Chemistry MCQs for Class 12 with Answers Chapter 3 Electrochemistry 2022

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Chemistry MCQs for Class 12 with Answers Chapter 3 Electrochemistry 2022
Chemistry MCQs for Class 12 with Answers Chapter 3 Electrochemistry 2022

Free PDF Download of CBSE Chemistry Multiple Choice Questions for Class 12 with Answers Chapter 3 Electrochemistry. Chemistry MCQs for Class 12 Chapter Wise with Answers PDF Download was Prepared Based on Latest Exam Pattern. Students can solve NCERT Class 12 Chemistry Electrochemistry MCQs Pdf with Answers to know their preparation level.

MCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers :-

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Question 1. Which of the statements about solutions of electrolytes is not correct ?

(A) Conductivity of solution depends upon size of ions.
(B) Conductivity depends upon viscosity of solution.
(C) Conductivity does not depend upon solvation of ions present in solution.
(D) Conductivity of solution increases with temperature.

Answer: Option

Question 2. When 0.1 mol CoCl3(N3)5 is treated with excess of AgNO3, 0.2 mol of AgCl are obtained. The conductivity of solution will correspond to:

(A) 1: 3 electrolyte
(B) 1: 2 electrolyte
(C) 1: 1 electrolyte
(D) 3: 1 electrolyte A

Answer: Option

Question 3. The cell constant of a conductivity cell

(A) Changes with change of electrolyte.
(B) Changes with change of concentration of electrolyte.
(C) Changes with temperature of electrolyte.
(D) Remains constant for a cell.

Answer: Option

Question 4. Which of the following statement is correct?

(A)ECell and Gibb’s energy of cell reaction both extensive properties.
(B) ECell and Gibb’s energy of cell reaction both intensive properties.
(C) ECell is an intensive property while Gibb’s energy of cell reaction is an extensive property.
(D) ECell is an extensive property while Gibb’s energy of cell is an intensive property

Answer: Option

Question 5. An electrochemical cell behaves like an electrolytic cell when:

(A) Ecell = Eexternal
(B) Ecell = 0
(C) Eexternal > Ecell
(D) Eexternal < Ecell

Answer: Option

Question 6. In an electrochemical process, a salt bridge is used:

(A) as a reducing agent
(B) as an oxidizing agent
(C) to complete the circuit so that current can flow
(D) None

Answer: Option

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

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: (c) 101 Ω-1 cm² mol-1

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: (d) all of these

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: (b) 1.166 cm-1

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: (d) Equivalent weight of electrolyte

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: (d) 0.001 M

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: (c) Specific conductance of = S m²

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: (b) 1.42 h

Question 15.
The charge required for reducing 1 mole of MnO\(_{4}^{-}\) to Mn2- is

(a) 1.93 × 105 C
(b) 2.895 × 105 C
(c) 4.28 × 105 C
(d) 4.825 × 105 C


Answer: (d) 4.825 × 105 C

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: (d) 5F

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: (c) 1.01 × 1023 electrons

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: (b) 6 × 96500 C

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: (b) 0.177 M

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: (c) 18.7 s

Question 21.
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: (b) 31.76 gm of Cu

Question 22.
Fused NaCl on electrolysis gives ………….. on cathode.

(a) Chlroine
(b) Sodium
(c) Sodium amalgam
(d) Hydrogen


Answer: (b) Sodium

Question 23.
The standard electrode potentials for the half cell reactions are:

Zn → Zn2-– 2e E° = 0.76 V
Fe → Fe2- + 2 E° = -0.41 V
The emf of the cell reaction
Fe2- + Zn → Zn2- + Fe is
(a) -0.35 V
(b) +0.35 V
(c) -1.17 V
(d) +1.17 V


Answer: (b) +0.35 V

Question 24.
Which of the following is a secondary cell?

(a) Leclanche cell
(b) Lead storage battery
(c) Concentration cell
(d) All of these


Answer: (b) Lead storage battery

Question 25.
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: (c) ΔG° is negative, K is greater than 1

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