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Understanding the Behavior of Solids, Liquids, and Gases: Kinetic Theory Explained

This overview delves into the kinetic theory of gases, detailing the constant motion of tiny particles and the nature of gas pressure resulting from collisions. It explains how pressure is measured in pascals, atmosphere, and mm Hg, including conversions. We explore the average kinetic energy of particles related to temperature, the behavior of liquids including the attractive forces between particles, and the processes of vaporization and vapor pressure. A deeper understanding of these concepts is essential for grasping the states of matter and their interactions.

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Understanding the Behavior of Solids, Liquids, and Gases: Kinetic Theory Explained

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  1. S-L-G Solids Liquids Gases

  2. Kinetic Theory-Gases • All matter consists of tiny particles that are in constant motion • Particles in a gas are considered to be small, hard spheres with an insignificant volume • The motion of the particles in a gas is rapid, constant and random • All collisions between particles in a gas are perfectly elastic

  3. Gas Pressure • Result of simultaneous collisions of billions of rapidly moving particles in a gas with an object • No particles = no collisions = no pressure is a vacuum • SI unit is a “pascal” (Pa) • 101.3 kPa = 1 atm = 760 mm Hg

  4. Do the following: • What pressure, in kPa and atm, does a gas exert at 385 mm Hg? • 101.3 kPa = 1 atm = 760 mm Hg

  5. Average Kinetic Energy • Related to temperature in °Kelvin (°K) • It is directly proportional, particles at 200 °K have twice the average kinetic energy as particles at 100 °K • 0 °K means the particles have no average kinetic energy

  6. Liquids • Unlike gases, there are attractive forces between particles in a liquid • Reduced space between particles means that liquids are not affected by increased pressures.

  7. Vaporization • Conversion of a liquid to a gas • When boiling is not involved, it is called evaporation • Only those particles with a certain minimum kinetic energy are going to escape the surface of the liquid.

  8. Vapor Pressure • Force exerted by a gas over a liquid evaporation • Liquid Gas condensation Eventually rate of evaporation will equal the rate of condensation

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