chem ch 8

1/2massvelocity²

kinetic energy=

temp

ke of a gas is directly proportional to

gas molecules

in continous, rapid, random motion, collide with each other and walls of container but no energy is lost (elastic)

molecular masses

gases with different _ must have same average kinetic energy at same temp, heavier must move slowly, light must move faster

speeds of gases

at given temp, molecules have high and low speeds, but have max (peak), as temp increase common speed increases, as temp increases, more molecules will be moving faster

square root u²=square root 3rt/molar mass

mean square speed

diffusion

mixing of gas molecules as a result of random motion, gas of oe mixture interacts with gas of other mixture

effusion

movement of gas molecules through tiny openings

square root molar mass gas 2/molar mass gas 1

rate of effusion of gas 1/rate of effusion of gas2

same

equal volumes of gas at same temp and pressure contain same number of molecules regardless of chemical nature and physical properties

6.022×10²³

one mole