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Gas Laws

Gas Laws. Kinetic theory Particles of matter are in constant motion no matter the form (s, l, g). A gas is composed of particles, in the form of molecules or atoms. The particles of a gas move rapidly in constant, random motion. All collisions are perfectly elastic.

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Gas Laws

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  1. Gas Laws

  2. Kinetic theoryParticles of matter are in constant motion no matter the form (s, l, g) A gas is composed of particles, in the form of molecules or atoms. The particles of a gas move rapidly in constant, random motion. All collisions are perfectly elastic.

  3. Physical behavior of a gas depends on: volume temperature pressure

  4. Volume How much space occupied volume of a gas in a sealed container is the volume of the container gases not in sealed containers are uncontained Units can be milliliters, liters, cubic centimeters

  5. TemperatureMeasure of the average kinetic energy of particles in a substance same temperature = same average kinetic energy temperature measured using Kelvin scale Kelvin temperature = 0°C + 273 no upper limit for temperature lower limit = absolute zero 0 K = -273°C (no motion of particles)

  6. To convert from Celsius to Kelvin—add 273 To convert from Kelvin to Celsius– subtract 273

  7. Pressureforce per area result of simultaneous collisions of billions of gas particles units of pressure atmospheres mm Hg Torr Pascal

  8. Standard Temperature and Pressure (STP) Standard temperature = 0°C = 273 K Standard pressure = 1 atm = 760 mm Hg = 760 Torr = 101 kPa

  9. Avogadro’s Law equal volumes of gases at the same temperature and pressure contain equal numbers of particles at STP 1 mole (6.02 X 1023 particles) of any gas occupies 22.4 liters

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