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. A displacement reaction is attempted by placing a copper strip in solution. No deposit of zinc appears. The best redox interpretation is:

a) copper is not reactive enough to reduce

b) copper always displaces every metal from solution

c) zinc ions are spectator ions in every possible reaction

d) copper must oxidise to zinc metal

2 / 50

2. 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) change subscripts to make coefficients disappear

d) simplify to the lowest whole-number coefficients

3 / 50

3. In basic medium, chlorine disproportionates as . The oxidation number of chlorine in is:

4 / 50

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

5 / 50

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

a) gains electrons and one loses electron

b) gains electrons and two lose electrons

c) loses electrons and two gain electrons

d) remains unchanged and chlorine only changes physical state

6 / 50

6. A sample of has mass . Its molar mass is , and in acidic medium . The number of equivalents present in the sample is:

7 / 50

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

a) do not change formulas; balance with coefficients

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

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

d) oxygen atoms should be ignored in redox equations

8 / 50

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

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

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

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

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

9 / 50

9. The decomposition is redox because:

a) potassium changes from to

b) all elements keep the same oxidation number

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

d) chlorine is reduced and oxygen is oxidised

10 / 50

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

a) undergo reduction at the cathode

b) donate electrons as a metal in every equation

c) act as a spectator ion

d) undergo oxidation at the anode

11 / 50

11. In a graph for one element during a reaction, the y-axis shows oxidation number and the x-axis shows reaction progress from reactant to product.

The plotted value falls from at the reactant side to at the product side.

The graph represents:

a) no redox change, because both values are positive

b) oxidation, because the element still has a positive value

c) reduction, because the oxidation number decreases

d) oxidation, because the line moves downward

12 / 50

12. An integrated reaction record says:

Copper metal is placed in solution. A grey deposit forms, and the solution becomes blue. The simplified ionic reaction is .

The best complete interpretation is:

a) no redox occurs because the total number of ions in solution changes

b) is oxidised, is reduced, copper acts as reducing agent, and silver deposits

c) is reduced, is oxidised, copper acts as oxidising agent, and silver dissolves

d) nitrate ions are oxidised, copper is a spectator, and the grey deposit is

13 / 50

13. 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:

14 / 50

14. 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

15 / 50

15. A claim says, “The -factor of is always .” The best correction is:

a) -factor is always equal to the number of oxygen atoms

b) -factor depends on the reduction product and medium

c) -factor is not used in redox calculations

d) -factor is always equal to the ionic charge of

16 / 50

16. A half-reaction in acidic medium is:

When this half-reaction is converted to basic medium, what is the first repair step?

a) Add to both sides

b) Remove without adding anything

c) Move to the product side

d) Change into

17 / 50

17. In the halogen order is more reactive than , and is more reactive than . Which reaction is expected to occur?

18 / 50

18. A simplified corrosion note contains these half-processes:

The species reduced in the second half-process is:

19 / 50

19. A compound contains an element with average oxidation number . This is possible because oxidation number can:

a) show only the charge of a free ion

b) show an average value in some compounds

c) replace the molecular formula completely

d) never be fractional

20 / 50

20. 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) cannot be a product of oxalate oxidation

c) should be written as elemental carbon

d) should have no oxygen atoms

21 / 50

21. A formula list gives , , , and . The sequence of oxidation numbers is:

22 / 50

22. A cell is represented as . Why is platinum used in both half-cells?

a) It supplies all ions needed for charge balance

b) It changes into by reacting chemically

c) an inert conductor for redox couples without solid electrodes

d) It acts as a salt bridge between the two solutions

23 / 50

23. A claim says, “Paint protects iron only by changing iron's oxidation number to a safer value.” The better explanation is:

a) paint converts all iron atoms into

b) paint forces oxygen to be oxidised instead of reduced

c) paint acts as a salt bridge for rusting

d) paint forms a barrier to air and moisture

24 / 50

24. A reaction record for acidified permanganate and iron is shown.

Feature	Value or role
Manganese change
Iron change
Medium species
Balanced ratio

The supported conclusion is:

a) is reduced and is the reducing agent

b) is oxidised and is the oxidising agent

c) is reduced and is the reducing agent

d) no redox reaction occurs because acid is present

25 / 50

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

a) the statement is complete for all redox reactions

b) an incomplete early definition of oxidation

c) the statement is useless even for burning reactions

d) the statement applies only to reactions in water

26 / 50

26. A redox titration end point should be close to the equivalence point, where:

a) equal volumes of both solutions must have been mixed

b) reactants have met the redox stoichiometric ratio

c) all ions in the flask must become neutral atoms

d) both solutions must have the same molarity

27 / 50

27. A reaction is called redox mainly because it involves what linked change?

a) Colour change and gas evolution occurring together

b) Heating and cooling occurring at equal rates

c) Dissolving and crystallisation occurring in the same vessel

d) Oxidation and reduction occurring together

28 / 50

28. The net ionic equation shows:

a) both magnesium and copper ions are reduced

b) magnesium is reduced and copper ions are oxidised

c) no redox change because the total charge is balanced

d) magnesium is oxidised and copper ions are reduced

29 / 50

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

a) and

b) and

c) and

d) and

30 / 50

30. In the reaction , the change is best described classically as:

a) reduction, because copper becomes black

b) oxidation, because copper gains oxygen

c) reduction, because oxygen is removed

d) oxidation, because hydrogen is present

31 / 50

31. The Roman numeral in iron chloride tells us that:

a) iron has atomic number

b) iron has oxidation state

c) chlorine has oxidation state

d) the compound contains three chlorine molecules

32 / 50

32. In the acidic half-reaction , nitrogen changes from:

a) to , so electrons are gained

b) to , so electrons are lost

c) to , so electron is gained

d) to , so electron is lost

33 / 50

33. Study the charge record for a proposed ionic equation.

Side	Species written	Total charge
Reactant side
Product side

What does this record show?

a) charge is conserved in the zinc-copper ionic equation

b) redox equations do not need atom balance

c) zinc and copper have no oxidation-number change

d) the equation is impossible because neutral copper appears

34 / 50

34. For the reaction , the oxidising agent is:

35 / 50

35. 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 flow from cathode to anode only in a cell

b) electrons flow anode to cathode for reduction

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

d) electrons do not flow in a galvanic cell

36 / 50

36. The energy conversion in a simple galvanic cell is best described as:

a) redox chemical energy changes into electrical energy

b) electrical energy converted into chemical energy only

c) heat energy converted into nuclear energy

d) light energy converted into oxidation number

37 / 50

37. In the electron-transfer definition, oxidation means:

a) loss of electrons

b) loss of neutrons

c) gain of electrons

d) gain of protons

38 / 50

38. 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 Q and R only

c) Rows R and S only

d) Rows P and Q only

39 / 50

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

a) oxidation because the oxidation number increases from to

b) oxidation because the oxidation number decreases from to

c) no redox change because iron remains iron

d) reduction because the oxidation number increases from to

40 / 50

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

a) electrons add mass to the zinc electrode

b) zinc atoms enter solution as

c) ions plate out as zinc metal

d) sulphate ions become zinc atoms

41 / 50

41. Assertion: is a disproportionation reaction.
Reason: Oxygen in has oxidation number , and it changes to both and .

a) Assertion is true, but Reason is false

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

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

d) Assertion is false, but Reason is true

42 / 50

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

a) false; -factor can depend on reaction and medium

b) false, because equivalent mass is never used in redox

c) true, because equivalent mass is always the same as molar mass

d) true, because -factor is always equal to valency

43 / 50

43. A record gives the change . What does it show?

a) is reduced because it gains an electron

b) is reduced because it loses a proton

c) is oxidised because an electron is written

d) is oxidised because its charge decreases

44 / 50

44. 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 Q

b) Row R

c) Row S

d) Row P

45 / 50

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

46 / 50

46. In , the oxidation number of manganese is:

47 / 50

47. A reaction record says . The best redox classification is:

a) non-redox; oxidation numbers do not change

b) redox, because carbon dioxide is present

c) redox, because calcium oxide contains oxygen

d) redox, because one product is formed

48 / 50

48. A reaction has and . The smallest whole-number ratio of atoms of to atoms of needed for electron balance is:

49 / 50

49. The equivalent mass of an oxidising or reducing agent in a given redox reaction is calculated by:

50 / 50

50. In a simple galvanic cell, the external electron flow is:

a) from salt bridge to both electrodes

b) from cathode to anode

c) from electrolyte to salt bridge only

d) from anode to cathode

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Redox Reactions Mock Test – Class 11 Chemistry

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