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| 1 atm in Pascal(Pa);kilopascal (kPa) |
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| 4 variables of the gas law: |
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-pressure
-temperature
-volume
-amount(in moles) |
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a gas that exhibits linear relationships among these variables
-no ideal gas actually exists |
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at a constant temperature, the volume occupied by a fixed amount of gas is inversely proportional to the external pressure
PV=constant @fixes T and n
P decreases as V increases |
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| as temperature increases volume increases |
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is the temperature at which an ideal gas would have zero volume because gas is directly proportional to its absolute(kelvin) temperature
V/T=Constant |
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standard temperature and pressure
1 atm, 0 degrees celsius |
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a gas that exhibits linear relationships between pressure, temperature, volume, and amount in moles.
-an ideal gas doesn't exist |
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The ideal gas law can also be expressed by the
combined equation:
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Dalton’s Law of Partial Pressures
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• The total pressure of a mixture of gases is
equal to sum of the partial pressures of each
gas
• The intermolecular forces (IMFs) between gas
molecules are considered to be negligible
• Therefore the partial pressure of a particular
gas is independent of the presence of any other
gas in the same container
• The partial pressure of that gas is dependent
only the moles of that gas |
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The Kinetic-Molecular Theory:
A Model for Gas Behavior
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Postulate 1:
Gas particles are tiny with large spaces between them. The volume
of each particle is so small compared to the total volume of the gas
that it is assumed to be zero.
Postulate 2:
Gas particles are in constant, random, straight-line motion except
when they collide with each other or with the container walls.
Postulate 3:
Collisions are elastic, meaning that colliding particles exchange
energy but do not lose any energy due to friction. Their total kinetic
energy is constant. Between collisions the particles do not influence
each other by attractive or repulsive forces. |
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Kinetic Energy and Gas Behavior
At a given T, all gases in a sample have |
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the same
average kinetic energy.
Kinetic energy depends on both the mass and the
speed of a particle.
At the same T, a heavier gas particle moves more
slowly than a lighter one. |
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is the process by which a gas escapes
through a small hole in its container into an evacuated
space.
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| Graham’s law of effusion states |
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that the rate of effusion
of a gas is inversely proportional to the square root of its
molar mass.
A lighter gas moves more quickly and therefore has a
higher rate of effusion than a heavier gas at the same T.
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