[PHYSICAL PHARMACY] PACOP PINK

D

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

A. Accurate

B. Approximate

C. Estimate

D. Precise

C

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

A. Debye

B. London

C. Keesom

D. H-bond

A

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

molecules

A. Debye

B. London

C. Keesom

D. H-bond

B

A type of Van der Waals forces of attraction which involves the dispersion of charges to induce polarity

between non-polar molecules

A. Debye

B. London

C. Keesom

D. H-bond

C

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

solution by the addition of salts

A. Debye

B. Ion-dipole interaction

C. Ion-induced dipole interaction

D. H-bonds

B

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

A. Debye

B. Ion-dipole interaction

C. Ion-induced dipole interaction

D. H-bonds

D

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

I. Stronger than ionic bonds

II. Responsible for the formation of water molecules

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

A. I only

B. I and II only

C. II and III only

D. III only

E. I, II and III

A

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

A. Boyles

B. Charles

C. Gay-Lussac

D. Ideal Gas Law

C

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

I. Boyle

II. Charles

III. Gay-Lussac

A. I only

B. I and II only

C. II and III only

D. III only

E. I, II and III

A

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?

A. 12ml

B. 8ml

C. 20ml

D. 25ml

B

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

A. 43ml

B. 58ml

C. 112.5ml

D. 22ml

D

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

same number of molecules

A. Boyles

B. Charles

C. Gay-Lussac

D. Avogadro

A

This is/are true values of the molar gas constants

I. 0.08205 L-atm / mole-degree

II. 8.314 cal / mole-degree

III. 1.987 joules / mole-degree

A. I only

B. I and II only

C. II and III only

D. III only

B

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?

A. 0.05g

B. 49g

C. 5g

D. 30g

B

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

I. Regnault

II. Victor-Meyer

III. Gieger-Muller

A. I only

B. I and II only

C. II and III only

D. III only

C

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

volume at STP?

A. 269L

B. 150L

C. 27.1L

D. 100L

A

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

A. 1.21

B. 9.21

C. 2.51

D. 0.42

B

The following is/are true statements regarding the kinetic molecular theory

I. Volume of gas is negligible in relation to the volume of the space in which the gas is confined

II. Particles exhibit continuous random motion owing to their kinetic energy

III. Speed is lost every time particles go into collision with each other or with the walls of the vessels

A. I only

B. I and II only

C. II and III only

D. III only

B

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

A. Ideal Gas Equation

B. Van der Waals Equation

C. Noyes-Whitney Equation

D. Freundlich Equation

C

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

A. Ideal Gas Law

B. Raoult's Law

C. Graham's Law

D. Dalton's Law

D

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

the individual gases

A. Ideal Gas Law

B. Raoult's Law

C. Graham's Law

D. Dalton's Law

A

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

A. Critical temperature

B. Critical pressure

C. Eutectic point

D. Triple point

B

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

A. Critical temperature

B. Critical pressure

C. Eutectic point

D. Triple point

A

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

H2Oand helium gas

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

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

III. Water and Helium have similar critical temperature and critical pressure

A. I only

B. I and II only

C. II and III only

D. III only

B

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

A. Ethylene dioxide

B. Ethyl chloride

C. Nitrous oxide

D. Lidocaine

D

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

A. Ideal Gas Equation

B. Van der Waals Equation

C. Noyes-Whitney Equation

D. Clausius-Clapeyron Equation

B

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

A. Molar Heat of Fusion

B. Molar Heat of Vaporization

C. Boiling point

D. Entropy

B

. 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

A. 2.73atm

B. 4.88atm

C. 7.5atm

D. 5.9atm

C

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

A. 362°C

B. 80°C

C. 89°C

D. 120°C

B

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

A. Melting point

B. Boiling point

C. Freezing point

D. Sublimation

D

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

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

II. All the heat absorbed is used to change the liquid to vapour and the temperature does not

rise until the liquid is completely vaporized

III. Boiling point of hydrocarbons, simple alcohols and carboxylic acids increase with an increase

in molecular weight

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

C

This is the heat lost when the vapours condense to liquids

A. Heat of Condensation

B. Heat of Fusion

C. Heat of Vaporization

D. Heat of Fission

B

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

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

II. Crystalline solids are compressible unlike gases and liquids

III. Show definite and sharp melting points

A. I only

B. III only

C. I and II

D. II and III

E. I, II and II

A

An example of a tetragonal crystal system is

A. Urea

B. Iodoform

C. Iodine

D. Sodium Chloride

D

Boric acid is an example of a __________ crystal system

A. Cubic

B. Hexagonal

C. Monoclinic

D. Triclinic

A

This is the crystal lattice formation of NaCl

A. Cubic

B. Hexagonal

C. Monoclinic

D. Triclinic

C

Sucrose possess this type of crystal formation

A. Cubic

B. Hexagonal

C. Monoclinic

D. Triclinic

A

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

I. Diamonds and Graphite

II. NaCl

III. Solid CO2 and NaphthaleneA. I only

B. III only

C. I and II

D. II and III

E. I, II and III

B

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

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

II. Molecular crystals are hard, brittle and have high melting points

III. Metallic crystals may be soft or hard

A. I only

B. III only

C. I and II

D. II and III

E. I, II and III

A

The hardness and strength of metals are dependent on

A. Lattice defects

B. Electron gas

C. Attractive forces

D. Proton content

C

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

compound

I. Freezing point

II. Melting point

III. Boiling point

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

B

This is the heat lost when the liquid freezes into solid

A. Heat of Condensation

B. Heat of Fusion

C. Heat of Vaporization

D. Heat of Combustion

A

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

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

II. This is generally high for crystals held together by Van der Waals forces than crystals held together by

covalent bonds

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

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

C

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

stable beta form

A. 37°C

B. 35°C

C. 33°C

D. 30°C

D

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

I. One polymorph is chemically different from another polymorph

II. One polymorph may be biologically active than the other polymorph

III. Polymorphism may affect the dissolution rate of drugs

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

A

These are compounds which are also known as pseudopolymorphs

A. Solvates

B. Amorphous solid

C. Liquid crystals

D. Isomers

D

This is the reversible change from one polymorphic form to another

A. Monotropic

B. Isotropic

C. Anisotropic

D. Enantiotropic

A

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

A. Monotropic

B. Isotropic

C. Anisotropic

D. Enantiotropic

C

Crystals showing different characteristics in various directions along the crystal are

A. Monotropic

B. Isotropic

C. Anisotropic

D. Enantiotropic

B

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

A. Monotropic

B. Isotropic

C. Anisotropic

D. Enantiotropic

E

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

I. These are supercooled liquids

II. They don't have a definite melting point

III. Have faster rate of dissolution than crystalline solids

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

C

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

I. Properties of which are intermediate between the liquid and solid states

II. Will flow if sufficient pressure is applied

III. They are also known as the mesophase

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

A

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

A. Smectic

B. Nematic

C. Cholesteric

D. Thermotropic

B

This is also known as the thread-like crystals

A. Smectic

B. Nematic

C. Cholesteric

D. Thermotropic

C

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

A. Smectic

B. Nematic

C. Cholesteric

D. Thermotropic

C

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

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

II. Considered as the mesophase of the most pharmaceutical significance

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

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

D

This is/are characteristics of molecules that forms the mesophase

I. Are inorganic in nature

II. Possess strong dipoles and easily polarizable groups

III. Are elongated, rectilinear in shape and rigid

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

C

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

A. Smectic

B. Nematic

C. Lyotropic

D. Thermotropic

D

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

mesophase

A. Smectic

B. Nematic

C. Lyotropic

D. Thermotropic

A

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

A. Cholesteryl benzoate

B. Calcium sterate

C. Sodium benzoate

D. Potassium acetate

C

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

A. Refraction

B. Polymorphism

C. Birefringence

D. Isomerism

B

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

A. Le Chatelier's Principle

B. Gibb's Phase Rule

C. Triangular Planar

D. Phase Diagram

A

This represents the number of homogenous, physically distinct portion of a system that is separated from

other portions of the system by bounding surfaces

A. Number of phases

B. Number of components

C. Degrees of freedom

D. Number of intermediates

C

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

A. Number of phases

B. Number of components

C. Degrees of freedom

D. Number of intermediates

B

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

A. Number of phases

B. Number of components

C. Degrees of freedom

D. Number of intermediates

E

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

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

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

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

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

B

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

A. 1

B. 2

C. 3

D. 0

A

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

A. 1

B. 2

C. 3

D. 0

D

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

of freedom of the system

A. 1

B. 2

C. 3

D. 0

B

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

their vapours

A. 1

B. 2

C. 3

D. 0

C

Which of the following represents the vapour pressure curve (Refer to diagram for #71-74)

A. Curve WX

B. Curve UX

C. Curve ZX

B

Which of the following is the deposition curve

A. Curve WX

B. Curve YX

C. Curve ZX

C

Which of the following represents the condensation curve

A. Curve WX

B. Curve YX

C. Curve ZX

B

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

A. W

B. X

C. Y

D. Z

A

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

A. Condensed System

B. Solid-Liquid Equilibrium System

C. Bivariant System

D. Conservative System

C

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

I. Upper Consolute Temperature

II. Critical Solution Temperature

III. Upper Miscibility Temperature

A. I only

B. II only

C. I and II

D. II and III

E. I, II and III

C

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 (Refer to diagram for #77-79)

A. 4 g water and 1 g phenol

B. 28 g phenol and 72 g water

C. 40 g water and 10 g phenol

D. 72 g phenol and 28 g water

B

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

A. 3 g water and 7 g phenol

B. 22.5 g water and 52.5 g phenol

C. 53 g phenol and 47 g water

D. 47 g phenol and 53 g water

A

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

amount of each component?

A. 36 g water and 64 g phenol

B. 50 g water and 50 g phenol

C. 64 g phenol and 36 g water

D. 9 g phenol and 16 g water

D

In the diagram which region represents the region where both components are present as pure solid phases (Refer to Diagram for #80-87)

A. I

B. II

C. III

D. IV

B

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

A. I

B. II

C. III

D. IV

C

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

A. I

B. II

C. III

D. IV

A

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

A. I

B. II

C. III

D. IV

C

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?

A. 50 g salol and 25 g thymol

B. 25 g salol and 50 g thymol

C. 47 g salol and 28 g thymol

D. 28 g salol and 47 g thymol

B

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?

A. 50 g salol and 25 g thymol

B. 35 g salol and 35 g thymol

C. 25 g salol and 50 g thymol

D. 40 g salol and 30 g thymol

C

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?

A. 50.5 g salol and 24.5 g thymol

B. 24.5 g salol and 50.5 g thymol

C. 31.25 g salol and 43.75 g thymol

D. 43.75 g salol and 31.25 g thymol

A

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

A. 45 g salol and 30 g thymol

B. 30 g salol and 45 g thymol

C. 25 g salol and 50 g thymol

D. 50 g salol and 25 g thymol

D

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

A. Heat of Condensation

B. Heat of Fusion

C. Heat of Vaporization

D. Heat of Combustion

A

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

A. Adiabetic

B. Isothermal

C. Isobaric

D. Reversible

B

A reaction where in temperature is held constant

A. Adiabetic

B. Isothermal

C. Isobaric

D. Reversible

A

Which law of thermodynamics states that the total energy of a system and its immediate surroundings

remain constant during any operation

A. 1st Law

B. 2nd Law

C. 3rd Law

C

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

A. 1st Law

B. 2nd Law

C. 3rd Law

B

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

A. 1st Law

B. 2nd Law

C. 3rd Law

C

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

A. Enthalpy

B. Molar Heat of Fission

C. Molar Heat Capacity

D. Molar Heat of Combustion

A

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

A. Enthalpy

B. Molar Heat of Fision

C. Molar Heat Capacity

D. Molar Heat of Combustion

B

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

A. Phosphorescence

B. Chromophore

C. Photoluminescence

D. Fluorescence

C

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

A. Phosphorescence

B. Chromophore

C. Photoluminescence

D. Fluorescence

B

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

A. System

B. True Solution

C. Mixture

D. Colloidal Dispersion

A

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

experimentation

A. System

B. True Solution

C. Phase

D. Colloidal Dispersion

C

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

system

A. System

B. True Solution

C. Phase

D. Colloidal Dispersion