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Gas **
Part 3
| Question | Answer |
|---|---|
| Earth's radius | 6370 Km |
| Earth's barometric pressure | 760 mm Hg (density of Hg = 13.6 g/cm^3) |
| Molecular mass of air | 29 g/mol |
| partial pressure of a gas | the pressure exerted by a component of a mixture of gases |
| mole fraction | n1/nt (partial pressure of one component of gas/total pressure) |
| Equation for partial pressure involving mole fraction | (n1/nt)Pt = X1Pt |
| 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). |
| 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. |
| To to measure hardness of that the molecules hit the wall | V*M (velocity times mass of molecules) |
| if the temp. of a gas is doubled, then the kinetic energy of its molecules is...? | doubled |
| root mean square speed | = 1/2 mu^2 |
| What happens when volume increases but the temp. is constant? | pressure will decrease |
| What happens when temp. increase at a constant volume | increase in pressure. |
| root mean square (rms) speed: | (sqrt(3RT/M) M is the molar mass |
| effusion | rate of escape of a gas through a tiny or or pinhole in its container |
| diffusion | the speed of one substance through space, or through a second substance (such as the atm) |
| Which will effuse more rapidly, a lighter gas or a heavy gas | a lighter gas |
| which will diffuse faster, lighter molecules or heavy ones | lighter ones |
| Effusion rate equation | (sqrt(1/M)) |
| mean free path | average distance traveled by a molecule |
| The higher the density of gas, the (blank) the mean free path | smaller. (more likelyhood of a collision) |
| The deviation from ideal gas behavior is (blank) at high pressure | large |
| As temp. increases the deviation from ideal behavior (blank) | decreases |
| characteristics of ideal gases | occupy no set volume, gas molecules have no attraction or repulsion for each other |
| Is the ideal gas equation good at high pressures? | not really |
| How are P and V related at constant P? | inversely proportional |
| How are P and T related at constant V? | directly proportional |
| P and n are related how at constant V? | directly proportional |
| how are gas density related to molar mass and pressure? | density is proportional to molar mass and pressure |
| how are gas density related to temperature? | density is inversely proportional to temperature |
| Molar mass = | Density*R*T/P |
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