1. GASES

2. 5 Assumptions of Kinetic Theory 1.Gases- large numbers of tiny particles that are far apart for their size They occupy a volume 100 times greater than gases or liquids They occupy a volume 100 times greater than gases or liquids Most of a gases’ vol is empty space, which accounts for gas’ lower density than that of liquids and solids, and explains why gases can be compressed Most of a gases’ vol is empty space, which accounts for gas’ lower density than that of liquids and solids, and explains why gases can be compressed

3.  All collisions are perfectly elastic, there is a transfer of kinetic energy

4. 3. The particles of a gas are in continuous, rapid, and random motion

5. 4. Between gas particles, there are no attractive or repulsive forces.

6.  The average kinetic energy of gas particles depend on the temperature of the gas.  Kinetic energy= ½ mv 2  KE depends only on a gases’ mass, since they have constant velocity  Speeds increase when temp increases, decrease when it decreases  All gases at the same temperature have the same average KE  Lighter gas particles have higher speeds

7. Kinetic Theory of and Nature of Gases  Many gases behave closer to ideally at lower pressures and higher temperatures

8. 5 Properties of gases  Expansion  Fluidity  Low Density  Compressibility  Diffusion and Effusion

9. Expansion  Gases will fill any container to take its shape

10. Fluidity  Gas particles glide easily past each other, so they flow easily

11. Low Density  1/1000 the density of a liquid or solid

12. Compressibility  Particles can be crowded close together by increasing the pressure

13. Diffusion and Effusion  Diffusion-Spontaneous mixing of particles of 2 substances, caused by random motion  Effusion- gas particles passing through a small opening by random motion

14. Real gas  Gases that don’t behave as ideal gases.  They deviate from ideal gas befavior because the particles occupy space and exert atractive forces on each other  Deviate the greatest when:  Pressure is high and temperature is low—the particles are closest together

15. Gases that behave most closely to ideal  Those whose particles do not attract  Nonpolar gases and noble gases  #4. Which gases deviate the most from ideal behavior (the ones that are polar and do attract) He, O 2, H 2, H 2 O, N 2, HCl, NH 3  Answer: H 2 O, HCl, NH 3