Exam 2 Content (Feb 14th)

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