PHYSICAL PHARMACY PACOP 5

A data set in which there is a considerable closeness among the values

A. Accurate

B. Approximate

C. Estimate D. Precise

A type of Van der Waals forces of attraction resulting from the tendency of molecules to align themselves with oppositely charged ends of their neighbour

Debye

London

Keesom

H-bond

Keesom

A data set in which there is a considerable closeness among the values

A. Accurate

B. Approximate

C. Estimate D. Precise

A type of Van der Waals forces of attraction resulting from the tendency of molecules to align themselves with oppositely charged ends of their neighbour

Debye

London

Keesom

H-bond

Keesom

A type of Van der Waals forces of attraction which involves permanent dipoles inducing polarity in non-polar molecules

Debye

London

Keesom

H-bond

Debye

A type of Van der Waals forces of attraction which involves the dispersion of charges to induce polarity between non-polar molecules

Debye

London

Keesom

H-bond

London

The intermolecular forces of attraction responsible for the solubility of non-polar molecules such as Iodine in solution by the addition of salts

Debye

Ion-dipole interaction

Ion-induced dipole interaction

H-bonds

Ion-induced dipole interaction

This is responsible for the solubility of ionic crystalline substance in polar solvents like water

Debye

Ion-dipole interaction

Ion-induced dipole interaction

H-bonds

Ion-induced dipole interaction

H-bond is the interaction between a molecule containing a hydrogen atom and a strongly electronegative atom such as fluorine, oxygen and nitrogen. This is/are true statements regarding H-bonds

Stronger than ionic bonds

Responsible for the formation of water molecules

Can be both occurring as an intramoleecular and intermolecular force of attraction

I only

I and II only

II and III only

III only

I, II and III

III only

This law relates the volume and pressure of given mass of gas at constant temperature

Boyles

Charles

Gay-Lussac

Ideal Gas Law

Boyles

The equation B α T or V=kT, was explained by which gas law?

Boyle

Charles

Gay-Lussac

I only

I and II only

II and III onl

II and III only

Gas X is an ideal gas occupying a volume of 15ml at a temperature of 55°F and a pressure of 700mmHg. What is the volume of a gas at 0° and 800mmHg?

12ml

8ml

20ml

25ml

12ml

At constant pressure a gas occupies volume of 50ml at a temperature of 40°C. What will be the volume occupied by the gas at 90°C

43ml

58ml

112.5ml

22ml

58ml

A gas law which states that gases of equal volumes at the same temperature and pressure contain the same number of molecules

Boyles

Charles

Gay-Lussac

Avogadro

Avogadro

This is/are true values of the molar gas constants

0.08205 L-atm / mole-degree

8.314 cal / mole-degree

1.987 joules / mole-degree

I only

I and II only

II and III only

III only

I only

Assuming that a 1.5g gas occupying a volume of 500ml at a pressure of 175 atm and a temperature of 75°C is behaving like an ideal gas. What is the molecular weight of the gas?

0.05g

49g

5g

30g

49g

A method used to determine the molecular weight of easily vaporized liquids

Regnault

Victor-Meyer

Gieger-Muller

I only

I and II only

II and III only

III only

I and II only

A given quantity of gas at a pressure of 750mmHg and a temperature of -25°C occupies 25L. What is its volume at STP?

269L

150L

27.1L

100L

27.1L

How many moles of gas are present in a 25L chamber containing a pressure of 750mmHg at -25°C

1.21

9.21

2.51

0.42

1.21

How many moles of gas are present in a 25L chamber containing a pressure of 750mmHg at -25°C

1.21

9.21

2.51

0.42

1.21

This equation is used for real gases, where it accounts for the interactions of gas molecules hence affecting the pressure and volume of an ideal gas

Ideal Gas Equation

Van der Waals Equation

Noyes-Whitney Equation

Freundlich Equation

Van der Waals Equation

This states that the rate of diffusion of the gas and the speed of the gas molecules are inversely proportional to the square root of their density

Ideal Gas Law

Raoult's Law

Graham's Law

Dalton's Law

Graham's Law

This law gives the relationship between the total pressure in a mixture of gases and the partial pressure of the individual gases

Ideal Gas Law

Raoult's Law

Graham's Law

Dalton's Law

Dalton's Law

This is the point above which it is impossible to liquefy a gas irrespective of the pressure applied

Critical temperature

Critical pressure

Eutectic point

Triple point

Critical temperature

This is the highest vapour pressure that the liquid can have which is also the force er unit are required to liquefy a gas at critical temperature

Critical temperature

Critical pressure

Eutectic point

Triple point

Critical pressure

This is/are true statements regarding the comparison of the critical temperature and critical pressure of H2Oand helium gas

The critical temperature and critical pressure of water is much higher than that of helium

The critical temperature and critical pressure of helium is much higher than that of water

Water and Helium have similar critical temperature and critical pressure

I only

I and II only

II and III only

III only

I only

This is used as local anaesthetic agent for minor surgical operations administered as an aerosol. This substance cools sufficiently on expansion when sprayed on the skin and freezes the tissue to provide anaesthesia

Ethylene dioxide

Ethyl chloride

Nitrous oxide

Lidocaine

Ethyl chloride

This equation shows the relationship between the vapour pressure and the absolute temperature of a liquid

Ideal Gas Equation

Van der Waals Equation

Noyes-Whitney Equation

Clausius-Clapeyron Equation

Clausius-Clapeyron Equation

This is the heat absorbed by 1 mole of liquid when it passes into the vapour state

Molar Heat of Fusion

Molar Heat of Vaporization

Boiling point

Entropy

Molar Heat of Vaporization

Determine the vapour pressure of water at 150°C. The vapour pressure of water at 110°C is 1.5atm and molar heat of vaporization of 9500cal/mole

2.73atm

4.88atm

7.5atm

5.9atm

4.88atm

The vapour pressure of acetone at 100°C is 1.5atm and a molar heat of vaporization of 9750cal/mole. Determine the temperature at which its pressure will drop at sea level

362°C

80°C

89°C

120°C

89°C

The temperature at which the vapour pressure of the liquid equals the external or atmospheric

Melting point

Boiling point

Freezing point

Sublimation

Boiling point

Which of the following is/are true statement(s) about boiling point

At higher elevations the atmospheric pressure decreases, hence the boiling point increases

All the heat absorbed is used to change the liquid to vapour and the temperature does not rise until the liquid is completely vaporized

Boiling point of hydrocarbons, simple alcohols and carboxylic acids increase with an increase in molecular weight

I only

II only

I and II

II and III

I, II and III

II and III

This is the heat lost when the vapours condense to liquids

Heat of Condensation

Heat of Fusion

Heat of Vaporization

Heat of Fission

Heat of Vaporization

Which of the following is/are statement(s) that describes crystalline solids

They are made of structural units arranged in a loose geometric patterns or lattices

Crystalline solids are compressible unlike gases and liquids

Show definite and sharp melting points

I only

III only

I and II

II and III

I, II and III

III only

An example of a tetragonal crystal system is

Urea

Iodoform

Iodine

Sodium Chloride

Urea

Boric acid is an example of a __________ crystal system

Cubic

Hexagonal

Monoclinic

Triclinic

Triclinic

This is the crystal lattice formation of NaCl

Cubic

Hexagonal

Monoclinic

Triclinic

Cubic

Sucrose possess this type of crystal formation

Cubic

Hexagonal

Monoclinic

Triclinic

Monoclinic

The units that constitute the crystal structure can be atoms, molecules or ions. Which of the following substance(s) is/are crystal formation made of atoms

Diamonds and Graphite

NaCl

Solid CO2 and Naphthalene

I only

III only

I and II

II and III

I, II and III

I only

This is/are statement(s0 which characterized different crystal formation

Atomic and ionic crystals are generally soft and have low melting points

Molecular crystals are hard, brittle and have high melting points

Metallic crystals may be soft or hard

I only

III only

I and II

II and III

I, II and III

III only

The hardness and strength of metals are dependent on

Lattice defects

Electron gas

Attractive forces

Proton content

Lattice defects

This is the temperature at which the liquid state is at equilibrium with the solid state of a pure crystalline compound

Freezing point

Melting point

Boiling point

I only

II only

I and II

II and III

I, II and III

I and II

This is the heat lost when the liquid freezes into solid

Heat of Condensation

Heat of Fusion

Heat of Vaporization

Heat of Combustion

Heat of Fusion

This is/are true statement(s) about melting point

This is higher for alkanes with an even number of carbon atoms than those with odd number of carbons

This is generally high for crystals held together by Van der Waals forces than crystals held together by covalent bonds

This is the heat required to increase the intermolecular and intramolecular distances in crystals

I only

II only

I and II

II and III

I, II and III

I only

This is the lowest possible temperature in melting cacao butter so as not to destroy the crystal nuclei of the stable beta form

37°C

35°C

33°C

30°C

33°C

This is/are true statement(s) about the effect of polymorphism in a drug

One polymorph is chemically different from another polymorph

One polymorph may be biologically active than the other polymorph

Polymorphism may affect the dissolution rate of drugs

I only

II only

I and II

II and III

I, II and III

II and III

These are compounds which are also known as pseudopolymorphs

Solvates

Amorphous solid

Liquid crystals

Isomers

Solvates

This is the reversible change from one polymorphic form to another

Monotropic

Isotropic

Anisotropic

Enantiotropic

Enantiotropic

If the direction of change from one polymorphic form to another involves one direction, this is said to be a

Monotropic

Isotropic

Anisotropic

Enantiotropic

Monotropic

Crystals showing different characteristics in various directions along the crystal are

Monotropic

Isotropic

Anisotropic

Enantiotropic

Anisotropic

Crystalline substances that exhibit similar properties and characteristics in all directions are

Monotropic

Isotropic

Anisotropic

Enantiotropic

Isotropic

Which of the following statement(s) describe/s an amorphous solid

These are supercooled liquids

They don't have a definite melting point

Have faster rate of dissolution than crystalline solids

I only

II only

I and II

II and III

I, II and III

I, II and III

Which of the following describe(s) the fourth state of matter

Properties of which are intermediate between the liquid and solid states

Will flow if sufficient pressure is applied

They are also known as the mesophase

I only

II only

I and II

II and III

I, II and III

I and II

This is are types of liquid crystals which are also known as the soap-like or grease-like crystals

Smectic

Nematic

Cholesteric

Thermotropic

Smectic

This is also known as the thread-like crystals

Smectic

Nematic

Cholesteric

Thermotropic

Nematic

This is the third type of liquid crystals, which may be considered as a special case of the nematic type

Smectic

Nematic

Cholesteric

Thermotropic

Cholesteric

This is/are statements which describe(s) the smectic crystals

The molecules of this crystals are mobile in two directions and can rotate in one axis

Considered as the mesophase of the most pharmaceutical significance

This phase easily forms binary systems or simple mixtures with other additives

I only

II only

I and II

II and III

I, II and III

I and II

This is/are characteristics of molecules that forms the mesophase

Are inorganic in nature

Possess strong dipoles and easily polarizable groups

Are elongated, rectilinear in shape and rigid

I only

II only

I and II

II and III

I, II and III

II and III

These are liquid crystsals obtained from the action of certain solvents on solids

Smectic

Nematic

Lyotropic

Thermotropic

Lyotropic

These are forms of liquid crystals obtained from the application of sufficient heat on solids sto form the mesophase

Smectic

Nematic

Lyotropic

Thermotropic

Thermotropic

This was the first recorded type of liquid crystals that was derived through the application of heat

Cholesteryl benzoate

Calcium sterate

Sodium benzoate

Potassium acetate

Cholesteryl benzoate

This is the property of crystals which the mesophase also possess characterized as the ability to let light pass through and divide into two components with different velocities and refractive index

Refraction

Polymorphism

Birefringence

Isomerism

Birefringence

This is used for relating the effect of the least number of independent variables (e.g. temperature, pressure and concentration) upon the various phases that can exist in an equilibrium system containing a given of components

Le Chatelier's Principle

Gibb's Phase Rule

Triangular Planar

Phase Diagram

Gibb's Phase Rule

This represents the number of homogenous, physically distinct portion of a system that is separated from other portions of the system by bounding surfaces

Number of phases

Number of components

Degrees of freedom

Number of intermediates

Number of phases

This is the least number of intensive variables that must be fixed to describe the system completely

Number of phases

Number of components

Degrees of freedom

Number of intermediates

Degrees of freedom

This is the smallest number of constituents by which the composition of each phase in the system at equilibrium can be expressed in the form of a chemical formula or equation

Number of phases

Number of components

Degrees of freedom

Number of intermediates

Number of components

This is/are true generalization(s) in the Gibbs' phase rule for a single-component system

The number of the degrees of freedom increases with the increase in the number of components

The number of the degrees of freedom decreases with the increase in the number of phases

It is necessary to fix mor variable as the system becomes more complex

I only

II only

I and II

II and III

I, II and III

I, II and III

Determine the degrees of freedom of a system containing either ice, water or water vapour

1

2

3

0

2

What is the degree of freedom for a system containing a water in equilibrium with its vapour

1

2

3

0

1

Assuming that we have system wherein ice-water-water vapour are in equilibrium. What will be the degrees of freedom of the system

1

2

3

0

0

Determine the degrees of freedom for a system containing liquid water, liquid ethanol in equilibrium with their vapours

1

2

3

0

2

Which of the following represents the vapour pressure curve

Curve WX

Curve UX

Curve ZX

Curve ZX

Which of the following is the deposition curve

Curve WX

Curve YX

Curve ZX

Curve YX

Which of the following represents the condensation curve

Curve WX

Curve YX

Curve ZX

Curve ZX

This is the point at which variables are unnecessary to define the system

W

X

Y

Z

X

These are systems where in only the solid and liquid states are considered and the vapour state is ignored

Condensed System

Solid-Liquid Equilibrium System

Bivariant System

Conservative System

Condensed System

In the phase diagram of a two-component system containing two liquid phases, the maximum temperature at which the two-phase region exist is called the

Upper Consolute Temperature

Critical Solution Temperature

Upper Miscibility Temperature

I only

II only

I and II

II and III

I, II and III

I and II

Determine the amount of component X (water) and component Y(Phenol) needed in preparing 50g of a system that would contain 28% by weight phenol and 72% by weight water

4 g water and 1 g phenol

28 g phenol and 72 g water

40 g water and 10 g phenol

72 g phenol and 28 g water

40 g water and 10 g phenol

What will be the weight of phenol and water to be used in a 75g system containing 53% by weight of phenol and 47% by weight of water

3 g water and 7 g phenol

22.5 g water and 52.5 g phenol

53 g phenol and 47 g water

47 g phenol and 53 g water

22.5 g water and 52.5 g phenol

In preparing a 100g system containing equal portions of water and phenol, how much will be the required amount of each component?

36 g water and 64 g phenol

50 g water and 50 g phenol

64 g phenol and 36 g water

9 g phenol and 16 g water

36 g water and 64 g phenol

In the diagram which region represents the region where both components are present as pure solid phases

I

II

III

IV

IV

Which region is composed of solid salol and its conjugate liquid phase

I

II

III

IV

II

This is the region which represents the solid thymol and its conjugate liquid phase

I

II

III

IV

III

This is the region in which both thymol and salol will be present as a single liquid phase

I

II

III

IV

I

What will be the weight of thymol and salol at 35°C to be sued in a 75g system containing 75% by weight of phenol and 25% by weight of salol?

50 g salol and 25 g thymol

25 g salol and 50 g thymol

47 g salol and 28 g thymol

28 g salol and 47 g thymol

47 g salol and 28 g thymol

What will be the weight of thymol and salol at 27°C to be used in a 75g system containing 75% by weight of phenol and 25% by weight of salol?

50 g salol and 25 g thymol

35 g salol and 35 g thymol

25 g salol and 50 g thymol

40 g salol and 30 g thymol

35 g salol and 35 g thymol

What will be the weight of thymol and salol at 20°C to be used in a 75g system containing 75% by weight of phenol and 25% by weight of salol?

50.5 g salol and 24.5 g thymol

24.5 g salol and 50.5 g thymol

31.25 g salol and 43.75 g thymol

43.75 g salol and 31.25 g thymol

31.25 g salol and 43.75 g thymol

What will be the weights of thymol and salol required to prepare a 75g system at eutectic point

45 g salol and 30 g thymol

30 g salol and 45 g thymol

25 g salol and 50 g thymol

50 g salol and 25 g thymol

45 g salol and 30 g thymol

The heat involved in the complete oxidation of 1 mole of a compound at 1 atm pressure is known as

Heat of Condensation

Heat of Fusion

Heat of Vaporization

Heat of Combustion

Heat of Combustion

This is a condition where in heat is neither lost nor gained during a reaction

Adiabetic

Isothermal

Isobaric

Reversible

Adiabetic

A reaction where in temperature is held constant

Adiabetic

Isothermal

Isobaric

Reversible

Isothermal

Which law of thermodynamics states that the total energy of a system and its immediate surroundings remain constant during any operation

1st Law

2nd Law

3rd Law

1st Law

Which law of thermodynamics states that the entropy of a pure crystalline substance is zero at absolute zero because the crystal arrangement mush show the greatest orderliness at this temperature

1st Law

2nd Law

3rd Law

3rd Law

This law of thermodynamics is concerned about the entropy and spontaneity of a system

1st Law

2nd Law

3rd Law

2nd Law

This is the heat required to raise the temperature of 1 mole of a substance by 1 degree

Enthalpy

Molar Heat of Fission

Molar Heat Capacity

Molar Heat of Combustion

Molar Heat Capacity

The heat required to increase the internal energy and to perform work of expansion

Enthalpy

Molar Heat of Fision

Molar Heat Capacity

Molar Heat of Combustion

Enthalpy

These are any molecules which are associated with the absorption of ultraviolet or visible light

Phosphorescence

Chromophore

Photoluminescence

Fluorescence

Chromophore

A molecule that initially absorbs ultraviolet light to reach an excited state and then emits ultraviolet or visible light in returning to ground state is generally manifesting the process known as

Phosphorescence

Chromophore

Photoluminescence

Fluorescence

Photoluminescence

This is defined as a mixture of two or more components that form a homogenous molecular dispersion

System

True Solution

Mixture

Colloidal Dispersion

True Solution

This is defined as a bounded space or a definite quantity of substance that is under observation and experimentation

System

True Solution

Phase

Colloidal Dispersion

System

This is a distinct homogenous part of a system separated by definite boundaries from other parts of the system

System

True Solution

Phase

Colloidal Dispersion

Phase