KMT Kinetic Molecular Theory

Kinetic Molecular TheoryKinetic energy = energy from motionKinetic theory = the particles that make up

matter are in constant motionMotion and temperature are directly

proportional

GasTake shape and volume from

container, can be compressed, and expand limitlesslyfar apart = less attraction between

particlesparticles move quickly and

randomly lots of MOTION = lots of ENERGY

vapor - gas that would normally be a liquid (or solid) at room temp

pressure –the force with which gas particles hit the container

Liquidfixed volume, shape of

container, expand when heatedparticles in contact, but can

flow past each othercloser together = more

attraction particles move slower

less motion = less energy

SolidDefinite shape & volume

particles packed tightly packed tight = very high

attractionparticles vibrate in a fixed

position little motion = less energy

ONLINE DEMOhttp://www.chamotlabs.co

m/Phases.html

Phase ChangesEnergy Flow causes Phase Changes:

To change state particles must absorb or release energythis energy IS CONSERVED

Phase Change GraphsShow how temp increases as heat is added

Link: http://mutuslab.cs.uwindsor.ca/schurko/animations/waterphases/status_water.htm

when the temp increases (slope), the heat is going to speed particles up Kinetic Energy (KE) increases

when melting or boiling (flat lines), the heat is used to break particle attractions and spread them apart Potential Energy (PE) increases

Phase DiagramsShows pressure vs

temperature – shows when the different phases exist

Important points on a phase diagram ‘Normal’ freezing and boiling

points – pressure of 1 atm Triple point – the temp and

pressure where all 3 phases co-exist

Critical point – indicates the highest temp and pressure that a substance can be liquid

Supercritical fluid – a substance BEYOND the critical point Has properties of a gas and

a liquid