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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. 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

0.0796

0.0199

1.99

0.282

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

Unstable

Solids

Stable

At very high temperature

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

Law of active mass

All of these

Law of mass action

Law of mobile equilibrium

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

High temperature and high pressure

Low temperature and low pressure

Low temperature and high pressure

High temperature and low pressure

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

Common ion effect

Dissociation constant for an acid

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

Concentrations of the reactants and products continue to change

Rates of the forward and backward reactions change

Equilibrium constant changes

Reactants and products keep reacting

7. A buffer solution can be prepared by mixing

A strong acid and weak base

A strong acid and its salt

A weak acid and weak base

A weak base and its salt with strong acid

8. Kc > Products / Reactants favours

Equilibrium

Forward reaction

Backward reaction

Reaction completed

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

Higher side

Lower side

Optimum side

Constant

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

Randomly

Fast

Moderately

Slowly

11. Idea of PH and POH was put forward by

Einstein

Gibbs

Chadwiick

Sorenson

12. 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

Common on effect

Lowery Bronsted concept

Law of mass action

13. Conjugate base of a very weak acid is

Do not ionize

Salt

Weak base

Strong base

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

More water is formed

More ice is formed

Equilibrium is not disturbed

Water evaporates

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

4 x 10¯⁴

3.6 x 10¯⁵

7.2 x 10¯⁶

3.6 x 10¯⁶

16. Which pH is considered as basic?

17. Units of Kc is

Moles⁺² dm¯⁶

Moles² dm⁺⁶

Kc may or may not have units

Moles¯² dm⁺⁶

18. 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

None of all

Le – Chatelier’s principle

Law of mass action

Law of conservation of energy

19. pH of milk is

6.5

7.5

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

Na₂CO₃

Na₂SO₄

NaCl

Fecl₃₋

21. The state of equilibrium refers to

Stationary state

Dynamic state

State of inertness

State or rest

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

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

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

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

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

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

K = 10¯²

K = 10

K = 10³

K = 10⁰

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

Solution of CuSO4

Glue

Blood

Brine

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

Strong acid and strong base

Weak acid and strong base

Weak acid and its salt with a strong base

Weak base and its salt with a strong acid

Page 2 of 3

26. The relationship between Kp and Kc is give by

Kp = Kc (RT)∆n

Kp = Kc (RT)∆

Kc = Kp (RT)∆n

Kp = Kc (RT)-∆n

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

None

Individually

Both a and b

Simultaneously

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

Becomes one fourth

Remains the same

Also be doubled

Be halved

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

Depends on the initial concentration of the reactants

Depends on the concentration of one of the products at equilibrium

Does not depend on the initial concentrations of reactants

Is not characteristic of the reaction

30. Reaction which proceed in both the directions is called

Non spontaneous

Spontaneous

Irreversible

Reversible

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

Product side

Fluctuate

Reactant side

Remains unchanged

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

More ice will be formed

Equilibrium will not be formed

Water will evaporate

More water will be formed

33. Which of the following is more acidic?

Apples

Lemons

Bananas

Bread

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

Pressure

Impurity

Temperature

Concentration

35. 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]

36. 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

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

No effect

Less than 7

More than 7

Equal to 7

38. Addition of CH3COOH and CH3COONa gives in water

Acidic buffer solution

Standard solution

Buffer solution

Both b and c

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

Increase in concentration of one of the products

Increase in concentration of one of the reactants

Removal of one of the products regularly

None of these

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

Total pressure

Amounts of A₂ and B₂

Temperature

Catalyst

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

Equal volumes of N₂ and H₂ are reacting

The reaction has stopped

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

Equal masses of N₂ and H₂ are reacting

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

Favour the formation of N₂O₄

Favour the decomposition of N₂O₄

Not alter the equilibrium

Stop the reaction

43. What is the relationship between kp and kc?

kp = kc (RT)-∆n

kp = kc (RT)∆n

Kc - kp (RT)∆n

kc = kp (P)-∆n

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

10¯²⁰

10¯¹⁰

10¹⁰

10¯¹⁴

45. 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

0.2

0.02

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

Produce some increase in Kc

Decrease the value of equilibrium constant

Double the value of Kc

Not produce any change in Kc

47. 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, II and III only

I and II only

I and III only

II and III only

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

3.0

0.5

0.25

1.0

49. Which of the following gives a basic buffer?

NaOH + NaCl

NH₄OH + NH₄Cl

NaCl + CH₃ COOH

NaOH + CH₃ COONa

50. Solubility of any salt can be determined from

Ksp

Page 3 of 3

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

Water will formed

More water will be formed

Equilibrium will not be disturbed

More ice will be formed

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

0.4 mole of NH3 with 0.2 mole of HCl

0.0002M HCl

0.2 mole of NaCl with 0.2 mole of HNO3

0.4 mole of CH3COOH with 0.4 mole of NaOH

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

Constant Reaction

Decomposition Reaction

Irreversible Reaction

Reversible Reaction

54. 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

Weak base and its salt with strong acid

Strong base and its salt with weak acid

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

None of these

Catalyst

Temperature

Pressure

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

Equilibrium will established

Reaction stops after some time

Reaction goes backward

Reaction goes forward

57. Who studied the effect of temperature on equilibrium?

Arrhenius

Vant Hoff

Lewis

Van der Waal

58. Temperature for preparation of SO₃ is

200 °C

400 – 500 °C

400 °C

600 °C

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

None of all

Dynamic equilibrium

Static equilibrium

Chemical equilibrium

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

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

None of these

HI dissociation stops

The reaction stops completely

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

Conversion of A to B is only 50% complete

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

Only 10% conversion of A to B has taken place

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

Law of Mass Action

None of these

Law of reaction

Law of Equilibrium

63. PH of human blood is

7.80

7.00

7.35

7.50

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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

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