Exam-Style Mock Test | Class 11 Chemistry: Redox Reactions

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Quiz: Redox Reactions – Progressive Test
Total questions: 480
Questions in this round: 50
Time allotted: 70 minutes
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Total rounds: 10
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Quiz: Redox Reactions – Certificate Challenge
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1 / 50

1. A species changes from to . The electron-transfer interpretation is:

a) no redox change, because the element symbol remains

b) reduction, because the positive charge increases

c) reduction, because the species gains electrons

d) oxidation, because the species loses electrons

2 / 50

2. Assertion: In a galvanic cell, oxidation and reduction are spatially separated.
Reason: The two half-reactions occur at different electrodes connected by an external circuit and an ionic path.

a) Assertion is false, but Reason is true

b) Assertion is true, but Reason is false

c) Both Assertion and Reason are true, but Reason does not explain Assertion

d) Both Assertion and Reason are true, and Reason explains Assertion

3 / 50

3. The most reliable sequence for solving a standard cell-potential problem is:

a) add all listed potentials, multiply by coefficients, then choose the larger formula mass

b) decide the answer from colour change, then ignore electrode notation

c) choose anode/cathode, use the cell-potential equation, interpret sign

d) choose the electrode with more atoms as cathode and the other as anode

4 / 50

4. For the reaction , using and , the standard cell potential is:

5 / 50

5. In the reaction , the oxidation-number change of tin is:

a) , so tin is reduced

b) , so tin is reduced

c) , so tin is oxidised

d) , so tin is oxidised

6 / 50

6. In a titration, of solution requires of acidified . Using , the concentration of is:

7 / 50

7. Match the reaction feature in Column I with the redox interpretation in Column II.

Column I	Column II
P.	1. Electron loss
Q.	2. Electron gain
R. Reaction without but with ion change	3. Need for broader redox definition
S. Electron loss and gain in the same equation	4. Coupled redox process

a) P-3, Q-4, R-1, S-2

b) P-2, Q-1, R-4, S-3

c) P-1, Q-2, R-3, S-4

d) P-4, Q-3, R-2, S-1

8 / 50

8. The pair in which both oxidation numbers are assigned correctly is:

a) in elemental sodium ;

b) ;

c) ;

d) ;

9 / 50

9. Study the table and select the row with the correct agent identification.

Row	Reaction	Electron donor	Reducing agent
P
Q
R
S

a) Row R

b) Row P

c) Row S

d) Row Q

10 / 50

10. A qualitative redox table is shown.

Row	Given information	Conclusion
P	accepts electrons more readily than	is the stronger oxidising agent
Q	loses electrons more readily than	is the stronger reducing agent
R	is oxidised more easily than	is the stronger reducing agent
S	is reduced more readily than	is the stronger oxidising agent

The row that needs correction is:

a) Row Q

b) Row P

c) Row S

d) Row R

11 / 50

11. A acidified solution is used where . What is its normality?

12 / 50

12. A graph for a working galvanic cell plots moles of deposited at the cathode on the y-axis against moles of electrons arriving at the cathode on the x-axis.

The graph is a straight line through the origin, and moles of electrons deposit mole of copper.

The graph is best interpreted as:

a) copper deposition does not involve reduction

b) the salt bridge is the source of electrons for copper deposition

c) electron flow deposits zinc at the copper electrode

d) copper deposition increases as gains electrons at the cathode

13 / 50

13. In , oxygen is assigned oxidation number . What is the average oxidation number of iron, and what does this value mean?

a) ; every iron atom must have oxidation number

b) ; every iron atom must have oxidation number

c) ; a formal average oxidation number

d) ; iron is reduced because oxygen is negative

14 / 50

14. Study the table and identify the row with the wrong electron-transfer label.

Row	Change	Label
P		Oxidation
Q		Reduction
R		Reduction
S		Reduction

a) Row S

b) Row R

c) Row Q

d) Row P

15 / 50

15. In the reaction , what is the smallest electron-balanced ratio of reduced chlorine atoms to oxidised chlorine atoms?

16 / 50

16. A species accepts electrons during a reaction. The same species is best described as:

a) oxidised and acting as an oxidising agent

b) reduced and acting as an oxidising agent

c) oxidised and acting as a reducing agent

d) reduced and acting as a reducing agent

17 / 50

17. A reaction note says:

An element in oxidation state forms two products. In one product, has oxidation state ; in the other, has oxidation state .

The note describes:

a) ionic precipitation

b) acid-base neutralisation

c) single displacement

d) disproportionation

18 / 50

18. In , the species oxidised is:

19 / 50

19. The pattern represents:

a) disproportionation because forms two products

b) comproportionation to an intermediate oxidation state

c) neutralisation because positive ions are present

d) precipitation because charges disappear

20 / 50

20. Assertion: Moisture often increases the rate of rusting of iron.
Reason: Moisture can support ionic movement needed for the electrochemical corrosion process.

a) Both Assertion and Reason are true, and Reason explains Assertion

b) Assertion is false, but Reason is true

c) Both Assertion and Reason are true, but Reason does not explain Assertion

d) Assertion is true, but Reason is false

21 / 50

21. A compact oxidation-number comparison gives , , and . The oxidation numbers of oxygen are respectively:

22 / 50

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

a) both zinc and copper lines rising by units

b) both zinc and copper lines remaining horizontal

c) zinc line rising from to , copper line falling from to

d) zinc line falling from to , copper line rising from to

23 / 50

23. In , the oxidation numbers of hydrogen and oxygen are:

a) ,

b) ,

c) ,

d) ,

24 / 50

24. The oxidation state of an element in a disproportionation reaction is usually intermediate because:

a) it must be able to increase and also decrease

b) it must already be the maximum possible value

c) it must already be the minimum possible value

d) it must be zero in every disproportionation reaction

25 / 50

25. In reductions, the product is important because:

a) it makes the charge on disappear before reaction

b) it fixes the manganese oxidation-number change and -factor

c) it changes the atomic mass of manganese

d) it fixes for every medium

26 / 50

26. A reaction record gives . The element reduced is:

a) bromine, because changes to

b) iodine, because changes to

c) neither iodine nor bromine, because both remain unchanged

d) both iodine and bromine, because both gain electrons

27 / 50

27. A formula note gives . Using the common fixed oxidation number of aluminium, what value is assigned to aluminium?

28 / 50

28. A comparison of cold dilute alkali and hot concentrated alkali reactions of chlorine shows different products. The redox reason is that:

a) chlorine keeps oxidation number in every product

b) chlorine can reach different positive oxidation states

c) undergoes the disproportionation change

d) chloride ions are always oxidised to

29 / 50

29. In the reaction , what is the mole ratio ?

30 / 50

30. The decomposition is redox because:

a) oxygen is removed from the formula, so no oxidation occurs

b) all elements keep the same oxidation number

c) chlorine is reduced and oxygen is oxidised

d) potassium changes from to

31 / 50

31. In broad redox language, respiration of glucose is described as oxidation of glucose because:

a) water formed in respiration keeps oxygen at

b) carbon ends at a higher oxidation number in

c) glucose only dissolves in blood without electron transfer

d) oxygen atoms in are oxidised to water

32 / 50

32. The half-reaction represents:

a) neither oxidation nor reduction because oxygen is absent

b) reduction because chlorine gains electrons

c) oxidation because chlorine loses electrons

d) oxidation because the number of chlorine atoms changes

33 / 50

33. In , oxygen is . Which interpretation is most suitable for the oxidation number of lead?

a) Lead has average , consistent with mixed lead states

b) Lead must be on every atom because there are four oxygen atoms

c) Lead has oxidation number because the compound is neutral

d) Lead must be on every atom because there are three lead atoms

34 / 50

34. Match the Stock name in Column I with the suitable formula in Column II.

Column I	Column II
P. iron oxide	1.
Q. iron oxide	2.
R. copper oxide	3.
S. copper oxide	4.

a) P-4, Q-2, R-3, S-1

b) P-1, Q-2, R-3, S-4

c) P-1, Q-3, R-2, S-4

d) P-2, Q-1, R-4, S-3

35 / 50

35. Rusting of iron is classified as corrosion because:

a) iron remains at oxidation number throughout

b) iron changes into a noble gas

c) oxygen is always oxidised from to

d) iron undergoes slow oxidation

36 / 50

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

a) the sulphate ion has charge

b) iron has oxidation state

c) the compound contains two iron atoms per formula unit

d) the total charge on the compound is

37 / 50

37. A reaction can be recognised as disproportionation when:

a) one metal displaces another metal from solution

b) two different elements exchange ions without oxidation-number change

c) an acid and a base form salt and water

d) one oxidation state forms two different oxidation states

38 / 50

38. The set containing only non-redox reactions is:

a) and

b) and

c) and

d) and

39 / 50

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

40 / 50

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

a) oxidation and reduction cannot be written as half-reactions

b) no net standard driving force in the written direction

c) the equation must contain no atoms

d) the cell potential must be multiplied by coefficients to become positive

41 / 50

41. For hot concentrated alkali, chlorine can disproportionate as:

The fraction of chlorine atoms oxidised is:

42 / 50

42. The standard reduction potentials are and . For the cell , is:

43 / 50

43. In , a note calls the oxidising agent. The best correction is:

a) is the reducing agent because manganese is reduced

b) is the oxidising agent because it contains hydrogen

c) is the reducing agent; chloride is oxidised

d) no redox process occurs because water is formed

44 / 50

44. The notation for a galvanic cell is written with the anode on the left and cathode on the right. For the reaction , the suitable notation is:

45 / 50

45. The row with the wrong central-atom oxidation number is:

Row	Species	Central atom	Given oxidation number
P
Q
R
S

a) Row Q

b) Row R

c) Row S

d) Row P

46 / 50

46. A reaction has changing to and changing to . Before balancing oxygen and hydrogen, what must be noticed?

a) chromium is reduced and iron is oxidised

b) both chromium and iron are oxidised

c) chromium is oxidised and iron is reduced

d) neither chromium nor iron changes oxidation number

47 / 50

47. An equation-error record shows:

What is the main defect in this proposed acidic-medium equation?

a) is missing, so H and charge are unbalanced

b) should have no oxygen atoms

c) should be written as elemental carbon

d) cannot be a product of oxalate oxidation

48 / 50

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

Column I	Column II
P. Oxidised species	1. Species that undergoes oxidation
Q. Reduced species	2. Species that undergoes reduction
R. Oxidising agent	3. Substance that brings about oxidation of another substance
S. Reducing agent	4. Substance that brings about reduction of another substance

a) P-3, Q-4, R-1, S-2

b) P-4, Q-3, R-2, S-1

c) P-1, Q-2, R-3, S-4

d) P-2, Q-1, R-4, S-3

49 / 50

49. A solution is used in acidic medium, where . What volume of this solution contains equivalents of oxidising capacity?

50 / 50

50. A claim says, “In a galvanic cell, electrons flow from the cathode to the anode because reduction needs electrons.” The best repair is:

a) electrons do not flow in a galvanic cell

b) electrons flow from cathode to anode only in a cell

c) electrons flow through the salt bridge from cathode to anode

d) electrons flow anode to cathode for reduction

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Redox Reactions Mock Test – Class 11 Chemistry

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