Gas Laws Summary PDF

GAS LAWS DiFFusion GAY LUSSAC’S LAW is the spontaneous spreading out of a When gases react, the volumes consumed substance due to the natural movement of in the reaction bear a simple whole number the particles of that substance. ratio to each other, and to the volumes of any gaseous products of the...

GAS LAWS DiFFusion GAY LUSSAC’S LAW is the spontaneous spreading out of a When gases react, the volumes consumed substance due to the natural movement of in the reaction bear a simple whole number the particles of that substance. ratio to each other, and to the volumes of any gaseous products of the reaction, all BOYLE’S LAW volumes being measured under the same conditions of temperature & pressure. states that, at constant temperature, the volume of a fixed mass of any gas is inversely proportional to the pressure of the gas. AVOGADRO’S LAW Equal volumes of gases, under the same conditions of temperature & pressure, CHARLE’S LAW contain equal numbers of molecules. states that, a constant pressure, the volume of a given mass of any gas is directly proportional to the Kelvin temperature. Kinetic Theory of GASES This theory is based on 5 assumptions: 1. Gases are made up of particles whose volumes are negligible compared to the distances between them. 2. There are no attractive or repulsive forces between gases. 3. The particles are in constant rapid the combined gas law random motion, colliding with each other & with the walls of the container. 4. The average kinetic energy of the Combining Boyle’s Law & Charles’ Law particles is proportional to the Kelvin gives us the combined gas law: temperature. p₁ V₁ p₂ V₂ a particle collides with the wall of the = T₁ T₂ Notes: All temp’s must be in K Units on either side of the equation must be consistent. 5. All collisions are perfectly elastic (ie. If container at a certain speed, it will rebound at that speed). GAS LAWS ideal gas is a gas that obeys all the assumptions of the kinetic theory under all conditions of temperature & pressure. real gas Real gases greatest deviation from the kinetic theory of gases happens at low temperature & high pressure The Equation of State for an Ideal Gas PV = nRT n = number of moles R is the universal gas constant R = 8.31 K.K⁻¹.mol⁻¹