Chemistry Chapter No.8 Chemical Equilibrium 1st Year MDCAT MCQs

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Book Name : Chemistry
Chapter No. 08
Chapter Name : Chemical Equilibrium
Total MCQ from Text Book : 48
Book Version : 2022
Published By : Punjab Text Book Board Lahore
Approved By : Govt of the Punjab and Federal Ministry for Education
Test Type : MCQ’s
Exam conduct By : Inter Boards of Sindh, KPK, Balochistan, AJK, Gilgit Baltistan, Punjab & Federal
Class / Grade : 11 ( F.Sc. Intermediate)
Total Marks : 48
Total Time : 48 minutes

GRADE 11 - CHEMISTRY - CHAPTER NO. 8 - CHEMICAL EQUILIBRIUM

1 / 48

Consider the following reaction: N₂ + 3H₂? 2NH₃ H = -92.46 kJ/mol Which of the following conditions will increase the yield of NH₃?

increase in ptessure

decrease in temperature

continuous removal of NH3

all of these

2 / 48

A buffer solution can be prepared by mixing:

strong base and its salt with weak acid

weak acid and its salt with weak

weak base and its salt with strong acid

strong acid and its salt with weak base

3 / 48

When HCl is added to aqueous solution of H₂S, its ionization:

Remain constant

Unpredictable

Decreased

Increased

4 / 48

What is the value of Ksp for the reaction? AgCl ? Ag^{+^{+ Cl^-}}

s2

4s2

2s2

5 / 48

What is Kc expression for? N₂ + 3H₂ ? 2NH₃

Kc= 4x2.v / (a - 2x)2(b - x)

Kc= x2 / (a - b)(b - x)

Kc= 4x2.v2 / (a - x)(b - 3x)3

Kc= 4x2 / (a - x)V

6 / 48

If Kc is small, then product is:

Normal amount

Large amount

Small amount

Unpredictable

7 / 48

Units of Kw are:

mol2 dm-3

mol2 dm-6

mol3 dm-3

mol dm-3

8 / 48

The pH of 10^-3 mol dm^-3 of an aqueous solution of H₂ SO₄ is:

1.5

2.7

9 / 48

Highest pH is of:

0.1 M H2SO4

0.02 M CH3COONa

0.01 M NaOH

0.01 M NaHCO3

10 / 48

Cr^- ion is the conjugate base of:

HOCl

HCl

HClO4

HClO3

11 / 48

A solution having pH = 0 indicates molar concentration of H⁺ ions

10-14

10-7

107

12 / 48

pH of 0.2 M HCl solution which is 50% dissociated:

13 / 48

The ionic product of water will rise if:

Both H+ and OH- ions are added

H+ ions are added

OH- ions are added

Temperature is increased

14 / 48

For which system does the equilibrium constant, K_c has units of (concentration) ^-1 ?

H2 + I2------ 2HI

2NO2 ------ N2O2

N2 + 3H2------ 2NH3

2HF ------ H2 + F2

15 / 48

When we add NH₄Cl in a solution of ammonium hydroxide in water, ionization of NH₄OH is:

Increased

Unpredictable

Not charged

Decreased

16 / 48

When BiCl ₃ reacts with water, white precipitate of BiOCI (Artificial milk) is formed: BiC1₃ + H₂O ? BiOC1 + 2HC1 White ppt. disappears when:

HCl is removed

more H2O is added

more HCl is added

more BiCl3 is added

17 / 48

The specie acting both as Bronsted acid and base is:

OH-

NH3

Na2CO3

HSO-4

18 / 48

Relationship between Kp and Kc for the reaction is: N₂ + 3H₂ ? 2NH₃

Kc = Kp (RT)2

Kc = Kp (RT)

Kp = Kc (RT)

Kp = Kc (RT)-2

19 / 48

If value of Kc is large, equilibrium position is:

Remains unchanged

Towards left

Towards right

None of these

20 / 48

Ka and Kb of a conjugate acid and base are related as:

None of these

Ka &#8733 1/Kb

Ka = Kb

Ka &#8733 Kb

21 / 48

pH of a solution is 13, the solution is:

Strong base

Weak base

Strong acid

Weak acid

22 / 48

The Conjugate acid of NH^- ₂ is:

NH2OH

NH+3

NH-2

NH3

23 / 48

pH and pOH of pure water at 25 C:

1 x 10-14

24 / 48

Law of mass action was given by:

Landsberger

Le-Chatelier

Raoult

Guldberg and Waage

25 / 48

How many million tons of ammonia is produced annually by Haber's prcess:

170

220

110

26 / 48

What is the value of Ksp for the reaction? Al(OH)3 ? Al^{+++^{+ 3OH^-}}

3s3

27s4

9s3

27 / 48

What would be the solubility product of AB₂, when solubility of A is '2' ?

28 / 48

The term 'pH' was introduced by:

J.J Thomson

Chadwick

Sorenson

Dalton

29 / 48

Law of mass action was given by Guldberg and Waage in:

1964

1864

1857

1888

30 / 48

The solubility product of AgC1 is 2.0 x 10^-10 mol² dm^-6. The maximum concentration of Ag⁺ ions in the solution is:

1.41 x 10 -5 mol dm-3

2.0 x 10 -10 mol dm-3

4.0 x 10 -20 mol dm-3

1.0 x 10 -10 mol dm-3

31 / 48

Which of the following is not affected by increase in pressure at equilibrium?

2O3 ⇋ 3O2

PCl5 ⇋ PCl3 + Cl2

N2O4 ⇋ 2NO2

H2 + I2 ⇋ 2HI

32 / 48

For Kc =4x²v² / (a - x)(b - 3x)³ Then the system will move on:

backward direction

none of these

forward direction

both directions

33 / 48

Which statement about the following equilibrium is correct? 2SO_2(g) + O_2(g) ? 2SO_3(g) H= -188.3 kJ mol^-1

The value of Kp falls with increasing pressure.

Adding V2O5 catalyst increase the equilibrium yield of sulphur trioxide

The value of Kp falls with a rise in temperature.

The value of Kp is equal to Kc

34 / 48

Strength of an acid can be determined by:

pKw

pOH

35 / 48

With increase in temperature, ionic product of water increases and pH value:

Increase

Decrease

May increase or decrease

Remains same

36 / 48

An excess of aqueous silver nitrate is added to aqueous barium chloride and precipitate is removed by filtration. What are the main ions in the filtrate?

Ba2+ and NO3- and Cl

Ba2+ and NO3- only

Ag+ and Ba2+ and NO3-

Ag+ and NO3- only

37 / 48

H_2(g) + I_2(g) ?2HI _(g) The unit for the above reaction is:

mol dm-3

mol-2 dm+6

mol-2

no unit

38 / 48

pH of human blood is:

6.5

7.35

39 / 48

The unit of Kc for the formation of NH_{3_{: N₂ + 3H₂? 2NH₃ H= -92.46 kJ}}

mol-2 dm +3

mol2 dm +3

mol dm-3

mol-2 dm +6

40 / 48

The increase in dilution of solution:

decreases the degree of dissociation

has no effect on degree of dissociation

increases the degree of dissociation

depends upon nature of solute

41 / 48

Of the given anions, the strongest Bronsted base is:

CIO-3

CIO-2

CIO-

CIO-4

42 / 48

Which one is basic buffer solution?

H2CO3 + NaHCO3

C6H5COOH + C6H5COONa

H3PO4 + NaH2PO4

NH4OH + NH4Cl

43 / 48

Kp and Kc are related:

Kc = RT

Kp = Kc (RT)&#916n

Kp = Kc (RT)-&#916n

Kc = Kp (RT)&#916n

44 / 48

pH of 0.005 molar aqueous solution of H₂SO₄ is

0.005

0.1

45 / 48

N₂ and O₂ are in 10dm³ flask and equilibrium constant for the following reaction is 40: N₂ + O₂?2NO If volume of the flask is doubled, the equilibrium constant will be:

Zero

46 / 48

pH of gastric juice is:

47 / 48

pH of acid 'A' is 2 and pH of acid 'B' is 4. Strength of acid A and B is:

10 time stronger

2 time stronger

100 time stronger

2 time weaker

48 / 48

Acid is weak if:

ka = 10

ka = 10+2

ka = 1

ka = 10-3

Your score is

The average score is 33%

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