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KMT

KMT. Kinetic Molecular Theory. Kinetic Molecular Theory. Kinetic energy = energy from motion Kinetic theory = the particles that make up matter are in constant motion Motion and temperature are directly proportional. Gas.

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KMT

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  1. KMT Kinetic Molecular Theory

  2. Kinetic Molecular Theory • Kinetic energy = energy from motion • Kinetic theory = the particles that make up matter are in constant motion • Motion and temperature are directly proportional

  3. Gas • Take shape and volume from container, can be compressed, and expand limitlessly • far apart = less attraction between particles • particles 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

  4. Liquid • fixed volume, shape of container, expand when heated • particles in contact, but can flow past each other • closer together = more attraction • particles move slower • less motion = less energy

  5. Solid • Definite shape & volume • particles packed tightly • packed tight = very high attraction • particles vibrate in a fixed position • little motion = less energy • ONLINE DEMO • http://www.chamotlabs.com/Phases.html

  6. Phase Changes • Energy Flow causes Phase Changes: • To change state particles must absorb or release energy • this energy IS CONSERVED

  7. Phase Change Graphs • Show 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

  8. Phase Diagrams • Shows 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

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