Unit 6 Gases Review

We're diving into Unit 6: Gases today. This review covers kinetic theory, phase diagrams, and gas laws. Every question from the study guide is answered here.Let's explore kinetic molecular theory. Gases move constantly in straight lines and are mostly empty space. Collisions are elastic, and kinetic energy depends only on temperature.Here's how we differentiate solids, liquids, and gases. Solids are dense, incompressible; liquids are almost as dense, barely compressible; gases have low density and are easily compressible.Understanding Kelvin and standard pressure is crucial. To convert Celsius to Kelvin, add 273. Standard atmospheric pressure is 760 torr, 101.3 kPa, or 1 atm.Pressure conversions are easy if you multiply by a fraction worth one. We use this method to switch between various units like mmHg, atm, kPa, and psi.Explore phases and their changes. Melting and freezing, vaporization and condensation, sublimation and deposition all represent transitions between solid, liquid, and gas.Reading a path on a phase diagram reveals the triple and critical points. The triple point is where all three phases coexist; the critical point defines the limit of liquid existence.Boyle's law states that at constant temperature, pressure and volume are inversely proportional. We can use P1V1 = P2V2 to solve for unknown values.Charles's and Gay-Lussac's laws show how volume, pressure, and temperature interact. Charles's Law relates volume and temperature, while Gay-Lussac's Law connects pressure and temperature.When pressure, volume, and temperature all change, we use the combined gas law: P1V1/T1 = P2V2/T2. Remember to convert all temperatures to Kelvin.