Diffusion vs. Effusion Diffusion - The tendency of the molecules of a given substance to move from regions of higher concentration to regions of lower concentration Examples: A scent spreading throughout a room or people entering a theme park Effusion - The process by which gas particles under pressure pass through a tiny hole Examples: Air slowly leaking out of a tire or helium leaking out of a balloon
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Diffusion vs. Effusion Diffusion - The tendency of the molecules of a given substance to move from regions of higher concentration to regions of lower.
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Diffusion vs. EffusionDiffusion - The tendency of the molecules of a given substance to move from regions of higher concentration to regions of lower concentrationExamples: A scent spreading throughout a room
or people entering a theme park
Effusion - The process by which gas particles under pressure pass through a tiny holeExamples: Air slowly leaking out of a tire or
helium leaking out of a balloon
Effusion
Particles in regions of high concentrationspread out into regions of low concentration,
filling the space available to them.
NETNET MOVEMENT
To use Graham’s Law, both gases must be at same temperature.
diffusiondiffusion: particle movement from
high to low concentration
effusioneffusion: diffusion of gas particles
through an opening
For gases, rates of diffusion & effusion obey Graham’s law: more massive = slow; less massive = fast
Graham’s Law
KE = ½mv2
Speed of diffusion/effusionSpeed of diffusion/effusion– Kinetic energy is determined by the temperature of
the gas.
– At the same temp & KE, heavier molecules move more slowly.
A molecule of oxygen gas has an average speed of 12.3 m/s at a given temp and pressure. What is the average speed of hydrogen molecules at the same conditions?