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18 Cards in this Set
- Front
- Back
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Characteristics of Ideal Gasses |
-Negligible attractive forces between molecules - pt. sized molecules - perfectly elastic collisions (No Ideal Gas exists) |
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Near-Ideal Gasses (Noble) |
(Ne, He, Ar, Kr, Ra, Xe) - mono-atomic - pure - lightweight |
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Gas Laws rely on 4 variables: |
- Pressure, P - Volume, V - Temp. T - # of moles, n |
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Mole |
An amount of a substance having a mass in grams that is equal to it's molecular mass, MM |
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Molecular Mass |
MM, the sum of all the atomic masses of the atoms making up a molecule |
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Atomic mass |
The mass of one atom measured in Atomic Mass Units |
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Atomic Mass Unit |
(u) 1/12 the mass of a single carbon 12 atom |
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Isotope |
Atoms of the same element having a different number of neutrons |
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Atomic Number |
The number of protons in the nucleus of an atom. This determines what element the atom is. |
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Avagadro's Number |
1 mole of any substance contains the same number of molecules. -6.022 x 10²³ mol/mole |
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S.T.P. |
P - 1 atm = 14.7 lb/in² = 76 cm Hg T - 0°C = 273K |
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Gas Laws only work for... |
Absolute temperature and pressure! |
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Boyle's Law |
As pressure increases, volume decreases P1V1 = P2V2 |
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Charles' Law |
As temperature increases, volume increases. V1/T1 = V2/T2 |
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Gay-Lussac's Law |
As pressure increases in a sealed container, temperature increases. P1/T1 = P2/T2 |
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Converting guage pressure: |
Pabsolute = Pguage + Patm
If problem asks for guage P, add Patm in beginning, subtract it at end. |
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Equation for finding # of moles |
n = m / MM |
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Equation for finding Number of molecules |
N = n(NA) |
