CHEM 1A Chapter Notes - Chapter 5: Van Der Waals Equation, Ideal Gas, Stoichiometry
Document Summary
Pressure: the result of molecular collisions (p. 196) The simple gas laws: boyle"s law, charles"s law, and avogadro"s law (p. 199) Applications of the ideal gas law: molar volume, density, and molar mass of a gas (p. 209) Mixtures of gases and partial pressures (p. 213) Gases in chemical reactions: stoichiometry revisited (p. 219) Kinetic molecular theory: a model for gases (p. 222) Mean free path, diffusion, and effusion of gases (p. 229) Real gases: the effects of size and intermolecular forces (p. 230) Gas pressure is the force per unit area that results from gas particles colliding with the surfaces around. Pressure is measured in a number of units including mmhg, torr, pa, psi, inhg, and atm: the simple gas laws (5. 3) The simple gas laws express relationships between pairs of variables when other variables are held constant. Boyle"s law states that the volume of a gas is inversely proportional to its pressure.
