10.2 Ideal Gas Law and Kinetic Theory of Gases | General Physics
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Chad provides a lesson on
Chad provides a lesson on the Ideal Gas Law and the Kinetic Theory of Gases. The lesson begins with the postulates of the Kinetic Theory of Gases:
1. A gas is comprised of a large number of atoms/molecules moving randomly.
2. Gas particles are point-like having negligible volume.
3. Gas molecules do not exert long range forces on one another.
4. All collisions between molecules and with the walls are elastic.
These provide the theoretical foundation from which the Ideal Gas Law stands, PV=nRT. A variety of individual gas laws are first presented including the following:
Boyle's Law: pressure is inversely proportional to volume at constant temperature.
Charles' Law: volume is proportional to temperature at constant pressure.
Avogadro's Law: volume is proportional to the moles of gas at constant pressure and temperature.
Guy Lussac's Law: pressure is proportional to temperature at constant volume.
Overall, these are all encompassed by the Ideal Gas Law: PV=nRT. Chad then solves a couple of ideal gas law practice problems.
Chad then presents the equation for pressure derived from the molecular model for ideal gases and uses it to show the linear relationship between kinetic energy and temperature for a gas. The relationship between the root mean square speed of a gas, temperature, and molar mass is derived. The Maxwell Distribution of Speeds is then presented graphically both with varying temperature and varying molar mass. Finally, the rms speed of a gas is solved for given the temperature and its molar mass.
00:00 Lesson Introduction
00:54 Kinetic Theory of Gases
06:58 Introduction to the Ideal Gas Law
10:52 Individual Gas Laws: Boyle's, Charles, Avogadro's, Guy Lussac's
21:01 Ideal Gas Law Calculations
27:44 Kinetic Energy, Temperature, and rms Speed of a Gas
34:06 Maxwell Distribution of Speeds
Check out Chad's General Physics Master Course: https://courses.chadsprep.com/courses...
1. A gas is comprised of a large number of atoms/molecules moving randomly.
2. Gas particles are point-like having negligible volume.
3. Gas molecules do not exert long range forces on one another.
4. All collisions between molecules and with the walls are elastic.
These provide the theoretical foundation from which the Ideal Gas Law stands, PV=nRT. A variety of individual gas laws are first presented including the following:
Boyle's Law: pressure is inversely proportional to volume at constant temperature.
Charles' Law: volume is proportional to temperature at constant pressure.
Avogadro's Law: volume is proportional to the moles of gas at constant pressure and temperature.
Guy Lussac's Law: pressure is proportional to temperature at constant volume.
Overall, these are all encompassed by the Ideal Gas Law: PV=nRT. Chad then solves a couple of ideal gas law practice problems.
Chad then presents the equation for pressure derived from the molecular model for ideal gases and uses it to show the linear relationship between kinetic energy and temperature for a gas. The relationship between the root mean square speed of a gas, temperature, and molar mass is derived. The Maxwell Distribution of Speeds is then presented graphically both with varying temperature and varying molar mass. Finally, the rms speed of a gas is solved for given the temperature and its molar mass.
00:00 Lesson Introduction
00:54 Kinetic Theory of Gases
06:58 Introduction to the Ideal Gas Law
10:52 Individual Gas Laws: Boyle's, Charles, Avogadro's, Guy Lussac's
21:01 Ideal Gas Law Calculations
27:44 Kinetic Energy, Temperature, and rms Speed of a Gas
34:06 Maxwell Distribution of Speeds
Check out Chad's General Physics Master Course: https://courses.chadsprep.com/courses...
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