Studied by 2 peoplegas
no defenite volume or shape
do gasses have high ot low densities
low; particles are so much farther away from each other because gasses take up a lot of space
gas particles
flow and mix by random motion (diffusion)
1st part of kinetic molecular theory
gases consist of large #s of tiny particles
2nd part of kinetic molecular theory
the particles of a gas are in constant motion, moving rapidly in straight lines in all directions, and thus possess kinetic energy
3rd part of kinetic molecular theory
the collisions between particles of a gas and container walls are elastic collisions
in gasses, when kenetic energy is transferred between two particles
the total energy of the particles remain the same. there is no net loss of kinetic energy
4th part of kinetic molecular theory
there are no forces of attraction or repulsion between particles of gas
5th part of kinetic molecular theory
the average kinetic energy of the particles of a gas is directy proportional to the kelvin temperature of gas
pressure
the force exerted per unit p = f/a
pressure units
atmospheres (atm) pascals (pa) bars (bar) torr (torr) millimeters of mercury (mm hg) pounds per square inche (psi)
standard temperature and pressure (stp)
0 degrees celsius, 273 kelvin, 760 mm hg
particles would have no kinetic energy at
absolute zero
barometer
measures atomspheric pressure
manometer
measues the pressure in a container
liquids
definite volume no definite shape
have stronge intermolecular forces than gases
liquids
why do liquids have a higher density than gases
because particles are closer together
can liquids diffuse slower or faster than gasses
slower
how are particles arranged in liquids
they are not in fixed positions and can slide past eachother
soilds
defenite shape and volume
solids have the strongest and highest
intermolecular forces and densities (water is an exception)
how are particles arranged in a solid
in a relatively fixed position. they can vibrated a little, but not much
crystalline
particles are arrnaged in a competing pattern (salts)
amorphous
particles are arranged randomly (waxes, plastics, glass)
vaporizaion
the process by which a liquid or a solid changes into a gas
in vaporization, particles gain enough energy to
overrcome the attractive forces holding them together
evaporation
the process by which particles escape the surface of a nonboiling liquid and enter the gas state
condensation
the process by which a gas changes into a liquid
boiling
the change of a liquid to a gas
boiling point
the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure
freezing
the physical change of a liquid to a solid by the removal of heat
freezing point
the temperature at which solid and liquid are at equuilibrium
melting
the physical change of a solid to a liquid by the addition of heat
during melting, particles gain enough energy to
overcome the attractive forces holding them together
sublimation
change of state from a solid directly to a gas (dry ice)
deposition
change the state from a gas directly to a solid (frost)
phase diagram
a graph of pressure versus temperature that shows the condition under which the phases of a substance exit
triple point
the temp and pressure at which all 3 states can coexist at equilibrium
critical point
temp and pressure where only a gas can exit
normal boiling point
boiling point at standard pressure
normal freezing/melting point
the freezing/melting point at standard pressure
Note
Flashcard