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# GASES - PowerPoint PPT Presentation

GASES. 5 Assumptions of Kinetic Theory. Gases- large numbers of tiny particles that are far apart for their size They occupy a volume 100 times greater than gases or liquids

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Presentation Transcript

### GASES

• Gases- large numbers of tiny particles that are far apart for their size

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

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

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

• The average kinetic energy of gas particles depend on the temperature of the gas.

• Kinetic energy= ½ mv2

• 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

• Many gases behave closer to ideally at lower pressures and higher temperatures

• Expansion

• Fluidity

• Low Density

• Compressibility

• Diffusion and Effusion

• Gases will fill any container to take its shape

• Gas particles glide easily past each other, so they flow easily

• 1/1000 the density of a liquid or solid

• Particles can be crowded close together by increasing the pressure

• Diffusion-Spontaneous mixing of particles of 2 substances, caused by random motion

• Effusion- gas particles passing through a small opening by random motion

• 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

• 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, O2, H2, H2O, N2, HCl, NH3