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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. 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

Law of mass action

Common on effect

Le – Chatelier’s principle

Lowery Bronsted concept

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

Temperature

Impurity

Pressure

Concentration

3. 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

4. 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

5. Solubility of any salt can be determined from

Ksp

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

Low temperature and low pressure

High temperature and low pressure

High temperature and high pressure

Low temperature and high pressure

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

Only 10% conversion of A to B has taken place

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

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

Temperature

Pressure

None of these

Catalyst

9. pH of milk is

6.5

7.5

10. Temperature for preparation of SO₃ is

200 °C

400 °C

400 – 500 °C

600 °C

11. Which of the following gives a basic buffer?

NaCl + CH₃ COOH

NH₄OH + NH₄Cl

NaOH + CH₃ COONa

NaOH + NaCl

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

Irreversible Reaction

Constant Reaction

Reversible Reaction

Decomposition Reaction

13. 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

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

Chemical equilibrium

None of all

Static equilibrium

Dynamic equilibrium

15. Addition of CH3COOH and CH3COONa gives in water

Both b and c

Standard solution

Acidic buffer solution

Buffer solution

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

Total pressure

Amounts of A₂ and B₂

Catalyst

Temperature

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

Equal masses of N₂ and H₂ are reacting

Equal volumes of N₂ and H₂ are reacting

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

The reaction has stopped

18. Who studied the effect of temperature on equilibrium?

Arrhenius

Van der Waal

Lewis

Vant Hoff

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

Decrease the value of equilibrium constant

Produce some increase in Kc

Double the value of Kc

Not produce any change in Kc

20. 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

Becomes one fourth

Also be doubled

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

Solution of CuSO4

Glue

Blood

Brine

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

Reactants and products keep reacting

Concentrations of the reactants and products continue to change

Equilibrium constant changes

Rates of the forward and backward reactions change

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

Law of mass action

Law of mobile equilibrium

All of these

Law of active mass

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

More water will be formed

Water will evaporate

More ice will be formed

Equilibrium will not be formed

25. 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

II and III only

I and II only

I and III only

I, II and III only

Page 2 of 3

26. 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

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

0.5

0.25

3.0

1.0

28. A basic Buffer solution can be prepared by mixing

Strong acid and its slat wit weak base

Weak base and its salt with strong acid

Weak acid and its slat with strong base

Strong base and its salt with weak acid

29. PH of human blood is

7.00

7.80

7.35

7.50

30. Which pH is considered as basic?

31. A buffer solution can be prepared by mixing

A weak acid and weak base

A weak base and its salt with strong acid

A strong acid and weak base

A strong acid and its salt

32. 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 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

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

33. Which of the following is more acidic?

Apples

Bread

Lemons

Bananas

34. Conjugate base of a very weak acid is

Salt

Strong base

Weak base

Do not ionize

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

HI dissociation stops

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

The reaction stops completely

None of these

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

No effect

Less than 7

More than 7

Equal to 7

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

NaCl

Fecl₃₋

Na₂CO₃

Na₂SO₄

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

10¯¹⁰

10¯²⁰

10¹⁰

10¯¹⁴

39. 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

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

Is not characteristic of the reaction

Does not depend on the initial concentrations of reactants

Depends on the initial concentration of the reactants

Depends on the concentration of one of the products at equilibrium

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

Individually

None

Both a and b

Simultaneously

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

Randomly

Fast

Moderately

Slowly

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

Dissociation constant

Common ion effect

Solubility product

Dissociation constant for an acid

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

K = 10

K = 10¯²

K = 10³

K = 10⁰

45. The state of equilibrium refers to

State or rest

Stationary state

State of inertness

Dynamic state

46. Units of Kc is

Kc may or may not have units

Moles⁺² dm¯⁶

Moles¯² dm⁺⁶

Moles² dm⁺⁶

47. Kc > Products / Reactants favours

Equilibrium

Reaction completed

Forward reaction

Backward reaction

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

7.2 x 10¯⁶

3.6 x 10¯⁶

3.6 x 10¯⁵

4 x 10¯⁴

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

More ice is formed

Equilibrium is not disturbed

Water evaporates

More water is formed

50. The relationship between Kp and Kc is give by

Kp = Kc (RT)∆n

Kc = Kp (RT)∆n

Kp = Kc (RT)∆

Kp = Kc (RT)-∆n

Page 3 of 3

51. What is the relationship between kp and kc?

kp = kc (RT)-∆n

kc = kp (P)-∆n

Kc - kp (RT)∆n

kp = kc (RT)∆n

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

None of these

Law of Equilibrium

Law of reaction

Law of Mass Action

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

Constant

Lower side

Optimum side

Higher side

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

Unstable

Solids

At very high temperature

Stable

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

Stop the reaction

Not alter the equilibrium

Favour the formation of N₂O₄

Favour the decomposition of N₂O₄

56. Idea of PH and POH was put forward by

Einstein

Chadwiick

Sorenson

Gibbs

57. Reaction which proceed in both the directions is called

Non spontaneous

Spontaneous

Reversible

Irreversible

58. 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

Law of mass action

Le – Chatelier’s principle

Law of conservation of energy

None of all

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

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

0.4 mole of NH3 with 0.2 mole of HCl

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

Fluctuate

Reactant side

Remains unchanged

Product side

61. 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] > [C]

[B] = [C]

[A] < [B]

[A] = [B]

62. Preparation of buffer solution can be done by mixing

Strong base and its salt with weak acid

Weak base and its salt with strong acid

Strong acid and its salt with weak base

Weak acid and its salt with weak base

63. 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

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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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