Exam-Style Mock Test | Class 11 Chemistry: Equilibrium

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Quiz: Equilibrium – Certificate Challenge
Total questions: 453
Questions to attempt: 100 random
Time allotted: 100 minutes
Certificate pass score: 70%
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Certificate: Yes
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Progressive Test — Guest First Round

Equilibrium – Progressive Test

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1 / 50

1. For , of is taken initially. If the degree of dissociation is and total pressure is , is

2 / 50

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

a) all concentrations become equal

b) become zero at fixed temperature

c) more products form until increases further

d) reactants form until returns to

3 / 50

3. A physical equilibrium can be recognized most safely by

a) formation of a new chemical substance

b) complete absence of molecular motion

c) constant properties with rate balance

d) equal masses of the two phases

4 / 50

4. A solution at has . The hydrogen ion concentration is

5 / 50

5. The blank in the statement is best filled by: At dynamic equilibrium, the forward rate is ______ the reverse rate.

a) greater than

b) unrelated to

c) smaller than

d) equal to

6 / 50

6. For the same pure liquid in a closed vessel, vapour pressure at equilibrium is higher at than at because

a) higher temperature helps molecules escape the liquid

b) higher temperature removes all vapour molecules from the vessel

c) condensation becomes impossible at

d) temperature changes the chemical identity of every liquid molecule

7 / 50

7. The table lists four descriptions of physical systems.

System	Description
P	Water in an open dish slowly evaporates into the room
Q	Ice and water coexist at the melting point under fixed pressure
R	Dry salt is heated until it decomposes
S	Gas escapes continuously from an uncorked soda bottle

The system best representing physical equilibrium is

a) P

b) Q

c) S

d) R

8 / 50

8. A solution is made by mixing of with of . If , the initial precipitation decision is

a) exactly saturated

b) impossible because the volumes are unequal

c) precipitation occurs

d) no precipitation occurs

9 / 50

9. 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

10 / 50

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

a) is a product with coefficient

b) is the third letter in the equation

c) aqueous species always receive exponent

d) there are three different species in the reaction

11 / 50

11. A reversible reaction is written as . If the temperature is increased, the equilibrium shifts

a) toward

b) toward the side with lower concentration only

c) neither way because heat is not a substance

d) toward

12 / 50

12. A weak acid has and concentration . Using , the approximate is

13 / 50

13. In a closed vessel containing liquid water and its vapour, the measurable property that becomes constant at fixed temperature is

a) the chemical formula of water

b) the colour of water

c) the vapour pressure of water

d) the molar mass of water

14 / 50

14. A solution of a salt of weak acid and strong base has parent acid . At , using , the approximate is closest to

15 / 50

15. A solution contains less dissolved solute than its solubility limit at the same temperature. The best description of the solution is

a) in solid-solution equilibrium with excess solid

b) unable to dissolve any more solute

c) saturated

d) unsaturated

16 / 50

16. The molar solubility of a sparingly soluble salt means

a) the mass of undissolved solid only

b) the concentration of solvent molecules

c) moles per litre in saturated solution

d) the value of for every salt

17 / 50

17. A reversible reaction has at a fixed temperature. This value most directly suggests that

a) the reaction has no forward or reverse movement

b) product and reactant terms are comparable

c) all individual concentrations must be exactly

d) the reaction can never respond to disturbance

18 / 50

18. A reversible reaction has at a certain temperature. The sign of for the written reaction is

a) negative

b) unrelated to

c) positive

d) always zero

19 / 50

19. For , at . Using , is closest to

20 / 50

20. A metal hydroxide has . If , the needed to just begin precipitation is

21 / 50

21. Equilibrium constants for two reactions are given:

For , the equilibrium constant is

22 / 50

22. The unit of for , when concentration is reported in , is

a) no unit because every is unitless

23 / 50

23. A data record gives two equilibrium mixtures for the same reaction at the same temperature.

Mixture
P
Q

The best conclusion is that

a) only mixture Q can be at equilibrium

b) neither can be at equilibrium because

c) both give the same ratio

d) only mixture P can be at equilibrium

24 / 50

24. A claim about equilibrium says, “The reaction has finished because the composition is constant.” The better interpretation is that

a) constant composition means the reaction is dynamic but balanced

b) constant composition means the reactants and products are equal in mass

c) constant composition means every molecule has stopped moving

d) constant composition means the reverse reaction is impossible

25 / 50

25. A basic buffer contains of and of . If of strong acid is added, , and , the final at is closest to

26 / 50

26. Selective precipitation is possible when

a) all salts have exactly the same

b) common ions increase the solubility of every salt equally

c) is never compared with

d) precipitates form at different ion-product values

27 / 50

27. A basic buffer has , , and the temperature is . Its is

28 / 50

28. A strong electrolyte differs from a weak electrolyte because a strong electrolyte

a) always has a higher concentration than a weak electrolyte

b) never forms ions in water

c) ionizes almost completely in water

d) conducts only in the solid state

29 / 50

29. A table summarizes four equilibrium disturbances.

Case	System	Disturbance	Expected response
P	Weak acid	Add	Ionization suppressed
Q		Add	Solubility decreases
R		Increase volume	Shifts toward
S	Exothermic forward reaction	Increase temperature	Shifts forward

The row that needs correction is

a) P

b) S

c) Q

d) R

30 / 50

30. 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) use for every ion in the solution

b) assume is always neutral

c) choose the relevant equilibrium constant

d) use for any weak base

31 / 50

31. A sealed soda bottle contains dissolved under pressure. When the bottle is opened, bubbles appear mainly because

a) lower pressure reduces its solubility

b) changes into solid carbon instantly

c) the external pressure on suddenly increases

d) water stops containing molecules

32 / 50

32. A solution contains and . The ionic product for is

33 / 50

33. For a salt of a weak acid and weak base at , and . Using , the solution is

a) strongly basic with

b) acidic with

c) basic with

d) neutral with

34 / 50

34. A catalyst is added to a reversible reaction already at equilibrium. The catalyst will

a) increase the equilibrium constant

b) decrease the equilibrium constant

c) change the equilibrium composition toward products

d) leave the equilibrium composition unchanged

35 / 50

35. A catalyst is added to a reversible reaction mixture before equilibrium is reached. The most suitable effect is that the catalyst

a) helps both directions proceed faster and equilibrium is reached sooner

b) increases only the reverse reaction rate

c) changes the required condition from equal rates to equal concentrations

d) increases only the forward reaction rate

36 / 50

36. 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) P

b) R

c) none of the stages

d) Q

37 / 50

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

a) dilution always makes every solution neutral

b) becomes zero on dilution

c) water removes all conjugate base from solution

d) depends on the concentration ratio

38 / 50

38. Two equilibria are given:

For the overall reaction , the equilibrium constant is

39 / 50

39. A weak acid has . Without using the small- approximation, the equation for is

40 / 50

40. In an ICE table for an equilibrium calculation, the letter represents

a) the catalyst used in the reaction

b) the concentration unit written in the table only

c) the colour of the equilibrium mixture

d) the concentration change toward equilibrium

41 / 50

41. A liquid-vapour equilibrium fails to establish in an open container mainly because

a) pressure has no connection with vapour particles

b) the liquid becomes a solid at ordinary temperature

c) vapour is not retained for condensation

d) the liquid molecules cannot escape from the surface

42 / 50

42. An electrolyte is a substance that conducts electricity in aqueous solution mainly because it

a) changes water into a metal

b) produces only neutral molecules in solution

c) prevents movement of all particles

d) produces ions in solution

43 / 50

43. A solution contains and . Adding can precipitate , while adding can precipitate . The correct calculation choice is

a) use because only two ion symbols appear

b) use the correct expression for each salt

c) use the same expression for both salts

d) use for every salt

44 / 50

44. At , a salt is formed from a weak acid with and a strong base. The hydrolysis constant of its anion is

45 / 50

45. A solution of and a solution of are compared. The safer statement is that

a) is stronger despite being more dilute

b) a dilute acid can never be strong

c) is stronger because its concentration is larger

d) both acids have equal strength because both contain hydrogen

46 / 50

46. The conjugate acid of is

47 / 50

47. For , the reaction quotient is

a) using current concentrations

b) using equilibrium concentrations only

c) using current concentrations

d) using current concentrations

48 / 50

48. The ionization of a monoprotic weak acid is represented as . The expression for is

49 / 50

49. For , the value of at a fixed temperature depends on

a) the total mass of the balance used in the laboratory

b) the equilibrium concentrations of the three gases

c) the order in which formulas are copied in a notebook

d) the colour of the reaction vessel

50 / 50

50. For , . The equilibrium constant for is

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Equilibrium Mock Test – Class 11 Chemistry

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Equilibrium – Progressive Test

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