10.3 Dalton's Law of Partial Pressure, Gas Density, & Graham's Law of Effusion | General Chemistry

Chad provides a lesson on some additional gas laws. The lesson begins with Dalton's Law of Partial Pressure showing how the partial pressure of a gas in a mixture is proportional to its mole fraction. The condition of STP (standard temperature and pressure; T = 273K, P = 1atm) is then introduced and how 1 mole of any gas behaving ideally will have a volume of 22.4L at STP. The relationship and formula between gas density, pressure, temperature, and the gas's molar mass is presented along with a sample calculation. Finally, the lesson is concluded with Graham's Law of Effusion with an example calculation demonstrating that H2 gas would escape from a balloon 4 times faster than O2 gas.

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00:00 Lesson Introduction
00:55 Dalton's Law of Partial Pressure
05:31 Molar Volume at STP (22.4L)
10:02 Gas Density and Molar Mass
16:30 Graham's Law of Effusion

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