Question 1.
If 96500 coulomb electricity is passed through CuSO₄ solution, it will liberate
(a) 63.5 gm of Cu
(b) 31.76 gm of Cu
(c) 96500 gm of Cu
(d) 100 gm of Cu

Answer

Answer: (b) 31.76 gm of Cu

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Question 2.
Fused NaCl on electrolysis gives ………….. on cathode.
(a) Chlroine
(b) Sodium
(c) Sodium amalgam
(d) Hydrogen

Answer

Answer: (b) Sodium

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Question 3.
The standard electrode potentials for the half cell reactions are:
Zn → Zn^2-– 2e^– E° = 0.76 V
Fe → Fe^2- + 2^– E° = -0.41 V
The emf of the cell reaction
Fe^2- + Zn → Zn^2- + Fe is
(a) -0.35 V
(b) +0.35 V
(c) -1.17 V
(d) +1.17 V

Answer

Answer: (b) +0.35 V

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Question 4.
Which of the following is a secondary cell?
(a) Leclanche cell
(b) Lead storage battery
(c) Concentration cell
(d) All of these

Answer

Answer: (b) Lead storage battery

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Question 5.
For a certain redox reaction, E° is positive. This means that
(a) ΔG° is positive, K is greater than 1
(b) ΔG° is positive, K is less than 1
(c) ΔG° is negative, K is greater than 1
(d) ΔG° is negative, K is less than 1

Answer

Answer: (c) ΔG° is negative, K is greater than 1

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Question 6.
Cell reaction is spontaneous, when
(a) E\(_{red}^{0}\) is negative
(b) ΔG° is negative
(c) E\(_{oxid}^{0}\) is Positive
(d) ΔG° is positive

Answer

Answer: (b) ΔG° is negative

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Question 7.
Equilibrium constant K is related to E\(_{cell}^{0}\) and not E\(_{cell}\) because
(a) E\(_{cell}^{0}\) is easier to measure than E\(_{cell}\)
(b) E\(_{cell}\) becomes zero at equilibrium point but E\(_{cell}^{0}\) remains constant under all conditions
(c) at a given temperature, E\(_{cell}\) changes hence value of K can’t be measured
(d) any of the terms E\(_{cell}\) or E\(_{cell}^{0}\) can be used

Answer

Answer: (b) E\(_{cell}\) becomes zero at equilibrium point but E\(_{cell}^{0}\) remains constant under all conditions

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Question 8.
Molar conductivity of 0.15 M solution of KCl at 298 K, if its conductivity of 0.0152 S cm^-1 w ill be
(a) 124 Ω^-1 cm² mol^-1
(b) 204 Ω^-1 cm² mol^-1
(c) 101 Ω^-1 cm² mol^-1
(d) 300 Ω^-1 cm² mol^-1

Answer

Answer: (c) 101 Ω^-1 cm² mol^-1

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Question 9.
Electrical conductance through metals is called metallic or electronic conductance and is due to the movement of electrons. The electronic conductance depends on
(a) the nature and structure of the metal
(b) the number of valence electrons per atom
(c) change in temperature
(d) all of these

Answer

Answer: (d) all of these

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Question 10.
The specific conductivity of N/10 KCl solution at 20°C is 0.0212 ohm^-1 cm^-1 and the resistance of the cell containing this solution at 20°C is 55 ohm. The cell constant is
(a) 3.324 cm^-1
(b) 1.166 cm^-1
(c) 2.372 cm^-1
(d) 3.682 cm^-1

Answer

Answer: (b) 1.166 cm^-1

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Question 11.
Faraday’s law of electrolysis is related to
(a) Atomic number of cation
(b) Speed of cation
(c) Speed of anion
(d) Equivalent weight of electrolyte

Answer

Answer: (d) Equivalent weight of electrolyte

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Question 12.
The molar conductivity is maximum for the solution of concentration
(a) 0.004 M
(b) 0.002 M
(c) 0.005 M
(d) 0.001 M

Answer

Answer: (d) 0.001 M

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Question 13.
Units of the properties measured are given below. Which of the properties has been not matched correctly?
(a) Molar conductance = Sm² mol^-1
(b) Cell constant = m^-1
(c) Specific conductance of = S m²
(d) Equivalence conductance = S m² (g eq)^-1

Answer

Answer: (c) Specific conductance of = S m²

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Question 14.
How long would it take to deposit 50 g of Al from an electrolytic cell containing Al₂O₃ using a current of 105 ampere?
(a) 1.54 h
(b) 1.42 h
(c) 1.32 h
(d) 2.15 h

Answer

Answer: (b) 1.42 h

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Question 15.
The charge required for reducing 1 mole of MnO\(_{4}^{-}\) to Mn^2- is
(a) 1.93 × 10⁵ C
(b) 2.895 × 10⁵ C
(c) 4.28 × 10⁵ C
(d) 4.825 × 10⁵ C

Answer

Answer: (d) 4.825 × 10⁵ C

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Question 16.
How much electricity in in terms of Faraday is required to produce 100 g of Ca from molten CaCl₂?
(a) 1F
(b) 2F
(c) 3F
(d) 5F

Answer

Answer: (d) 5F

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Question 17.
If a current of 1.5 ampere flows through a metallic wire for 3 hours, then how many electrons would flow through the wire?
(a) 2.25 × 10²² electrons
(b) 1.13 × 10²³ electrons
(c) 1.01 × 10²³ electrons
(d) 4.5 × 10²³ electrons

Answer

Answer: (c) 1.01 × 10²³ electrons

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Question 18.
How many coulombs of electricity is required to reduce 1 mole of Cr₂O\(_{7}^{2-}\) in acidic medium?
(a) 4 × 96500 C
(b) 6 × 96500 C
(c) 2 × 96500 C
(d) 1 × 96500 C

Answer

Answer: (b) 6 × 96500 C

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Question 19.
A current of 1.40 ampere is passed through 500 mL of 0.180 M solution of zinc sulphate for 200 seconds. What will be the molarity of Zn²⁺ions after deposition of zinc?
(a) 0.154 M
(b) 0.177 M
(c) 2 M
(d) 0.180 M

Answer

Answer: (b) 0.177 M

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Question 20.
How much time is required to deposit 1 × 10^-3 cm thick layer of silver (density of 1.05 g cm^-3) on a surface of area 100 cm² by passing a current of 5 A through AgNO₃ solution?
(a) 125 s
(b) 115 s
(c) 18.7 s
(d) 27.25 s

Answer

Answer: (c) 18.7 s

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