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11 Cards in this Set
- Front
- Back
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When dealing with gases what do we assume?
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We assume they have nonexistent intermolecular forces and occupy no volume. Volume of gases change extensively with changes in pressure and temperature.
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What are the distinct properties of gases?
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They expand to fill their container.
They are quite compressible under pressure. they form homogenous mixtures with each other regardless of their identities. |
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What does STP stand for (Gas laws)?
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Standard Temperature and pressure.
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0.0 Celsius = ? K
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273.15 K
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Pressure = 1 ?
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1 atmosphere = pressure
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What is the kinetic molecular theory of gases?
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Attractive and repulsive forces between gas molecules are negligible.
The volume of all molecules of the gas is negligible compared to the volume in which the gas is contained. Collisions between gas molecules are elastic; henceforth there is no gain or loss of energy. Gas molecules collide with each other and the walls of their container in a random, continuous motion. |
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What is Graham's law of effusion?
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Graham's law states that the rates of effusion are inversely proportional to the square roots of the densities of the gases.
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What does Dalton's law state?
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It states that the total pressure of a mixture of gases is equal to the sum of the individual pressures exerted by all the gases.
P(total) = RT/V (N1 + N2 + N3 + ...) R = 0.0821 L-atm/K-mol T = Kelvin temperature n = Number of moles. |
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What is Boyle's law?
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Pressure and volume are inversely proportional to one another and the temperature is constant.
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What is Charle's law?
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It states that volume and absolute temperature are directly proportional and pressure is constant.
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What is the ideal gas law?
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PV = nRT
This law assumes that each gas occupies the entire volume of the vessel with its own partial pressure. We can use this relationship to find the density and molar mass of the gas. |
