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MDCAT Chemistry Chemical Equilibrium Test Online

Malik TahirLast Updated: May 24, 2025

Chemistry Chemical Equilibrium MCQS Online Test

MDCAT Chemistry Chemical Equilibrium Chapter Online Test

Total Questions:	63
Time Allowed:	30 Minutes
Total Marks:	63
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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MDCAT Chemistry Chemical Equilibrium Test

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Page 1 of 3

Chemistry

1. AgCl dissolved with cone (2 x 10¯²) Ksp will be

3.6 x 10¯⁶

7.2 x 10¯⁶

4 x 10¯⁴

3.6 x 10¯⁵

2. Which one of the following is a buffer solution?

Brine

Blood

Solution of CuSO4

Glue

3. When H₂ and I₂ are mixed and equilibrium is attained, then

Amount of HI formed is equal to the amount of H₂ dissociated

The reaction stops completely

None of these

HI dissociation stops

4. When ever a week a base is dissolved in water, it gives its conjugate acid similarly a weal acid in water products its conjugate base. The conjugate acid base pair is stated by

Le – Chatelier’s principle

Lowery Bronsted concept

Common on effect

Law of mass action

5. When sparingly soluble salt is in equilibrium with molar concentration of its oppositely charged ion when the product is called

Dissociation constant

Solubility product

Dissociation constant for an acid

Common ion effect

6. Which of the following is more acidic?

Bananas

Lemons

Apples

Bread

7. The factor which changes equilibrium constant o the reaction A₂(g) + B₂(g) → 2 AB(g) is

Total pressure

Temperature

Amounts of A₂ and B₂

Catalyst

8. The equilibrium constant in a reversible chemical reaction at a given temperature

Is not characteristic of the reaction

Depends on the initial concentration of the reactants

Does not depend on the initial concentrations of reactants

Depends on the concentration of one of the products at equilibrium

9. Solubility of any salt can be determined from

Ksp

10. Who studied the effect of temperature on equilibrium?

Van der Waal

Vant Hoff

Arrhenius

Lewis

11. Reaction which proceed in both the directions is called

Non spontaneous

Irreversible

Spontaneous

Reversible

12. What is the relationship between kp and kc?

kp = kc (RT)-∆n

kp = kc (RT)∆n

Kc - kp (RT)∆n

kc = kp (P)-∆n

13. Chemical equilibrium is referred to as dynamic because, at equilibrium, the

Reactants and products keep reacting

Equilibrium constant changes

Concentrations of the reactants and products continue to change

Rates of the forward and backward reactions change

14. Which statements are correct for a reaction at equilibrium?
(I) The forward and reverse reactions both continue
(II) The rates of the forward and reverse reactions are equal
(III) The concentrations of reactants and products are equal

I and III only

I and II only

I, II and III only

II and III only

15. Synthesis of ammonia by Habor process is an example of ___________

Decomposition Reaction

Reversible Reaction

Irreversible Reaction

Constant Reaction

16. Idea of PH and POH was put forward by

Chadwiick

Gibbs

Einstein

Sorenson

17. Preparation of buffer solution can be done by mixing

Strong acid and its salt with weak base

Weak acid and its salt with weak base

Weak base and its salt with strong acid

Strong base and its salt with weak acid

18. Addition of CH3COOH and CH3COONa gives in water

Standard solution

Both b and c

Acidic buffer solution

Buffer solution

19. In reversible reactions, if the forward reaction occur very fast then reactant (s) is (are) __________

At very high temperature

Unstable

Stable

Solids

20. In a chemical reaction N₂ + 3H₂ ⇌ 2NH₃ at equilibrium point

Equal volumes of N₂ and H₂ are reacting

The same amount of ammonia is formed as is decomposed into N₂ and H₂

Equal masses of N₂ and H₂ are reacting

The reaction has stopped

21. Temperature for preparation of SO₃ is

600 °C

400 – 500 °C

400 °C

200 °C

22. The state of equilibrium refers to

State or rest

Stationary state

State of inertness

Dynamic state

23. At certain temperature, 50% of HI is dissociated into H₂ and I₂ the equilibrium constant is

3.0

0.5

0.25

1.0

24. Which pH is considered as basic?

25. In which of the following cases, the reaction goes farthest to completion?

K = 10

K = 10⁰

K = 10³

K = 10¯²

Page 2 of 3

26. For the reaction 2A(g) + B(g) ⇌ 3C(g) + D(g) two moles each of A and B were taken into a flask. The following must always be true when the system attained equilibrium

[A] < [B]

[A] = [B]

[B] = [C]

[A] > [C]

27. A buffer solution can be prepared by mixing

A weak acid and weak base

A strong acid and its salt

A weak base and its salt with strong acid

A strong acid and weak base

28. The product of [0H¯][H⁺] at 25C° is

10¯¹⁴

10¯¹⁰

10¹⁰

10¯²⁰

29. If the value of kc is very low then the forward reaction will occur __________

Randomly

Moderately

Slowly

Fast

30. In an exothermic reversible reaction increase in temp shifts the equilibrium to

Fluctuate

Remains unchanged

Reactant side

Product side

31. For a reaction H₂ + I₂ ⇌ 2HI at 721 K, the value of equilibrium constant is 50. If 0.5 moles each of H₂ and I₂ is added to the system the value of equilibrium constant will be

0.02

0.2

32. The equilibrium will shift towards right by increasing ___________ of reactants

Temperature

Impurity

Concentration

Pressure

33. Which of the following factors will favour the reverse reaction in a chemical equilibrium?

Increase in concentration of one of the reactants

Increase in concentration of one of the products

None of these

Removal of one of the products regularly

34. In a reversible chemical reaction having two reactants in equilibrium, if the concentration of the reactants are doubled then the equilibrium constant will

Remains the same

Be halved

Also be doubled

Becomes one fourth

35. The rate at which a substance reacts is directly proportional to its active mass and the rate of reaction is directly proportional to the product of the active mass of reacting substances is known as

Le – Chatelier’s principle

Law of conservation of energy

Law of mass action

None of all

36. When pressure is applied to the equilibrium system Ice ⇌ Water? Which of the following phenomenon will happen?

More water will be formed

More ice will be formed

Water will evaporate

Equilibrium will not be formed

37. When pressure is applied to the given equilibrium ice water which of the following will happen

More water will be formed

Water will formed

More ice will be formed

Equilibrium will not be disturbed

38. If a buffer solution of higher PH than seven is to be made we use

Weak acid and its salt with a strong base

Strong acid and strong base

Weak base and its salt with a strong acid

Weak acid and strong base

39. Which of the following aqeous solution will be basic?

Na₂SO₄

NaCl

Na₂CO₃

Fecl₃₋

40. For equilibrium 2NO₂(g) ⇌ N₂O₄(g) + 14.6 kcal increase of temperature would

Stop the reaction

Not alter the equilibrium

Favour the decomposition of N₂O₄

Favour the formation of N₂O₄

41. The relationship between Kp and Kc is give by

Kp = Kc (RT)∆n

Kc = Kp (RT)∆n

Kp = Kc (RT)-∆n

Kp = Kc (RT)∆

42. In reversible reaction the changes in forward and backward reaction occur _________

Simultaneously

Both a and b

None

Individually

43. In an exothermic reaction, a 10° rise in temperature will

Not produce any change in Kc

Decrease the value of equilibrium constant

Produce some increase in Kc

Double the value of Kc

44. When rate of forward reaction is equal to rate of backward reaction, then the equilibrium established is called

Dynamic equilibrium

Static equilibrium

Chemical equilibrium

None of all

45. Conjugate base of a very weak acid is

Salt

Strong base

Weak base

Do not ionize

46. pH of milk is

7.5

6.5

47. PH of human blood is

7.35

7.50

7.80

7.00

48. Which of the following gives a basic buffer?

NaOH + NaCl

NaCl + CH₃ COOH

NaOH + CH₃ COONa

NH₄OH + NH₄Cl

49. Two moles of HI was heated in a sealed tube at 440°C till the equilibrium was reached. HI was found to be 22% decomposed. The equilibrium constant for dissociation is

0.282

0.0199

0.0796

1.99

50. If rate of concentration of reaction is equal to rate of concentration of products in reversible reaction the __________

Reaction stops after some time

Equilibrium will established

Reaction goes backward

Reaction goes forward

Page 3 of 3

51. An equilibrium constant of 10¯⁴ for a reaction means that the reaction is

One that will have 50% product and 50% reactant at equilibrium

The equilibrium constant only relates to the speed of a reaction and not to the amount of product formed

One that is unfavourable and will not have very much product at equilibrium

One that is very favorable and will have mostly product at equilibrium

52. What can affect the magnitude of equilibrium constant Kp of a reversible gaseous reaction

Catalyst

None of these

Temperature

Pressure

53. Le-Chatelier’s principle is sometime known as

Law of mass action

Law of active mass

Law of mobile equilibrium

All of these

54. Water and ice are in equilibrium at 0C° and pressure is applied at this stage, then

More ice is formed

More water is formed

Water evaporates

Equilibrium is not disturbed

55. By the addition of base in water pH will be

Equal to 7

No effect

Less than 7

More than 7

56. Kc > Products / Reactants favours

Reaction completed

Equilibrium

Forward reaction

Backward reaction

57. A basic Buffer solution can be prepared by mixing

Strong acid and its slat wit weak base

Weak acid and its slat with strong base

Strong base and its salt with weak acid

Weak base and its salt with strong acid

58. The reaction 2SO₂ + 2O₂ ⇌ 2SO will be favoured by

Low temperature and low pressure

High temperature and low pressure

Low temperature and high pressure

High temperature and high pressure

59. At start of reaction, concentration of reactants are on

Lower side

Higher side

Optimum side

Constant

60. Units of Kc is

Kc may or may not have units

Moles² dm⁺⁶

Moles¯² dm⁺⁶

Moles⁺² dm¯⁶

61. Which set of solutes will form a buffer when dissolved in water to make 1 litter of solution?

0.4 mole of CH3COOH with 0.4 mole of NaOH

0.0002M HCl

0.4 mole of NH3 with 0.2 mole of HCl

0.2 mole of NaCl with 0.2 mole of HNO3

62. A chemical reaction A ⇌ B is said to be in equilibrium when

The rate of transformation of A to B is just equal to rate of transformation of B to A in the system.

Complete conversion of A to B has taken place

Conversion of A to B is only 50% complete

Only 10% conversion of A to B has taken place

63. The rate of chemical reaction is directly proportional to the active mass of reactant this statement is known as ___________

Law of Equilibrium

Law of reaction

None of these

Law of Mass Action

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Malik TahirLast Updated: May 24, 2025

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MDCAT Chemistry Chemical Equilibrium Test Online

Chemistry Chemical Equilibrium MCQS Online Test

MDCAT Chemistry Chemical Equilibrium Chapter Online Test

MDCAT Chemistry Chemical Equilibrium Test

Chemistry

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Malik Tahir

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Chemistry Chemical Equilibrium MCQS Online Test

MDCAT Chemistry Chemical Equilibrium Chapter Online Test

MDCAT Chemistry Chemical Equilibrium Test

Chemistry

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