Redox Reactions Mock Test – Class 11 Chemistry

1. A complete redox cell answer should identify electrode processes before applying the voltage formula because:

2. The net ionic equation shows:

3. A proposed galvanic cell has under standard conditions. The safest interpretation is:

4. A metal displaces from solution, but cannot displace from solution. The best conclusion is:

5. A standard reduction potential table gives:

The strongest oxidising agent in the table is:

6. The decomposition is redox because:

7. In , using , the oxidation number of nitrogen is:

8. In the neutral compound , the oxidation number of sulphur is:

9. A metal reacts with dilute acid to liberate , but metal does not. A suitable redox interpretation is:

10. The fully balanced acidic half-reaction for is:

11. A bottle label reads iron sulphate. The Roman numeral means:

12. A metal reacts with ions as . The broader redox idea is needed here because:

13. In the cell, the zinc electrode gradually loses mass because:

14. A redox titration graph plots volume of titrant on the x-axis and amount of analyte remaining on the y-axis. Before the equivalence point, the graph falls because:

15. The half-reactions and are combined. The smallest common electron count is:

16. A redox titration calculation must use the balanced redox equation mainly because:

17. The electron count is balanced in which paired set of half-reactions?

18. The salt bridge in a simple galvanic cell mainly:

19. Rusting of iron is classified as corrosion because:

20. Standard electrode potential is mainly a measure of:

21. In , what fraction of chlorine atoms is oxidised?

22. In a permanganate titration in acidic medium, reacts with in the ratio . If of is used, the moles of oxidised are:

23. In a reaction, an element changes from oxidation number to . The change represents:

24. In the corrosion of iron in moist air, the metal atom that undergoes oxidation is:

25. A metal displaces silver from solution according to . The electron balance is:

26. In the reaction , oxidation and reduction are coupled because:

27. The half-reaction is written in a notebook. The best repair is:

28. Match the basic redox terms in Column I with their meanings in Column II.

29. A metal has , while has . For , the likely role of is:

30. A half-reaction is written as . The change is best described as:

31. A compound has formula . Its Stock name is:

32. For the reaction , the oxidising agent is:

33. A statement says, “In redox, equivalent mass can be calculated without knowing the reaction.” The best evaluation is:

34. A bleaching process uses an oxidising substance to remove the colour of a dye. The redox interpretation is that the dye molecules are usually:

35. A cell is made from and the standard hydrogen electrode. If , the reaction has:

36. A half-reaction at one electrode is . This electrode is:

37. The paired changes and occur in the same reaction. What is the most suitable redox interpretation?

38. In the reaction , the element oxidised is:

39. A learner calculates the oxidation number of iron in as by writing . The correction is:

40. The row that applies the oxygen exception correctly is:

41. Study the table and select the row in which the oxidation-number equation is properly written.

42. For , the oxidation-number graph would show:

43. A data note gives the qualitative reduction tendency order . The strongest oxidising agent among these ions is:

44. The coefficient of in the acidic reaction of with is . The electron-balance reason is:

45. In , using , the oxidation number of nitrogen is:

46. In acidic medium, oxidises to . If of reacts completely, the moles of consumed are:

47. A qualitative redox table is shown.

The row that needs correction is:

48. A reaction changes into . Using oxidation numbers, this change is:

49. The acidic-medium reduction half-reaction requires how many ions after oxygen is balanced?

50. In the reaction , the electron transfer count is: