1 / 9

Kinetic Molecular Theory

Kinetic Molecular Theory. ki⋅net⋅ic. Origin: 1850–55; < Gk kīnētikós moving, equiv. to kīnē - ( verbid s. of kīneîn to move) + - tikos. Source: Websters Dictionary. Particles of matter are ALWAYS in motion Volume of individual particles is  zero.

oya
Download Presentation

Kinetic Molecular Theory

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Kinetic Molecular Theory ki⋅net⋅ic Origin: 1850–55; < Gk kīnētikós moving, equiv. to kīnē- (verbid s. of kīneîn to move) + -tikos Source: Websters Dictionary

  2. Particles of matter are ALWAYS in motion Volume of individual particles is  zero. Collisions of particles with container walls cause the pressure exerted by gas. Particles exert no forces on each other. Average kinetic energy is proportional to Kelvin temperature of a gas. Kinetic Molecular Theory

  3. Kinetic Energy of Gas Particles At the same conditions of temperature, all gases have the same average kinetic energy. m = mass v = velocity  At the same temperature, small molecules move FASTER than large molecules

  4. Gases expand to fill their containers Gases are fluid – they flow Gases have low density 1/1000 the density of the equivalent liquid or solid Gases are compressible Gases effuse and diffuse The Nature of Gases

  5. The Nature of Gases Effusion is going from a “crowded” room to a less crowded room through a small hole.

  6. The Nature of Gases Diffusion is one gas spreading out within another. (Skunk smell)

  7. Diffusion • Diffusion describes the mixing of gases. The rate of diffusion is the rate of gas mixing. • Diffusion is the result of random movement of gas molecules • The rate of diffusion increases with temperature • Small molecules diffuse faster than large molecules

  8. Graham’s Law of Diffusion M1 = Molar Mass of gas 1 M2 = Molar Mass of gas 2

  9. Purification of Uranium-235 Using Gaseous Diffusion

More Related