MOD 2 Flashcards

RESET

1
Q

Molecules PACKED close together closely, vibrating in FIXED POSITION

A

SOLID

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2
Q

Molecules are close but RANDOMLY ARRANGED

Flows and ASSUMES SHAPE of container

A

LIQUID

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3
Q

Molecules are FAR APART

Fills any container completely

A

GAS

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4
Q

In order for molecules to exist in aggregates in gases, liquids, and solids, __________ must exist

A

INTERMOLECULAR FORCES

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5
Q

responsible for the behavior of molecules in solid, liquid, and gas

A

INTERMOLECULAR FORCES

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6
Q

Solid → liquid → gas

A

BREAKING OF BONDS

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7
Q

Gas → liquid → solid

A

FORMATION OF BONDS

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8
Q

factors that would make bonds either broken or established

A

TEMPERATURE & PRESSURE

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9
Q

Transition of a substance directly from SOLID state TO a GAS state

A

SUBLIMATION

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10
Q

A process in which a GAS does DIRECTLY to a SOLID, BYPASSING THE LIQUID PHASE

A

DEPOSITION

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11
Q

for VASODILATION, volatile, formulated in closed glass tube

A

AMYL NITRITE (liquid state)

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12
Q

Described as molecules that have HIGHER KINETIC ENERGY (energy in movement) that produces RAPID MOTION

A

GASEOUS STATE

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13
Q

ENERGY IN MOTION

A

KINETIC ENERGY

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14
Q

A FORCE per unit area (dynes/cm2) as they COLLIDE to ONE ANOTHER and to WALLS OF THE CONTAINER to which they are confined.

A

PRESSURE (gas)

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15
Q

Normal atmospheric level within sea level

A

1 atm or 760 mmHg

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16
Q

PROPERTIES OF GAS

A

pressure
volume
temperature

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17
Q
  • perfectly ELASTIC collision
  • NO intermolecular forces of attraction
A

IDEAL GAS LAW

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18
Q

PRESSURE and VOLUME of gases are INVERSELY PROPORTIONAL
- the lower the volume, the higher the pressure

A

BOYLE’S LAW

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19
Q

BOYLE’S LAW

A

pressure & volume are inversely proportional at constant temperature

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20
Q

states that the PRESSURE (p) of a given quantity of gas varies INVERSELY with its VOLUME (v) at CONSTANT TEMPERATURE

A

ROBERT BOYLE

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21
Q

Volume - Temperature relationship at constant Pressure
- the higher the volume, the higher the temperature

A

CHARLES’ LAW

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22
Q

CHARLES’ LAW

A

volume & temperature are directly proportional

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23
Q

what is constant in boyle’s law

A

TEMPERATURE

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24
Q

what is constant in charles’ law

A

PRESSURE

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25
Q

what is constant in gay lussac’s law

A

VOLUME

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26
Q

Pressure - Temperature relationship at constant Volume
- the higher the pressure, the higher the temperature

A

GAY-LUSSAC’S LAW

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27
Q

States that the PRESSURE of a given amount of gas held at CONSTANT VOLUME is DIRECTLY PROPORTIONAL to the Kelvin TEMPERATURE.

A

GAY-LUSSAC

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28
Q

States that the VOLUME of an ideal gas is DIRECTLY PROPORTIONAL to the absolute TEMPERATURE at CONSTANT PRESSURE.

A

CHARLES

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29
Q

IDEAL GAS LAW equation

A

PV = nRT

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30
Q

unit for volume

A

L

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31
Q

unit for Temperature

A

K

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32
Q

unit for Pressure

A

atm

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33
Q

unit for n

A

mol

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34
Q

formula if molwt hinahanap

A

PV = nRT/molwt

molwt = nRT/PV

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35
Q

Describes how gases consist of tiny particles in constant motion, with their behavior influenced by factors like temperature and pressure.

A

KINETIC MOLECULAR THEORY

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36
Q

The theory that was developed to EXPLAIN THE BEHAVIOR OF GASES and to lend additional support to the VALIDITY OF THE GAS LAWS.

A

KINETIC MOLECULAR THEORY

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37
Q

The volume of gas is (kinetic mol theo)

A

NEGLIGIBLE

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38
Q

Who showed that a LIGHTER GAS DIFFUSES MORE RAPIDLY through a porous membrane than does a heavier one

A

GRAHAM’S LAW

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39
Q

NOT composed of infinitely small and perfectly elastic non-attracting spheres

A

REAL GASES

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40
Q

▪ Have finite volume
▪ Tend to attract one another
* There is an intermolecular binding force.

A

REAL GASES

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41
Q

formula for REAL GAS

A

[P + an2/v2] (V - nb) = nRT

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42
Q

ATTRACTION BETWEEN THE GAS PARTICLES, brought about by intermolecular binding forces that may exist

A

INTERNAL PRESSURE [an2/v2)

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43
Q

VOLUME OCCUPIED BY THE GAS PARTICLES; volume lost when molecules are held closely together

A

EXCLUDED VOLUME (nb)

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44
Q

incompressability of molecules

A

nb - excluded volume

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45
Q

The TEMPERATURE to LIQUEFY THE GAS and establish intermolecular binding forces is

A

LOW ↓

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46
Q

The PRESSURE to LIQUEFY THE GAS and establish intermolecular binding forces is

A

HIGH ↑

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47
Q

↓ temperature
↑ pressure

A

LIQUEFACTION OF GASES

GAS → LIQUID

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48
Q
  • Possess LESS kinetic energy than gases
  • Occupy a DEFINITE VOLUME denser than gas
  • Take the shape of the container
  • INCOMPRESSIBLE
A

LIQUID STATE

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49
Q

Gas molecules LOSE their kinetic energy in the form of

A

HEAT

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50
Q
  • Temperature above which LIQUID NO LONGER EXISTS
A

CRITICAL TEMPERATURE

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51
Q
  • Pressure required to liquefy a gas at Tcrit
A

CRITICAL PRESSURE

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52
Q

critical temperature of water

A

374 °C

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53
Q

critical pressure of water

A

218atm

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54
Q

volume is approx 0

A

NEGLIGIBLE VOLUME

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55
Q

the particles of GAS DO NOT ATTARCT ONE ANOTHER at ___ pressures

A

LOW PRESSURES

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56
Q

one of the most obvious ways to liquefy a gas is to subject it to

A

INTENSE COLD using FREEZING MIXTURES

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57
Q

a rapid EXPANSION of ideal gas to which no heat could enter the system (gas)

A

ADIABATIC EXPANSION

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58
Q

Adiabatic expansion can be carried out by using ______ which effectively INSULATES the contents of the flask from the external environment

A

DEWAR or VACUUM FLASK

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59
Q

A ____ is observed when a HIGHLY COMPRESSED NONIDEAL GAS EXPANDS into a region of low pressure

A

COOLING EFFECT

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60
Q

the COOLING EFFECT that is observed when a HIGHLY COMPRESSED NONIDEAL GAS EXPANDS into a region of low pressure and differs from the cooling produced in adiabatic expansion

A

JOULE-THOMSON EFFECT

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61
Q

to bring about liquefaction by the Joule-Thomson effect, it may be necessary to __________ before allowing it to expand

A

PRECOOL THE GAS

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62
Q

a material that is LIQUID under the pressure conditions existing inside the container but that forms a GAS under normal atmospheric conditions

A

PROPELLANT

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63
Q

traditionally been utilized as propellants but is now BANNED

A

CHLOROFLUOROCARBONS & HYDROFLUOROCARBONS

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64
Q

Inside the aerosol

A

REAL GAS

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65
Q

outside the aerosol

A

IDEAL GAS

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66
Q

Subjecting the propellant into an EXTREME COLD TEMPERATURE and EXTREME HIGH PRESSURE

A

ADIABATIC EXPANSION

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67
Q

expanding the volume of gas using ideal gas

A

ADIABATIC EXPANSION

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68
Q

COMPRESSED real gas into an area with LOW PRESSURE

A

JOULE-THOMSON EFFECT

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69
Q

REMOVING ENERGY FROM THE SYSTEM will provide extreme cold temperature, wherein movement of gaseous molecule will become extremely slow and compress high pressure until intermolecular will exist and gas will be converted to liquid state

A

JOULE-THOMSON EFFECT

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70
Q

when the rate of condensation EQUALS the rate of vaporization at a definite temperature, the vapor becomes ________ and a dynamic _______ is established

A

SATURATED, EQUILIBRIUM

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71
Q

the PRESSURE OF SATURATED VAPOR above the liquid

A

EQUILIBRIUM VAPOR PRESSURE

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72
Q

Absorb heat energy → translated to kinetic energy → gas molecules move and oscillate → bonds are broken → molecules evaporate and converted to gaseous state (water vapor)

A

OPEN SYSTEM

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73
Q

high pressure (compressed system) → molecules of water vapor are held closed → vapor pressure returns to liquid state

A

CLOSED SYSTEM

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74
Q

equal evaporation and condensation

A

EQUILIBRIUM VAPOR PRESSURE

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75
Q

water is lost, all liquid will be converted to GASEOUS STATE

A

TEMP INCREASES, PRESSURE CONSTANT

76
Q

NO more liquid state, ONLY VAPOR PRESSURE will exist

A

PRESSURE INCREASES, TEMP IS CONSTANT

77
Q

the relationship between the VAPOR PRESSURE and the ABSOLUTE TEMPERATURE of a liquid is expressed by

A

CLAUSIUS-CLAPEYRON EQUATION

78
Q

____________ by MOLECULES OF LIQUID so that it will be converted to the GASEOUS STATE

A

HEAT ABSORBED

79
Q

_________ by the WATER VAPOR so that it will be converted to LIQUID STATE

A

HEAT LIBERATED

80
Q

compute the CHANGE IN TEMPERATURE such as boiling point WHEN THERE IS A CHANGE IN PRESSURE

A

CLAUSIUS-CLAPEYRON EQUATION

81
Q

heat absorbed by 1 mole of liquid when it passes to gas

A

MOLAR HEAT OF VAPORIZATION

82
Q

the boiling point of water at 1 atm

A

100C

83
Q

vapor pressure = atmospheric pressure

A

BOILING POINT

84
Q

Drug substances in liquid state

A

problematic, volatile

85
Q

Most of the drug substances exists in

A

CRYSTALLINE OR AMORPHOUS FORM

86
Q
  • They are MOST FAVORABLE drug substance since they are stable.
  • Easiest to manipulate and to handle
A

SOLID

87
Q

VASODILATOR (liquid) but can formulate as SUBLINGUAL TABLET (under the tongue), VOLATILE IF NOT SEALED PROPERLY

A

NITROGLYCERIN

88
Q

They have a definite shape and GEOMETRICAL FORM

A

CRYSTALLINE

89
Q

Crystalline solids have a _____ melting point

A

SHARP

90
Q

a SOFT solid

A

GRAPHITE

91
Q

crystalline solids have ____ cleavage

A

CLEAN

92
Q

They have a DEFINITE HEAT OF INFUSION.

A

CRYSTALLINE SOLIDS

93
Q

crystalline solids are _____

A

ANISTROPIC

94
Q

amorphous solids are ______

A

ISOTROPIC

95
Q

different arrangements of lattices/crystalline

A

HABIT

96
Q
  • Arranged in LATTICES – fixed geometric pattern
  • Definite melting points
  • Rate and stability
  • Habit
A

CRYSTALLINE SOLIDS

97
Q

6 CRYSTAL SYSTEMS

A

CUBIC
TETRAGONAL
HEXAGONAL
RHOMBIC
MONOCLINIC
TRICLINIC

98
Q

IDENTIFY THE CRYSTAL SYSTEM:
sodium chloride

A

CUBIC

99
Q

IDENTIFY THE CRYSTAL SYSTEM:
urea

A

TETRAGONAL

100
Q

IDENTIFY THE CRYSTAL SYSTEM:
iodoform

A

HEXAGONAL

101
Q

IDENTIFY THE CRYSTAL SYSTEM:
iodine

A

RHOMBIC

102
Q

IDENTIFY THE CRYSTAL SYSTEM:
sucrose

A

MONOCLINIC

103
Q

IDENTIFY THE CRYSTAL SYSTEM:
boric acid

A

TRICLINIC

104
Q

morphology of a crystalline form

A

HABIT

105
Q

Same elemental substances, but different crystalline forms

A

POLYMORPHISM

106
Q

the ability for a compound to exist in MORE THAN ONE CRYSTAL FORM with different unit cell parameters

A

POLYMORPHISM

107
Q

the existence of a chemical element in two or more forms

A

ALLOTROPY

108
Q

examples of polymorphs

A

CARBON & SULFUR

109
Q

a special case of polymorphism

A

ALLOTROPIC

110
Q

a polymorphous natural fat
- consists mainly of a single glyceride

A

THEOBROMA OIL OR CACAO BUTTER

111
Q

Theobroma oil is capable of existing in how many polymorphic forms

A

4

112
Q

Melting point:
UNSTABLE GAMMA FORM

A

18C

113
Q

Melting point:
ALPHA FORM

A

22C

114
Q

Melting point:
BETA PRIME FORM

A

28C

115
Q

Melting point:
STABLE BETA FORM

A

34.5C

116
Q
  • Crystalline structure containing WATER MOLECULE
  • Hydrous form
  • Anhydrous form
A

HYDRATES

117
Q
  • Crystalline structure containing solvent molecules
A

SOLVATES

118
Q

Another term for amorphous solid

A

SUPERCOOLED LIQUIDS

119
Q
  • Has a YIELD VALUE and no definite melting point
  • Difference in rate of dissolution of antibiotic novobiocin
A

AMORPHOUS SOLIDS

120
Q

faster rate of dissolution

A

AMORPHOUS FORM OF NOVOBIOCIN

121
Q

slower rate of dissolution

A

CRYSTALLINE FORM OF NOVOBIOCIN

122
Q

heat absorbed so that solid can be converted to liquid state; heat liberated so that liquid is converted to solid state

A

LATENT HEAT OF FUSION

123
Q
  • For solids and liquids
  • Compute for change in FREZZING and MELTING POINT
A

CLAPEYRON EQUATION

124
Q
  • The position of equilibrium will move in such a way as to COUNTERACT THE CHANGE
  • The system in equilibrium will adjust to REDUCE STRESS.
  • Volume of solid > Volume of liquid
A

LA CHATELIER’S PRINCIPLE

125
Q

exhibit SIMILAR PROPERTIES in ALL DIRECTIONS

A

ISOTROPIC

126
Q

showing DIFFERENT CHARACTERISTICS in VARIOUS DIRECTIONS along the crystal

A

ANISTROPIC

127
Q
  • Molecules are immobile and no rotations
A

CRYSTAL

128
Q
  • One of the mesophases or intermediate states
  • Intermediate state between solid and liquid
A

LIQUID CRYSTAL

129
Q

Two types of liquid crystals

A

SMECTIC
NEMATIC

130
Q

mobile in 2 directions and rotate about 1 axis

A

SMECTIC

131
Q

mobile in 3 directions and rotate about 1 axis

A

NEMATIC

132
Q

special type of NEMATIC

A

CHOLESTERIC

133
Q

Molecules are mobile in 3 directions and rotate about 3 axes

A

LIQUID

134
Q

the temperature at which a liquid passes into the solid state

A

FREEZING POINT

135
Q

a system at equilibrium READJUSTS to REDUCE THE EFFECT of an external stress

A

LE CHATELIER’S PRINCIPLE

136
Q

ability of drug to be ABSORBED

A

BIOAVAILABILITY

137
Q

antibacterial

A

SULFAMETER

138
Q

antiviral na nagprecipitate

A

RITONAVIR

139
Q

mas maganda from 2 pero most products that are available in the market is in form 3

A

SULFAMETER

140
Q

solid + liquid properties

A

LIQUID CRYSTALLINE STATE

141
Q

4th state of matter

A

LIQUID CRYSTALLINE STATE / MESOPHASE

142
Q

solid compounds but MOLECULES ARE MOVING

A

LIQUID CRYSTALS

143
Q

SOAP LIKE OR GREASE LIKE

A

SMECTIC

144
Q

THREAD LIKE

A

NEMATIC

145
Q

gas + liquid properties

A

SUPERCRITICIAL FLUID STATE

146
Q

supercritical fluid state movement

A

LIKE GAS

147
Q

a supercritical fluid is a _______ formed from the gaseous state where the gas is held under a combination of temperature and pressures that EXCEED THE CRITICAL POINT

A

MESOPHASE

148
Q

LCD meaning

A

LIQUID CRYSTALLINE DISPLAY

149
Q

for EMULSION STABILITY as well as increase in SOLUBILIZATION

A

SMECTIC

150
Q

for LCD displays

A

NEMATIC

151
Q
  • Solubilization and dissolution of cholesterol found in GALLSTONES
  • Used as BIOPHYSICAL model for the structure and functionality of cell membranes
A

LIQUID CRYSTALS

152
Q
  • Gas-like since it can go through spaces
  • Liquid-like since it is dense
  • BEYOND CRITICAL TEMPERATURE and when you keep applying pressure, this will increase in density and since it cannot be converted to liquid state, the VISCOSITY REMAINS AS A GAS.
  • It has the DENSITY OF LIQUID, but the VISCOSITY IS GASEOUS.
A

SUPERCRITICAL FLUIDS

153
Q

supercritical fluid density

A

liquid

154
Q

supercritical fluid viscosity

A

gaseous

155
Q

a point where it can exist as solid, liquid, gas

A

TRIPLE POINT

156
Q

TEMP:
solid & gas

A

LOW TEMP

157
Q

TEMP:
liquid & gas

A

MIDDLE TEMP

158
Q
  • Extraction
  • Crystallization
  • Preparation of formulations (for micro and nanoparticles)
  • Decaffeination of coffee (has replaced methylene chloride)
A

SUPERCRITICAL FLUID

159
Q

defined by a series of independent variables

A

PHASES OF MATTER

160
Q
  • Different phases are coexisting, such as coexistence of water and gas, coexistence of solid and gas, or coexistence of 3 states of matter AT THE SAME TIME
A

PHASE EQUILIBRIA & PHASE RULE

161
Q

who formulated the PHASE RULE

A

J. WILLARD GIBS

162
Q

a relationship for determining the LEAST NUMBER OF INTENSIVE VARIABLES that CAN BE CHANGED without changing the equilibrium state of the system, or, alternatively, the LEAST NUMBER required to define the state of the system

A

PHASE RULE

163
Q

PHASE RULE EQUATION

A

F = C - P + 2

164
Q

number of degrees of freedom

A

F

165
Q

no of components

A

C

166
Q

no of phases

A

P

167
Q

the SMALLEST NUMBER OF CONSTITUENTS by which the composition of each phase in the system at equilibrium

A

NUMBER OF COMPONENTS

168
Q

a HOMOGENOUS portion of a system that is SEPARATED from other portions of the system by bounding surfaces

A

PHASE

169
Q

the LEAST NUMBER of INTENSIVE VARIABELS that must be FIXED/KNOWN to describe the system completely

A

NUMBER OF DEGREES OF FREEDOM

170
Q

TWO variables (temp
and pressure) must be fixed to define the system

A

BIVARIANT

171
Q

ONE variable (temp or
pressure) must be fixed to define the system

A

UNIVARIANT

172
Q

temp and pressure are
already fixed and defined

A

INVARIANT (0)

173
Q

hexane + water (phase)

A

2 PHASES

174
Q

Two-Component System is also known as

A

CONDENSED SYSTEM

175
Q
  • System in which VAPOR PHASE IS IGNORED and only the SOLID and/or LIQUID phases are CONSIDERED
A

TWO-COMPONENT SYSTEM / CONDENSED SYSTEM

176
Q

Containing Solid-Liquid Phases

A

EUTECTIC MIXTURES

177
Q

area within the curve represents a two-phase system; Any point beyond it is a single phase

A

BINODAL CURVE

178
Q

temperature beyond which every proportion of A & B will exist as 1-phase; maximum temperature to obtain a one phase system

A

CRITICAL SOLUTION TEMPERATER (UPPER CONSOLUTE TEMPERATURE)

179
Q

line from which a system separates into phases of constant composition; used to approximate the proportions of components A & B existing at a particular temperature

A

TIE LINE

180
Q

phases of constant composition that separate when a mixture is prepared within the boundary of the 2-phase system

A

CONJUGATE PHASE

181
Q

the COMPOSITION OF TWO OR MORE COMPOUNDS that exhibits a melting temperature lower than that of any other mixture of the compounds.
o MPA+B < MPA or MPA+B < MPB

A

EUTECTIC MIXTURE

182
Q

the point at which the liquid and solid phases have the SAME COMPOSITION, CO-EXISTING

A

EUTECTIC POINT

183
Q

phenomenon of LOWERING THE MELTING POINT due to COMBINATION OF COMPONENTS (thymol-salol; camphor-menthol)

A

EUTEXIA

184
Q

a system consisting 3 components existing in phase equilibrium.

A

THREE COMPONENT SYSTEM / TERNARY SYSTEM

185
Q

In a three component system, Temperature and pressure are both made ______

A

CONSTANT

186
Q

Consists of two liquids that are PARTIALLY MISCIBLE TO EACH OTHER and the third component acts as co-solvent which has the affinity to both immiscible layers

A

THREE COMPONENT SYSTEM