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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. Le-Chatelier’s principle is sometime known as

All of these

Law of mobile equilibrium

Law of mass action

Law of active mass

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

Produce some increase in Kc

Double the value of Kc

Decrease the value of equilibrium constant

Not produce any change in Kc

3. pH of milk is

6.5

7.5

4. 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

5. The relationship between Kp and Kc is give by

Kp = Kc (RT)∆

Kp = Kc (RT)∆n

Kc = Kp (RT)∆n

Kp = Kc (RT)-∆n

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

Increase in concentration of one of the products

Removal of one of the products regularly

None of these

Increase in concentration of one of the reactants

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

10¯²⁰

10¹⁰

10¯¹⁰

10¯¹⁴

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

High temperature and high pressure

Low temperature and low pressure

High temperature and low pressure

Low temperature and high pressure

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

Impurity

Concentration

Temperature

Pressure

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

Pressure

None of these

Temperature

Catalyst

11. Kc > Products / Reactants favours

Forward reaction

Backward reaction

Equilibrium

Reaction completed

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

Static equilibrium

None of all

Dynamic equilibrium

Chemical equilibrium

13. Reaction which proceed in both the directions is called

Reversible

Irreversible

Spontaneous

Non spontaneous

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

Total pressure

Temperature

Amounts of A₂ and B₂

Catalyst

15. 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

16. 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

Common on effect

Lowery Bronsted concept

Le – Chatelier’s principle

Law of mass action

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

Weak base and its salt with a strong acid

Strong acid and strong base

Weak acid and strong base

Weak acid and its salt with a strong base

18. Which pH is considered as basic?

19. Solubility of any salt can be determined from

Ksp

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

Also be doubled

Remains the same

Becomes one fourth

Be halved

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

Higher side

Constant

Optimum side

Lower side

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

Product side

Reactant side

Remains unchanged

Fluctuate

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

None

Both a and b

Simultaneously

Individually

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

Decomposition Reaction

Irreversible Reaction

Reversible Reaction

Constant Reaction

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

Rates of the forward and backward reactions change

Concentrations of the reactants and products continue to change

Equilibrium constant changes

Reactants and products keep reacting

Page 2 of 3

26. 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] = [B]

[A] > [C]

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

Fecl₃₋

Na₂CO₃

Na₂SO₄

NaCl

28. Which of the following gives a basic buffer?

NH₄OH + NH₄Cl

NaCl + CH₃ COOH

NaOH + CH₃ COONa

NaOH + NaCl

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

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 is very favorable and will have mostly product at equilibrium

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

31. Temperature for preparation of SO₃ is

400 – 500 °C

200 °C

400 °C

600 °C

32. 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

33. Addition of CH3COOH and CH3COONa gives in water

Both b and c

Buffer solution

Acidic buffer solution

Standard solution

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

4 x 10¯⁴

3.6 x 10¯⁵

3.6 x 10¯⁶

7.2 x 10¯⁶

35. 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 its salt

A strong acid and weak base

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

Solubility product

Dissociation constant

Dissociation constant for an acid

Common ion effect

37. The state of equilibrium refers to

Dynamic state

Stationary state

State or rest

State of inertness

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

No effect

Equal to 7

More than 7

Less than 7

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

None of these

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

The reaction stops completely

HI dissociation stops

40. 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.

Complete conversion of A to B has taken place

Only 10% conversion of A to B has taken place

Conversion of A to B is only 50% complete

41. 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

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

Stable

Solids

Unstable

At very high temperature

43. PH of human blood is

7.00

7.35

7.80

7.50

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

Water will evaporate

More water will be formed

More ice will be formed

Equilibrium will not be formed

45. 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 conservation of energy

Law of mass action

Le – Chatelier’s principle

None of all

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

Reaction stops after some time

Reaction goes backward

Equilibrium will established

Reaction goes forward

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

Equal volumes of N₂ and H₂ are reacting

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

48. 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

49. Which of the following is more acidic?

Bread

Apples

Lemons

Bananas

50. 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

Page 3 of 3

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

Slowly

Randomly

Moderately

Fast

52. Idea of PH and POH was put forward by

Gibbs

Chadwiick

Einstein

Sorenson

53. Who studied the effect of temperature on equilibrium?

Arrhenius

Van der Waal

Lewis

Vant Hoff

54. Preparation of buffer solution can be done by mixing

Weak base and its salt with strong acid

Weak acid and its salt with weak base

Strong base and its salt with weak acid

Strong acid and its salt with weak base

55. Conjugate base of a very weak acid is

Strong base

Weak base

Salt

Do not ionize

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

More ice is formed

Equilibrium is not disturbed

More water is formed

Water evaporates

57. 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

58. 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

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

0.5

0.25

3.0

1.0

60. 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

0.282

0.0199

1.99

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

K = 10⁰

K = 10³

K = 10

K = 10¯²

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

Glue

Solution of CuSO4

Brine

Blood

63. Units of Kc is

Moles² dm⁺⁶

Kc may or may not have units

Moles⁺² dm¯⁶

Moles¯² dm⁺⁶

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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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