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I. Physical Properties

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This article explores the Kinetic Molecular Theory (KMT), which explains the behavior of gases based on particle motion and interactions. It differentiates between ideal and real gases, highlighting their characteristics, such as volume, attractive forces, and kinetic energy related to temperature. We examine gas properties, including expansion to fill containers, low density, and compressibility. Additionally, we discuss diffusion and effusion processes, and the significance of temperature and pressure measurements, including standard conditions. Understanding these principles is crucial for mastering gas behavior in various applications.

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I. Physical Properties

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  1. 12.1- Gases I. Physical Properties

  2. A. Kinetic Molecular Theory • kinetic-molecular theory:(def) theory of the energy of particles and the forces that act between them; based on idea that particles of matter are always in motion • Kinetic molecular theory describes the motion of an ideal gas

  3. A. Kinetic Molecular Theory • ideal gas: (def) imaginary gas that perfectly fits the assumptions of the kinetic-molecular theory

  4. A. Kinetic Molecular Theory • Particles in an ideal gas… • have no volume. • have elastic collisions. • are in constant, random, straight-line motion. • don’t attract or repel each other. • have an avg. KE directly related to Kelvin temperature.

  5. B. Real Gases • Particles in a REAL gas… • have their own volume • attract each other • proposed by van der Waals • Gas behavior is most ideal… • at low pressures • at high temperatures • in nonpolar atoms/molecules

  6. C. Characteristics of Gases • Gases expand to fill any container. • random motion, no attraction • Gases are fluids (like liquids). • no attraction • Gases have very low densities. • no volume = lots of empty space

  7. C. Characteristics of Gases • Gases can be compressed. • no volume = lots of empty space • Gases undergo diffusion & effusion. • random motion

  8. C. Characteristics of Gases • Diffusion: (def) process by which gases spontaneously spread out and mix with other gases; lighter gases diffuse more quickly • Effusion: (def) process by which gases particles under pressure pass through a tiny opening; lighter gases effuse faster

  9. A. Temperature K = ºC + 273.15 ºF -459 32 212 ºC -273 0 100 K 0 273 373 • Always use absolute temperature (Kelvin) when working with gases.

  10. B. Pressure SI unit of force is the Newton Which shoes create the most pressure?

  11. . Pressure Mercury Barometer • Barometer • measures atmospheric pressure - at sea level, height of column is 760 mm - P of Hg is equal to the P of the atmosphere

  12. E. Pressure U-tube Manometer • Manometer • measures contained gas pressure - difference in height of tubes indicates the gas pressure

  13. E. Pressure • KEY UNITS AT SEA LEVEL 101.325 kPa (kilopascal) 1 atm 760 mm Hg 760 torr 14.7 psi

  14. Pressure

  15. C. STP Standard Temperature & Pressure 0°C273.15 K 1 atm101.325 kPa -OR- STP

  16. D. Dalton’s law • Dalton’s law of partial pressure: • Ptotal = P1 + P2 + P3…+Pn (n = number of gases in mixture) **Total P exerted by collection gases is sum of pressure exerted by each gas

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