Study your flashcards anywhere!

Download the official Cram app for free >

  • Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off
Reading...
Front

How to study your flashcards.

Right/Left arrow keys: Navigate between flashcards.right arrow keyleft arrow key

Up/Down arrow keys: Flip the card between the front and back.down keyup key

H key: Show hint (3rd side).h key

A key: Read text to speech.a key

image

Play button

image

Play button

image

Progress

1/9

Click to flip

9 Cards in this Set

  • Front
  • Back
Charles Law
CONSTANT PRESSURE
as Temp Increase, Volume Increases (DIRECT)

V/T=K

V1/T1=V2/T2
Boyle's Law
(robert Boyle)
CONATANT TEMPERATURE
(INVERSE) PTV

PV=K

P1V1=P2V2
Gay Lussac's Law
CONSTANT VOLUME
Temp Increases, Pressure Increases
(DIRECT)

P/T=K

P1/T1=P2/T2
Combined Gas Laws
PV=K
V/T=K PV/T or P1V1/T1=P2V2/T2
P/T=K


*PTV*
Dalton's Law of Partial
(DUH!)
Total PRESSURE exerted by a mixture of gases = Sum of the partial Pressure of each gas
Ideal Gas Laws
PV=nRT .0821 LxATM/MOLxL

R= constant (.0821)
P= pressure (atm)
V= volume (l) one of everything
n= # of moles no change!
t= temperature (k)
Avogadro's Hypothesis
EQUAL VOLUMES of any gas at the same TEMPERATURE and PRESSURE contain EQUAL # OF MOLES

DIFFERENT MASS...

@stp= 6.02x10 to the 23
Kinetic Molecular Theory of Gases
Ideal gases:*molecules in random straight-line motion *have moleculesthat collide w/no net energy loss *molecules that have no attraction for one another *have molecules with no Volume....
Real Gases act like ideal gases when: high temps, low press, small molecules, PLIGHT, BBUUTT differ or deviate when LT and HP
Graham's Law of Diffusion
MASS Increases, RATE Decreases
If more mass (bigger molecules) move slower than smaller molecules.

r1/r2= m2/m1

m= mass
r= rate