Gas Laws Flashcards
Kinetic Molecular Theory
a theory used to
explain the usual behavior
of gases.
The theory describes the
relationship among;
- Pressure, Volume, Temperature, Velocity, Frequency of Collisions
IDEAL GAS LAWS
Gases contain particles that are in constant, random,
straight-line motion
Gas particles collide with each other and with the walls of
the container
-Results in a transfer of energy
Gas particles are separated by great distances
-No Definite Volume, No Definite Shape
Gas particles DO NOT attract each other
Ideal Gases
(Particles spread out); Gases are most Ideal at Low Pressure and High Temperature
- Hydrogen & Helium are always Ideal
gases (low Density)
Real Gases
(Particles are closer together); Gas particles DO attract each other; Gas particles DO occupy volume; Gases are most Real at High Pressure
and Low Temperature
Negligible
indefinite
AVOGADRO’S HYPOTHESIS
- If two gases are at the same exact temperature and
pressure - the volumes that the gases occupy are the same
- AND the # moles (#molecules) are also same
equation of ideal gases
PV = nRT (n=# of moles) (R= gas constant 0.08206 atm L/mol K)
Pressure
the amount of force over area
Volume
the amount of space an object takes up
Robert Boyle
discovered the relationship between volume and pressure of a gas
STP of Pressure
760 mm Hg = 760 Torr = 1 atm = 101.3 Kpa
Boyles Law
at constant temp; as pressure is added to a gas, the volume decreases; so inversely proportional
Boyles Law Equation
P1V1 = P2V2
Jacques Charles
discovered the relationship between temp and volume of a gas; so directly proportional bc as volume increases so does temp; MUST BE IN KELVIN
