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35 Cards in this Set
- Front
- Back
phases
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solid liquid gas
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gases and liquids are defined as _____
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fluids
they both can 'flow' |
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gas particles have ___ intermolecular forces between them
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weak
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both gases/liquids can take the shape of the container
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know this
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gases are ______, unlike solids and liquids
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compressible
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define gas based on 4 variables
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pressure
temperature moles volume |
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1 atm =
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760mm Hg = 760torr = 100kPa
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gases occur under STP
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273K and 1 atm
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ideal gases have
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1. no intermolecular forces/interactions
2. occupy no volume 3. low pressure 4. high temperature |
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non ideal gas situation?
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high pressure and low temperature
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kinetic molecular theory
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all gases show similar physical characteristics and behavior irrespective of their chemical identity
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rules of kinetic molecular theory
1. gases are made up of particles whose volumes are ____ compared to volume of container |
1. negligible
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2. gas atoms/molecules exhibit no ________ or _______
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2. intermolecular attractions or repulsions
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3. gas particles are in continuous ____ motion
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3. random
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4. collisions between molecules are _____ meaning conservation of momentum and KE
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4. elastic
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5. the average KE is ____ to the temperature
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proportional
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6.the KE is ____ of all gases at a given temperature, regardless of chemical identity or mass
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6. identical
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average molecular speeds =
KE = 1/2mv^2 = (3/2kT) |
know this
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speed = (3RT/MM)^1/2
trend? |
speed is inversely proportional to molecular mass...hence the heavier an atom is, the slower it will move
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as temperature increases, the average speed of molecules ____
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increase
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diffusion = effusion =
r1/r2 = (MM2/MM1)^1/2 |
r = rates (proportion)
MM = molecular mass |
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all gas particles have the ____ KE at the same temperature
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same
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effusion =
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flow of a gas particles under pressure from one compartment to another through a small opening
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avogadro's principle with constant pressure and temperature
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equal amts of all gases at the same temperature and pressure will occupy equal volumes
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volume at STP
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22.4L/mol
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n1/V1 = n2/V2 = k
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proportional moles to volumes
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ideal gas law EQ
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PV = nRT
R = 8.314J or .0821atm |
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density
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mass/volume = g/L
OR [P(MM)] / RT |
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PV/T =P2V2 / T2
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know this
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Boyle's Law
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PV =PV
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Charles' Law
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V/T = V/T
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partial pressures
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P(A) = P(T)*X(A)
P(T) = total pressure X = moles |
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real gases deviate with
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pressure
temperature |
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real gases and pressure
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as pressure increases, take up LARGER volume than predicted
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real gases and temperature
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as the temperature is decreased, the particles have a SMALLER volume than predicted
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