gas laws Flashcards
kinetic molecular theory (ideal gas laws)
a theory used to explain / describe the usual behavior of gases
- theory describes the relationship among:
- pressure
- volume
- temp
- velocity
- frequency of collisions
ideal gas laws (kmt)
- gases contain particles that are in constant, random, and “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 or shape
- gas particles DO NOT attract each other
ideal vs real gas laws
ideal : kmt
- gases are most ideal at low pressure and high temp
- hydrogen and helium are always ideal gases (low density)
real:
- gas particles DO attract each other
- gas particles DO occupy volume
- gases are most REAL at high pressure and low temp
avogadro’s hypothesis
if two gases are at the same exact temp and pressure…
- the volume that the gases occupy are the same AND the # moles (# molecules) are also the same
- if gases happen to be at STP, every 1 moles of gas would occupy 22.4 L
boyle’s law
P1V1 = P2V2
at constant temp:
- as pressure increases on a gas, volume will decrease
- pressure and volume are inversely proportional
charles’ law
V1 / T1 = V2 / T2
at constant pressure:
- volume is directly proportional to its change in temp
temp must be measured in KELVIN
lussac’s law
P1 / T1 = P2 / T2
at constant volume:
- as temp increases, pressure exerted by the gas will increase
- directly proportional