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

Depends on the concentration of one of the products at equilibrium

Is not characteristic of the reaction

Depends on the initial concentration of the reactants

Does not depend on the initial concentrations of reactants

2. 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

3. Solubility of any salt can be determined from

Ksp

4. A basic Buffer solution can be prepared by mixing

Strong base and its salt with weak acid

Strong acid and its slat wit weak base

Weak acid and its slat with strong base

Weak base and its salt with strong acid

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

Temperature

Pressure

Concentration

Impurity

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

Unstable

Stable

At very high temperature

Solids

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

Decrease the value of equilibrium constant

Double the value of Kc

Not produce any change in Kc

Produce some increase in Kc

8. The relationship between Kp and Kc is give by

Kc = Kp (RT)∆n

Kp = Kc (RT)∆

Kp = Kc (RT)-∆n

Kp = Kc (RT)∆n

9. 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

10. PH of human blood is

7.35

7.80

7.00

7.50

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

Moderately

Randomly

Fast

Slowly

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

K = 10

K = 10³

K = 10¯²

K = 10⁰

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

The reaction has stopped

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

Equal volumes of N₂ and H₂ are reacting

Equal masses of N₂ and H₂ are reacting

14. Temperature for preparation of SO₃ is

600 °C

400 – 500 °C

200 °C

400 °C

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

No effect

More than 7

Equal to 7

Less than 7

16. Kc > Products / Reactants favours

Backward reaction

Equilibrium

Reaction completed

Forward reaction

17. 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

0.2 mole of NaCl with 0.2 mole of HNO3

0.4 mole of NH3 with 0.2 mole of HCl

0.0002M HCl

18. 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

19. 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

20. pH of milk is

7.5

6.5

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

Remains unchanged

Reactant side

Product side

Fluctuate

22. 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]

[A] < [B]

[A] = [B]

[B] = [C]

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

Water will evaporate

Equilibrium will not be formed

More water will be formed

More ice will be formed

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

None of these

The reaction stops completely

HI dissociation stops

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

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

Law of reaction

Law of Equilibrium

Law of Mass Action

None of these

Page 2 of 3

26. 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

27. Which of the following gives a basic buffer?

NaOH + NaCl

NaCl + CH₃ COOH

NH₄OH + NH₄Cl

NaOH + CH₃ COONa

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

Constant Reaction

Irreversible Reaction

Decomposition Reaction

Reversible Reaction

29. What is the relationship between kp and kc?

kp = kc (RT)-∆n

kc = kp (P)-∆n

kp = kc (RT)∆n

Kc - kp (RT)∆n

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

Law of mass action

Law of mobile equilibrium

All of these

Law of active mass

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

1.0

0.5

0.25

3.0

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

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

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

33. Idea of PH and POH was put forward by

Sorenson

Chadwiick

Einstein

Gibbs

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

Individually

None

Both a and b

Simultaneously

35. 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

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

Water evaporates

More ice is formed

Equilibrium is not disturbed

More water is formed

37. 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

Be halved

Also be doubled

38. Who studied the effect of temperature on equilibrium?

Van der Waal

Arrhenius

Lewis

Vant Hoff

39. 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

0.0199

0.282

1.99

0.0796

40. Preparation of buffer solution can be done by mixing

Weak acid and its salt with weak base

Weak base and its salt with strong acid

Strong acid and its salt with weak base

Strong base and its salt with weak acid

41. Conjugate base of a very weak acid is

Strong base

Do not ionize

Salt

Weak base

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

Blood

Glue

Brine

Solution of CuSO4

43. A buffer solution can be prepared by mixing

A strong acid and its salt

A weak base and its salt with strong acid

A strong acid and weak base

A weak acid and weak base

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

Increase in concentration of one of the products

None of these

Increase in concentration of one of the reactants

Removal of one of the products regularly

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

More ice will be formed

Water will formed

More water will be formed

Equilibrium will not be disturbed

46. 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, II and III only

I and III only

47. Addition of CH3COOH and CH3COONa gives in water

Buffer solution

Both b and c

Acidic buffer solution

Standard solution

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

High temperature and low pressure

Low temperature and low pressure

High temperature and high pressure

Low temperature and high pressure

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

Static equilibrium

Dynamic equilibrium

None of all

Chemical equilibrium

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

NaCl

Na₂SO₄

Na₂CO₃

Fecl₃₋

Page 3 of 3

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

Temperature

None of these

Catalyst

Pressure

52. 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

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

53. 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

Lowery Bronsted concept

Le – Chatelier’s principle

54. Which pH is considered as basic?

55. Reaction which proceed in both the directions is called

Irreversible

Reversible

Non spontaneous

Spontaneous

56. Units of Kc is

Moles¯² dm⁺⁶

Moles⁺² dm¯⁶

Moles² dm⁺⁶

Kc may or may not have units

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

Favour the decomposition of N₂O₄

Favour the formation of N₂O₄

Stop the reaction

Not alter the equilibrium

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

Optimum side

Higher side

Lower side

Constant

59. The state of equilibrium refers to

Stationary state

State or rest

Dynamic state

State of inertness

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

3.6 x 10¯⁶

3.6 x 10¯⁵

7.2 x 10¯⁶

4 x 10¯⁴

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

10¯¹⁴

10¹⁰

10¯¹⁰

10¯²⁰

62. 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

Solubility product

Dissociation constant

Common ion effect

63. Which of the following is more acidic?

Bananas

Bread

Lemons

Apples

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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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Malik Tahir

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