PRELIM 02 - States of Matter Flashcards
Total heat lost or gained in the conversion involving solid and liquid by 1 mole of substance
Molar heat of fusion
2 heat processes
Endothermic, Exothermic
Refers to when heat is absorbed
Endothermic
Refers to when heat is released
Exothermic
Term used to describe the total heat content of a particular system
Enthalpy
Term used to describe the molecular randomness/disorderliness of a particular system
Entropy
Total heat required for the conversion involving liquid and gas by 1 mole of liquid substance
Molar heat of vaporization
Graphs that relate pressure and temperature to the state of matter
Phase diagrams
Other name for phase diagrams
Temperature-composition diagram
Rule that determines the relationship for the least number of intensive variables
Gibb’s phase rule
A homogenous part of the system, physically separated by distinct boundaries
Phase
Composition (one, two, or three components)
Component
Do not depend on the amount of matter present of the phases
Independent variables
The number of independent parameters that define its configuration
Degrees of freedom
No pressure is involved; vapor phase is ignored
Condensed system
Pressure is considered; involves gas
Noncondensed system
Originates from measurements using a barometer
Millimeters of mercury (mmHg)
Other name for mmHg
Torr
Person who invented torr
Evangelista Torricelli
1 mmHg = _____ Torr
1 torr
Average atmospheric pressure at sea level
Atmosphere (atm)
1 atm = _____ mmHg
760 mmHg
SI unit for pressure
Pascal (Pa)
Average air pressure at sea level
101,325 Pa
1 Pa = _____ N/m^2
1 N/m^2
1 atm = _____ in Hg (inches of mercury)
29.92 in Hg
1 atm = _____ psi (pounds power square inch)
14.7 psi
The pressure exerted by a single component in a mixture of gases
Partial pressure (Pn)
The average distance that a gas particle travels between collisions
Mean free path
Process by which gas particles spread out in response to a concentration gradient
Diffusion
Process by which gas particles escape from a container into a vacuum through small hole
Effusion
Means that no heat enters the system
Adiabatic
Where the gas does external work
Joule-Thomson effect
The temperature at which the vapor pressure of the liquid equals the external or atmospheric pressure
Boiling point
Found that a dissolved solute lowers the vapor pressure of the solvent
FM Raoult
States that the partial pressure exerted by solvent vapor above an ideal solution (Pa) is the product of the mole fraction of solvent solution (Xa) and the vapor pressure of the pure solvent at the given temperature (PoA)
Raoult’s law
Supercooled liquids in which the molecules are arranged in a somewhat random manner
Amorphous solids
Where substances exist in more than one crystalline form, and are said to be allotropic
Polymorphism
Change from one form to another is reversible
Enantiotropic
When transition takes place in one direction only (metastable to stable)
Monotropic
Exhibit similar properties in all directions
Isotropic
Shows different characteristics in various directions along the crystal
Anisotropic
States that if a system at equilibrium is disturbed by a change in concentration, pressure, or temperature; the system will shift its equilibrium position so as to counter the effect of the disturbance
Le Chatelier’s principle
Formed using solvents
Lyotropic
Formed using temperature
Thermotropic
Predicted by Satyendra Nath Bose and Albert Einstein; dilute gas cooled to temperature very near to absolute zero
Bose-Einstein condensates
Refers to the temperature when the liquid phase no longer exists
Critical temperature
Refers to the pressure needed to liquify a gas at its critical temperature
Critical pressure
Critical temperature of water
647 K
Critical pressure of water
218 atm
A eutectic mixture that is the most widely use topical anesthetic
EMLA
Refers to the point that is the lowest temperature at which the liquid phase is present in a system
Eutectic point
