MDCAT XI Chemistry Chemical Equilibrium Online Test

544

Created on July 25, 2025 By

📚 Test Details

Subject: Chemistry
Class: 1st year / XI
Chapter: Chemical Equilibrium
Test: 2
Book: Sindh Textbook
Total No. Of MCQs: 50 MCQs
Time Allowed: 50 Minutes

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1 / 50

1. A large Kc value indicates that at equilibrium:

a) mostly products

b) mostly reactants

c) equal amounts

d) none

2 / 50

2. For H₂ + I₂ ⇌ 2HI, which condition increases HI yield?

a) raise pressure

b) lower temperature

c) add I₂

d) add catalyst

3 / 50

3. In exothermic equilibrium, increasing temperature shifts the reaction toward:

a) reactants

b) products

c) no change

d) catalyst side

4 / 50

4. Units of Kₚ vs. Kc differ due to:

a) phases

b) pressure vs concentration

c) temperature

d) catalysts

5 / 50

5. Kc has no units when:

a) equal gas moles

b) more reactants

c) more products

d) solids present

6 / 50

6. In NH₄OH + NH₄Cl buffer, adding NH₄Cl reduces OH⁻ due to:

a) common ion effect

b) oxidation

c) hydrolysis

d) Le Chatelier’s principle

7 / 50

7. For N₂ + 3H₂ ⇌ 2NH₃, equilibrium shifts right when:

a) T↑ and P↑

b) T↓ and P↑

c) P↓

d) temp unaffected

8 / 50

8. Expression for 2A + B ⇌ 3C:

a) [C]³/[A]²[B]

b) [C]/[A]²[B]

c) [A]²[B]/[C]³

d) [C]²/[AB]

9 / 50

9. Which does affect Kc?

a) catalyst

b) temperature

c) pressure

d) concentration

10 / 50

10. When Q < Kc:

a) shifts to reactants

b) to products

c) at equilibrium

d) stops

11 / 50

11. Buffer action works due to:

a) Le Chatelier

b) ion product

c) common ion

d) dynamic equilibrium

12 / 50

12. A large Kc means reaction favors:

a) forward

b) reverse

c) unchanged

d) catalyst

13 / 50

13. Solubility of Ca(OH)₂ decreases with:

a) ↑T

b) ↓T

c) ↑P

d) adding salt

14 / 50

14. Not a reversible reaction property:

a) ⇌ arrow

b) one direction

c) dynamic

d) products re-form reactants

15 / 50

15. In N₂ + 3H₂ ⇌ 2NH₃, adding N₂ shifts reaction move

a) right

b) left

c) unchanged

d) stops

16 / 50

16. Law of Mass Action by:

a) Guldberg & Waage

b) Arrhenius

c) Le Chatelier

d) Bronsted

17 / 50

17. Kₚ falls with rising T in which exothermic equilibrium?

a) 2SO₂ + O₂ ⇌ 2SO₃

b) N₂ + 3H₂ ⇌ 2NH₃

c) H₂ + Cl₂ ⇌ 2HCl

d) all

18 / 50

18. Dynamic equilibrium:

Dynamic equilibrium:

a) forward = reverse rates

b) equal concentration

c) stops

d) reversible becomes irreversible

19 / 50

19. Q gives:

a) Kc

b) reaction direction

c) catalyst effect

d) speed of reaction

20 / 50

20. Catalyst:

a) speeds both sides

b) increases products

c) changes Kc

d) raises temp

21 / 50

21. Kc units for H₂ + I₂ ⇌ 2HI:

a) mol·dm⁻³

b) mol²·dm⁻⁶

c) mol²·dm⁻³

d) none

22 / 50

22. Equal moles both sides → Kc units:

a) dm⁻³

b) mol·dm⁻³

c) mol²·dm⁻⁶

d) none

23 / 50

23. C ⇌ A + B; Kc increase if temperature increases then reaction is:

a) endothermic

b) exothermic

c) neutral

d) irreversible

24 / 50

24. Which reaction doesn’t reach equilibrium?

a) irreversible

b) closed system

c) reversible

d) buffered

25 / 50

25. If Q > Kc, reaction shifts:

a) reactants side

b) products side

c) no shift

d) catalyst

26 / 50

26. Weak acid ionization constant:

a) Kw

b) Kb

c) Ka

d) Kc

27 / 50

27. Acid strength best shown by:

a) pKa

b) pH

c) Ka

d) Kb

28 / 50

28. By reducing pressure reaction moves to

a) fewer moles

b) more moles

c) inert gas

d) catalyst

29 / 50

29. Kp = Kc(RT)^Δn applies to:

a) gases

b) liquids

c) solids

d) buffers

30 / 50

30. IN ENDOTHERMIC REACTION IF TEMPERATURE IS INCREASED THEN REACTION SHIFT TO

a) forward

b) backward

c) no change

d) side with catalyst

31 / 50

31. Kc units for PCl₃ + Cl₂ ⇌ PCl₅:

a) mol·dm⁻³

b) mol⁻¹·dm³

c) mol²·dm⁻³

d) none

32 / 50

32. At equilibrium:

a) Q = K

b) Q > K

c) Q < K

d) Q = 0

33 / 50

33. Inert gas at constant pressure:

a) no effect

b) fewer moles side

c) increases Kc

d) speeds up reaction

34 / 50

34. Strong acid added to buffer:

a) slight pH decrease

b) large pH decrease

c) pH increase

d) destroyed

35 / 50

35. Catalyst effect:

a) speeds equilibrium

b) increases yield

c) changes Kc

d) raises T

36 / 50

36. At equilibrium, the rate of the forward reaction is:

a) Greater than the backward reaction

b) Equal to the backward reaction

c) Zero

d) Less than the backward reaction

37 / 50

37. Which of the following is NOT a characteristic of a chemical equilibrium?

a) Dynamic in nature

b) Closed system required

c) Concentrations of reactants and products change continuously

d) Rate of forward reaction equals rate of backward reaction

38 / 50

38. Remove heat from exothermic reaction shift equilibrium

a) right

b) left

c) increases temp

d) none

39 / 50

39. For Δn in Kp = Kc(RT)^Δn, 2A ⇌ 3B:

a) +1

b) -1

c) 0

d) +2

40 / 50

40. If Q < K, reaction proceeds:

a) forward

b) backward

c) stops

d) fast

41 / 50

41. Chemical equilibrium can be established only in:

a) An open system

b) A closed system

c) A system with a catalyst

d) A system with excess reactants

42 / 50

42. When a reversible reaction reaches equilibrium, the concentrations of reactants and products become:

a) Zero

b) Constant

c) Equal

d) Variable

43 / 50

43. Which factor does NOT affect the equilibrium position of a reaction?

a) Temperature

b) Pressure

c) Catalyst

d) Concentration of reactants

44 / 50

44. According to Le Chatelier’s Principle, if the concentration of a reactant is increased, the equilibrium will shift:

a) To the left

b) To the right

c) Remain unchanged

d) Toward formation of reactants

45 / 50

45. If heat is added to an endothermic reaction at equilibrium, the reaction will shift:

a) To the left

b) To the right

c) Stop completely

d) Not affected

46 / 50

46. The equilibrium constant (Kc) is affected only by:

a) Catalyst

b) Pressure

c) Temperature

d) Concentration

47 / 50

47. Which of the following will shift the equilibrium to the product side in an exothermic reaction?

a) Increase in temperature

b) Addition of catalyst

c) Decrease in temperature

d) Removal of product

48 / 50

48. In a gaseous equilibrium, increasing pressure favors the side:

a) With more moles of gas

b) With less moles of gas

c) With equal moles of gas

d) With no gases

49 / 50

49. If the equilibrium constant Kc >> 1, it means:

a) Reactants are favored

b) Products are favored

c) System is at equilibrium

d) Forward and backward reactions are equal

50 / 50

50. At equilibrium, the concentration of reactants and products depends on:

a) Catalyst used

b) Reaction mechanism

c) Temperature and reaction conditions

d) Pressure

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MDCAT XI Chemistry Chemical Equilibrium Online Test

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