Chemistry 1st Year Chapter 10 Electrochemistry Notes MCQs Bank

chemistry 11th notes chapter 10

1. During the electrolysis of aqueous KNO₃, H₂ is produced at cathode instead of potassium due to:

 
 
 
 

2. “Al” metal is extracted from its ________ during electrolysis.

 
 
 
 

3. The oxidation number of sulphur in Na₂S₄O₆ is:

 
 
 
 

4. If a strip of Cu-metals is placed in a solution of FeSO₄ then:

 
 
 
 

5. Gold and silver are the least reactive due to:

 
 
 
 

6. The change in oxidation state of nitrogen in the following reaction is: Cu + HNO₃ —> Cu(NO₃)₂ + NO₂ + H₂O

 
 
 
 

7. Which of the following cannot conduct electricity:

 
 
 
 

8. The electrolysis product of molten NaCl at electrodes:

 
 
 
 

9. The colour of K₂MnO₄ solution is:

 
 
 
 

10. In a galvanic cell, the electrode occupying a lower position in the electrochemical series:

 
 
 
 

11. In superoxides, the oxidation number of oxygen is:

 
 
 
 

12. Which of the following has same oxidation state in all of its compounds:

 
 
 
 

13. Value of standard reduction potential for strong reducing agent is:

 
 
 
 

14. Down’s cell is used for the extraction of:

 
 
 
 

15. When Brine solution is electrolysed which of the following ions get discharged at anode:

 
 
 
 

16. Magnesium metal is extracted by the electrolysis of its:

 
 
 
 

17. The ability of elements to act as reducing agent _________ down to electrochemical series.

 
 
 
 

18. The oxidation state of Mn in K₂MnO₄ is:

 
 
 
 

19. The oxidation potential of Mg and Al are +2.37 and 1.66V, respectively. The Mg is a chemical reaction:

 
 
 
 

20. Standard hydrogen electrode has an arbitrarily fixed potential of:

 
 
 
 

21. A normal aluminum electrode coupled with a normal hydrogen electrode gives an emf of 1.66 volts and deflection of the needle towards Hydrogen. The standard electrode potential of aluminum is:

 
 
 
 

22. The increase in positive oxidation state is called:

 
 
 
 

23. Which one metal shows the maximum oxidation state?

 
 
 
 

24. Which of the following is a primary cell:

 
 
 
 

25. In lead accumulator, cathode is made up of:

 
 
 
 

26. In which compound oxidation state of chlorine is +5:

 
 
 
 

27. In silver oxide battery anode is made up of:

 
 
 
 

28. Four metals A, B, C, and D are having standard electrode potential as -3.05, -1.66, -0.4, and 0.8V respectively. Which one will be the best reducing agent:

 
 
 
 

29. Which of the following is not the reduction:

 
 
 
 

30. Fuel cell are the means by which chemical energy is converted into:

 
 
 
 

31. Iron can be prevented from rusting by:

 
 
 
 

32. The cell in which a non-spontaneous redox reaction takes place as a result of electricity is known as:

 
 
 
 

33. The oxidation state of carbon is C₆H₁₂O₆ is:

 
 
 
 

34. If the sum of Eo values of the two half cells is negative, then:

 
 
 
 

35. Which of the following is a reducing agent in following reaction: P + HNO₃ —-> H₃PO₄+ NO + H₂O

 
 
 
 

36. In a reaction Zn + HNO₃ → Zn(NO₃)₂ + NO + H₂O:

 
 
 
 

37. Which of the following statement is correct?

 
 
 
 

38. The overall positive reaction potential value predicts that process is:

 
 
 
 

39. Which of the following statement is true about galvanic cell:

 
 
 
 

40. Which of the following is a secondary cell:

 
 
 
 

41. Electrochemical series is useful in:

 
 
 
 

42. The correct order of equivalent conductance at infinite dilution among LiCl, NaCl, and KCl is:

 
 
 
 

43. The cell in which electrical energy is converted int⁰Chemical energy is:

 
 
 
 

44. When an element is in contact with 1M aqueous solution of its own ions, at 298K then the potential is called?

 
 
 
 

45. During electrolysis reaction that take place at cathode:

 
 
 
 

46. In which of the following compounds oxidation number of sulphur is negative:

 
 
 
 

47. In which of the following reactions, hydrogen behave as an oxidizing agent:

 
 
 
 

48. The oxidation state of carbon-atom in glucose is:

 
 
 
 

49. Greater the value of the standard reduction potential of the given species:

 
 
 
 

50. SHE acts as an anode when connected with Cu electrode but cathode with Zn electrode because:

 
 
 
 

51. Which can replace hydrogen from dilute acids?

 
 
 
 

52. Coinage metals have the least reactivity because they have:

 
 
 
 

53. Which of the following cell can convert chemical energy directly into electrical energy:

 
 
 
 

54. Halogens are placed at the lower level of electrochemical series, this indicates that:

 
 
 
 

55. Reduction potential of SHE is 0.00 volts its oxidation potential will be:

 
 
 
 

Short Questions

1. A porous plate or a salt bridge is not required in lead storage cell. Why?
2. A salt bridge maintains the electrical neutrality in the cell. Justify it?
3. Calculate the oxidation number of Mn in KMnO₄ and MnO₂?
4. How copper can be purified electrolytically?
5. How does electrochemical series tell us the distinction between the oxidation and reducing agents?
6. How in electrochemical cells, SHE can act as anode and cathode both?
7. How is Al anodized in an electrolytic cell?
8. How is the Daniel cell represented?
9. How the chemical energy is converted into electrical energy in a Galvanic cell or voltaic cell?
10. How the electrolysis of aqueous solutions of KNO₃ gives hydrogen and oxygen at cathode and anode, respectively?
11. How the galvanic cell can be reversed by an external source of e.m.f.?
12. How we can say that a voltaic cell is reversible cell?
13. It is true that Mg⁺² + ZnO → MgO+ Zn⁺² is spontaneous reaction?
14. Lead accumulator is a chargeable battery. Comment on it?
15. Na and K can displace hydrogen from acids but pt, pd and Cu cannot. Why?
16. Sodium metal is softer than copper but both are very good electrical conductors. Explain why?
17. Standard hydrogen electrode (SHE) is the reference electrode to assign the reduction potential to the electrodes. Comment upon it?
18. The electrodes above SHE in electrochemical series undergo oxidation, when connected with SHE. The e.m.f. of the cell so obtained is equal to the standard reduction potential of the electrode. Why?
19. The electrolyte in the presence of inert electrodes gives different results than the situation when the electrodes also take part in the reaction. Why?
20. The oxidation number of some of the elements vary from compound t⁰Compound. Justify it?
21. The standard oxidation potential of Zn is 0.76 V and its reduction potential is ―0.76 V Justify it?
22. What are electrochemical series?
23. What are electrode reactions of dry cell?
24. What are electrode reactions of silver oxide battery?
25. What are the electrode reactions in lead stage battery?
26. What is electrolyte? Give examples of fused NaCl?
27. What is salt bridge?
28. What is SHE?
29. What is the difference between a cell bad a battery?
30. Why the positively charged ions moves towards the cathode and negatively charged ions go to the anode to complete the oxidation reduction process in an electrolytic cell?
31. Why the products of electrolysis in molten electrolyte are different from the products of electrolysis in the solution state?

Long Questions

1. Define oxidation number. Describe the rules used for the calculation of oxidation number of an element in molecules and ions.
2. Give steps for balancing the Redox equation by oxidation number method.
3. Describe the electrolysis of molten NaCl and a concentrated solution of NaCl.
4. Give the industrial importance of electrolysis process in detail
5. Describe the construction and working of standard hydrogen electrode.
6. Describe Nickel Cadmium Cell.
7. Write a note on construction and working of fuel cells.
8. What is electrochemical series? Give its three applications.
9. What is standard hydrogen electrode? Give its construction and working.
“10. Balance the following oxidation number method.
Cu + HNO₃ —-> Cu(NO₃)₂ + NO₂ + H₂O
NaCl + H₂SO₄ + MnO₂ ——-> Na₂SO₄+MnSO₄ + H₂O + Cl₂”
11. Describe the process to determine the electrode potential using SHE.
12. How does a fuel cell generate electricity?
13. What are the advantages of fuel cells?
14. Determine the oxidation state of Cr in K₂CrO₄ and Cr₂O₇⁻²
15. Describe the construction and working of a Galvanic cell
16. What type of metals are more reactive? Explain with reference to electrochemical series.
17. Write down the rules for assigning oxidation states to elements in a compound.

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