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Molecules Cause Pressure
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Molecules Cause Pressure
Kinetic Molecular Theory
Particles of matter are ALWAYS in motion
Volume of individual particles is zero. Collisions of particles with container
walls cause pressure exerted by gas.
Particles exert no forces on each other.
Average kinetic energy µ Kelvin temperature of a gas.
Kinetic Energy of Gas Particles
At the same conditions of temperature, all gases have the same average kinetic energy.
2
2
1mvKE
Different Gases at Same Temp.
Same Gas - Two Temperatures
Distribution of Molecular Speeds
Maxwell’s equation relates molecular mass, average speed, and temperature together.
Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing.
Diffusion
EffusionEffusion: describes the passage of gas into an evacuated chamber.
Rate of effusion for gas 1Rate of effusion for gas 2
2
1
MM
Distance traveled by gas 1Distance traveled by gas 2
2
1
MM
Effusion:
Diffusion:
Graham’s LawRates of Effusion and Diffusion
Real Gases
[ ]P a V nb nRTobs2( / ) n V
corrected pressure corrected volume
Pidea
l
Videa
l
Must correct ideal gas behavior when at high pressure (smaller volume) and low temperature (attractive forces become important).