lecture24_chem110_sas

lecture24_chem110_sas - Chapter 10: Gases Part 3: Real...

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Chapter 10: Gases Part 3: Real Gases CH110 FA11 SAS 1 Prepare for Recitation October 20 th ALEKS Objective 8 due October 18 th ANGEL Quiz 8, October 20 th Lecture 22: October 12 th Lecture 23: October 14 th Lecture 24: October 17 th Read: Ch. 10.1-10.9 Additional Preparation: BLB 10 : 5,23,30,45,71,75,82-84; Packet 10 : 1-15 BLB 25 : 11,12,25
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CH110 FA11 SAS 2 By the end of Today’s Lecture you should know: Kinetic-molecular theory Real gases (van der Waals) KEY QUESTIONS: THE BIG PICTURE Chapter 10: Gases Part 3: Real Gases What does partial pressure mean? What type of mixtures do gasses form? What state equation can we use to describe mixtures of gasses? Remember: macroscopic properties come from microscopic origins How does the energy of a molecule in a gas compare with intermolecular forces? How can we describe mixtures of gasses? How do real gasses differ from ideal gasses?
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Effusion and Diffusion CH110 FA11 SAS 3 Note: Diffusion is more complicated due to collisions between gas molecules, but it also obeys Graham’s Law. Graham’s Law of Effusion: M 2 M 1 r 1 r 2 = Effusion: Diffusion: Heavy molecules diffuse (or effuse) more ______ than lighter ones. 1 M r proportional to
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Practice Problem CH110 FA11 SAS 4 An unknown gas effuses at a rate 1.49 times faster than Cl 2 . What is the molecular weight of the gas? A. 16.0 g/mol B. 31.9 g/mol C. 47.6 g/mol D. 106 g/mol E. 157 g/mol
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CH110 FA11 SAS 5 The rate of diffusion follows Graham’s Law At STP molecules collide ~ 10 10 times per second N 2 speed = 500 m/s but … … in 1 s it collides 10 10 times What happens to the MFP as density and pressure decrease? Mean Free Path (MFP):
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lecture24_chem110_sas - Chapter 10: Gases Part 3: Real...

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