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31 Cards in this Set
- Front
- Back
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Why are gases weiord?
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invisible
low density ( 1000 * less dense) diffuse/expansion fill any container they are in volume is meaningless particals 1000 m/s |
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pressure
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force/ surface area
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force in gases
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collisions of particles against you/ container
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surface area
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where the container/ you is
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atmosphere
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1 atm typical day at sea level pressure of the atmosphere
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Kinetic energy
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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 |
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measurements
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760 mm HG = 1 atm = 76 cm Hg= 101.3 kPa
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Boyles law
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the volume of a sample of gas is inversely proportional to its presure if the temperature remains constant
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equation for Boyles law
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PV = K
P= pressure V= the volume of the sample K= a constant |
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inverse relationships
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PV = K inverse
V/P = K direct |
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equations to inverse relationships
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P1 V1 = P2 V2
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Charles law
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at a constant pressure the volume of a gas is directly proportional to its Kelvin temperature
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absotlute zero
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- 273 so you must add 273 to the temperature is in Celsius
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Charles law equation
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V1 V2 or v
--- = --- ---- = K T1 T2 T |
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No name law
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compares presssure and temperature
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equation for no name law
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P1 P2
--- = ---- T1 T2 |
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Combined gas laws
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P1 V1 = P2 V2
P1 V1 P2 V2 ------ = ------- T1 T2 |
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Gas stoichiometry
What is the difference |
using volume
but volumes are meaningless |
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molar volume
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the size of 1 mole of any gas at STP is 22.4 liters
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Golden Figure
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1 mile gas--6.02*10(23)particals
22.4 liter ------------- 1 GMM |
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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 |
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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 |
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non STp
volume to mass |
balance equation
gas laws P1 V1 T1 constant =P2 V2 T2 stoich |
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non STP
mass to volume |
balance equation
stoich gas laws P1 V1 T1 constant P2 V2 T2 |
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Another way
volume to mass |
PV= n RT
(p* cons) -------- (V)=(X)( 8.31) (T+273) (760) Stoich start in middle |
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Another way
mass to volume |
PV= n RT
stoich for moles stop in middle ( P) (X )= (m stoi)(8.31)(T+273) |
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Avogadro's Principle
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equal volumes of gases at equal conditions contain equal numbers of particles
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Changing conditions
Gas laws |
P1 V1 T1 P2 V2 T2
before after |
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changing conditions
STP |
given M or V want M or v
chemical equations |
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changing conditions
non STP |
same as STP with conditions given
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changing conditions
ideal gas laws |
1 gas mentioned conditions given
no before and after |
