Studied by 5 peoplekinetic theory - gas
molecules constantly move in random motion at high speeds
random motion
molecules travel in no specific path and undergo sudden changes if they collide
brownian motion
random motion of tiny particles
pressure in gases
as they move randomly they collide with the walls of the container they occupy and produce a net force
gas at high pressure
more frequent collisions and a greater force
what does the amount of pressure that a gas exerts on its container depend on
temperature of gas
increased temperature
particles move with more energy
decreased temperature of gas
pressure of container decreases
absolute zero
the temperature at which the molecules in a substance have zero kinetic energy
absolute zero to C
-273
is it possible to have a temperature lower than 0 K
no
can kelvin be a negative value
no
division between kelvin and celsius scale
change in a temperature of 1 K = change in temperature of 1 C
0 C to K
237 K
hotter gas
faster movement of molecules and more collisions
increase in kinetic energy
increased temperature of system
change of state
internal energy of gas
sum of kinetic energy of all molecules
is temperature (kelvin) directly proportional to kinetic energy
yes
gas laws - pressure and volume
in constant gas temperature, the pressure changes when it's compressed and expanded
gas laws - pressure and volume (compressed)
decrease in volume
increase in pressure
gas laws - pressure and volume (expanded)
increase in volume
decrease in pressure
what does a vacuum pump do
remove air from a sealed container
can change in pressure cause a change in volume
yes
gas laws - pressure and volume (compressing gas)
increase in pressure gas particles collide more frequently
gas laws - pressure and temperature (increase in temperature)
increase in speed of molecules
gas laws - pressure and volume (hotter gas)
higher kinetic energy
gas laws - pressure and volume (cooler gas)
lower kinetic energy
what should be constant for pressure and volume
temperature
what should be constant for pressure and temperature
volume
pressure law
pressure is directly proportional to temperature
relationship between the pressure and (Kelvin) temperature for a fixed mass of gas at constant volume
P1 / T1 = P2 / T2
boyle's law
for a fixed mass of a gas held at a constant temperature: pV = constant
pressure and volume - directly or inversely proportional
inversely proportional
relationship between the pressure and volume of a fixed mass of gas at constant temperature
P1V1 = P2V2
Note
Flashcard