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Understanding the Kinetic Molecular Theory and Properties of Gases

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camden-leblanc
10 diapositives · 266 Views · Nov 19, 2014

The Kinetic Molecular Theory explains gas behavior based on the idea that particles are always in motion. Key assumptions include that gases consist of tiny, far-apart particles, are in random motion, and that their kinetic energy increases with temperature. Gases are compressible, low in density, and will expand to fill any container. While ideal gases conform to all assumptions of this theory, real gases deviate under certain conditions like low temperature and high pressure. Understanding these principles is crucial for studying gas behavior in various scientific fields.

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  1. Properties of Gases Kinetic Molecular Theory

  2. Kinetic-Molecular Theory • Based on idea that particles of matter are always in motion. • Provides reasoning for the behavior of gases and their physical properties.

  3. Assumptions of the Kinetic-Molecular Theory • 1. Gases consist of a large number of tiny particles that are far apart relative to their size. • Most of the volume of a gas is empty space. • Accounts for lower density of gases in comparison to solids and liquids. • Explains fact that gases are easily compressed.

  4. Assumptions of the Kinetic-Molecular Theory • 2. Gas particles are in continuous rapid, random motion • Kinetic energy is the energy of motion. • 3. There are no forces of attraction or repulsion between gas particles. • Kinetic energy of the gas particles overcomes the attractive forces between the individual particles.

  5. Assumptions of the Kinetic-Molecular Theory • 4. The average kinetic energy (KE) of gas particles depends on the temperature of the gas. • As temperature increases, KE increases. • KE = ½mv2 (m = mass, v = velocity). • At the same temperature: • Lighter gases have higher average speeds. • Heavier gases have lower average speeds.

  6. Assumptions of the Kinetic-Molecular Theory • 5. Collisions between gas particles and between particles and container walls are elastic collisions. • In elastic collisions, there is no loss of kinetic energy. • Kinetic energy is transferred between two gas particles during collisions. http://my.hrw.com/sh/hc6_003036809x/student/ch10/sec01/vc00/hc610_01_v00fs.htm

  7. Ideal versus Real Gases • Ideal gases conform to all of the assumptions of the kinetic-molecular theory of gases. • Gases that behave ideally have the following properties: • Low mass. • Low polarity. • Gases behave most ideally under the following conditions: • High temperature. • Low pressure.

  8. Ideal versus Real Gases • Real gases do not obey all of the assumptions of the kinetic-molecular theory. • Gases that behave like real gases have the following properties: • High mass. • High polarity. • Gases behave like real gases under the following conditions: • Low temperature. • High pressure.

  9. Properties of Gases • Expansion and compression: • Gases can expand or compress to fit any size container. • Gases have no definite shape or volume. • Fluidity: • Gas particles easily flow past one another. • Low density: • The gaseous state of a substance is 1/1000th the density of the same substance as a solid or liquid.

  10. Properties of Gases • Diffusion and effusion: • Diffusion is the mixing of the particles of two gaseous substances caused by their random motion. • Effusion is the process by which gas particles pass through a tiny opening. • Both occur spontaneously. http://my.hrw.com/sh/hc6_003036809x/student/ch10/sec01/vc05/hc610_01_v05fs.htm