Ideal Gas Law - Explaining the governing principles behind the ideal gas equation.pptx

This presentation describes the principles that are behind the ideal gas law relationship, and how the math and relationships correspond to actual physical properties.

1. The container starts out with a certain number of molecules in the container. These molecules bounce off themselves and the walls of the container to produce a certain pressure When the volume is reduced at constant temperature, the gas molecules bounce more frequently off the walls, increasing the previous pressure. This is the basis for Boyle’s Law. Pressure and volume are inversely proportional Boyle’s Law

2. Gay Lussac’s Law T = 300K The first diagram has a certain number of molecules at 300 Kelvin, with a certain amount of kinetic energy, so the molecules push against the container to exert a pressure T = 450K This diagram has increased temperature, while volume remained constant. This provides the gas molecules with more energy (represented by the darker shade of red of each molecule), so they collide with the walls of the container with greater energy, increasing pressure.Pressure is directly proportional to temperature

3. Charles’s Law T = 300K The first diagram has a certain number of molecules at 300 Kelvin, with a certain amount of kinetic energy, so the molecules push against the container to exert a pressure T = 450K This diagram has increased temperatur e. If we want to maintain constant pressure, the molecules have to push out against the piston with the energy from the increased temperature. Hence, at constant pressure, volume and temperature ate proportional