up of

Cadmium

AgO2

MnO2

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

193000

96500

10000

48250

97. 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)

0.333

0.0033

33.3

3.33

98. Vant Hoff’s factor of Ca(NO₃)₂ is

99. In alkaline battery anode is made up of

AgO₂

MnO₂

Cadmium

100. Voltaic cell can be recharged by

By heating it

By replacing external circuit with external source of electricity

By removal of solution

By addition of fresh solution

Page 5 of 8

101. 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)₄Cl₂]Cl₂

[Pt(NH₃)₄Cl]Cl₃

[Pt(NH₃)₄Cl₃]Cl

[Pt(NH₃)₄Cl₄]

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

Na, Pt and graphite

Na and Hg

Pt and graphite only

Na and S only

103. 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

104. Colligative properties are the properties of

Both a and b

Dilute solution which behave as nearly ideal solution

Concentration solutions behave as nearly non – ideal solutions

Neither a nor b

105. Alkaline battery has a voltage of

1.5V

3.5V

4.5V

2.5V

106. Strong reducing agents have

Lesser positive value of standard reduction potential

Greater positive value of standard reduction potential

Greater negative value of standard reduction potential

None of these

107. 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

108. The best reducing agent is

F¯

I¯

Cl¯

Br¯

109. 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

110. 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

111. 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

112. 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

113. 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

39.6

40.5

114. 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

115. 96500 C of electricity liberates from CuSO₄ solution

100 g of Cu

31.75 g of Cu

96500 g of CU

63.5 g of Cu

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

Gains electrons

pH is changed

Acts as a catalyst

Loses electrons

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

1 g

4 g

5 g

2 g

118. Stronger the oxidizing agent, greater is the

Redox potential

Reduction potential

Oxidation potential

e.m.f of cell

119. Oxidation number of carbon in NaHCO₃ is

-6

120. 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

0.281 V

0.176 V

0.222 V

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

Gold has lower reduction potential then iron

Gold is denser

Iron rusts

Gold has higher reduction potential then iron

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

0.25

0.05

2.05

0.5

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

Oxidation

Reduction

Neither oxidation and reduction

Both oxidation and reduction

124. When common salt is dissolved in water

B.P of water increase

B.P of water remain constant

Any possibility

B.P of water decrease

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

NH₄Cl

Na₂SO₄

NaCl

CH₃ CooNH₄

Page 6 of 8

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

Making leather

Rust removal

Manufacture of bleach

Electroplating

127. 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

128. During a redox reaction, an oxidizing agent

Is oxidized

Is hydrolysed

Gains electrons

Loses electrons

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

1.5

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

Cl¯

Na⁺

Both Na⁺ and CI¯

None of these

131. 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

132. Pure water does not conduct electricity because it

Is neutral

Is almost unionized

Is readily decomposed

Has low boiling point

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

None of these

One gm. Equivalent weight

Electrochemical equivalent

One gm. atomic weight

134. 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

1.5

0.5

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

0.512

0.0512

0.186

0.80

136. The depression of freezing point is directly proportional to

Molality of the solution

Molarity of the solution

Mole fraction of the solution

Molarity of the solvent

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

Pure distilled water

Dilute solution of glucose

Chloroform

Molten NaCl

138. 8 g of NaOh is dissolved in 500 cm³ of solution, its molarity is:

0.4 M

0.2 M

0.8 M

0.04 M

139. 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 10³

1.06 x 10²

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

Galvanization

Electrolysis

Photo electrolysis

Cathodic protection

141. Salt bridge transfers

Anion

Electrons

Ions

Current

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

Standard oxidation potential

Ionization potential

Cell voltage

Standard reduction potential

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

A voltaic cell

A chemical cell

A galvanic cell

An electrolytic cell

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

145. What are the ions present in water?

H+ and OH-

H2O

H2 and O

H and OH

146. Which has maximum oxidation number

147. 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

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

0.0521

1.86

0.521

0.0186

149. 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

11.2 cm³

550 cm³

5.6 cm³

150. 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:

224 cm³

22400 cm³

112 cm³

1.008 g

Page 7 of 8

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

∆ G = 0, ∆E = 0

∆ G = -ve, ∆ E = 0

∆ G = -ve

∆ G = +ve, ∆ E = 0

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

Chloride

Chlorine

Oxygen

Hydrogen

153. In electrolytic cell, electricity in carried out by

Neutralization

Non-spontaneous reaction

All

Spontaneous reaction

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

MgCl₂

BaCl₂

KCl

NaCl

155. Corrosion is basically a

Interaction

Electrochemical phenomenon

Altered reaction in presence of H₂O

Union between two light metals and a heavy metal

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

Cathode

Anode

None of these

Electrode

157. 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

240 C

120 C

4 C

20 C

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

None

159. Which of the following statements is FALSE?

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

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

160. Potential of Zn is called

Redox

Oxidation

It has not potential

Reduction

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

12.1 atm

1.21 atm

2.46 atm

24.6 atm

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

Hydrolyzed

Reduced

Oxidized

Precipitated

163. In a Galvanic cell

Chemical energy is converted into heat

Electrical energy is converted into heat

Electrical energy is converted into chemical energy

Chemical energy is converted into electricity

164. In an electrolytic cell current flows

From cathode to anode in outer circuit

From cathode to anode inside the cell

From anode to cathode inside the cell

From anode to cathode in an outer circuit

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

0.1 N NaCl

Graphite

Glass

0.1 N HCl

166. 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

167. Oxidation in a chemical reaction involves

Decrease in oxidation number

Increase in oxidation number

Both are possible

Increase in oxidation number of all the elements on reactant side

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

169. At room temperature, the mole fraction of a solution in 0.25 and the vapour pressure of the solvent is 0.80 atm. Then the lowering of vapour pressure is

0.60

0.20

0.80

0.75

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

5.58g NaCl/100m

58.5g NaCl/100ml

20g NaCl/100ml

10.0g NaCl/100ml

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

5.51

6.1

1.32

5.65

172. 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

173. 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

Greater

Lesser

None

174. 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

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

Increases gradually

Drops to zero

Does not change

Increases rapidly

Page 8 of 8

176. The unit of specific conductivity is

Ohm cm¯¹

Ohm cm¯²

Ohm¯¹ cm¯¹

Ohm¯¹ cm

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

2Br– → Br₂ + 2e –

Na⁺ + e– → Na

Na → Na⁺ + e–

Br₂ + 2e – → 2Br –

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

Sublimation point

Boiling point

Melting point

Inversion point

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

1 M

1 N

1 f

2 M

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

All

1 molar

1 normal

1 molal

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

Weak acid and its salt of weak base

Weak acid and its salt of strong base

Strong acid and its salt of weak base

A strong acid and its salt of a strong base

182. Standard hydrogen electrode has an arbitrarily fixed potential

0.00 volt

0.10 volt

1.00 volt

None of these

183. Metals usually conduct electricity because

Metals have high resistance

In metals the ions are free to more

Metals are decomposed by current

They are mobile electrons in the metallic structure

184. Which of the following is a strong electrolyte?

NH₄OH

Ca(NO₃)₂

CH₃COOH

HCN

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

Electrorefining

Both A and B

None of these

Electroplating

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

Equal to that of water

More than that of H₂O

Equal to that of ethanol

Less than that of water

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

510 sec

12157.48 sec

102 sec

642 sec

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

Galvanic cell

Fuel cell

Dry cell

Electrolytic cell

189. 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

190. Molarity of water is

55.5

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

Chemical energy

Heat energy

Electrical energy

None of these

192. 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°

0.186 c°

1.86 c°

Sufficient date not given

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Malik TahirLast Updated: May 24, 2025

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Chemistry Electrochemistry MCQS Online Test

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