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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 ?
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?
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
pressure and volume are indirectly proportional
volume and temperature are directly proportional
pressure and temperature are directly proportional
a gas in which the particles undergo elastic collisions (when particles collide, there is no loss in the speed of the particles)
a measure of how much the volume of matter decreases under pressure
Pressure goes up when you add molecules because...
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
Ability of gases to mix
Example of diffusion
A process by which gas particles pass through a tiny opening
a gas that does not behave completely according to the assumptions of the kinetic-molecular theory
1 atm and 273 K
The coldest temperature, 0 Kelvin, that can be reached. It is the hypothetical temperature at which all molecular motion stops.
Pressure and Volume Law
Volume v.s. Temperature
after flipping, if a given H atom started up, it will end up
(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)
The smaller the mass the faster the
rateA/rateB=squareroot of MMb/MMa
Heavy gases are
light gases are
A catalyst causes the product to form...?
Law of Partial pressures
at STP 1 mol/
at the same temperature and pressure, equal volumes of all gases contain the same number of molecules.
Density is measure in
(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
Volume and temperature directly proportional
P₁/T₁ = P₂/T₂
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