Kinetic Molecular Theory of Matter Kala Costin, Kyra Safrin, trell Fennell, Alison Cannon, Jesus Ramirez

Can you smell the perfume? Raise your hand when you first smell the perfume. Try to explain the motions of the molecules floating around the room when the perfume was sprayed.

What is Kinetic-Molecular theory of matter? The kinetic-molecular theory of matter can be used to explain the properties of gases, liquids, and solids.

Real and Ideal Gases An Ideal Gas is a hypothetical gas that perfectly fits all the assumptions of the kinetic- molecular theory. A Real Gas is a gas that does not behave completely according to the assumptions of the kinetic-molecular theory.

The nature of gases Expansion- Gases do not have a definite shape or volume. Gas particles move rapidly in all directions. They take shape of the container they are put into. Move in all directions without attraction between them. Fluidity- Gas particles slide past each other easily. The attraction between them are insignificant. Gases are considered fluids because they possess the same abilities as liquids do.

The nature of gases continued Low Density- Particles are so much farther apart in gaseous states, so this leads to atmospheric temp in gases to be about 1/1000 the density of the same substance in liquid or solid states. Compressibility- Gas particles are crowded close together in compressibility, where normally they would be spread far apart. Thus, the volume of the sample of gas will greatly decrease.

Diffusion and effusion Gases spread out and mix together. Random continuous motions of gas particles carry them throughout the space available. Diffusion- the spontaneous mixing of the particles of two substances caused by the random motion Effusion- Gas particles passing through a tiny opening. The rate of effusion of different gases is directly proportional to the velocities of their particles. In other words, the molecules of low mass effuse at a faster rate than molecules at a higher mass.

Fun facts about this subject Molecular motion is completely random. Particles in motion possess kinetic energy. Molecular motion is greatest in gases, less in liquids, and least in solids.