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14 Cards in this Set
- Front
- Back
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Kinetic Molecular Theory
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1. Ignore volume
2. No intermolecular forces (elastic collisions) 3.KE ~ T |
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Ideal gas
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Gas that satisfies all requirements of kinetic molecular theory
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STP
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standard temperature and pressure -0 C (273 K) and 1 atm (760 mm Hg = 760 torr)
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Ideal Gas Law
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PV= nRT
P1V1/T1= P2V2/T2 |
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Charles Law
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If the pressure is constant, volume is proportional to temperature
V1/T1 = V2/T2 |
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Boyles Law
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if the temperature is constant, pressure is inversely proportional to volume
P1V1=P2V2 |
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Constant volume
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Pressure is proportional to temperature
P1/T1=P2/T2 |
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1 mole ideal gas
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22.4 L at STP
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Daltons Law of Partial Pressures
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Total pressure is sum of partial pressures of all the constituent gases
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Partial pressure of gas
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Mole fraction * total pressure
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Effusion
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The escape of gas molecules through a tiny hole to the vacuum
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Diffusion
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Mixing of the gases (not vacuum)
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Grahams Law of Effusion
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rate of effusion of gas A/rate of effusion of gas B = sqrt (molar mass of gas B/molar mass of gas A)
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At what conditons do gases approach ideal gases behavior?
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low pressure and high temperature
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