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

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Quiz: Redox Reactions – Progressive Test
Total questions: 480
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1 / 50

1. In the reaction , the oxidising agent and reducing agent are respectively:

a) and

b) and

c) and

d) and

2 / 50

2. A balancing note for a redox equation says, “The formula was changed to to balance oxygen.” The best correction is:

a) oxygen atoms should be ignored in redox equations

b) do not change formulas; balance with coefficients

c) changing subscripts is the standard way to balance redox equations

d) the charge on an ion is never important in balancing

3 / 50

3. Use the arrangement described below.

A zinc rod is dipped in solution and a copper rod is dipped in solution. The two solutions are connected by a salt bridge, and the rods are connected by a wire.

If the net reaction is , the zinc electrode acts as:

a) cathode, because electrons leave it

b) salt bridge, because zinc conducts charge

c) anode, because zinc is oxidised

d) cathode, because zinc ions are reduced

4 / 50

4. During a redox titration, using directly as if it were would make the calculated moles:

a) times too small

b) times too large

c) negative

d) unchanged

5 / 50

5. A proposed redox equation has all atoms balanced but the coefficients can all be divided by . The best reporting step is to:

a) leave the larger coefficients because they are still balanced

b) remove all ions from the equation

c) simplify to the lowest whole-number coefficients

d) change subscripts to make coefficients disappear

6 / 50

6. A simple galvanic cell is made from and half-cells. The redox idea behind its operation is:

a) the salt bridge carries electrons from zinc solution to copper solution

b) chemical electron transfer is separated into two electrode processes

c) zinc changes into copper at the anode

d) no oxidation or reduction occurs at either electrode

7 / 50

7. Read the reaction description below.

A strip of metal is placed in a solution containing ions. A coating of metal appears, and ions enter the solution. The net change is .

In this reaction, the electron donor is:

8 / 50

8. A proposed half-reaction is:

The most important correction is:

a) remove oxygen atoms from

b) change into

c) place on the reactant side

d) write on the reactant side

9 / 50

9. In , oxygen is assigned . The average oxidation number of iron is:

10 / 50

10. An equivalent-based titration calculation says . This equality is valid at equivalence because:

a) both solutions must have the same -factor

b) molarities must always be equal

c) oxidising and reducing equivalents are equal

d) volumes of the two solutions must always be equal

11 / 50

11. In the reaction , nitrogen is:

a) reduced from to

b) unchanged at

c) reduced from to

d) oxidised from to

12 / 50

12. A compound contains , , and no peroxide linkage is indicated. The most suitable first assignments for are:

a) ,

b) ,

c) ,

d) ,

13 / 50

13. A standard reduction potential table gives:

Half-reaction

The strongest oxidising agent in the table is:

14 / 50

14. In comparing values, the species with the more positive reduction potential is more likely to:

a) undergo reduction at the cathode

b) act as a spectator ion

c) undergo oxidation at the anode

d) donate electrons as a metal in every equation

15 / 50

15. The electron-flow direction in a simple redox reaction is best stated as:

a) from reducing agent to oxidising agent

b) from the substance with more atoms to the substance with fewer atoms

c) from oxidising agent to reducing agent

d) from reduced product to oxidised product only

16 / 50

16. A balanced equation is reported as . The main reporting issue is:

a) chlorine cannot appear as

b) use lowest whole-number coefficients

c) iron cannot have different oxidation states

d) the equation is not atom-balanced

17 / 50

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

18 / 50

18. In acidic medium, can be reduced either to or to . The -factors of nitrate in these two cases are respectively:

a) and

b) and

c) and

d) and

19 / 50

19. Copper shows different oxidation states in and . The oxidation numbers of copper in these compounds are:

a) and

b) and

c) and

d) and

20 / 50

20. The balanced equation is supported by which electron-change relation?

a) loses electrons and two gain electrons

b) gains electrons and one loses electron

c) remains unchanged and chlorine only changes physical state

d) gains electrons and two lose electrons

21 / 50

21. A proposed acidic half-reaction is . The error is:

a) water should never appear in acidic medium

b) manganese atoms are not balanced

c) oxygen atoms are not balanced

d) electrons are on the product side

22 / 50

22. Rusting of iron is commonly introduced as an oxidation process because iron:

a) loses its metallic colour only

b) separates from oxygen to form pure metal

c) combines with oxygen in moist air

d) changes into a liquid

23 / 50

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

a) reduction by gain of two electrons

b) no redox change because both values are positive

c) oxidation by gain of two electrons

d) oxidation by loss of two electrons

24 / 50

24. The reaction has . The oxidised and reduced species are respectively:

a) and

b) and

c) and

d) and

25 / 50

25. Study the exception table and choose the row that needs correction.

Row	Species	Oxidation number asked	Assigned value
P
Q
R
S

a) Row R

b) Row Q

c) Row S

d) Row P

26 / 50

26. Rusting of iron is classified as corrosion because:

a) oxygen is always oxidised from to

b) iron changes into a noble gas

c) iron undergoes slow oxidation

d) iron remains at oxidation number throughout

27 / 50

27. In a balanced redox equation, electrons do not appear in the final overall equation because:

a) electrons are ignored when ionic equations are written

b) electrons are not involved in redox reactions

c) electrons lost and gained cancel during addition

d) electrons are converted into atoms during balancing

28 / 50

28. A neutral compound has the formula . If oxygen is assigned , the oxidation number of is:

29 / 50

29. Use the situation below.

An iron nail is left in moist air for several days. A reddish-brown coating forms. A similar dry iron nail kept in a sealed dry tube changes very little over the same time.

The best explanation is:

a) water prevents all electron transfer

b) dry air changes iron directly into faster

c) rusting is only a physical deposition of dust

d) moisture helps the redox corrosion process occur on iron

30 / 50

30. 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 R

b) Row S

c) Row P

d) Row Q

31 / 50

31. 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 S

c) Row P

d) Row Q

32 / 50

32. A student sees and says aluminium ion is the strongest oxidising agent because the magnitude is large. The best correction is:

a) aluminium cannot take part in redox reactions

b) negative makes the strongest oxidising agent

c) is hard to reduce; is reductant

d) magnitude alone decides oxidising strength without sign

33 / 50

33. Assertion: When changes to , reduction occurs.
Reason: Reduction can decrease the positive charge on a species by gain of electrons.

a) Assertion is true, but Reason is false

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

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

d) Assertion is false, but Reason is true

34 / 50

34. 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:

a) analyte is consumed by redox stoichiometry

b) titrant volume has no relation to reaction progress

c) redox titrations do not follow mole ratios

d) analyte concentration increases as titrant is added

35 / 50

35. The molar mass of is . Its equivalent mass is calculated for three media: acidic , neutral , and strongly basic . The correct order of equivalent masses is:

a) neutral acidic strongly basic

b) strongly basic neutral acidic

c) acidic neutral strongly basic

d) acidic neutral strongly basic

36 / 50

36. For , the oxidation number of oxygen is:

37 / 50

37. A combination reaction is redox when:

a) one product forms with an oxidation-number change

b) a precipitate forms from two aqueous salt solutions

c) two or more reactants form one product without any oxidation-number change

d) an acid and a base form salt and water

38 / 50

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

39 / 50

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

40 / 50

40. Cell notation represents:

a) only a precipitation reaction between and

b) zinc half-cell left, copper half-cell right, salt bridge between

c) a single solution containing all species mixed together

d) copper half-cell on the left and zinc half-cell on the right, with no salt bridge

41 / 50

41. The pattern represents:

a) neutralisation because positive ions are present

b) disproportionation because forms two products

c) comproportionation to an intermediate oxidation state

d) precipitation because charges disappear

42 / 50

42. 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, but Reason does not explain Assertion

b) Assertion is true, but Reason is false

c) Assertion is false, but Reason is true

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

43 / 50

43. The substance acting as the oxidising agent is identified by which oxidation-number change?

a) The reactant containing the maximum number of oxygen atoms in all cases

b) The substance containing the atom whose oxidation number decreases

c) The product with the largest coefficient

d) The substance containing the atom whose oxidation number increases

44 / 50

44. Oxidation-number change can identify redox reactions because:

a) increase in oxidation number means oxidation and decrease means reduction

b) increase in oxidation number means reduction and decrease means oxidation

c) every reaction with ions is automatically non-redox

d) every reaction with oxygen is automatically non-redox

45 / 50

45. A table lists acidic half-reactions. Which row has the electron side correct?

Row	Half-reaction type	Electron placement
P		on reactant side
Q		on reactant side
R		on reactant side
S		on reactant side

a) Row P only

b) Rows P and Q only

c) Rows Q and R only

d) Rows R and S only

46 / 50

46. In metal extraction using carbon monoxide, , the practical role of is:

a) oxidising agent, because carbon changes from to

b) spectator gas, because carbon oxidation number is unchanged

c) precipitating agent, because iron forms a solid

d) reducing agent, because carbon changes from to

47 / 50

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

a) changes oxidation into reduction

b) supplies electrons directly to the cathode

c) prevents any ions from moving between half-cells

d) ions move to maintain electrical neutrality

48 / 50

48. The thermal decomposition is redox because:

a) mercury decreases from to , while oxygen increases from to

b) oxygen is present on both sides, so no redox change occurs

c) mercury and oxygen both remain unchanged

d) mercury increases from to , while oxygen decreases from to

49 / 50

49. A reducing agent has molar mass . In a given reaction, one formula unit of loses electrons. What mass of contains equivalents?

50 / 50

50. Match the displacement feature in Column I with the correct interpretation in Column II.

Column I	Column II
P.	1. oxidation of the displacing metal
Q.	2. reduction of the displaced ion
R. unchanged	3. spectator ion behaviour
S.	4. net ionic redox equation

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

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Redox Reactions Mock Test – Class 11 Chemistry

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