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21 Cards in this Set
- Front
- Back
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What is the SI unit for pressure |
it is pascals, 1 atm= 101.325 pascals. |
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what is the STP (standard temperature and pressure for a gas) |
it is at 273 K (0 celisus) and 1ATM. |
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Standard state conditions is for enthlapy and entropy an free energy changes and are? |
298 K. and 1M concentration AND 1 atm. |
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IDEAL gas |
PV=nRT. |
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Combined gas law/ what is it and where is it used |
used to find the change in the volume or pressure or temp from the standard. |
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avogadro's principle
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at constant temperature and pressure, as number of moles increases the volume increases as well. N/V= n2/V2. K(which in this case is constant pressure over constant temperature) = N/V. derive it from Ideal gas law its not hard. |
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Boyle's law |
P goes up, V goes down and vice versa in constant temperature. |
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Charles' law |
V/T =V/T K= V/T |
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Gay-Lussac's law |
If constant volume and moles, then Pressure increases with temperature. |
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Combined Gas law. |
PV/T. |
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Dalton's law of partial pressure. |
In a container that contains a mixture of gasses, the total pressure exerted is equal to the partial pressure of each gas. Ptotal= Pa+Pb+Pc... Pa= Ptotal * molar fraction of a. molar fraction of a= Moles of gas a/ Total moles of gas. |
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Henry's law |
Look it up [A]= kH (henry constant)* Partial pressure A. and in case of changing pressure A1/P1=A2/P2 - pay attention to use MOLAR VALUE for A's not moles (aka divide moles by volume). |
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vapor pressure |
pressure exerted by the evaporated molecules on the surface of the liquid. |
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Graham's law of diffusion and effusion |
movement of molecules from high concentrations to low concentrations. |
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If a gas particles travel at the SAME average kinetic energy, what does that mean....especially if one is faster. hint* according to KE= 1/2 MV^2* |
since they both have the same KE, then the one traveling faster MUST be less in mass (ligher).
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Pleural effusion |
fluid flows into the pleural space through small openings in the capillaries or lymphatic vessels. This causes pressure to build up around the lungs which hinders breathing. |
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Deviation of the Ideal Gas Law (Due to pressure). |
1- at moderately high pressure, a gas' volume would be less than that predicted by the gas law. 2-At extremely high pressure, The gas molecule's size becomes large relative to the distance between them causing them to have a larger volume than that predicted by the ideal gas law. for example, the ideal gas law assumes that a gas can be compressed to take up a zero volume; this is not possible because gas particles have volume themselves. |
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Deviations of the ideal gas law due to temperature. |
AS temperature goes down, the intermolecular forces causes molecules to attract. the attraction causes the volume to be less than predicted by the Ideal gas law, |
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The closer a gas gets to its boiling point, the less ideally it acts. True or False.f |
True. |
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Van Der Waals Equation of STATE |
it is a correction to the IDEAL GAS LAW EQUATION. Look it up on page 271. |
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The kinetic molecular theory |
summary for the chapter theories. |
