| GAS
PRESSURE AND ITS MEASUREMENT |
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Pressure |
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Units of pressure |
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Measuring pressure |
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Atmospheric pressure |
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Pressure of gases |
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Closed-tube manometer |
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Open-ended manometer |
| EMPIRICAL
GAS LAWS |
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Boyle’s Law:
Pressure-Volume relationship |
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Charles’ Law: Temperature-Volume
relationship |
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Gay-Lussac’s Law:
Temperature-Pressure relationship |
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Avogadro’s Law:
Quantity-Volume relationship |
| DERIVED
GAS LAWS |
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Combined Gas Law |
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Ideal Gas Law |
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Mathematical derivation |
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Calculations using the Ideal Gas
Law |
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Calculations involving just P, V,
n, and T |
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Calculations involving mass or molar mass,
P, V, n, and T |
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Calculations involving density and molar mass |
| STOICHIOMETRY
AND THE IDEAL GAS LAW |
| GAS
MIXTURES |
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Partial pressures and mole
fractions |
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Dalton’s Law of Partial Pressures |
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Partial pressure |
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Mole fraction |
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Relationship between mole fraction
and partial pressure |
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Gases collected over water |
| KINETIC
THEORY |
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Definition |
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The five postulates of the Kinetic
Theory of Ideal Gases |
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Gases are composed of particles,
atoms or molecules, whose size can be considered to be negligible. |
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Gas particles are in continuous
random motion. |
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The attractive forces between
particles have a negligible effect on their behavior. |
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Collisions between gas particles
are elastic. |
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The average kinetic energy of a
particle is directly proportional to the absolute temperature. |
| EXPLAINING
THE GAS LAWS FROM THE KINETIC THEORY |
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Explaining Gay-Lussac’s Law |
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Explaining Boyle’s Law |
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Explaining Charles’ Law |
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Explaining Avogadro’s Law |
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Explaining the Ideal Gas Law |
| DIFFUSION
AND EFFUSION AND THE KINETIC THEORY |
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Diffusion |
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Effusion |
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Graham’s Law |
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Root-mean-square molecular speed |
| REAL GASES |
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Conditions under which real gases
deviate from ideal gases |
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Two assumptions that do not hold
true for real gases |
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That the volume of the gas particles themselves
is effectively zero |
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That there is no force of attraction between
gas particles |
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Two conditions under which the
behavior of real gases deviate significantly from the behavior of ideal
gases. |
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High pressure |
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Low temperature |
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In general, the closer a gas is to
the liquid state the more it will deviate from the Ideal Gas Law. |
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Real gases adhere to a corrected
form of the Ideal Gas Law Equation called the van der Waals Equation. |
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