Kinetic Molecular Theory - Kinetic Molecular Theory and the Nature of Gases A Applies only to ideal gases(do not actually exist B Gases will behave

Kinetic Molecular Theory - Kinetic Molecular Theory and the...

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Kinetic Molecular Theory and the Nature of Gases A. Applies only to ideal gases (do not actually exist) B. Gases will behave nearly ideally if pressure is not very high and temperature isn’t very low C. Expansion 1. Gases have no definite volume; they fill up the container D. Fluidity 1. Particles glide past one another 2. Liquids and gases are both called fluids E. Low Density 1. Particles of a gas are much further apart than solids/liquids F. Compressibility 1. Gas particles are initially far apart 2. This means lots of room for them to compress together G. Diffusion and Effusion 1. Diffusion - spontaneous mixing of particles of two substances caused by their random motion 2. Rate of diffusion depends on: speed, diameter, and attraction of particles
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Unformatted text preview: a. ex. Hydrogen diffuses quickly because its particles move faster 3. Effusion- Process by which gas particles pass through a tiny opening 4. Rate of effusion directly proportional to velocity of particles a. particles with a low mass will effuse faster 2. At high pressures/ low temperatures the difference is considerable a. particles too close to overcome attractive forces C. Gases with little attraction behave almost ideally 1. Noble gases, which are monatomic and nonpolar 2. Diatomic gasses, like hydrogen, also behave almost ideally 3. The more polar a gas is, the more it will deviate from the “ideal”...
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  • Fall '08
  • Young
  • Mole, gas particles

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