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Chemistry LibreTexts

Chapter 6: Properties of Gases

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  • 6.1: Kinetic Molecular Theory: A Model for Gases
  • 6.2: Pressure
    how pressure is measured, units of pressure, atmospheric gas pressure
  • 6.3: The Gas Laws
    The volume of a gas is inversely proportional to its pressure and directly proportional to its temperature and the amount of gas. Boyle showed that the volume of a sample of a gas is inversely proportional to pressure (Boyle’s law), Charles and Gay-Lussac demonstrated that the volume of a gas is directly proportional to its temperature at constant pressure (Charles’s law), and Avogadro showed that the volume of a gas is directly proportional to the number of moles of gas (Avogadro’s law).
  • 6.4: The Ideal Gas Law
    The empirical relationships among the volume, the temperature, the pressure, and the amount of a gas can be combined into the ideal gas law, PV = nRT. The proportionality constant, R, is called the gas constant. The ideal gas law describes the behavior of an ideal gas, a hypothetical substance whose behavior can be explained quantitatively by the ideal gas law and the kinetic molecular theory of gases. Standard temperature and pressure (STP) is 0°C and 1 atm.
  • 6.5: Dalton's Law of Partial Pressures
  • 6.6: Gas Volumes and Stoichiometry
  • 6.7: Non-ideal (Real) Gases


Chapter 6: Properties of Gases is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts.

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