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21 Cards in this Set
- Front
- Back
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Gases
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Least dense form of matter Fluid and conform to the shape of their container Easily compressible
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Variables to Describe Gases
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Temperature, pressure, volume, number of moles
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Standard Temperature and Pressure
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273 K and 1 atm
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Equations for Ideal Gases
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Assume negligible volume and mass of gas molecules
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Ideal Gas Law
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Avogadro’s Principle
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Pressure and temperature held constant
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Boyle’s Law
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Temperature and number of moles held constant
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Charles’s Law
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Pressure and number of moles held constant
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Gay-Lussac’s Law
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Volume and number of moles held constant
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Combined Gas Law
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Combination of other gas laws
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Density
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Dalton’s Law of Partial Pressure
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Henry’s Law
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Amount of gas dissolved in solution is directlyproportional to the partial pressure of that gas at the surface |
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Kinetic Molecular Theory Assumptions
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Gas particles have negligible volume, lack intermolecular attractions and repulsions, have elastic collisions, average kinetic energy is directly proportional to temperature
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Average Molecular Speeds
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Rule of Thumb Gas Molecule Speed
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Higher temp, faster the molecule
Larger molecule, slower the molecule |
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Graham’s Law
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Gases with lower molar masses will diffuse or effuse faster than gases with higher molar masses at the same temperature
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Real Gases
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Deviate from ideal behavior under high pressure (low volume) and low temperature conditions
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Real Gases Occupy Less Volume
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At moderately high pressures, low volumes, or low temperature because of intermolecular forces
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Real Gases Occupy More Volume
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At extremely high pressures, low volumes, or low temperatures because particles occupy physical space
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Van der Waals Equation of States
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Corrects the ideal gas law for intermolecular forces (a) and molecular volume (b)
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