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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. A basic Buffer solution can be prepared by mixing

Weak acid and its slat with strong base

Weak base and its salt with strong acid

Strong acid and its slat wit weak base

Strong base and its salt with weak acid

2. Reaction which proceed in both the directions is called

Non spontaneous

Spontaneous

Irreversible

Reversible

3. Solubility of any salt can be determined from

Ksp

4. Conjugate base of a very weak acid is

Strong base

Do not ionize

Salt

Weak base

5. 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 II only

II and III only

I, II and III only

I and III only

6. 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

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

More ice is formed

Water evaporates

More water is formed

Equilibrium is not disturbed

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

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

Equal volumes of N₂ and H₂ are reacting

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

Concentrations of the reactants and products continue to change

Reactants and products keep reacting

Equilibrium constant changes

Rates of the forward and backward reactions change

10. 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

11. Addition of CH3COOH and CH3COONa gives in water

Buffer solution

Standard solution

Acidic buffer solution

Both b and c

12. What is the relationship between kp and kc?

Kc - kp (RT)∆n

kp = kc (RT)∆n

kc = kp (P)-∆n

kp = kc (RT)-∆n

13. Units of Kc is

Moles⁺² dm¯⁶

Moles² dm⁺⁶

Kc may or may not have units

Moles¯² dm⁺⁶

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

Blood

Brine

Solution of CuSO4

Glue

15. 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] > [C]

[B] = [C]

[A] = [B]

16. 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

17. A buffer solution can be prepared by mixing

A weak base and its salt with strong acid

A strong acid and weak base

A strong acid and its salt

A weak acid and weak base

18. 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

19. 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.

Conversion of A to B is only 50% complete

Only 10% conversion of A to B has taken place

Complete conversion of A to B has taken place

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

Law of active mass

Law of mobile equilibrium

All of these

Law of mass action

21. The state of equilibrium refers to

Dynamic state

Stationary state

State of inertness

State or rest

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

Catalyst

Temperature

None of these

Pressure

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

Constant Reaction

Decomposition Reaction

Irreversible Reaction

Reversible Reaction

24. Which of the following is more acidic?

Bananas

Bread

Lemons

Apples

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

High temperature and high pressure

High temperature and low pressure

Low temperature and high pressure

Low temperature and low pressure

Page 2 of 3

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

Not produce any change in Kc

Produce some increase in Kc

Double the value of Kc

Decrease the value of equilibrium constant

27. Kc > Products / Reactants favours

Forward reaction

Backward reaction

Reaction completed

Equilibrium

28. Temperature for preparation of SO₃ is

600 °C

400 – 500 °C

200 °C

400 °C

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

At very high temperature

Stable

Solids

Unstable

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

More than 7

Equal to 7

No effect

Less than 7

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

3.0

0.5

0.25

1.0

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

7.2 x 10¯⁶

4 x 10¯⁴

3.6 x 10¯⁶

3.6 x 10¯⁵

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

Not alter the equilibrium

Favour the formation of N₂O₄

Stop the reaction

Favour the decomposition of N₂O₄

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

None of these

The reaction stops completely

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

HI dissociation stops

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

10¯¹⁴

10¹⁰

10¯¹⁰

10¯²⁰

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

Fluctuate

Reactant side

Remains unchanged

Product side

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

Constant

Higher side

Optimum side

Lower side

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

K = 10³

K = 10⁰

K = 10

K = 10¯²

39. Which of the following gives a basic buffer?

NaOH + CH₃ COONa

NH₄OH + NH₄Cl

NaCl + CH₃ COOH

NaOH + NaCl

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

Temperature

Pressure

Impurity

Concentration

41. PH of human blood is

7.35

7.50

7.00

7.80

42. 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

Also be doubled

Be halved

Becomes one fourth

43. 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

44. pH of milk is

6.5

7.5

45. The relationship between Kp and Kc is give by

Kp = Kc (RT)-∆n

Kp = Kc (RT)∆

Kc = Kp (RT)∆n

Kp = Kc (RT)∆n

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

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

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

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

Law of Equilibrium

None of these

Law of reaction

Law of Mass Action

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

Increase in concentration of one of the reactants

None of these

Removal of one of the products regularly

Increase in concentration of one of the products

49. Who studied the effect of temperature on equilibrium?

Lewis

Arrhenius

Van der Waal

Vant Hoff

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

Na₂SO₄

Na₂CO₃

NaCl

Fecl₃₋

Page 3 of 3

51. 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

Law of mass action

Lowery Bronsted concept

Common on effect

52. Preparation of buffer solution can be done by mixing

Weak base and its salt with strong acid

Strong base and its salt with weak acid

Strong acid and its salt with weak base

Weak acid and its salt with weak base

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

Equilibrium will not be disturbed

More ice will be formed

Water will formed

More water will be formed

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

Depends on the initial concentration of the reactants

Is not characteristic of the reaction

Depends on the concentration of one of the products at equilibrium

Does not depend on the initial concentrations of reactants

55. Idea of PH and POH was put forward by

Chadwiick

Einstein

Sorenson

Gibbs

56. 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

0.0796

1.99

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

Randomly

Slowly

Moderately

Fast

58. 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

Dissociation constant

Common ion effect

Solubility product

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

None

Simultaneously

Both a and b

Individually

60. 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 mass action

None of all

Law of conservation of energy

61. Which pH is considered as basic?

62. 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

63. 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

Equilibrium will not be formed

More ice will be formed

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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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