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UNIT 10 gases - Coggle Diagram
UNIT 10 gases
Together (mixtures:)
Basically all partial moles and partial pressures will add up to total amount and pressure of the mixture.
But remember that a given volume of gas will always expand to fit its container, so you have to use proportionality equations to find out new values for pressure/stuff.
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OVER WATER: must account for vapor pressure at equilibrium of water; must adjust container so water level is same outside/inside so Patm = Ptotal = Pgas + PH20
HOW do gases behave:
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Molar mass eq: PM = dRT (d = density of gas) (to get here from ideal gas law, divided by n and V, then multiplied by mass.)
Characteristics defined:
Pressure: P = F/A. Basically net force against a given area (the container walls.) ATM pressure is just air's pressure pushing on everything.
Temperature: proportional to average kinetic energy (will have different energies, but average stays.)
Volume: size of container (gas will always fill this; volume of gas = volume of container.. remember when doing partials)
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MISC
STP = 760 torr/1 atm, @ 0 C (273 K). Gases occupy 22.4L per mole here.
R = .0821 (atm), 62.4 (torr)
FORMULAS WERE DERIVED IN KELVINS, SO ALWAYS CONVERT TO KELVINS (ABSOLUTE TEMPERATURE.) OR ELSE WON'T WORK (R is a kelvin unit).. proportionality only works with an absolute measurement (from 0.)
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I MISSED:
CONVERT TO CORRECT TEMP UNIT (K for calculations, C if needed).
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Effusion/Diffusion:
1/2mv^2 states that at at given kin. nrg, lighter molecules move faster to compensate for mass. Faster = faster effusion AND diffusion (hitting and spreading.)