1.
The standard electrode potential of Zn²⁺/Zn is –0.76 V and of Cu²⁺/Cu is +0.34 V. The EMF of the cell Zn | Zn²⁺ || Cu²⁺ | Cu is:
a) 1.10 V
b) –1.10 V
c) 0.42 V
d) –0.42 V
2.
Which of the following is used as a primary cell?
a) Lead storage battery
b) Nickel–cadmium cell
c) Dry cell
d) Fuel cell
3.
Kohlrausch’s law is related to:
a) Solubility product
b) Conductivity of electrolytes at infinite dilution
c) Cell potential
d) Gibbs free energy
4.
Which electrode is used in a hydrogen electrode?
a) Platinum black
b) Copper
c) Silver
d) Graphite
5.
In the Daniel cell, electrons flow from:
a) Copper to zinc
b) Zinc to copper
c) Electrolyte to copper
d) Electrolyte to zinc
6.
The relationship between ΔG° and E°cell is:
a) ΔG° = –nFE°cell
b) ΔG° = nFE°cell
c) ΔG° = –E°cell/F
d) ΔG° = –RT ln E°cell
7.
The conductivity of a solution decreases with:
a) Increase in temperature
b) Decrease in temperature
c) Increase in concentration
d) Increase in dilution
8.
At infinite dilution, molar conductivity of weak electrolyte:
a) Becomes zero
b) Becomes infinite
c) Remains constant
d) Cannot be determined directly
9.
The unit of molar conductivity (Λm) in SI is:
a) ohm⁻¹ cm⁻¹
b) ohm⁻¹ cm² mol⁻¹
c) S m² mol⁻¹
d) S cm mol⁻¹
10.
Electrochemical equivalent is expressed in:
a) g C⁻¹
b) C mol⁻¹
c) g mol⁻¹
d) g A⁻¹
11.
Which of the following cells is a fuel cell?
a) Daniel cell
b) H₂–O₂ cell
c) Dry cell
d) Lead storage battery
12.
For the reaction:
2Ag++Cu→2Ag+Cu2+2Ag^+ + Cu \rightarrow 2Ag + Cu^{2+}2Ag++Cu→2Ag+Cu2+
If E°(Ag⁺/Ag) = +0.80 V and E°(Cu²⁺/Cu) = +0.34 V, E°cell = ?
a) 0.46 V
b) 0.80 V
c) 1.14 V
d) 0.34 V
13.
Which of the following is not a secondary cell?
a) Lead–acid battery
b) Nickel–cadmium cell
c) Mercury cell
d) None of these
14.
Which of the following quantities remains constant during electrolysis?
a) Number of electrons
b) Charge of electrons
c) Mass of substance deposited
d) Volume of electrolyte
15.
Faraday’s first law of electrolysis states:
a) Mass deposited ∝ time
b) Mass deposited ∝ charge passed
c) Mass deposited ∝ atomic mass
d) Mass deposited ∝ current density
16.
In a concentration cell, EMF is:
a) Zero
b) Positive
c) Negative
d) Depends on concentration difference
17.
In the electrolysis of molten NaCl:
a) Na is liberated at cathode
b) Cl₂ is liberated at cathode
c) H₂ is liberated at anode
d) O₂ is liberated at cathode
18.
The slope of molar conductivity (Λm) vs √c graph for weak electrolytes gives:
a) Λm°
b) Limiting molar conductivity
c) Degree of dissociation
d) Ionic conductivity
19.
The resistance of a conductivity cell filled with 0.1 M KCl solution is 100 Ω. The cell constant is 1.29 cm⁻¹. What is the conductivity (κ)?
a) 0.0129 S cm⁻¹
b) 0.129 S cm⁻¹
c) 0.00129 S cm⁻¹
d) 1.29 S cm⁻¹
20.
In a galvanic cell, salt bridge is used to:
a) Maintain electrical neutrality
b) Increase EMF
c) Provide electrons
d) Prevent leakage of solution
21.
Which of the following has the highest molar conductivity at infinite dilution?
a) NaCl
b) KCl
c) LiCl
d) CsCl
22.
The quantity of electricity required to deposit 1 mole of silver (Ag⁺ + e⁻ → Ag) is:
a) 96500 C
b) 48250 C
c) 193000 C
d) 965 C
23.
The decrease in molar conductivity of a strong electrolyte with increase in concentration is due to:
a) Decrease in number of ions
b) Increase in ionic mobility
c) Increase in inter-ionic attraction
d) Increase in solvation
24.
The emf of a galvanic cell is related to equilibrium constant (K) by:
a) E°cell = RT/nF ln K
b) E°cell = –RT/nF ln K
c) nFE°cell = RT ln K
d) ΔG° = –RT ln K
25.
Which of the following metals is extracted by electrolysis of its molten salt?
a) Copper
b) Silver
c) Sodium
d) Iron
Answer Key
- a
- c
- b
- a
- b
- a
- c
- d
- c
- a
- b
- a
- c
- b
- b
- d
- a
- c
- a
- a
- d
- a
- c
- c
- c
Sarvan sir- Chemistry For All 