Electrochemistry Quiz

15 Questions

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Electrochemistry Quiz

Electrochemistry is a branch of Chemistry that concentrates in the study of the relationship between electrical and chemical components. How well have you mastered this study? The quiz below dives deep into the details. All the best.


Questions and Answers
  • 1. 
    Which of the following decreases with dilution:
    • A. 

      Molar Conductance

    • B. 

      Conductance

    • C. 

      Specific Conductance

    • D. 

      Equivalent Conductance

  • 2. 
    An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to:
    • A. 

      Increase in number of ions

    • B. 

      Increase in ionic mobility of ions

    • C. 

      100% ionisation of electrolyte at normal dilution

    • D. 

      Increase in both i.e., number of ions and ionic mobility of ions

  • 3. 
    • A. 

      The standard reduction potential of Li+/Li is lower than that of Cu+/Cu

    • B. 

      The standard reduction potential of Cu+/Cu is lower than that of Li+/Li

    • C. 

      The standard oxidation potential of Li+/Li is lower than that of Cu+/Cu

    • D. 

      Li is smaller in size as compared to Cu

  • 4. 
    The standard electrode potential is measured by:
    • A. 

      Electrometer

    • B. 

      Voltmeter

    • C. 

      Pyrometer

    • D. 

      Galvanometer

  • 5. 
    • A. 

      KNO3 is highly soluble in water

    • B. 

      Velocity of (NO3)- is greater than that of K+

    • C. 

      Velocity of K+ is greater than that of (NO3)-

    • D. 

      Velocity of both K+ and (NO3)- are nearly the same

  • 6. 
    What would happen if the electrodes used in the electrolysis process rective:
    • A. 

      Electrode does not participate in the chemical reaction

    • B. 

      Electrodes only act as source and sink for electrons

    • C. 

      Electrodes participate in the electrode reaction

    • D. 

      Electrodes are burnt up

  • 7. 
    • A. 

      5 x 10-4

    • B. 

      1 x 10-4

    • C. 

      5 x 10-5

    • D. 

      1 x 10-5

  • 8. 
    • A. 

      1240 x 10-4 S m2 mol-1

    • B. 

      124 x 10-4 S m2 mol-1

    • C. 

      12.4 x 10-4 S m2 mol-1

    • D. 

      1.24 x 10-4 S m2 mol-1

  • 9. 
    The reduction potential of hydrogen half-cell will be negative if:
    • A. 

      P(H2) = 1 atm and [H+] =  M

    • B. 

      P(H2) = 1 atm and [H+] = 2 M

    • C. 

      P(H2) = 2 atm and [H+] = 1 M

    • D. 

      P(H2) = 2 atm and [H+] = 2 M

  • 10. 
    The hydrogen electrode is dipped in a solution of pH 3 at 25°C. The potential would be (the value of 2.303 RT/F is 0.059 V)
    • A. 

      0.177 V

    • B. 

      - 0.177 V

    • C. 

      0.059 V

    • D. 

      - 0.059 V

  • 11. 
    Which of the following reaction is preferred during electrolysis of dilute sulphuric acid:
    • A. 

      2H2O (l) → O2 (g) + 4H+ (aq) + 4e-

    • B. 

      2SO42- (g) → S2O82- (g) + 2e-

    • C. 

      2H2 (g) + 4OH- (aq) → 4H2O (l) + 4e-

    • D. 

      2SO42- (aq) → S2O82- (aq) + 2e-

  • 12. 
    The standard electrode potential for the half cell reactions are: The E.M.F. of the cell reaction
    • A. 

      – 1.20 V

    • B. 

      + 1.20 V

    • C. 

      + 0.32 V

    • D. 

      – 0.32 V

  • 13. 
    Al2O3 is reduced by electrolysis at low potentials and high currents. If 4.0 × 104 amperes of current is passed through molten Al2O3 for 6 hours, what mass of aluminum is produced? (Assume 100% current efficiency, atomic mass of Al = 27 g/mol)
    • A. 

      9.0 x 103 g

    • B. 

      8.1 x 104 g

    • C. 

      2.4 x 105 g

    • D. 

      9.0 x 103 g

  • 14. 
    When KMnO4 acts as an oxidizing agent and ultimately forms MnO42–, MnO2, Mn2O3 and Mn2+, then the number of electrons transferred in each case is:
    • A. 

      1, 3, 4, 5

    • B. 

      3, 7, 1, 5

    • C. 

      4, 3, 1, 5

    • D. 

      1, 5, 7, 3

  • 15. 
    For a cell reaction involving two electrons change, the standard E.M.F. of the cell is found to be 0.295 V at 25°C. The equilibrium constant of the reaction at 25°C is:
    • A. 

      2.95 x 10-2

    • B. 

      2.95 x 102

    • C. 

      1 x 1010

    • D. 

      1 x 10-10