35 terms

# Gas Laws

###### PLAY
decreases
When pressure increases, volume _____.
increases
When temperature increases, pressure _____.
increases
When temperature increases, volume _____.
unit of pressure
mm Hg
unit of pressure
atm
unit of pressure
psi
unit of temperature
Kelvin
unit of temperature
Celsius
unit of volume
liter
unit of volume
milliliter
Ideal Gas Law
PV = nRT
pressure
P
volume
V
number of moles
n
gas constant
R
temperature
T
1) Particles do not take up space.
2) Particles bounce off of each other without losing energy.
3) Particles are not attracted to one another. (no intermolecular forces)
3 Rules for ideal gases (vs real gases)
Combined Gas Law
P₁V₁ / T₁ = P₂V₂ / T₂
1) Particles are small and inert.
2) Temperature is high.
3) Pressure is low.
3 Conditions when real gases act almost exactly like ideal gases.
1) Temperature must be in kelvins
2) Units for P1 must match P2 (and units for V1 must match V2)
2 Rules for units on the combined gas law (P₁V₁ / T₁ = P₂V₂ / T₂)
Graham's Law
Rate₁/Rate₂ = sq rt(M₂)/sq rt (M₁)
1) The right side of the equation flips so that 2 is over 1.
2) Rate = amount/time
2 Rules for on Graham's Law
Rate₁/Rate₂ = sq rt(M₂)/sq rt (M₁)
(all units must match the gas constant R)
1) Temperature must be in kelvins.
2) Pressure must be in atm.
3) Volume must be in L.
3 Rules for units on Ideal gas law
(PV = nRT)
Mass can be used to find n (or conversely, n can be used to find mass) by converting between moles and grams.
Mass in the ideal gas law
(PV = nRT)
effusion
the process that occurs when a gas escapes through a tiny hole in its container
rate (described in terms of time)
= 1/time (inverse)
rate (described in terms of amount)
= amount
specific heat formula
q = mc delta T
specific heat (variable)
c