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Lecture 8

CHM 1045 Lecture 8: Gases

2 Pages

Chemistry and Biochemistry
Course Code
Cameroun Robert

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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-Lussacs 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 Charless 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 Boyles law - Volume is inversely related to pressure with constant temperature - When pressure increase, volume decrease - p1v1=p2v2 Avogadros 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 11 22 1 = 2 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 1 2 - = 2 1 - mw= molecular weight. 0.08206 L atm mol1 K1 and 8.314 kPa L mol1 K1. The Kinetic molecular theory: 1. Gases molecule travel in continuous motion. And only change direction when colliding with another molecule or the wall of the container. 2. The volume of gas is negligible 3. Molecule exert pressure when collide with the wall of container and other molecule. 4. Gas exert no force when colliding. Therefore lost no energy. Gas are elastic. 5. The average
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