3 phases and gases - STP(0 ° C and 1atm 1 mole gas = 22.4L...

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Phases Physical Changes Phase Transitions Endo- vs. Exothermic Entropy Changes Calorimetry (q = mc T) Diagram Phase Diagrams General H 2 O CO 2
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Gases Kinetic Molecular Theory Ideal Gas Assumptions 1) Gas molecules themselves have no volume 2) No intermolecular attractions between molecules (all collisions are elastic) Kinetic energy T Characteristics of Gases Volume (Liters; 1cm 3 = 1mL) Temperature ( ° C or K) Pressure (1atm = 760 torr = 760mmHg)
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Unformatted text preview: STP (0 ° C and 1atm) 1 mole gas = 22.4L @ STP Ideal Gas Law PV = nRT (Works best at low P, high T, and for non-polar gases) Boyle’s Law P ∝ V 1 Charle’s Law V ∝ T Avogadro’s Law V ∝ n Combined gas law 2 2 2 2 1 1 1 1 T n V P T n V P = Dalton’s Law of Partial Pressures P Tot = P A + P B + … P A = χ A P Tot Graham’s Law of Effusion 1 2 2 1 M M r r =...
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3 phases and gases - STP(0 ° C and 1atm 1 mole gas = 22.4L...

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