The Gas Laws Flashcards
Liquid
Br2
Gases Moles to Grams
H2 N2 O2 Fl2 Cl2 up
Solid
I2
Ionic Compounds
Solid
Covalent gases
CO CO2 SO4 SO3 PO3
Increase temperature
Increase Energy
Lower Temperature
Decrease Energy
What happens when Volume Increases?
Pressure Decreases
What does P 1 atm equal?
760 mmHg
What is volume in ?
L or ML 1L = 1x10 Negative 3
How do you convert T into K?
T= Degrees C+273 in K
PV/T n=?
P1 V1/ T1 = P2 V2/T2
n= constant not changing
V Increases P Decreases
P1 V1 are inversely proportional
Charles Law
V1/T1 (K) = V2/T2 (K)
Combination gas law
P1 V1/ T1 (K) = P2 V2/ T2 (K)
Boyle’s Law
P1 V1 = P2 V2
V,T directly proportional
PV=?
nRT
n=?
mole
One condition quantity
(Kg, g, left or right mole)
R=?
Ideal gas constant
atm/v
l/v ( change to the proper units before solving x)
Ionic Forces
Ionic Compounds
Covalent Compounds
London Forces
dipole-dipole interaction
H-bonds (FON)
Hydrogen bonds are ?
The strongest dipole dipole (polar)
R=PV/nT=?
0.0821 atmxL/molexK
Dalton’s law of partial pressure
States that the total pressure exerted by a mixture of gases is the sum of the partial pressures of the individual gases.
Partial Pressure
Is the pressure that a gas in a mixture would exert if it were present alone under the same conditions.
