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12 Cards in this Set
- Front
- Back
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Gas Pressure |
Results from collisions of molecules on the container |
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vapor |
The gaseous state of a substance that would otherwise be normally a solid or liquid at standard temperature and pressure |
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Equation for pressure in terms of height of a liquid |
P =dgh where (d) equals density, (g) equals gravity, (h) equals height |
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Ideal Gas Law |
PV= nRT where P=pressure, V=volume, n=amount of substance in moles, T=temperature, and R=the gas law constant Note: the three other major gas laws are variations on this gas law |
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Boyle's Law |
The volume of a fixed sample of gas at a given temperature is inverselyproportional to the applied pressure i.e. PV =k and P1V1 = P2V2 |
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Charles' Law |
The volume of a fixed sample of gas at constant pressure is directlyproportional to its absolute temperature ie. V= kT or V1/T1 = V2/T2 |
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Avogardo's Law |
The volume occupied by a fixed amount of gas is the same no matter whatthat gas is ie. v =kn |
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Partial Pressure |
The pressure of one gas in a mixture of different gases |
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Finding partial pressure |
for gases X,O,Z total P = Po+Px+Pz PzV = nzRT PxV = nxRT PoV = noRT |
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Graham's Law |
The rate of diffusion (or effusion) of two gases is inverselyproportional to their molar masses: (rate = same as velocity) ie: u̅2/u̅1=r2/r1= √ (M1/M2) |
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Effusion |
process in which a gas under pressure flows through a small hole in a container |
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Diffusion |
is the gradual mixing of molecules of one gas with molecules ofanother gas by virtue of their kinetic properties |
