Fahrenheit (F)
Celsius (C)
Kelvin (K)
Density (d)
1 amu =
Atomic weight
[(mass)(% fractional abundance)]
Percentage to decimal
Divide by 100
Percent composition
% element =
[(# of atoms)(molecular weight)/ molar mass of the compound] x 100
Avogadro’s number
atoms or molecules
Percent yield
(actual yield/theoretical yield) x 100
Empirical to molecular formula
given mass of molecular formula/ molar mass of empirical formula = multiplier
Molarity (M)
Dilution (before and after)
or
(c = concentrated, d = diluted)
If \Delta E >0
Endothermic
If \Delta E <0
Exothermic
Change in internal energy ()
Exchange of energy betweem system and surroundings
q = heat
w = work
Work
or
P = pressure
V = volume
Enthalpy (H)
Change in enthalpy ()
Enthalpy of reaction
Calorimetry
Specific heat for H2O
Hess’s law
Bond enthalpy
bonds broken - bonds formed
Speed of light (constant)
Speed of light (formula)
= wavelength
= frequency
Energy is proportional to frequency
= plank’s constant
= frequency
Plank’s constant ()
Dipole moment ()
= charge
= distance
Charge ()
= Coulomb
1 D =
1 A =
Formal charge
v.e. - lines - dots
6
octrahedral
Bond order
(bonding e - antibonding e)
Pressure (P)
Pascals
1 Pa = 1 N/m²
Bar
1 bar = 105
Pa =
100 kPa
Atmosphere
1 atm = 760 torr = 760 mmHg
Hg =
101.325 kPa = 1.10325 bar
STP 1
1 atm
760 torr (mmHg)
101.325 kPa
Boyle’s law
Charles’s law
Gay-Lussac’s law
Combined gas law
Avogadro’s law
STP 2
V = 22.4 L
T = 0°C = 273 K
P = 1 atm
Ideal gas law
R constant
n
moles
M
molar mass
m
mass
Density of gases
Dalton’s law of partial pressures
Mole fraction
= moles of compound (part)
= total mass (whole)
Pressure and mole fraction
X = mole fraction
Urms and molecular mass
R = 8.314 J/mol·K
R = 8.314 kg·m2/ s2·mol·K
Graham’s law describes diffusion and effusion