Gases
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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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GASES

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Gases

GASES


5 assumptions of kinetic theory

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

    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


Gases

  • All collisions are perfectly elastic, there is a transfer of kinetic energy


Gases

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


Gases

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


Gases

  • 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


Kinetic theory of and nature of gases

Kinetic Theory of and Nature of Gases

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


5 properties of gases

5 Properties of gases

  • Expansion

  • Fluidity

  • Low Density

  • Compressibility

  • Diffusion and Effusion


Expansion

Expansion

  • Gases will fill any container to take its shape


Fluidity

Fluidity

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


Low density

Low Density

  • 1/1000 the density of a liquid or solid


Compressibility

Compressibility

  • Particles can be crowded close together by increasing the pressure


Diffusion and effusion

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


Real gas

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


Gases that behave most closely to ideal

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, O2, H2, H2O, N2, HCl, NH3

  • Answer: H2O, HCl, NH3


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