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Kinetic Molecular Theory Definition




 
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More Lessons for High School Chemistry

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A series of free High School Chemistry Video Lessons and solutions.

In this lesson, we will learn

  • vapor pressure
  • kinetic-molecular theory of gases.
  • Avogadro's Principle
  • Dalton's Law of Partial Pressure
  • Graham's Law of Effusion

Vapor Pressure
Vapor pressure is the pressure caused by the evaporation of liquids. Three common factors that influence vapor press are surface area, intermolecular forces and temperature. The vapor pressure of a molecule differs at different temperatures.
The pressure caused by the evaporation of liquids.
Vapor Pressure, Volatility, and Evaporation



Gases
The gaseous state is one of the three phases of matte. Gases are obtained through vaporization from liquid and sublimation from solid. When a liquid vaporizes, it is often called boiling. Gases are the least dense state of matter because they contain high kinetic energy.
The phase at which matter has the highest kinetic energy.
Reviews kinetic energy and phases of matter, and explains the kinetic-molecular theory of gases.


 
Uses the kinetic theory of gases to explain properties of gases (expandability, compressibility, etc.)
Avogadro's Principle
Avogadro's Principle, also known as Avogadro's Law, is one of the gas laws. Avogadro's Principle states that equal volume of mass at the same temperature and pressure contain the same number of molecules. This principle can be expressed in mathematical terms as volume/amount of gas = proportionality constant.
Understanding and applying Avogadro's Principle.


Practice problems and examples, looking at the relationship between the volume and amount of gas (number of moles) in a gas sample.
Dalton's Law of Partial Pressure
Dalton's Law states that total pressure of a gaseous mixture is equal to the sum of the partial pressures of each substance present.
Understanding and applying Dalton's Law.


 
Dalton's Law of Partial Pressure
Graham's Law
Graham's Law states that the rate of effusion for a gas is inversely proportional to the square root of its molar mass.
Understanding and applying Graham's Law. Graham's Law of Effusion - Gases


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