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31 Cards in this Set

  • Front
  • Back
Why are gases weiord?
invisible
low density ( 1000 * less dense)
diffuse/expansion
fill any container they are in
volume is meaningless
particals 1000 m/s
pressure
force/ surface area
force in gases
collisions of particles against you/ container
surface area
where the container/ you is
atmosphere
1 atm typical day at sea level pressure of the atmosphere
Kinetic energy
gas is made of mostly space therefor it is easily compressed and can miz so readily
Gas molecules are always moving so the pressure of a gas is the effect of the molecules hitting the walls of the container
No energy is formed of used in the movement of the molecules KE remains thesame if temperature and volume does not change
Molecules have no attraction or rpulsion to one another
measurements
760 mm HG = 1 atm = 76 cm Hg= 101.3 kPa
Boyles law
the volume of a sample of gas is inversely proportional to its presure if the temperature remains constant
equation for Boyles law
PV = K
P= pressure
V= the volume of the sample
K= a constant
inverse relationships
PV = K inverse

V/P = K direct
equations to inverse relationships
P1 V1 = P2 V2
Charles law
at a constant pressure the volume of a gas is directly proportional to its Kelvin temperature
absotlute zero
- 273 so you must add 273 to the temperature is in Celsius
Charles law equation
V1 V2 or v
--- = --- ---- = K
T1 T2 T
No name law
compares presssure and temperature
equation for no name law
P1 P2
--- = ----
T1 T2
Combined gas laws
P1 V1 = P2 V2

P1 V1 P2 V2
------ = -------
T1 T2
Gas stoichiometry
What is the difference
using volume
but volumes are meaningless
molar volume
the size of 1 mole of any gas at STP is 22.4 liters
Golden Figure
1 mile gas--6.02*10(23)particals


22.4 liter ------------- 1 GMM
STP
mass to volume
X g gi/ 1 m gi/ X m w/ 22.4 l w
--------------------------------
/GMM g gi/X m gi/ 1 m w
STP
volume to mass
X l gi/ 1 m gi/ X m w/ GMM g w
-------------------------------
/22.4 l gi/ X m gi/ 1 m w
non STp
volume to mass
balance equation
gas laws P1 V1 T1
constant =P2 V2 T2
stoich
non STP
mass to volume
balance equation
stoich
gas laws P1 V1 T1
constant P2 V2 T2
Another way
volume to mass
PV= n RT
(p* cons)
-------- (V)=(X)( 8.31) (T+273)
(760)
Stoich start in middle
Another way
mass to volume
PV= n RT
stoich for moles stop in middle
( P) (X )= (m stoi)(8.31)(T+273)
Avogadro's Principle
equal volumes of gases at equal conditions contain equal numbers of particles
Changing conditions
Gas laws
P1 V1 T1 P2 V2 T2
before after
changing conditions
STP
given M or V want M or v
chemical equations
changing conditions
non STP
same as STP with conditions given
changing conditions
ideal gas laws
1 gas mentioned conditions given
no before and after