Chemical Equilibrium Test UHS MDCAT Preparation

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Chemical Equilibrium Test UHS MDCAT Preparation

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UHS MCAT & MDCAT Entry Tests Chemistry Preparations

Chemistry Chemical Equilibrium Test 1

Total No. of MCQs: 25
Time Limit: No

1 / 25

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?

Ag⁺ and Ba⁺⁺ and NO¯₃

Ag⁺ and NO¯₃ only

Ba²⁺ and NO¯₃ and CI¯₃

Ba²⁺ and NO¯₃ only

2 / 25

Which is not true about buffer is a solution?

Whose pH is constant

Whose pH may or may not change during a chemical reaction

Which resists change in its pH

Which resists enough to maintain its pH

3 / 25

The ionic product of solution is greater than solubility product. The solution is:

Supersaturated

Saturate

Unsaturated

None of all

4 / 25

The value of Kp is greater than Kc for a gaseous reaction when

Number of molecules of products is greater than that the reactants

Number of molecules of products is greater than the reactants

Number of molecules of reactants is greater than those of products

A catalyst is added

5 / 25

0.1 M HCI has pH = 1.0, it is about 100 times stronger than acetic acid. Then pH of acetic acid will be:

0.1

1.3

2.0

6 / 25

Neutralization of a strong acid with a strong base is:

Reversible process

None-spontaneous reaction

Chemical equilibrium

Spontaneous reaction

7 / 25

What is the unit of equilibrium constant kc for the following reaction? H₂ + I₂ Ĝ ≈ 2HI

None of these

Mol¯¹ dm³

Mol¯² dm³

Mol dm¯¹

8 / 25

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 masses of reacting substances in knows as?

None of all

Law of mass action

Le-Chatelier’s principle

Law of conservation of energy

9 / 25

Le-Chatelier’s principle is applied on the reversible reactions in order to:

Predict the reaction of reaction

Find the best condition of favorable shifting the position of equilibrium

Determine the rate reaction

Determine the extent of reaction

10 / 25

If the difference of pKa values of the two acids is 2, then:

Acid with greater pKa is 100 times stronger acid

Acid with greater pKa is 10 times stronger acid

Acid with smaller pKa is 10 times stronger acid

Acid with smaller pKa is 100 times stronger acid

11 / 25

Chemical equilibrium involving reactants and products is more than one phase is known:

Heterogeneous

Dynamic

Homogeneous

Static

12 / 25

The strongest base among the following is

LiOH

NaCH

RbOH

KOH

13 / 25

Which statement about the following equilibrium is correct? 2SO₂(g) + O₂(g) ≈2SO₃(g) ∆H≈ - 188.3 kJmol¯¹

The value of Kp is equal to Kc

The value of Kp falls with increasing pressure

Adding V₂O₅ catalyst increases the equilibrium yield of SO₃

The value of Kp falls with the rise in temperature

14 / 25

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

Dynamic equilibrium

Chemical equilibrium

Static equilibrium

None of all

15 / 25

Hydrogen gas and iodine vapours combine to form HI at 425°C. The same composition of mixture is present if we start with decomposition of HI. It suggests.

Law of mass action

Irreversible reaction

A dynamic equilibrium

A static equilibrium

16 / 25

For which system does the equilibrium constant Kc has units of (concentration)¯¹?

H₂ + 3H₂ = 2NH₃

2HF = H₂ + F₂

2NO₂ = N₂O₄

H₂ + I₂ = 2HI

17 / 25

Who introduced the term pH?

Sorenson

Goldstein

Thomson

Henderson

18 / 25

Law of mass action states that rate of chemical reaction is directly proportional to the product of active masses of the reactants. The term active mass means

Number of moles

Mass in grams converted to products

Total pressures of the reactants

Number of moles per dm³ of reactants

19 / 25

The solubility product of AgCI is 2 x 10¯¹⁰ mol² dm¯⁶. The maximum concentration of Ag⁺ in the solution is:

2 x 10¯¹⁰ mol dm¯³

1.41 x 10¯⁵ mol dm¯³

1 x 10¯¹⁰ mol dm¯³

2 x 10¯²⁰ mol dm¯³

20 / 25

The pH of buffer solution is 4.74. On adding 0.1 ml (0.00001M) HC1 solution, the pH of solution will be:

4.7

5.3

5.2

4.74

21 / 25

The pH of 10¯³ mol dm ¯³ of an aqueous solution of H₂OS₄ is

3.0

2.0

2.7

1.5

22 / 25

Which of the solution among the following has highest pH?

0.01 M NaHCO₃

0.02 M CH₃COONa

0.01 M NaOH

0.1 M H₂SO₄

23 / 25

Who studied the effect of temperature on equilibrium?

Lewis

Arrhenius

Vant Hoff

Van der Waal

24 / 25

The value of Kp is greater than Kc for a gaseous reaction when

Number of molecules of reactants is greater than those of products

Number of molecules of reactants and products are equal

Number of molecules of products is greater than those of reactants

Catalyst is added

25 / 25

All of the following are the postulates of Arrhenius theory of ionization except:

Ionization is reversible process

Electrical conductivity of a solution of an electrolyte depends on the extent to which the electrolyte ionize in solution

Strong electrolyte ionize to a greater extent in water

Electrolyte ionize in water to produce cations and anions

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Chemical Equilibrium Test UHS MDCAT Preparation

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