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Year 1 Gas Laws (GAS LAWS (Charles's law V α T (K = C + 273),…
Year 1 Gas Laws
GAS LAWS
Boyle's Law P α 1/V
Avogadro V α n
Inverse and proportional relationships
Charles's law V α T
K = C + 273
P α T
average KE α T
Ideal Gas Law :star:
PV=nRT
must be in a closed system
treat all particles the same, no matter the atom
temp must be Kelvin
molar mass of gas = densityRT/pressure
Partial Pressures
Vapor pressure α Boiling point
all the pressures add up
P1+P2+Pn=Ptotal
Mole Fraction
x=n1/ntotal = P1/Ptotal
Collecting a gas over water
Ptotal - Pof gas = Pwater
Kinetic Molecular Theory :hearts:
Gas particles have insignificant volume
the distances between the particles are so great compared to the particles size
Particles do not interact with each other
All collisions are elastic
average KE of particles is proportional to temperature
Quantities that affect gases
Volume
number of molecules
more molecules = more collisions
Pressure
increasing pressure increases collisions
UNITS: force over area (N/m^2)
760 mmHg/torr = 1 atm
temperature
increasing temp, increases the speed: t α v
Real Gases :smiley: NO NEED TO ADDRESS FOR HONORS
Do not behave ideally
behave more ideally at high temp and low pressure
Have IMFS
increased e- increases IMFS
Individual particles have volume
STP
1 atm/760 Kpa
273 K
1 mol of gas at STP = 22.4 L
Effusion and diffusion
Effusion
The passing of a gas through a tiny hole into an evacuated chamber
Diffusion
mixing of gases
gas stoich
If STP
1 mol = 22.4 L
If not STP
Use PV=nRT to find moles and then do stoich