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Electrochemistry JEE

The Quiz is a JEE mains Level quiz containing 25 questions.

In 25 questions 15 questions are single choice, 6 questions are Assertion reasons type, 04 questions are Match the following type,

The time allotted for the quiz is 60 minutes.

The number of attempts remaining is 3

1 / 25

1. When the sample of copper with zinc impurity is to be purified by electrolysis, the appropriate electrodes are:

a) Cathode → Impure sample; Anode → Pure copper

b) Cathode → Impure zinc; Anode → Impure sample

c) Cathode → Pure copper; Anode → Impure sample

d) Cathode → Pure zinc; Anode → Pure copper

2 / 25

2. Consider the following graph.

electro15

Here the limiting molar conductivity is:

a) 87.46

b) 148.6

c) 150

d) 147

3 / 25

3. Resistance of 0.2 M solution of an electrolyte is 50Ω. The specific conductance of the solution is 1.3 S m ^-1. If resistance of the 0.4 M solution of the same electrolyte is 260 Ω, its molar conductivity is :

a) 625 x 10^-4 S m² mol^-1

b) 6250 S m² mol^-1

c) 62.5 S m² mol^-1

d) 6.25 x 10^-4 S m² mol^-1

4 / 25

4. Statement I: Impure copper is converted into pure copper by electrolysis.
Statement II: Copper is dissolved at cathode and deposited at anode.

a) Statement I is true, Statement II is false.

b) Statement I is false, Statement II is true.

c) Statement I is true, Statement II is true; Statement II is NOT a correct explanation for statement-I.

d) Statement I is true, Statement II is true; Statement II is the correct explanation for Statement I.

5 / 25

5. Select the correct statement for the weak electrolyte:

a) The change in Λ_m with dilution is due to decrease in the degree of dissociation and number of ions in the solution that contain electrolyte.

b) Λ_m increases steeply on dilution near high concentration.

c) They have higher degree of dissociation at higher concentration.

d) At infinite dilution, electrolyte dissociate completely but at such low concentration the conductivity of solution is low and cannot be measured accurately.

6 / 25

6. Statement I: Electrical conductance through metals is called electronic conductance.
Statement II: This is due to movement of electrons.

a) Statement I is true, Statement II is false.

b) Statement I is true, Statement II is true; Statement II is NOT a correct explanation for statement-I.

c) Statement I is true, Statement II is true; Statement II is the correct explanation for Statement I.

d) Statement I is false, Statement II is true.

7 / 25

7. As a lead storage battery is charged:

a) The concentration of sulphuric acid decreases.

b) Sulphuric acid is regenerated

c) Lead electrode becomes coated with lead sulphate

d) Lead dioxide dissolves

8 / 25

8. Match the terms given in Column I with the units given in Column II.

electro50

a) A →3; B → 4; C → 1; D → 2

b) A →4; B → 3; C → 2; D → 1

c) A →3; B → 4; C → 2; D → 1

d) A →4; B → 3; C → 1; D → 2

9 / 25

9. Match the following Column I (expressions) with Column II and choose the correct option from the codes given below.

Electro45

a) A →4; B → 1; C → 3; D → 2

b) A →4; B → 3; C → 1; D → 2

c) A →3; B → 2; C → 4; D → 1

d) A →3; B → 4; C → 2; D → 1

10 / 25

10. The graph of molar conductivity versus √C is plotted.

electro14

Which type of electrolyte are used in A and B ?

a) A→ Weak electrolyte; B→ Weak electrolyte

b) A→ Weak electrolyte; B→ Strong electrolyte

c) A→ Strong electrolyte; B→ Weak electrolyte

d) A→ Strong electrolyte; B→ Strong electrolyte

11 / 25

11. The reduction potential of hydrogen half-cell will be negative if:

a) p(H₂) = 1 atm and [H⁺] = 1.0 M

b) p(H₂) = 2 atm and [H⁺] = 2.0 M

c) p(H₂) = 1 atm and [H⁺] = 2.0 M

d) p(H₂) = 2 atm and [H⁺] = 1.0 M

12 / 25

12. KCl solution is generally used to determine the cell constant because:

a) It is highly ionic in nature.

b) All of these reasons.

c) Size of cations and anion are comparable

d) Its conductivity is known accurately at various concentration and different temperatures.

13 / 25

13. Statement I: Platinum and gold are used as inert electrodes.
Statement II: Pt and Au do not participate in the reaction and provide the surface for oxidation or reduction.

a) Statement I is true, Statement II is true; Statement II is the correct explanation for Statement I.

b) Statement I is true, Statement II is false.

c) Statement I is false, Statement II is true.

d) Statement I is true, Statement II is true; Statement II is NOT a correct explanation for statement-I.

14 / 25

14. Match Column I with Column II related to the figure given below and then select the appropriate option from the codes given below.

fig Q47 A

electro47

a) A →2; B → 3; C → 1; D → 2

b) A →2; B → 1; C → 3; D → 2

c) A →1; B → 2; C → 1; D → 3

d) A →1; B → 2; C → 3; D → 1

15 / 25

15. Molar conductivities (Λ^°_m) at infinite dilution of NaCl, HCl and CH₃COONa are 126.4, 425.9 and 91.0 S cm² mol^-1respectively. Λ^°_mfor CH₃COOH will be

a) 425.5 S cm² mol^-1

b) 180.5 S cm² mol^-1

c) 390.5 S cm² mol^-1

d) 290.85 S cm² mol^-1

16 / 25

16. When 0.1 mole of MnO₄²^-is oxidized, the quantity of electricity required to completely oxidize MnO₄ ²^-to MnO₄^-1is:

a) 96500 C

b) 9650 C

c) 2 x96500 C

d) 96.50 C

17 / 25

17. Statement I: Conductivity of electrolytes decreases when dissolved in water.
Statement II: They furnish their own ions.

a) Statement I is false, Statement II is true.

b) Statement I is true, Statement II is false.

c) Statement I is true, Statement II is true; Statement II is NOT a correct explanation for statement-I.

d) Statement I is true, Statement II is true; Statement II is the correct explanation for Statement I.

18 / 25

18. Select the correct statement

a) Conductivity as well as molar conductivity decrease with decrease in concentration.

b) Conductivity decreases but molar conductivity increases with increase in dilution.

c) Conductivity decreases but molar conductivity increases with increase in concentration.

d) Conductivity increases but molar conductivity decreases with increase in dilution.

19 / 25

19. Which of the following equation(s) is/are incorrect?

a) Λ^°_m(NaBr)- Λ^°_m(NaCl)= Λ^°_m(KBr)- Λ^°_m(KCl)

b) None of the options mentioned.

c) Λ^°_m(KCl)- Λ^°_m(NaCl)= Λ^°_m(KBr)- Λ^°_m(NaBr)

d) Λ^°_m(KBr)- Λ^°_m(NaBr)= Λ^°_m(KI)- Λ^°_m(NaI)

20 / 25

20. Statement I: Conductivity of pure water is 3.5 x 10^-5 S m⁻¹
Statement II: High amounts of hydrogen and hydroxyl ions are present in water.

a) Statement I is true, Statement II is false.

b) Statement I is true, Statement II is true; Statement II is the correct explanation for Statement I.

c) Statement I is true, Statement II is true; Statement II is NOT a correct explanation for statement-I.

d) Statement I is false, Statement II is true.

21 / 25

21. For the generation of electrical potential of 1.1 V, the ideal concentration of zinc and copper ion (in mol dm ^-3) in the Galvanic cell is :

a) 2 and 1

b) 3 and 2

c) 1 and 1

d) 4 and 2

22 / 25

22. Match the items of Column I and Column II.

electro52

a) A →4; B → 3; C → 1; D → 2

b) A →3; B → 4; C → 2; D → 1

c) A →3; B → 4; C → 1; D → 2

d) A →4; B → 3; C → 2; D → 1

23 / 25

23. Statement I: Conductivity always increases with decrease in concentration for strong and weak electrolytes.
Statement II: Number of ions per unit volume decreases on dilution.

a) Statement I is true, Statement II is true; Statement II is the correct explanation for Statement I.

b) Statement I is true, Statement II is false.

c) Statement I is false, Statement II is true.

d) Statement I is true, Statement II is true; Statement II is NOT a correct explanation for statement-I.

24 / 25

24. Conductivity (Unit Siemen's 'S') is directly proportional to area of the vessel and the concentration of the solution in it and is inversely proportional to the length of the vessel, then the unit of constant of proportionality is:

a) S m² mol^-1

b) S m mol^-1

c) S^-2 m² mol

d) S² m² mol^-2

25 / 25

25. If the E^°_cellfor a given reaction has a negative value, then which of the following gives the correct relationships for the values of ∆G^° and K_eq?

a) ∆G^o< 1; K_eq < 1

b) ∆G^o< 1; K_eq > 1

c) ∆G^o> 1; K_eq < 1

d) ∆G^o< 1; K_eq > 1

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