Chemistry Unit 10

Pressure-

force exerted by gas particles when they collide with walls of container

Volume-

As Volume of gas decreases, pressure increases

Temperature-

As temperature increases, pressure increases. Gas particles move more quickly and collide with more energy

Amount of Gas-

As amount of gas increases, pressure increases

Gas particles are very small with

lots of space between them

All particles have same mass, but not same velocity, so

each particle has different kinetic energy

Particles in constant motion

move in straight paths

Collisions are elastic, meaning

no KE lost

Gases in constant motion so they

expand to fill containers

Gases have low density bc of

empty space between particles

Gases are easily compressible because of

lots of empty space between particles

Compressible-

forced into smaller volume

Diffusion-

Movement from area of high concentration to low concentration

Standard Temperature and Pressure (STP) for gases-

1 atm and 273K

All motion stops at absolute zero which is 0K which

can never be reached

Boyles Law-

at constant temperature, pressure of gas is inversely proportional to its volume

Charles Law-

At constant pressure, volume of gas is directly proportional to its temperature in Kelvin

Gay-Lussacs Law:

At constant volume, pressure of gas is directly proportional to its Kelvin temperature

In Combined gas Law-

amount of gas is constant

Graham Law of diffusion depends on mass of the particles;

the lighter the particle, the faster the diffusion

To compare one gas to another

temperature should remain constant

Effusion-

gases escape from container through hole then diffuse according to Graham's law