Finding n or mole fraction for each will give you the partial pressure if you know Ptot.
Used most often when gas is collected over water. Why See next
Try a few.
16 Ptot pgas pwater 17 Kinetic Molecular Theory
Large number of particles in constant random motion
Volume of particle is negligible
Forces between particles are negligible
Collisions are perfectly elastic
Average kinetic energy is proportional to average Kelvin temperature
18 KE Distribution 19 Speed of Different Gases same temperature 20 Equations
Average KE 1/2mu2
u is the root mean square speed which is almost the velocity or speed that we are used to.
Explain the three gas laws with this
21 Effusion and Diffusion
Average speed equation no derivation
The smaller the M the faster the average speed
Effusion escape of a gas from a tiny hole into an evacuated space
Diffusion spread of a gas into a space or another substance (we usually mean this!)
22 Comparing two gases
Derive ratio of speeds of gas a and gas b
This is diffusion
Same for effusion use r for rate
Calculate the ratio of the rates of effusion for N2 and O2 gases at the same temperatures.
24 Derivations from Ideal BehaviorIncreased Pressure
PV/RT n For 1 mole this ratio should be equal to 1
Pressure less than 10 atmospheres ideal behavior is seen.
After that what happens
Particles take up space within the volume of the gas.
25 Actually lowers pressure 26 Also causes attractive forces again lowering pressure 27 Decreased Temperature
Lower temperature what happens
Particles begin to attract each other.
Constants to correct for this available for each gas.
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