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18 Cards in this Set
- Front
- Back
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Conversion of Celsius to Kelvin |
Celcius + 273 |
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Atmospheric pressure at sea level |
1 atm= 100 kPascals = 760 torr = 760 mmHg |
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Standard Temperature and Pressure (STP) |
0 degrees celsius or 273 Kelvin 1 atm |
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Ideal Gas Law |
PV = nRT P= pressure V=volume n=moles of gas R=gas constant (0.08 L-atm/K-mol) T=Temp in Kelvins |
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Charles Law |
at a constant pressure: V1/T1 = V2/T2 |
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Boyles Law |
way to remember: Think boyles= boil = temperature at a constant temperature: P1V1 = P2V2 |
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Gas law at constant Volume (Ammonton's Law) |
P1/T1 = P2/T2 |
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Combined Gas Law |
(P1V1)/T1 = (P2V2)/T2 |
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van der Waals Equation (ideal gas law for real gases) |
(P + (an^2)/(V^2)) (V-nb) = nRT "an" term stands to serve as correction for intermolecular forces "nb" term stands to serve as correction for physical volume |
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What factors cause deviation from ideal behavior for gases? |
High pressures and low temperatures |
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What characteristics allow gases to behave ideally? |
weak intermolecular forces and small molecular weights and volumes |
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Standard molar volume at STP |
22.4 Liters Means that one mol of an IDEAL GAS occupies this much space |
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Assumptions made for ideal gases (Kinetic Molecular Theory) |
1.) All collisions are elastic 2.) there are not intermolecular forces 3.) The molecules themselves do not have a volume (volume is based on the container the gas is put in) 4.) Temp is directly related to kinetic energy |
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Ideal gas values are ALWAYS greater than real gas values |
yuh |
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Dalton's Law |
Sum of partial pressures equal total pressure |
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Effusion |
Gases escaping a container through a small hole Smaller / lighter gases effuse faster |
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Graham's Law |
(Effusion of gas A) / (Effusion of gas B) = Square root (molar mass B/ molar mass A) |
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What happens when a gas is compressed? |
it is warmed up |
