• 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

Card Range To Study

through

image

Play button

image

Play button

image

Progress

1/43

Click to flip

Use LEFT and RIGHT arrow keys to navigate between flashcards;

Use UP and DOWN arrow keys to flip the card;

H to show hint;

A reads text to speech;

43 Cards in this Set

  • Front
  • Back
Gases are one of...
the four phases of matter
what are the four phases of matter?
solid
liquid
gas
plasma
All gases are:
homogeneous
homogeneous:
mixed uniformly(same throughout)
compressible:
apply pressure to their container, their volume will change
pressure:
the force exerted over a certain area by the gas against the walls of the container
1atm= ____mmHg
760mmHg
1atm= 760mmHg= ____KPa
101.325 KPa
Ideal Gases are gases whose...
behavior exactly matches these relationships or gas laws in reality, ideal gases don't exist
Boyle's Law: at constant temperature the _____ of gas is ________ to pressure
volume, inversely proportional
equation for Boyle's Law
V(proportional to) (1/P) or

P*V=constant
Charle's Law: at constant pressure the _____ of gas varies _______________.
volume, directly with temperature
equation for Charle's Law
V(proportional to)T

as T increases V increases
Avogadro's Law: At fixed temperature and pressure the _____ of gas varies _________________.
volume, directly with the molar quantity
equation for Avogadro's law
V (proportional to) n

as n increases, V increases
Ideal Gas Law
PV=nRT
P=
pressure
V=
volume
n=
number of moles
R=
gas constant (.08206)
T=
temperature
Ideal gas law can be used to __________ if ___, ____, and ___ are known.
calculate the # of moles(n), P, V, T
Partial Pressure:
the pressure of one individual gaseous component of gaseous mixture
Dalton's Law of partial pressure
the total pressure of a system is equal to the sum of the individual gas pressures.
what is the pressure of each gas in our atmosphere?
Ptotal= Patm= PN2 + PO2 + PAr + PCO2 + .....

78% N2 * 1.0 atm = .78 atm N2
21% O2 * 1.0 atm = .21 atm O2
----------------
sum=1atm
if 2.00g of N2 gas has a volume of .40L and a pressure of 6.0 atm, what is its Kelvin temperature?
PV/nR=T

6.0*.40/.0714*.08206 = 409K
Used to express the __________ of gases in a _______(x)
individual concentration, mixture
X= mols of componentA/total mols of mixture(x)
nA/nA+nB+nC...
what would you get if you multiplied the mole fraction by 100?
you would get the percent mol concentration
Kinetic Molecular Theory of Gases
a theory that explains why gases behave like they do
1. Gases are made of _______moving at _______.
tiny particles, random
2. The volume of the ______ themselves is ______ in comparison to the total volume.
particles, small
3. Gas particles act ______ of each other.
independently
4. Collisions of the gas particles with _____ and the ____ of the _____ are ______.
each other, walls, container, elastic
5. The average Ek of the particles is ________ to ______ in ____.
proportional, temp, K
Kinetic energy
KE=(1/2)mV^2
Diffusion:
the mixing of gas molecules by random motion
Effusion:
the escape of gas molecules through a pinhole into a vacuum
Graham's Law:
the rate of effusion is inverselly proportional to the square root in its mass.
rate (proportional to) 1/ square root of mass
Graham's Law
Kinetic Molecular theory assumes small particle size
for real gases at high pressure
Kinetic Molecular theory assume no attractive forces between gas particles
this is not true at high pressure
Van der Waals Equation:
[P+(an^2/V^2)]*(V-nb)=nRT