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Kinetic Theory of Gases
- Ideal gas law: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R = 8.314 J/(mole. K) is the universal gas constant, and T is the temperature in K.
- The number of moles n = N/Na, where N is the number of atoms (or molecules), and Na is Avogadros number.
- The root mean square speed of a molecule, Vrms, is equal to the square root of 3RT/M, where M is the molecular mass of the gas.
- The translational kinetic energy of n moles of a gas is 3nRT/2.
- In a gas at a given temperature, there is a distribution of speeds of the molecules. Some molecules move relatively slowly and others move relatively fast.
Kinetic Theory of Gases
Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.
- Intro
- Ideal Gas Law
- Ideal Gas Definition
- 1 Mole of Gas
- Avogadro's Number
- Gas in a Container, Pressure Increases with Temperature
- Ideal Gas law
- Boltzmann's Constant
- Example
- Conceptual Example
- Shake and Open the Coke Bottle
- Quantitative Example: Container with Gas
- Heat the Gas to 127 Degrees
- Kinetic Theory
- Container in a Cube Shape
- Molecules Travelling with Velocity v
- Change in Momentum of Molecule Per Second
- Newton's Third law
- Example
- Distribution of Molecules
- Extra Example 1: Helium Gas in Balloon
- Extra Example 2: Oxygen Molecules
































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