Exam-Style Mock Test | Class 11 Chemistry: Equilibrium

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Quiz: Equilibrium – Certificate Challenge
Total questions: 453
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Time allotted: 100 minutes
Certificate pass score: 70%
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Equilibrium – Progressive Test

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1 / 50

1. The solubility of a gas in a liquid generally increases when the pressure of the gas above the liquid is increased at constant temperature because

a) pressure removes the need for gas-liquid equilibrium

b) the gas molecules lose their chemical identity

c) the liquid becomes a solid under all pressures

d) more gas particles contact the liquid surface

2 / 50

2. A graph record shows a sudden vertical drop in for , followed by gradual increases in and gradual decreases in and . The disturbance was most likely

a) removal of

b) increase in container volume only

c) addition of a catalyst only

d) addition of

3 / 50

3. In a mixed equilibrium problem, the solution contains a weak base , its conjugate acid , and a salt whose cation hydrolyses. The most reliable way to begin is to

a) assume is always neutral

b) use for any weak base

c) choose the relevant equilibrium constant

d) use for every ion in the solution

4 / 50

4. For , the initial concentration of is , and no is present. If , then is

5 / 50

5. For , each of and is taken initially, and . If is the equilibrium concentration of , the equation to solve is

6 / 50

6. At , the relation between and is

7 / 50

7. A expression for is being checked. The exponent on must be because

a) is the third letter in the equation

b) aqueous species always receive exponent

c) there are three different species in the reaction

d) is a product with coefficient

8 / 50

8. A solution of is basic because

a) acetate ion is the conjugate acid of a strong base

b) sodium acetate behaves as a strong acid salt

c) acetate ion produces by hydrolysis

d) forms completely in water

9 / 50

9. For , at . Using , is closest to

10 / 50

10. The quantity that most directly tells how much solute is present in a given volume of solution is

a) reaction rate

b) concentration

c) pressure

d) temperature

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11. A rate-time record for a reversible reaction is given below.

Stage	Forward rate	Reverse rate
P	High	Nearly zero
Q	Decreasing	Increasing
R	Equal to reverse rate	Equal to forward rate

The stage representing dynamic equilibrium is

a) none of the stages

b) R

c) Q

d) P

12 / 50

12. Two equilibria are given:

For the overall reaction , the equilibrium constant is

13 / 50

13. A mixed aqueous system contains a weak acid , its salt , and a sparingly soluble salt . The ion is important because it is

a) a gas whose pressure controls

b) absent from all equilibrium expressions

c) common to both equilibria

d) always a strong acid in water

14 / 50

14. A buffer contains of and of in . If of strong acid is added and volume change is neglected, , and , the new is closest to

15 / 50

15. The expression for a weak acid becomes when

a) is very close to

c) the acid is completely ionized

16 / 50

16. In expressions, a dissolved species such as is not written as a pressure term because

a) ions cannot take part in equilibrium

b) all dissolved ions have zero concentration

c) uses partial pressures only for gaseous species

d) aqueous species must always be placed in the numerator

17 / 50

17. A vessel contains . At equilibrium, and . The value of is

18 / 50

18. Assertion: Adding a product to an equilibrium mixture at fixed temperature can make the reaction shift in the reverse direction.
Reason: Adding product makes the reaction quotient larger than the equilibrium constant for many product-over-reactant expressions.

a) The assertion is false, but the reason is true

b) Both assertion and reason are true, and the reason explains the assertion

c) Both assertion and reason are true, but the reason does not explain the assertion

d) The assertion is true, but the reason is false

19 / 50

19. For a gaseous reaction, even though the reaction is not trivial. This can happen when

c) all reactants are removed

20 / 50

20. A graph shows suddenly becoming greater than after a disturbance. The next spontaneous change should make

a) reactants form until returns to

b) all concentrations become equal

c) become zero at fixed temperature

d) more products form until increases further

21 / 50

21. A weak acid has . Using , the degree of ionization is

22 / 50

22. Assertion: A catalyst does not change the equilibrium composition of a reversible reaction.
Reason: A catalyst changes the rates of both forward and reverse reactions without changing the equilibrium condition.

a) Both assertion and reason are true, but the reason does not explain the assertion

b) The assertion is false, but the reason is true

c) Both assertion and reason are true, and the reason explains the assertion

d) The assertion is true, but the reason is false

23 / 50

23. At , . If of a conjugate acid is , the of its conjugate base is

24 / 50

24. In a solution, the molar solubility of is calculated using . The approximate solubility is

25 / 50

25. A reaction has for . The value of for and for , respectively, is

a) and

b) and

c) and

d) and

26 / 50

26. The pressure equilibrium constant is most suitable when the equilibrium expression is written using

a) colour intensities of products

b) molar masses of all species

c) gaseous partial pressures

d) masses of pure solids only

27 / 50

27. In a saturated solution at fixed temperature, adding a small amount of would tend to

a) dissolve more because chloride is a product ion

b) decrease the solubility of

c) increase of

d) remove all solid instantly

28 / 50

28. A reaction has , , , and . The value of is closest to

29 / 50

29. A conductivity test is performed on equal-concentration aqueous solutions. One solution lights the bulb brightly, another lights it dimly, and a third does not light it. The most suitable classification is

a) bright: non-electrolyte; dim: strong electrolyte; no light: weak electrolyte

b) bright: pure solvent; dim: strong electrolyte; no light: strong electrolyte

c) bright: weak electrolyte; dim: non-electrolyte; no light: strong electrolyte

d) bright: strong electrolyte; dim: weak electrolyte; no light: non-electrolyte

30 / 50

30. The notation shows that acetic acid

a) ionizes partially and reversibly in water

b) forms only solid particles in water

c) ionizes completely like a strong electrolyte

d) is a non-electrolyte with no ions in solution

31 / 50

31. For a reversible reaction at equilibrium, the forward rate is . The reverse rate at the same instant is

32 / 50

32. A salt has . In one solution, and . The best conclusion is

a) precipitation does not occur because

b) precipitation occurs because

c) the solution is exactly saturated

d) precipitation occurs because one ion concentration is small

33 / 50

33. Use the table to identify the set that matches an equilibrium state.

Set	Forward rate	Reverse rate	Observed composition with time
P	Greater than reverse rate	Smaller than forward rate	Changing
Q	Equal to reverse rate	Equal to forward rate	Constant
R	Zero	Zero	Constant because all motion stops
S	Smaller than reverse rate	Greater than forward rate	Changing

a) Set R

b) Set Q

c) Set P

d) Set S

34 / 50

34. Equal volumes of and are mixed. If , the mixture is

a) unsaturated, so no precipitates

b) saturated exactly at equilibrium

c) supersaturated, so precipitates

d) impossible to judge because equal volumes are used

35 / 50

35. The molar solubility of a sparingly soluble salt means

a) the value of for every salt

b) moles per litre in saturated solution

c) the mass of undissolved solid only

d) the concentration of solvent molecules

36 / 50

36. For the equilibrium , , and initially , . Using the small- approximation, the approximate value of in , is

37 / 50

37. The table gives pressure disturbances for gaseous equilibria.

Case	Change	Reaction feature	Predicted shift
P	Compression	Products have fewer gaseous moles	Toward products
Q	Expansion	Products have more gaseous moles	Toward products
R	Compression	Both sides have equal gaseous moles	No pressure-based shift
S	Expansion	Reactants have fewer gaseous moles	Toward reactants

The row that does not match the pressure-volume rule is

a) Q

b) S

c) P

d) R

38 / 50

38. A sealed vessel contains a solid in equilibrium with its saturated solution at fixed temperature. If a few dissolved particles crystallize, the concentration of the solution does not fall permanently because

a) crystallization is impossible in a saturated solution

b) particles dissolve from the solid at the same rate

c) solvent particles change into solute particles

d) the system becomes chemically inactive

39 / 50

39. An acidic buffer is diluted by adding water, but the ratio remains unchanged. The will remain nearly unchanged because

a) becomes zero on dilution

b) depends on the concentration ratio

c) water removes all conjugate base from solution

d) dilution always makes every solution neutral

40 / 50

40. A salt solution is made from an anion that is the conjugate base of a weak acid and a cation from a strong base. The hydrolysis reaction most directly responsible for basicity is

41 / 50

41. The thermodynamic relation connecting standard Gibbs energy change and equilibrium constant is

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42. In the Contact process, is exothermic. Increasing pressure favours formation because

a) products have more gaseous moles than reactants

b) oxygen is omitted from pressure calculations

c) products have fewer gaseous moles

d) is a pure solid

43 / 50

43. A reaction list contains these equilibria:

Case	Equilibrium	Classification claim
P		Homogeneous
Q		Homogeneous
R		Homogeneous
S		Heterogeneous

The claim that needs correction is

a) S

b) R

c) Q

d) P

44 / 50

44. A comparison table for and is shown.

Case	Reaction feature	Expected relation
P
Q
R
S

The row that needs correction is

a) Q

b) P

c) S

d) R

45 / 50

45. For , . A current mixture has and . The system is

a) shifting in reverse

b) impossible because

c) at equilibrium

d) shifting forward

46 / 50

46. A product is removed from the equilibrium mixture at constant temperature. The immediate response is best described as

a) a shift toward products

b) a shift toward reactants

c) a change in without any shift

d) no change because product concentration is irrelevant

47 / 50

47. An equilibrium gas mixture has total pressure . The mole fractions are , , and . The partial pressure of is

48 / 50

48. A sample of undergoes . If , the equilibrium concentration of is

49 / 50

49. The statement “Changing temperature shifts equilibrium but never changes ” should be repaired as

a) temperature change changes only, while is always fixed

b) temperature change affects only solid equilibria

c) temperature change stops both forward and reverse reactions

d) temperature change can shift equilibrium and can change

50 / 50

50. The pair and is a conjugate acid-base pair because

a) one proton differs

b) they have the same charge

c) they differ by two protons

d) both must be strong acids

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Equilibrium Mock Test – Class 11 Chemistry

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