Chemistry Unit 10 Theories

Currently on Parts 1 & 2

Kintetic Theory of Matter

all particles of matter are in constant motion (even solids)

Kinetic Theory of Gas

1. Gases are of tiny particles; do not attract nor repel each other ; move independently of each other; have an attractive force between the particles of solids & liquids
2. Gas particles move very fact (thousands of km/hr); particles move randomly in a straight like until collision
3. Collisions between gas particles are elastic (not sticky); kinetic energy can be transferred from 1 particle to another without losing any KE

random walk

when gas particles move randomly in small straight lines until collisions with each other or objects in a room

Gas pressure

collision of gas particles w/ each other & the walls of their container (collision # increases → pressure increase)

vaccum

region of space where no pressure is exerted

atmospheric pressure (atm)

pressure cause by the air in our atmosphere; as altitude increases → atm decreases

standard pressure

average pressure as measured at sea levels

standard pressure units

1 atm

101\.3 kPa

760 mmHg

barometer

device used to measure atmospheric pressure

temperature

measure of the amount of kinetic energy a sample of matter has

average KE proportion

average KE is proportional to the Kelvin (K) temperature

Kelvin temperature formula

Kelvin = °C + 273

absolute zero idea

since temp. decreases, particles move slower & slower; therefore, particles would theoretically stop @ 0Kelvin (absolute zero); doesn’t happen due to kineti theory

STP

standard temperature & pressure; measured as 0°C or 273K