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
Pass score: 60%
Total rounds: 10
Current round: 1^st
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Quiz: Redox Reactions – Certificate Challenge
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1 / 50

1. For a balanced redox equation, the basic conservation requirement is that:

a) only the number of molecules must be equal on both sides

b) atoms and total charge must be conserved

c) only the mass of solid substances must be conserved

d) the same physical states must appear on both sides

2 / 50

2. Read the reaction record.

Chlorine gas reacts with cold dilute alkali to form chloride and hypochlorite ions. The simplified ionic change may be written as .

This reaction is called disproportionation because:

a) chlorine is only oxidised from to in the products

b) chlorine is only reduced from to in the products

c) chlorine is both reduced to and oxidised to

d) hydroxide ion is both oxidised and reduced

3 / 50

3. For elemental chlorine , chlorine is assigned the oxidation number:

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4. A statement says, “The cathode is always negative because it receives electrons.” The most careful correction is:

a) the cathode is defined by oxidation, so it cannot receive electrons

b) the cathode is always positive in every cell

c) cathode means reduction; its sign depends on cell type

d) the cathode is the salt bridge, so sign is meaningless

5 / 50

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

a) chlorine cannot appear as

b) the equation is not atom-balanced

c) iron cannot have different oxidation states

d) use lowest whole-number coefficients

6 / 50

6. Match each idea in Column I with its correct electron-transfer meaning in Column II.

Column I	Column II
P. Oxidation	1. Loss of electrons
Q. Reduction	2. Gain of electrons
R. Oxidising agent	3. Electron acceptor
S. Reducing agent	4. Electron donor

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

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

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

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

7 / 50

7. A acidified solution reacts with according to . If of is used, the moles of that reacted are:

8 / 50

8. A notebook pairs some changes with classical labels. The unsupported pairing is:

Row	Change	Label
P		Oxidation
Q		Reduction
R	Loss of hydrogen from a substance	Oxidation
S	Addition of hydrogen to a substance	Oxidation

a) Row P

b) Row Q

c) Row S

d) Row R

9 / 50

9. The thermal decomposition is redox because:

a) mercury and oxygen both remain unchanged

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

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

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

10 / 50

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

The fraction of chlorine atoms oxidised is:

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11. A reaction-classification table is prepared.

Row	Reaction	Classification
P		redox combination
Q		non-redox decomposition
R		disproportionation
S		redox displacement

The row that needs correction is:

a) Row S

b) Row P

c) Row R

d) Row Q

12 / 50

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

13 / 50

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

14 / 50

14. 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 converted into atoms during balancing

c) electrons are not involved in redox reactions

d) electrons lost and gained cancel during addition

15 / 50

15. The cell notation corresponds to which standard cell-potential expression?

16 / 50

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

17 / 50

17. A complete redox reaction can be built only when:

a) the charges of all individual ions become zero

b) both half-reactions have electrons on the product side

c) both half-reactions have electrons on the reactant side

d) the two half-reactions involve equal electrons

18 / 50

18. A table compares two reactions.

Reaction	Observation or type	Redox decision
P.	white precipitate	?
Q.	metal displacement	?

The correct decisions for P and Q are:

a) P = non-redox, Q = non-redox

b) P = non-redox, Q = redox

c) P = redox, Q = non-redox

d) P = redox, Q = redox

19 / 50

19. In , the total number of electrons lost by aluminium atoms is:

20 / 50

20. The coefficient before in affects:

a) electron balance, not

b) the standard reduction potential, making it

c) the charge on each ion

d) the identity of

21 / 50

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

22 / 50

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

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

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

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

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

23 / 50

23. A graph description is given for a working cell.

The x-axis shows time. One y-axis curve shows mass of zinc electrode, and another shows mass of copper electrode. The zinc curve slopes downward, while the copper curve slopes upward.

The graph is consistent with:

a) oxidation at zinc and reduction at copper

b) no redox reaction in either half-cell

c) reduction at zinc and oxidation at copper

d) electron flow through the salt bridge

24 / 50

24. Study the table and find the unsupported oxidation-number assignment.

Row	Species	Assigned oxidation number of the underlined element
P
Q
R
S

a) Row S

b) Row R

c) Row Q

d) Row P

25 / 50

25. A statement says, “The anode has the lower reduction potential in a spontaneous galvanic cell.” This is generally:

a) correct only if both electrodes are made of the same metal

b) lower reduction potential half-cell runs as oxidation

c) incorrect, because the anode must have the highest reduction potential

d) incorrect, because anodes are never involved in redox

26 / 50

26. 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) single displacement

b) acid-base neutralisation

c) disproportionation

d) ionic precipitation

27 / 50

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

a) oxidation by loss of two electrons

b) oxidation by gain of two electrons

c) reduction by gain of two electrons

d) no redox change because both values are positive

28 / 50

28. A cell note says:

The notation is . During operation, copper electrode mass decreases and silver deposits on the silver electrode.

The net reaction represented by the note is:

29 / 50

29. The standard hydrogen electrode is assigned a potential of:

30 / 50

30. A half-reaction pair is multiplied before adding because:

a) all coefficients in chemistry must be even numbers

b) coefficients must make the electrons cancel

c) oxidation half-reactions cannot contain ions

d) reduction half-reactions must be written without charge

31 / 50

31. Consider the following statements about oxidation number.
I. It helps identify oxidation and reduction in many reactions.
II. It is always identical to actual charge on an atom in a covalent molecule.
III. It is assigned by rules and used for electron bookkeeping.

a) II and III only

b) I, II and III

c) I and II only

d) I and III only

32 / 50

32. A reaction note contains the half-changes and . In this reaction, the reducing agent is:

33 / 50

33. Zinc placed in solution gives the reaction . Why is this reaction still treated as redox even though no oxygen or hydrogen transfer is shown?

a) precipitates with zinc

b) Copper forms a coloured solution

c) Zinc transfers electrons to

d) Zinc changes physical state to

34 / 50

34. Select the row that is not a disproportionation pattern.

Row	Oxidation-number pattern for one element	Decision
P	and	disproportionation
Q	and	disproportionation
R	and	disproportionation
S	for one element and for a different element	disproportionation

a) Row R

b) Row P

c) Row S

d) Row Q

35 / 50

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

a) separates from oxygen to form pure metal

b) loses its metallic colour only

c) combines with oxygen in moist air

d) changes into a liquid

36 / 50

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

37 / 50

37. A description says, “Oxidation always means addition of oxygen.” The most careful conclusion is:

a) the statement is complete for all redox reactions

b) the statement applies only to reactions in water

c) the statement is useless even for burning reactions

d) an incomplete early definition of oxidation

38 / 50

38. For the qualitative order as oxidising agents, the strongest reducing ion among , , and is:

39 / 50

39. A compact cell problem gives and . The standard cell has:

40 / 50

40. In ordinary oxides such as , , and , oxygen is generally assigned:

41 / 50

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

a) salt bridge, because charge appears

b) cathode, because metal ions are formed

c) cathode, because electrons are produced

d) anode, because oxidation occurs

42 / 50

42. A redox equation is atom-balanced but has unequal total charge on the two sides. What conclusion is most suitable?

a) The equation is fully balanced because atoms are enough

b) The equation is incomplete for an ionic redox reaction

c) The equation becomes balanced by changing subscripts in formulas

d) The equation must be non-redox

43 / 50

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

a) ,

b) ,

c) ,

d) ,

44 / 50

44. In acidic medium, is reduced to . What is the -factor of in this reaction?

45 / 50

45. In the redox reaction , of dichromate reacts with how many moles of ?

46 / 50

46. In electrode-process language, oxidation always occurs at the:

a) electrolyte surface only

b) anode

c) cathode

d) salt bridge

47 / 50

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

48 / 50

48. A table lists possible reduction products of .

Medium	Reduction product	-factor of
P. Acidic
Q. Neutral or mildly basic
R. Strongly basic
S. Acidic

Which row needs correction?

a) Row P

b) Row S

c) Row R

d) Row Q

49 / 50

49. 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

50 / 50

50. A solution is used in acidic medium. The -factor of dichromate is . Its normality is:

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Redox Reactions Mock Test – Class 11 Chemistry

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