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Gas Laws and Properties of Gases: Understanding Kinetic Theory

Learn about gas properties, pressure, kinetic-molecular theory, and gas laws in this comprehensive guide. Explore concepts such as boiling and melting points, fluidity, compressibility, and ideal gas behavior.

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Gas Laws and Properties of Gases: Understanding Kinetic Theory

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  1. Bell Work • Which line represents: • Boiling? • Freezing? • Liquid phase? • Solid phase? • Gas phase? • What are the boiling and melting points of this substance?

  2. Kelvin = Celsius + 273 In other words, add 273 to Celsius temperatures to get Kelvin temperatures Temperature Scales (p. 6)

  3. Properties of Gases • Gases are fluids (this just means that they flow) • Gases have low density • Lots of space between molecules • Volume taken up by a gas is mostly empty space • Gases are highly compressible • Gases completely fill their container

  4. Pressure • Pressure = Force per unit of area • Nail vs. dowel • Bottom of a pool • Pressure of a gas is caused by collisions between the molecules • Units for gas pressure: atm (atmospheres) • Also Pa or kPa (Pascales or kiloPascales)

  5. Standard Temperature and Pressure (STP) • STP means a temperature of 0 °C and a pressure of 1 atm

  6. Kinetic-Molecular Theory • Matter is made up of particles that are in constant random motion • Particles are attracted to each other - Attractions are weaker the farther apart they are • The higher the temperature, the faster the particles move

  7. Kinetic-Molecular Theory • Kinetic-molecular theory says ideal gas particles: • Are in constant, random, straight-line motion • Are very far apart from each other, so the volume of the particles is considered negligible • Have no attractive forces between them • Have collisions that may result in energy transfer, but NOT a loss or gain of energy • Gases are closest to being ideal at high temperatures and low pressures

  8. As we increase the volume of a gas' container, what will happen to the pressure? Gas Laws

  9. As we increase the temperature of a gas, what will happen to the volume of the gas' container (assuming the container is flexible)? Gas Laws

  10. As we increase the temperature of a gas, what will happen to the pressure of the gas? Gas Laws

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