Chapter 11 Flashcards
Kinetic molecular theory
Part 1 and 2
- Collection of particles in constant motion
2. No attractions or repulsions between particles; collisions like billiard ball collisions
Kinetic molecular theory
This model predicts the correct behavior for most gases under many conditions.
Kinetic molecular theory part 3 and 4
- A lot of space between the particles compared to the size of the particles themselves
- The speed of the particles increases with hear.
Pressure
Pressure=force/area
Force
.
Area
.
Atm
Atmosphere, the average pressure at sea level
Pascal
Pa, defined as 1 newton per square meter
1Pa=1N/m^2
1 atm=xpa
101,325 Pa
mmHg
Millimeter of mercury
1 ATM=x mm Hg
1atm=760 mm Hg
1mm Hg= xtorr
1mm=1 torr
Millimeter of mercury is also known as a ___
Torr
Psi
Pounds per square inch
1 ATM=xpsi
1atm=14.7 psi
Boules law
The volume of a gas and it’s pressure are inversely proportional.
The volume of a gas and it’s pressure are inversely proportional.
Bottles law
V is proportional to 1/P
Boules law mathematical formula
V=(constant/P)
Charles law
The volume of gas increases proportionally as it’s kelvin temperature increases
Charles formula
V=Constant*T
V1/t/1)=(V2/T2
Combined gas law
(P1V1/T1)=(P2V2/T2)
Applies when amount of gas is constant
Must use kelvins
Avogadro’s Law
The volume of a gas and the amount of the gas in miles are directly proportional.
(V1/n1)=(V2/n2)
The ideal gas law takes into account all three relationships:
Boyles
Charles
Avagadros
V is proportional too
Ideal gas
(nT/P)
Mathematical ideal gas formula
V=(RnT/P)
Or
PV=nRT
R=
.0821(Latm/molK)
Partial pressure of component=
Fractional composition of component * total pressure
