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For Kinetic-Molecular Theory of Gases what do we assume?
gas particles are small relative to the distance between them
forces between particles are negilbe expect during collisions
between collisions, particles move in straight lines at various speeds
collisions are elastic with no loss in keltic energy
What’s diffusion?
movement are particles from higher concentration to low concentration
what’s effusion?
the escape of gas particles through a small opening in containers
lighter molecules collide more frequently in a container thus,
they will effuse faster than heavier ones
heavy molecules collide not as frequent in a contain thus,
they will effuse slower than lighter ones.
What is the rate of effusion?
Urms = 1/ sqrt(molar mass)
What does each part of this equation mean?
Ave.KE → average kinetic engird of the molecules
Mm → molar mass in kg/mol
u² → average rms speed
R → Ideal gas constant
T → temp in Kelvin
if particles are moving slow the temperature will be?
colder
if particles are moving fast the temperture will be?
hotter
as volume increases pressure will?
decrease
as temp goes up, volume will?
go up but pressure will remain the same.
as temp goes down, volume will?
go down but pressure will remain the same
