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32 Cards in this Set
- Front
- Back
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Pressure
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-Defined as the force per unit area on a surface
-caused by collisions |
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Pascal
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-defined as the pressure exerted by a force of one newton acting on an area of one square meter
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newton
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the force that will increase the speed of a one kilogram mass by one meter per second each second it's applied
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millimeter of mercury
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-unit of pressure
-symbolized mm Hg |
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barometer
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-device used to measure atmospheric pressure
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atmosphere of pressure
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(atm) defined as being exactly quivalent to 760mm Hg
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ideal gas
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an imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory
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kinetic-molecular theory (4 constants)
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-based on the idea that pa rticles of matter are always in motion
1) gases consist of large #s of tiny particles that are far apart 2) elastic collisions 3) constant, rapid, random motion 4) no forces of attraction or repulision (weak dispersion forces) |
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real gas
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a gas that does not behave completely according to the assumptions of the kinetic-molecular theory
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fluid
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-gas particles glide easily past one another
-liquids and gases that flow |
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elastic collision
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- collisions between gas particles and between particles and container walls are elastic collisions
- no net loss of kinetic energy |
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effusion
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a process by which gas particles under pressure pass through a tiny opening
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ideal gas constant
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R= 0.0821 (L X atm / mol X k)
the constant R |
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diffusion
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spontaneous mixing of the particles of two substances caused by their random motion
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ideal gas law
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PV= nRT
R= 0.0821 L atm/ mol K the mathematical relationship of P,V,T and mols |
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standard molar volume of a gas
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the volume ocupied by one mole of a gas at STP
found to be 22.4 L |
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Avogadro's Law
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states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
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Guy-Lussac's law of combining volumes of gases
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states that at cosntant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers
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Graham's law of effusion
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R1 radical MW2
R2= radical MW1 |
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Boyle's law
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V1P1=V2P2
(n,T) |
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Charle's law
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V1T2=V2T1
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vaporization
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the process by which a liquid or solid changes to a gas
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expansion
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process of diffusion to where a gas fills its container
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mm --> atm
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divide by 760
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C --> K
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+ 273
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standard temperature and pressure
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scientists have agreed on standard conditions of 1 atm pressure and 0 degrees C
STP |
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absolute zero
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- 273. 15 degrees C
given a value of zero on the kelvin scale |
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gas laws
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simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas
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partial pressure
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preesure of each gas in a mixture
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Guy- Lussac's law
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T1-2=T2-1
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Dalton's law of partial pressures
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Pt= p1 + p2 +p3
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combined gas law
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V1P1T2=V2P2T1
(n) |
