Understanding Pressure and Partial Pressure in Gas Mixtures
Explore pressure conversions, Daltons Law, and the causes of gas pressure in a closed container. Learn how to calculate partial pressures and understand the impact of gas molecule interactions on pressure behaviors.
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Presentation Transcript
Topic: Pressure (and Partial Pressure) Do Now: Convert the following units of pressure 249 torr to atm 10432 Pa to kPa 2534 kPa to mmHg
What causes the pressure of a gas in a closed container? Impacts of gas molecules with walls of container Pressure depends on: # impacts per unit time Force each impact Microscopic View
Light molecules move faster and hit walls more often Heavy molecules hit walls with greater force These 2 effects essentially balance out **Gas pressure doesn t depend on the identity(light like He(g) or heavy like CO2(g))of the gas**
Molecular Speeds at 298 K H2 He 1.36 X 105 cm/sec O2 Ar 4.31 X 104 cm/sec Xe 2.38 X 104 cm/sec 48200 cm 1 in 1 ft sec 2.54 cm 12 in 1080 miles per hour 1.93 X 105 cm/sec 4.82 X 104 cm/sec * 1 mile 3600 sec = 5280 ft 1 hour
Daltons Law of Partial Pressure The sum of individual pressures of all the gasses that make up a mixture is equal to the total pressure of the mixture PT = P1 + P2 + P3+
1 atm = Pressure of N2 + Pressure of O2 + pressure of Ar + pressure of H2) (g) + .. In order to figure Partial Pressure of N2 = 1 atm (.7655) = .7655atm
