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Chapter 6
Pressure= Force / Aera
Factors that affect Pressure
- The number of gas molecules
- The volume of Container
- The average speed of molecules
(Higher the concentration, the greater pressure) (Lower the concentration, the pressure)
Gas I
Boyle's Law Pressure up Volume down
Pressure down Volume up
Ideal Gas Law: PV= NRT (r=0.0821)
Standard Conditions: 1 atm pressure, 273 K or O Cel
Density is directly proportional to the molar mass
Gas Law II
Partial Pressure: Ptotal= Pa + Pb+ Pc..... Pn= nn * RT/V
1 atm; 760 torr; 760 mmHg
Gas III
Kinetic Energy= 1/2 N^a * m * u^2
Gas particles are in constant motion and exhibit perfect elastic collisions
- Gas Sizes are very small
- Kinetic Energy is proportional to temperature
- Collision of gas are elastic
Molar Mass up Kinetic / Molecular SPeed down
Volume up Kinetic Energy up
Temperature up Kinetic Energy up
Mean Free Path
mean free path- the average distance a molecule travels before the collision
- the greater the pressure, the mean free path distance decreases
Density, Temperature, and Volume effect collision rate
Diffusion: particles moving high to low concentration
Effusion: the Escaping of particles through an opening
Grahams Law rate of a/ rate of b = sqrt of Ma/ Mb
Real Gas Behaviours: not all gases behave the same, at ideal settings
(P + a (n/v)^2) x ( v- nb) = NRT
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