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## Ignore words

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Charles's Law
A sample of oxygen occupies a volume of 160 mL at 91°C . What will be the volume of oxygen when the temperature drops to 0.00°C ?
Boyle's Law
A container holds 500. mL of CO₂ at 742 torr. What will be the volume of the CO₂ if the pressure is increased to 795 torr?
Gay-Lussac's Law
a directly proportional relationship between the temperature and pressure of a confined gas
Volume and # of moles; V₁/n₁ = V₂/n₂
volume and the number of molecules are directly proportional
Boyle's
pressure and volume are indirectly proportional
Charles's
volume and temperature are directly proportional
Gay-Lussac's
pressure and temperature are directly proportional
ideal gas
a gas in which the particles undergo elastic collisions (when particles collide, there is no loss in the speed of the particles)
compressibility
a measure of how much the volume of matter decreases under pressure
more collisions
Pressure goes up when you add molecules because...
its container
Gas takes the shape of...
set shape or volume
unlike liquids and soilds gas does not have a
liquids and solids
_ and _ share many similar characteristics
Diffusion
Ability of gases to mix
air fresner
Example of diffusion
effusion
A process by which gas particles pass through a tiny opening
real gas
a gas that does not behave completely according to the assumptions of the kinetic-molecular theory
STP
1 atm and 273 K
absolute zero
The coldest temperature, 0 Kelvin, that can be reached. It is the hypothetical temperature at which all molecular motion stops.
Boyles
Pressure and Volume Law
low volume
High pressure=
high Volume
Low pressure=
Charles
Volume v.s. Temperature
up
after flipping, if a given H atom started up, it will end up
half
(Boyle's) Double the pressure you....the volume
Combined gas law
A combination of Boyle's Law, Charles' Law, and Lussac's Law. V1P1/T1=V2P2/T2 (people vomit over toilets)
true
(ex mg)
gas molecules
The smaller the mass the faster the
Graham's Law
rateA/rateB=squareroot of MMb/MMa
slow
Heavy gases are
fast
light gases are
faster
A catalyst causes the product to form...?
Dalton's Law
Law of Partial pressures
22.4 L
at STP 1 mol/
at the same temperature and pressure, equal volumes of all gases contain the same number of molecules.
g/L
Density is measure in
g/mol
(Density)Convert from g/L to ... and back.
atm → kPa
1 atm/ 101.3 kPa
atm → mm Hg
1 atm/ 760 mm Hg
atm → torr
1 atm/ 760 torr
Charles' law
Volume and temperature directly proportional
P₁/T₁ = P₂/T₂
Gay-Lussac's Law
R = (kPa)
R = 8.31kPa x L/ K x mol
R = (atm)
R = 0.0821atm x L/ K x mol
Ptotal = PA+PB+PC
Dalton's Law of Partial Pressures
Graham's Law of Diffusion
rateA/ rateB = √MMB/ √MMA
Celsius → Kelvin
K = C+273