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Lecture 8

# CHM-1045 Lecture Notes - Lecture 8: Combined Gas Law, Ideal Gas Law, Kinetic Theory Of Gases

Department
Chemistry and Biochemistry
Course Code
CHM-1045
Professor
Cameroun Robert
Lecture
8

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CHM 1045- Lecture 8- Gases
Gas pressure is the result of the force of gas molecules when colliding with the surfaces of
objects
- 760 mm Hg = 760 torr = 1 atm = 101325 Pa
Gay-Lussac’s law.
- the pressure is directly related to temperature with constant volume
- When temperature increase, pressure increase.
- Temperature must be in Kelvin
- P1/T1=P2/T2
Charles’s law
- Volume is directly related to temperature with constant temperature.
- Volume increases as the temperature increases,
- Temperature must be in Kelvin
- v1/t1=v2/t2
Boyle’s law
- Volume is inversely related to pressure with constant temperature
- When pressure increase, volume decrease
- p1v1=p2v2
Avogadro’s law
- Mole of a gas is directly related to its volume with constant pressure and temperature.
- v1/n1=v2/n2
ideal gas law
- a relation between the pressure, volume, temperature, and number of moles of a gas:
- PV=nRT
- R value depend on pressure unit
Combined gas law

 =

R value= 0.08206 L atm mol1 K1 and 8.314 kPa L mol1 K1.
- Ideal gas happen under low pressure and high temperature.
Diffusion
- Spreading of gas molecule into surface area
- From high to low concentration
Rate of diffusion
Rate of diffusion= amount of gas passing through an area /unit of time
Effusion
- The escape of molecule through hole
- 
=

- mw= molecular weight.
0.08206 L atm mol1 K1 and 8.314 kPa L mol1 K1.
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