5 - Pressure : collisions with container cause this;...

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1 Kinetic Molecular Theory What is occurring at the microscopic level? How do individual particles exert force to give pressure? Why are gases compressible? And what happens on the molecular level? Why does the law of partial pressures work? What is the temperature effect on molecules? Why does Avogadro’s law work? Shouldn’t smaller molecules occupy less space than larger ones? What about pressure considerations? Kinetic Molecular Theory Particles have an average (or most probable ) speed: u mp increases with increasing T cT E K = So at a given T all gases have the SAME kinetic energy!
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Unformatted text preview: Pressure : collisions with container cause this; anything that causes them to ⇑ will cause ⇑ P; Compressibility : ⇓ space and molecules hit walls more often: ⇑ P; Partial Pressures : Simply an ⇑ in the number of molecules; more molecules to collide with walls (assume NO IMF’s!) Temp Effect : ⇑ energy and molecules move faster and hit walls more often: ⇑ P; Avogadro’s : ⇑ molecules, ⇑ collisions; ⇑ V until collisions per surface area gets to where it was before addition 2 3...
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This note was uploaded on 01/30/2012 for the course CHEM 6A taught by Professor Pomeroy during the Summer '08 term at UCSD.

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5 - Pressure : collisions with container cause this;...

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