Electrochemistry MCQ

Electrochemistry MCQ

Electrochemistry MCQ, Multiple Choice Questions on Electrochemistry, Engineering Chemistry MCQ, electrochemistry MCQ, electrochemistry MCQ class 12, electrochemistry MCQ pdf, electrochemistry MCQ with answers, electrochemistry MCQ class 12, electrochemistry MCQ for neet, electrochemistry MCQ, electrochemistry MCQ for neet, Engineering MCQ

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Multiple-choice Questions

Q.1. The effect of temperature increases on concentration is as follows:

  • Metallic conduction increases, electrolytic conduction decreases
  • electrolytic conduction increases, metallic conduction decreases
  • Both metallic and electrolytic conduction decreases
  • Both metallic and electrolytic conduction increases

Answer: electrolytic conduction increases, metallic conduction decreases

Q.2. The units of equivalent conductance are:

  • ohm−1
  • ohm−1 cm−2
  • ohm−1 cm2
  • mho cm2

Answer: ohm−1 cm2

Q.3. The cell constant is

  • \frac{1}{a}
  • \frac{a}{1}
  • a\times 1
  • \frac{K}{R}

Answer: \frac{1}{a}

Q.4. The effect of dilution on conduction is as follows:

  • Specific conductance increases, molar conductance decreases
  • Specific conductance decreases, molar conductance increases
  • Both increases with dilution
  • Both decreases with dilution

Answer: Specific conductance decreases, molar conductance increases

Q.5. The units of the cell constant is

  • cm−1
  • cm2
  • cm3
  • cm−2

Answer: cm−1

Q.6. The potential of a single electrode is a half cell is called as

  • Reduction potential
  • Half-wave potential
  • Single electrode potential
  • Cell potential

Answer: Reduction potential

Q.7. Which of the following constitutes Daniel Cell?

  • Zn − Ag cell
  • Cu − Ag cell
  • Zn − Cu cell
  • none of these

Answer: Zn − Cu cell

Q.8. EMF of a cell in terms of the reduction potential of its left and right electrode

  • E = Eleft + Eright
  • E = Eleft − Eright
  • E = Eright − Eleft
  • None of these

Answer: E = Eright − Eleft

Q.9. Which of the following is a secondary cell

  • Dry cell
  • Mercury cell
  • Ni–Cd cell
  • H2–O2 cell

Answer: Ni-Cd cell

Q.10. An electrochemical cell stops working after some time because

  • One of the electrodes is eaten away
  • electrode potentials of both electrodes becomes equal in magnitude
  • electrode potentials of both the electrodes go on decreasing
  • electrode potentials of both the electrodes go on increasing

Answer: electrode potentials of both electrodes becomes equal in magnitude

Q.11. The standard EMF (E°) for the cell reaction

Zn + Cu2+ → Zn2+ + Cu is 1.1 volt at 25 °C. The EMF(E) of the cell reaction when 0.1M Cu2+ and 0.1 M Zn2+ solutions are used, at 25 °C is

  • 1.10 V
  • 0.10 V
  • −1.10 V
  • −0.110 V

Answer: 1.10 V

Q.12. In an electrochemical cell

  • Potential energy decreases
  • Kinetic energy decreases
  • Potential energy changes into electrical energy
  • Chemical energy changes into electrical energy

Answer: Chemical energy changes into electrical energy

Q.13. As lead storage battery is charged

  • lead dioxide dissolves
  • sulphuric acid is regenerated
  • lead electrode becomes coated with lead sulphate
  • the concentration of sulphuric acid decreases

Answer: sulphuric acid is regenerated

Q.14. In an electrochemical series, electrodes are arranged in the

  • Increasing order (downwards) of standard reduction potential
  • Decreasing order of standard reduction potential
  • Increasing order of standard oxidation potential
  • Increasing order of equivalent weight

Answer: Increasing order (downwards) of standard reduction potential

Q.15. The electrode potential of standard calomel electrode is

  • 0.2422 V
  • 0.2400 V
  • 0.2810 V
  • 0.3335 V

Answer: 0.2422 V

Q.16. Silver – Silver chloride electrode is a type of

  • Redox electrode
  • Metal – Metal Ion electrodes
  • Metal – Amalgam electrode
  • Gas – ion electrode

Answer: Metal – Metal Ion electrodes

Q.17. Calomel electrode consists of calomel with a solution of

  • Saturated NaCl
  • Saturated Ca (OH)2
  • Saturated KCl
  • Saturated AgCl

Answer: Saturated KCl

Q.18. Which electrode is used for pH measurement

  • Silver electrode
  • Redox electrode
  • Glass electrode
  • Calomel electrode

Answer: Glass electrode

Q.19. Lachance cell is an example of

  • Primary cell
  • Secondary cell
  • Tertiary cell
  • Fuel cell

Answer: Primary cell

Q.20. A fuel cell converts

  • Chemical energy into electrical energy
  • Chemical energy into potential energy
  • Chemical energy into heat
  • Chemical energy into pressure

Answer: Chemical energy into electrical energy

Q.21. Which is produced during H2−O2 fuel cell

  • CH3OH
  • H2O
  • H2O2
  • H3O+

Answer: H2O

Q.22. The cathode of Ni-Cd cell is made up from

  • NiOH
  • Ni (OH)2
  • NiO2
  • NiO (OH)

Answer: NiO (OH)

Q.23. During Charging of lead-acid cell, the concentration of H2SO4

  • Increases
  • Decreases
  • Remains unchanged
  • First increases then decreases

Answer: Increases

Q.24. In a potentiometric titration, the graph is plotted between variations of

  • Electrode potential with temperature of titrant
  • Electrode potential with pressure of titrant
  • Electrode potential with volume of titrant
  • Electrode potential with concentration of titrant

Answer: Electrode potential with the volume of titrant

Q.25. At equilibrium, the EMF of the cell is

  • 0 V
  • 100 V
  • Less than 0 V
  • More than 0 V

Answer: 0 V

Q.26. In glass electrode, the glass membrane undergoes exchange of Na+ ion with

  • Ca2+
  • Mg2+
  • H+
  • NH4+

Answer: H+

Q.27. Quinhydrone – electrode consist of hydroquinone (QH2) and quinone (Q) in the ratio of

  • 1: 2
  • 1:1
  • 2:1
  • 1:15

Answer: 1:1

Q.28. The conductance of an electrode depends upon

  • Number of free ions present in solution
  • Number of free ions present in solvent
  • Concentration of the solution
  • Temperature of the solution

Answer: Number of free ions present in solution

Q.29. Four metals A, B, C, and D are having their reduction potentials as −3.05, −1.66, −0.40, and −0.80 V respectively. Which one of these will be the most reducing agent.

  • A
  • B
  • C
  • D

Answer: A

Q.30. Equivalent conductance of NaCl, HCl, and C2H5COONa at infinite dilution are 126.45, 426.16, and 91 ohm−1 cm2 respectively. The equivalent conductance of C2H5COOH at infinite dilution is

  • 201.28 ohm−1 cm2
  • 390.71 ohm−1 cm2
  • 698.28 ohm−1 cm2
  • 540.48 ohm−1 cm2

Answer: 390.71 ohm−1 cm2

Q.31. The saturated solution of KNO3 is used to make salt bridges because

  • Velocity of K+ is greater than that of NO3
  • Velocity of NO3 is greater than that of K+
  • Velocities of both K+ and NO3 are nearly the same
  • KNO3 is highly soluble in water

Answer: Velocities of both K+ and NO3 are nearly the same

Q.32. The specific conductance of N/50 solution of KCl at 25 °C is 0.002765 ohm−1. If the resistance of the cell is 400 ohms, then what is the value of cell constant

  • 2
  • 1.106
  • 3
  • 3.2

Answer: 1.106

Q.33. The EMF of the cell Ni | Ni2+ (1.0M) | Au3+ (1.0M) | Au

Given that

\begin{pmatrix} E^{o}=-0.25V for Ni^{2+}|Ni\\ E^{o}=+1.5V for Au^{3+}|Au \end{pmatrix}
  • 1.25 V
  • −1.25 V
  • 1.75 V
  • 2.00 V

Answer: 1.75 V

Q.34. The conductivity of a saturated solution of BaSO4 is 3.06 × 10−6 ohm−1 cm2 and its equivalent conductance is 1.53 ohm−1 cm2 equiv−1. The Ksp for BaSO4 will be

  • 4 × 10−12
  • 2.5 × 10−9
  • 2.5 × 10−13
  • 4 × 10−6

Answer: 4 × 10−6

Q.35. Which of the following does not conduct electricity

  • Molten NaCl
  • Aqueous NaCl
  • Solid NaCl
  • Aqueous NH4Cl

Answer: Solid NaCl

Q.36. On dilution specific conductance of an electrolyte

  • Increases
  • Decreases
  • First increases then decreases
  • Neither increases nor decreases

Answer: Decreases

Q.37. The unit of equivalent conductivity is

  • Mho
  • Ohm –1 cm–1
  • Ohm–1 cm–1 equiv –1
  • Ohm –1 cm2 equiv –1

Answer: Ohm –1 cm2 equiv –1

Q.38. The cell constant is defined as

  • Ratio of distance between electrodes and their area of cross–section
  • Ratio of specific conductance to the observed conductance
  • Both the above
  • None of the above

Answer: Both the above

Q.39. Which of the following statement is incorrect about an electrochemical cell?

  • Oxidation occurs at the anode and reduction occurs at the cathode.
  • Chemical energy converts into electrical energy and vice versa
  • Cell can work indefinitely
  • Salt bridge reduces the liquid junction potential of the cell

Answer: Cell can work indefinitely

Q.40. Glass electrode is an example of

  • Redox electrode
  • Ion-selective electrode
  • Metal insoluble salt electrode
  • Gas electrode

Answer: Ion-selective electrode

Q.41. A battery that remains in the inactive state and is activated immediately before use is the

  • Primary cell
  • Secondary cell
  • Reserve battery
  • Fuel cell

Answer: Reserve battery

Q.42. In a Leclanche cell, the anode is

  • Graphite rod
  • FeO and Fe(OH)3
  • Zinc container
  • MnO2 + C

Answer: Zinc container

Q.43. Which of the following is not an alkaline battery?

  • Nickel cadmium battery
  • Mercury battery
  • Zinc– air battery
  • Lead acid battery

Answer: Lead acid battery

Q.44. In a solid oxide fuel cell, the electrolyte is

  • NaOH or KOH
  • Ceramic compounds
  • H2SO4
  • Liquid phosphoric acid

Answer: Ceramic compounds

Q.45. Which of the following is not a secondary cell?

  • Lithium–MnO2 battery
  • Lead–acid battery
  • Nickel–cadmium battery
  • Nickel metal hydride battery

Answer: Lithium–MnO2 battery

Q.46. The specific conductance of a solution is 0.3568 ohm–1cm–1. When placed in a cell, the conductance is 0.0268 ohm–1. The cell constant is

  • 1.331cm–1
  • 13.31 cm–1
  • 0.665 cm–1
  • 6.65 cm–1

Answer: 13.31 cm–1

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