Part 3
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Earth's radius | 6370 Km
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| Earth's barometric pressure | 760 mm Hg (density of Hg = 13.6 g/cm^3)
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| Molecular mass of air | 29 g/mol
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| partial pressure of a gas | the pressure exerted by a component of a mixture of gases
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| mole fraction | n1/nt (partial pressure of one component of gas/total pressure)
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| Equation for partial pressure involving mole fraction | (n1/nt)Pt = X1Pt
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| The Kinetic-Molecular Theory (the theory of moving molecules by Calusius) | Gases consist of a lot of molecules (or atoms, in the case of the noble gases) that are in continuous random motion. Kinetic energy of the the molecules doesn't change w/time (as long as T is constant).
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| Kinetic-Molecular Theory - what if you have two gas samples, both at the same temp. | then the kinetic energy for the collection of gas molecules in one sample is equal to the kinetic energy for the collection of gas molecules in the other sample.
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| To to measure hardness of that the molecules hit the wall | V*M (velocity times mass of molecules)
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| if the temp. of a gas is doubled, then the kinetic energy of its molecules is...? | doubled
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| root mean square speed | = 1/2 mu^2
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| What happens when volume increases but the temp. is constant? | pressure will decrease
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| What happens when temp. increase at a constant volume | increase in pressure.
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| root mean square (rms) speed: | (sqrt(3RT/M) M is the molar mass
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| effusion | rate of escape of a gas through a tiny or or pinhole in its container
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| diffusion | the speed of one substance through space, or through a second substance (such as the atm)
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| Which will effuse more rapidly, a lighter gas or a heavy gas | a lighter gas
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| which will diffuse faster, lighter molecules or heavy ones | lighter ones
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| Effusion rate equation | (sqrt(1/M))
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| mean free path | average distance traveled by a molecule
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| The higher the density of gas, the (blank) the mean free path | smaller. (more likelyhood of a collision)
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| The deviation from ideal gas behavior is (blank) at high pressure | large
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| As temp. increases the deviation from ideal behavior (blank) | decreases
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| characteristics of ideal gases | occupy no set volume, gas molecules have no attraction or repulsion for each other
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| Is the ideal gas equation good at high pressures? | not really
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| How are P and V related at constant P? | inversely proportional
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| How are P and T related at constant V? | directly proportional
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| P and n are related how at constant V? | directly proportional
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| how are gas density related to molar mass and pressure? | density is proportional to molar mass and pressure
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| how are gas density related to temperature? | density is inversely proportional to temperature
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| Molar mass = | Density*R*T/P
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You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
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