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18 Cards in this Set
- Front
- Back
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assumptions of kienetic molecular theory of gases
(ideal gas) |
1. particles with negligible volume
2. no intermolecular attractions or repulsions 3. continuous, random motion (gas molecule collide with each other and wall of their container in a random continuous motion) 4. elastic collisions, conservation of kinetic energy (nogain or loss of energy) 5. avg kinetic energy of gas particles proportional to the absolute temp |
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at high T and low P real gas is like???
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ideal gas
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ideal gas equation
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PV=nRT
P = 1atm = 760mmHg =760 torr V = in L or mL T= T(K)=T(C)+273.15 |
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STP
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273.15K(0 C) and 1atm
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volume of 1 mole of any gas at STP
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22.4 L
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density
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g/L
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molar mass
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g/mol
(divide weight by volume then multiply by 22.4L/mol) |
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Boyle's law
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constant temp (isothermal condition)
P1V1=P2V2 |
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isothermal condition
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constant temp
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Dalton's law of partial pressure
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when two or more ideal gases are in one vessle withon chem interacton
Pt=Pa+Pb+Pc... |
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Mole fraction
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the mole fraction of gas A
Xa = number of moles of a /total number of moles of gases |
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partial pressure
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Ppartial of a = Ptotal Xa
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charles's law
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constant pressure
V1/T1 = V2/T2 |
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Avagadro's principle
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for all gases at constant T,P
n1/v1 = n2/v2 thus all gases have the same number of moles in the same volume. |
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effusion
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the flow of gas particles under pressure from one compartment to another through small opening
gives ration of the rates of two process how fast either occurs and relate to gas's molar masses. r1/r2 = SQR M2/M1 r = rate of effusion M = density |
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heavier the gas
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slow it to diffuse or effuse
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diffusion
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how quickly gas travel in open air( how gas expends)
more massive slow it moves and thus diffuse and effuse slowly) diffusion equation is same as effusion |
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maxwell-boltzmann distribution curve
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shows the distribution of speeds of all the gas particle in a sample at a gien temperature
bell curve flattening means at T inc, gas travel greate range speed thus small porporton of the movlecule will move at exactly the new average speed |
