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Kinetic Theory & Gas Laws

Kinetic Theory & Gas Laws. October 2014. Kinetic Theory of Matter. Kinetic Theory of Matter : all matter is made of tiny particles (atoms) which are in constant motion. Fluid Behavior. Fluids : any substance in which the particles are free to flow. (move past one another.)

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Kinetic Theory & Gas Laws

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  1. Kinetic Theory & Gas Laws October 2014

  2. Kinetic Theory of Matter Kinetic Theory of Matter: all matter is made of tiny particles (atoms) which are in constant motion

  3. Fluid Behavior • Fluids: any substance in which the particles are free to flow. (move past one another.) (Gases and Liquids) • All fluids exert pressure. • (examples: water pressure, atmospheric pressure, blood pressure) • The pressure of all fluids increases with depth. (More matter on top as you descend)

  4. Pressure • Pressure: The amount of force applied over a given area. • The SI unit of pressure is the Pascal, (Pa).  • One Pascal (Pa) is the force of 1 Newton exerted over an area of one square meter. • 1 Pa = 1Newton = 1N 1Meter 2 m2 • The English units for pressure are • Pounds Inches 2 Pounds per squared inch, (PSI) • http://www.youtube.com/watch?v=1FtLUdozmfA&feature=related (Head rush Balloon/Nails) • http://www.youtube.com/watch?v=P1zfktn4AzU&feature=related (Ellen show)

  5. Pressure

  6. Pressure and Altitude • The higher the altitude, the lower the pressure, air particles are less densely packed together at higher altitudes. • Air pressure decreases as altitude increases. 4,300 ft 14,000 ft 9,000 ft

  7. Pressure Equilibrium • Pressure Differentials: • When pressures are unbalanced, energy flows from high pressure areas to low pressure areas until balanced. • (Equilibrium is reached and there is no longer a difference.) • Equilibrium: a state of balance

  8. Properties of Gases • No definite shape or volume, they expand to fill their container • Particles move rapidly in all directions and constantly collide with each other and the walls of their container (creates pressure in container) • Low density because particles are far apart (often used to fill tires or balloons) Gases are mostly empty space. • Compressible

  9. Gas Laws- Boyle’s Law • Boyle’s law: (British; Robert Boyle) • As the volume of a container of gas decreases, the pressure inside the container increases. (fixed amount of gas at a constant temperature) • Volume ↓ then Pressure ↑ • (the reverse is also true) • V ↑ then P↓ • This relationship is inversely proportional

  10. Gas Laws- Boyle’s Law • Examples of Boyle’s Law: Squeezing a closed balloon increases pressure inside, deep sea fish die when brought to the surface, air compressors, our diaphragms/lungs, etc… • https://www.youtube.com/watch?v=27yqJ9vJ5kQ

  11. Gas Laws- Boyle’s Law

  12. Gas Laws- Charles’ Law • Charles’ law: (French; Jacques Charles) • The volume of a gas increases as the temperature increases. (Fixed amount of gas at a constant pressure) • Temperature ↑ then Volume ↑ • (the reverse is also true) • T ↓ then V ↓ • This relationship is directly proportional. • https://www.youtube.com/watch?v=7JKVtbe-hV8 • https://www.youtube.com/watch?v=GcCmalmLTiU

  13. Gas Laws- Charles’ Law • In theory, Charles could calculate the temperature at which volume would = zero. • This temperature is called absolute zero. At absolute zero, all particle motion stops and the volume of the gas equals 0. • Absolute zero = -273º C or 0 Kelvin. • In reality: Gases can’t be cooled to a volume of zero. They condense into liquids when they are cooled below their boiling points or solidify when cooled below their melting point. • Examples of Charles’ Law: hot air balloons, tires needing more gas in winter to be inflated fully, etc…

  14. Gas Laws- Charles’ Law

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