11.1: Supersonic Skydiving and the Risk of Decompression 11.2: Pressure- The Result of Particle Collisions Gases exert pressure, which is force per unit area. The pressure of a gas may be expressed in the SI unit of pascal or kilopascal, as well as in many other units including torr, atmosphere, and bar. Atmospheric pressure is measured using a barometer; other gas pressures can be measured using one of several types of manometers. 11.3: The Simple Gas Laws- Boyle’s Law, Charles’s Law and Avogadro’s Law 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). 11.4: The Ideal Gas Law 11.5: Applications of the Ideal Gas Law- Molar Volume, Density and Molar Mass of a Gas 11.6: Mixtures of Gases and Partial Pressures 11.7: A Particulate Model for Gases- Kinetic Molecular Theory 11.8: Temperature and Molecular Velocities 11.9: Mean Free Path, Diffusion, and Effusion of Gases 11.10: Gases in Chemical Reactions- Stoichiometry Revisited 11.11: Real Gases- The Effects of Size and Intermolecular Forces No real gas exhibits ideal gas behavior, although many real gases approximate it over a range of conditions. Gases most closely approximate ideal gas behavior at high temperatures and low pressures. Deviations from ideal gas law behavior can be described by the van der Waals equation, which includes empirical constants to correct for the actual volume of the gaseous molecules and quantify the reduction in pressure due to intermolecular attractive forces. 11.E: Exercises