Electrochemistry - NCERT Based MCQs for NEET

This article contains NCERT based 45 MCQ questions test on Chemistry chapter "Electrochemistry". You can attempt these questions in the form of an interactive quiz and calculate your score. Read the below quiz rules carefully before you start

General Instructions

• Quiz contains 45 questions of 4 marks each.
• Correct answer (✔) will award you +4 marks and Incorrect answer (✘) will give you -1 mark.
• Total test is of 180 marks.
• Tap on box in order to select any option that you think is correct.
• Press the Submit button given in the end of quiz to calculate your score.
• There is a PDF file attached in the end of quiz. You can see detailed solutions to all questions and do self analysis from that file as well.

Question 1. To deposit 0.6354 gm of copper by electrolysis of aqueous cupric sulphate solution, the amount of electricity required (in coulombs) is –

(1) 9650

(2) 4825

(3) 3860

(4) 1930

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Question 2. What is the amount of chlorine evolved when 2 amperes of current is passed for 30 minutes in an aqueous solution of NaCl –

(1) 66 g

(2) 1.32 g

(3) 33 g

(4) 99 g

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Question 3. The electrolytic cells, one containing acidified ferrous chloride and another acidified ferric chloride are connected in series. The ratio of iron deposited at cathodes in the two cells when electricity is passed through the cells will be –

(1) 3:1

(2) 2:1

(3) 1:1

(4) 3:2

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Question 4. When electricity is passed through the solution of AlCl₃, 13.5gm of Al are deposited. The no. of Faraday must be –

(1) 0.50

(2) 1.00

(3) 1.50

(4) 2.00

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Question 5. When 1F of electricity is passed through acidulated water, O₂ evolved is –

(1) 11.2 dm³

(2) 5.6 dm³

(3) 22.4 dm³

(4) 1.0 dm³

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Question 6. In electrolysis of dilute H₂SO₄ using platinum electrodes –

(1) H₂ is evolved at cathode

(2) NH₃ is produced at anode

(3) Cl₂ is obtained at cathode

(4) O₂ is produced at cathode

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Question 7. In the cell, the negative electrode is –

(1) Cu

(2) Cu²⁺

(3) Zn

(4) Zn²⁺

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Question 8. Saturated solution of KNO₃ is used to make ‘salt-bridge’ because

(1) Velocity of K⁺ is greater than that of NO₃^–

(2) Velocity of NO₃^– is greater than that of K⁺

(3) Velocities of both K⁺ and NO₃^– are nearly the same

(4) KNO₃ is highly soluble in water

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Question 9. The molar conductance of NaCl, HCl and CH₃COONa at infinite dilution are 126.45, 426.16 and 91ohm⁻¹cm²mol⁻¹ respectively. The molar conductance of CH₃COOH at infinite dilution is

(1) 201.28 ohm⁻¹ cm² mol⁻¹

(2) 390.71 ohm⁻¹cm²mol⁻¹

(3) 460.71 ohm⁻¹cm²mol⁻¹

(4) 540.48 ohm⁻¹cm²mol⁻¹

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Question 10. If a strip of Cu metal is placed in a solution of ferrous sulphate

(1) Copper will precipitate out

(2) Iron will precipitate out

(3) Copper will dissolve

(4) No reaction will take place

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Question 11. At 25°C specific conductivity of a normal solution of KCl is 0.002765 mho. The resistance of cell is 400 ohms. The cell constant is –

(1) 0.815

(2) 1.016

(3) 1.106

(4) 2.016

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Question 12. The standard reduction potential for Li⁺ / Li ; Zn²⁺ / Zn ; H⁺/H₂ and Ag⁺/Ag is

−3.05, − 0.762, 0.00 and +0.80V. Which of the following has highest reducing capacity –

(1) Ag

(2) H₂

(3) Zn

(4) Li

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Question 13. Given standard electrode potentials

Fe²⁺ + 2e⁻ → Fe; E^o = −0.440 V

Fe³⁺ + 3e⁻ → Fe; E^o = −0.036 V

The standard electrode potential (E°) for

Fe³⁺ + e⁻ → Fe²⁺

(1) -0.476 V

(2) -0.404 V

(3) +0.404 V

(4) +0.772 V

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Question 14. E° for the cell is 1.10V at 25°C, the equilibrium constant for the reaction

Zn + Cu²⁺⇌ Cu + Zn²⁺

is of the order of

(1) 10^-28

(2) 10^-37

(3) 10⁺¹⁸

(4) 10⁺¹⁷

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Question 15. Aluminum displaces hydrogen from dilute HCl whereas silver does not. The e.m.f. of a cell prepared by combining Al/Al³⁺ and Ag/Ag⁺ is 2.46 V. The reduction potential of silver electrode is +0.80V. The reduction potential of aluminum electrode is –

(1) +1.66V

(2) –3.26V

(3) +3.26V

(4) –1.66V

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Question 16. Which of the following is a highly corrosive salt

(1) FeCl₂

(2) PbCl₂

(3) Hg₂Cl₂

(4) HgCl₂

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Question 17. The passage of current liberates H₂ at cathode and Cl₂ at anode. The solution is

(1) Copper chloride in water

(2) NaCl in water

(3) H₂SO₄

(4) Water

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Question 18. Which of the following liberate hydrogen on reaction with dilute H₂SO₄

(1) Fe

(2) Cu

(3) Al

(4) Hg

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Question 19. When 96500 coulomb of electricity is passed through a copper sulphate solution, the

amount of copper deposited will be

(1) 0.25 mol

(2) 0.50 mol

(3) 1.00 mol

(4) 2.00 mol

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Question 20. An electrolytic cell contains a solution of Ag₂SO₄ and have platinum electrodes. A

current is passed until 1.6 gm of O₂ has been liberated at anode. The amount of silver deposited at cathode would be

(1) 107.88 gm

(2) 1.6 gm

(3) 0.8 gm

(4) 21.60 gm

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Question 21. When E°_Ag⁺/Ag= 0.8 volt and E°_Zn²⁺/Zn= −0.76 volt, which of the following is correct

(1) Ag⁺ can be reduced by H₂

(2) Ag can oxidize H₂ into H⁺

(3) Zn²⁺ can be reduced by H₂

(4) Ag can reduce Zn²⁺ ion

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Question 22. For a cell given below Ag | Ag⁺ || Cu²⁺ | Cu E° cell is

(1) x + 2y

(2) 2x + y

(3) y – x

(4) y – 2x

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Question 23. Λ^∞_AcOH using appropriate molar conductance of the electrolytes listed above at infinite dilution in H₂O at 25°C

(1) 552.7

(2) 517.2

(3) 217.5

(4) 390.7

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Question 24. The reduction potential of hydrogen half-cell will be negative if –

(1) p (H₂) = 1 atm and [H⁺] = 2.0 M

(2) p (H₂) = 1 atm and [H⁺] = 1.0 M

(3) p (H₂) = 2 atm and [H⁺] = 1.0 M

(4) p (H₂) = 2 atm and [H⁺] = 2.0 M

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Question 25. The standard reduction potentials for Zn²⁺/Zn, Ni²⁺/Ni and Fe²⁺/Fe are –0.76, –0.23 and –0.44 V respectively. The reaction X + Y²⁺ → X²⁺ + Y will be spontaneous when

(1) X = Ni, Y = Fe

(2) X = Ni, Y = Zn

(3) X = Fe, Y = Zn

(4) X = Zn, Y = Ni

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Question 26. Given :

E°_Cr³⁺/Cr= -0.74 V; E°_{MnO4^-/Mn²⁺}=1.51 V

E°_{Cr2O7^2-/Cr³⁺}= 1.33 V; E°_Cl/Cl⁻= 1.36 V

Strongest oxidizing agent will be –

(1) Cl

(2) Cr³⁺

(3) Mn²⁺

(4) MnO₄^–

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Question 27. The equivalent conductance of NaCl at concentration C and at infinite dilution are λ_C and λ_∞ respectively. The correct relationship between λ_C and λ_∞ is given as: (where the constant B is positive)

(1) λ = λ_∞ - (B)√C

(2) λ_C = λ_∞ + (B)√C

(3) λ_C = λ_∞ + (B)C

(4) λ_C = λ_∞ − (B)C

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Question 28. Given below are the half-cell reactions:

Mn²⁺ + 2e^– → Mn; E° = –1.18 V

2 (Mn³⁺ + e^– → Mn²⁺); E° = +1.51 V

The E° for 3 Mn²⁺ → Mn + 2 Mn³⁺ will be –

(1) –0.33 V; the reaction will not occur

(2) –0.33 V; the reaction will occur

(3) –2.69 V; the reaction will not occur

(4) –2.69 V; the reaction will occur

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Question 29. Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half-cell reactions and their standard potentials are given below:

MnO₄^-(aq) + 8H⁺ + 5e^- → Mn²⁺(aq) + 4H₂O(l); E= 1.51 V

Cr₂O₇^2-(aq) + 14H⁺(aq) + 6e^- → 2Cr³⁺(aq) + 7H₂O(l); E= 1.38 V

Fe³⁺(aq) + e^- → Fe²⁺(aq); E= 0.77 V

Cl₂(g) + 2e^- → 2Cl^-(aq); E= 1.40 V

Identify the only incorrect statement regarding the quantitative estimation of aq. Fe(NO₃)₂

(1) MnO₄^– can be used in aqueous HCl.

(2) Cr₂O₇^2– can be used in aqueous HCl

(3) MnO₄^– can be used in aqueous H₂SO₄

(4) Cr₂O₇^2– can be used in aqueous H₂SO₄

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Question 30. Zn|Zn²⁺ (a = 0.1 M) || Fe²⁺ (a = 0.01 M) | Fe.

The emf of the above cell is 0.2905 V. Equilibrium constant for the cell reaction is:

(1) 10^0.32/0.0591

(2) 10^0.32/0.0295

(3) 10^0.26/0.0295

(4) e^0.32/0.295

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Question 31. Given below are the standard electrode potentials of few half-cells. The correct order of these metals in increasing reducing power will be K⁺|K= –2.93 V, Ag⁺|Ag= 0.80 V,

Mg²⁺|Mg = – 2.37 V, Cr³⁺|Cr= – 0.74 V,

(1) K < Mg < Cr < Ag

(2) Ag < Cr < Mg < K

(3) Mg < K < Cr < Ag

(4) Cr < Ag < Mg < K

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Question 32. In which of the following electrochemical cell

the overall cell reaction is:

Zn(s) + H₂SO₄ (aq) → ZnSO₄ (aq) + H₂(g)

(1) Zn | H₂SO₄ (aq) | H₂ (g) | Pt

(2) Zn | ZnSO₄ (aq) | H₂ (g) | Pt

(3) Zn | ZnSO₄ (aq) | H₂SO₄ (aq) | H₂ (g) | Pt

(4) Zn | ZnSO₄ (aq) || H₂SO₄ (aq) | H₂ (g) | Pt

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Question 33. The equivalent conductivity of N/10 solution of acetic acid at 25°C is 14.3 ohm^–1 cm² equiv^–1. What will be the degree of dissociation of acetic acid? (CH₃COOH= 390.71 ohm^–1 cm² equiv^–1)

(1) 3.66%

(2) 3.9%

(3) 2.12%

(4) 0.008%

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Question 34. Which of the following is not an application of electrochemical series?

(1) To compare the relative oxidising and reducing power of substances

(2) To predict evolution of hydrogen gas on reaction of metal with acid

(3) To predict spontaneity of a redox reaction

(4) To calculate the amount of metal deposited on cathode.

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Question 35. Which of the following statements is correct?

(1) E_cell and Δ_rG of cell reaction both are extensive properties.

(2) E_cell and Δ_rG of cell reaction both are intensive properties.

(3) E_cell is an intensive property while Δ_rG of cell reaction is an extensive property.

(4) E_cell is an extensive property while Δ_rG of cell reaction is an intensive property.

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Question 36. Same amount of electric current is passed through the solutions of AgNO₃ and HCl. If 1.08 g of silver is obtained from AgNO₃ solution, the amount of hydrogen liberated at STP will be

(1) 1.008 g

(2) 11.2 g

(3) 0.01 g

(4) 1.1 g

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Question 37. Which of the following reactions does not take place during rusting?

(1) H₂CO₃ → 2H⁺ + CO₃^2–

(2) 4Fe²⁺ + O₂(dry) → Fe₂O₃

(3) 4Fe²⁺ + O₂ + 4H₂O → 2Fe₂O₃ + 8H⁺

(4) Fe₂O₃ + xH₂O → Fe₂O₃.xH₂O

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Question 38. E° for F₂ + 2e^– → 2F^– is 2.8 V, 

E° for ½ F₂ + e^– → F^– is-

(1) 2.8 V

(2) l.4 V

(3) –2.8 V

(4) –1.4 V

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Question 39. The correct Nernst equation for the given cell

Pt(s) | Br₂(l) | Br^–(M) || H⁺(M) | H₂(g)(1bar) |Pt(s)

is

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Question 40. Molar conductivity of NH₄OH can be calculated by the equation,

(1) Λ°NH₄OH = Λ°Ba(OH)₂ + Λ°NH₄Cl – Λ°BaCl₂

(2) Λ°NH₄OH = Λ°BaCl₂ + Λ°NH₄Cl – Λ°Ba(OH)₂

(3) Λ°NH₄OH=1/2 [Ba(OH)₂ + NH₄Cl - BaCl₂]

(4) Λ°NH₄OH = 1/2 [NH₄Cl+ Ba(OH)₂]

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Question 41. What will be the emf of the following

concentration cell at 25°C?

Ag(s)|AgNO₃(0.01 M) || AgNO₃(0.05M) |

Ag(s)

(1) 0.828 V

(2) 0.0413 V

(3) –0.0413 V

(4) –0.828 V

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Question 42. How many coulombs of electricity is required

to reduce 1 mole of Cr₂O₇^2– in acidic medium?

(1) 4 × 96500 C

(2) 6 × 96500 C

(3) 2 × 96500 C

(4) 1 × 96500 C

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Question 43. Which statement is true in regard to a

spontaneous redox reaction?

(1) E°_red is always negative

(2) E°_cell is always positive

(3) E°_Ox is always positive

(4) E°_red is always positive

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Question 44. Metals can be prevented from rusting by

(1) Connecting iron to more electropositive metal cathodic protection.

(2) Connecting iron to more electropositive metal anodic protection.

(3) Connecting iron to less electropositive metal anodic protection.

(4) Connecting iron to less electropositive metal cathodic protection.

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Question 45. E° values of three metals are listed below

Zn²⁺(aq) + 2e^– → Zn(s); E° = –0.76 V

Fe²⁺(aq) + 2e^– → 2Fe(s); E° = –0.44 V

Sn²⁺(aq) + 2e^– → Sn(s); E° = –0.14 V

Which of the following statements are correct on the basis of the above information?

(i) Zinc will be corroded in preference to iron if zinc coating is broken on the surface.

(ii) If iron is coated with tin and the coating is broken on the surface then iron will be corroded

(iii) Zinc is more reactive than iron but tin is less reactive than iron.

(1) (i) and (ii)

(2) (ii) and (iii)

(3) (i), (ii) and (iii)

(4) (i) and (iii)

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Detailed Solutions

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