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

Randomly

Slowly

Moderately

Fast

2. Units of Kc is

Moles¯² dm⁺⁶

Moles² dm⁺⁶

Kc may or may not have units

Moles⁺² dm¯⁶

3. Which pH is considered as basic?

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

Decomposition Reaction

Reversible Reaction

Constant Reaction

Irreversible Reaction

5. 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

None of all

Law of mass action

Law of conservation of energy

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

More ice is formed

More water is formed

Equilibrium is not disturbed

Water evaporates

7. 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

0.4 mole of CH3COOH with 0.4 mole of NaOH

0.2 mole of NaCl with 0.2 mole of HNO3

0.0002M HCl

8. Solubility of any salt can be determined from

Ksp

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

Dissociation constant for an acid

Common ion effect

Solubility product

Dissociation constant

10. The relationship between Kp and Kc is give by

Kp = Kc (RT)∆

Kc = Kp (RT)∆n

Kp = Kc (RT)∆n

Kp = Kc (RT)-∆n

11. Temperature for preparation of SO₃ is

400 – 500 °C

400 °C

600 °C

200 °C

12. PH of human blood is

7.80

7.35

7.50

7.00

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

3.6 x 10¯⁵

7.2 x 10¯⁶

3.6 x 10¯⁶

4 x 10¯⁴

14. Addition of CH3COOH and CH3COONa gives in water

Both b and c

Acidic buffer solution

Standard solution

Buffer solution

15. The state of equilibrium refers to

State or rest

Stationary state

Dynamic state

State of inertness

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

Less than 7

More than 7

No effect

Equal to 7

17. Which of the following is more acidic?

Bananas

Apples

Lemons

Bread

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

Removal of one of the products regularly

Increase in concentration of one of the reactants

None of these

Increase in concentration of one of the products

19. 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

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

None of these

HI dissociation stops

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

The reaction stops completely

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

Water will formed

More water will be formed

More ice will be formed

Equilibrium will not be disturbed

22. 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

Also be doubled

Be halved

Remains the same

23. 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

Reactants and products keep reacting

Equilibrium constant changes

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

3.0

0.25

1.0

0.5

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

Does not depend on the initial concentrations of reactants

Depends on the concentration of one of the products at equilibrium

Depends on the initial concentration of the reactants

Is not characteristic of the reaction

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

Higher side

Optimum side

Constant

Lower side

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

At very high temperature

Solids

Unstable

Stable

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

Not alter the equilibrium

Favour the formation of N₂O₄

Favour the decomposition of N₂O₄

Stop the reaction

30. pH of milk is

6.5

7.5

31. A buffer solution can be prepared by mixing

A strong acid and weak base

A weak base and its salt with strong acid

A weak acid and weak base

A strong acid and its salt

32. Conjugate base of a very weak acid is

Salt

Strong base

Weak base

Do not ionize

33. 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

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

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

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

Solution of CuSO4

Blood

Brine

Glue

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

Double the value of Kc

Decrease the value of equilibrium constant

Not produce any change in Kc

Produce some increase in Kc

36. Idea of PH and POH was put forward by

Chadwiick

Sorenson

Einstein

Gibbs

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

NaCl

Na₂SO₄

Fecl₃₋

Na₂CO₃

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

Amounts of A₂ and B₂

Total pressure

Temperature

Catalyst

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

Equilibrium will not be formed

More water will be formed

Water will evaporate

More ice will be formed

40. What is the relationship between kp and kc?

kc = kp (P)-∆n

kp = kc (RT)∆n

Kc - kp (RT)∆n

kp = kc (RT)-∆n

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

Weak acid and its salt with a strong base

Weak base and its salt with a strong acid

Strong acid and strong base

Weak acid and strong base

42. Who studied the effect of temperature on equilibrium?

Arrhenius

Van der Waal

Lewis

Vant Hoff

43. 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

44. 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

Lowery Bronsted concept

Common on effect

Law of mass action

Le – Chatelier’s principle

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

K = 10¯²

K = 10

K = 10⁰

K = 10³

46. 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

Strong base and its salt with weak acid

Weak base and its salt with strong acid

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

Temperature

None of these

Catalyst

Pressure

48. 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

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

Fluctuate

Reactant side

Product side

Remains unchanged

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

10¯¹⁴

10¯¹⁰

10¹⁰

10¯²⁰

Page 3 of 3

51. A basic Buffer solution can be prepared by mixing

Weak base and its salt with strong acid

Weak acid and its slat with strong base

Strong base and its salt with weak acid

Strong acid and its slat wit weak base

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

Simultaneously

Individually

Both a and b

None

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

Reaction goes forward

Equilibrium will established

Reaction stops after some time

Reaction goes backward

54. Which of the following gives a basic buffer?

NaCl + CH₃ COOH

NH₄OH + NH₄Cl

NaOH + NaCl

NaOH + CH₃ COONa

55. 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]

[B] = [C]

[A] > [C]

[A] = [B]

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

Low temperature and high pressure

High temperature and low pressure

Low temperature and low pressure

High temperature and high pressure

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

Dynamic equilibrium

Chemical equilibrium

None of all

Static equilibrium

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

Law of reaction

Law of Mass Action

None of these

Law of Equilibrium

59. Reaction which proceed in both the directions is called

Non spontaneous

Spontaneous

Reversible

Irreversible

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

Only 10% conversion of A to B has taken place

Conversion of A to B is only 50% complete

Complete 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.

61. Kc > Products / Reactants favours

Reaction completed

Forward reaction

Backward reaction

Equilibrium

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

Law of mass action

Law of active mass

All of these

Law of mobile equilibrium

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

Temperature

Impurity

Pressure

Concentration

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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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