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Boyle’s Law
P1V1 = P2V2
Charles’s Law
V1/T1 = V2/T2
Gay-Lussac’s Law
P1/T1 = P2/T2
Combined Gas Law
P1V1/T1 = P2V2/T2
Dalton’s Law of Partial Pressures
Ptotal = P1 + P2 + P3 + P4 + …
STP atm
1.00
STP kPa
101.325
STP mmHg/torr
760
STP temp (K)
273
Ideal Gas Law
PV = nRT
Ideal Gas Law + mass and molar mass
PVM = mRT
density of a gas
m/V
Avogadro’s Principle
22.4 L/ mol
expands
____________ to assume the shape and volume of its container
flows
readily ____________
straight lines
particles only move in ____________
compressible
molecules far apart but ____________
few
____________ attractive forces between particles
volume
space occupied by a gas sample
mL, L, cm^3, dm^3
volume units
1 cm^3
1 mL = ____________
1dm^3
1 L = ____________
temperature
a measure of the average kinetic energy of a group of particles
thermometer
measurement tool for temperature
kelvin (K)
temperature unit
amount
number of moles of the substance
mol
amount unit
pressure
force per unit area caused by the collision of the gas molecules with the walls of the container
manometer
measurement tool for pressure
pascal (Pa), atmosphere (atm), torr, millimeter of mercury (mmHg)
pressure units
kinetic molecular theory
a model that uses particle motion and interparticle forces to properties of different states of matter
no volume
individual gas particles have almost ____________
inter particle
gas particles have no ____________ forces
constant random
gas particles are in ____________ motion
elastic
collisions are ____________, no energy lost
average kinetic energy
all gases have the same ____________ at a given temperature
high temp and low pressure
real gases behave like ideal gases at:
avogadro’s principle
equal volume of all gases measured at the same temperature and pressure contain the same number of particles
Note 
Flashcard (77)