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Farenheit (F)
59(°C+32)
Celsius (C)
95(°F−32)
Kelvin (K)
°C+273
Density (d)
Vm
1 amu =
1.66054×11−24g
Atomic weight
Σ [(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
6.02×1023 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)
Vn
Dilution (before and after)
M1V1=M2V2 or McVc=MdVd
(c = concentrated, d = diluted)
If ΔE>0
Endothermic
If ΔE<0
Exothermic
Change in internal energy (ΔE)
Ef−E0
Exchange of energy betweem system and surroundings
ΔE=q+ω
q = heat
w = work
Work
PV or −PV
P = pressure
V = volume
Enthalpy (H)
E+PV
Change in enthalpy (ΔH)
ΔE+PΔV
Enthalpy of reaction
ΔHrxn=Hproducts+Hreactants
Calorimetry
q=mcΔT
Specific heat for H2O
4.184 J/g°C
Hess’s law
ΔH=∑products−∑reactants
Bond enthalpy
Σ bonds broken - Σ bonds formed
Speed of light (constant)
c=3.00×108m/s
Speed of light (formula)
c=λv
λ = wavelength
v = frequency
Energy is proportional to frequency
E=hv
h = plank’s constant
v = frequency
Plank’s constant (h)
6.626×10−34J⋅s
Dipole moment (μ)
Qr
Q = charge
r = distance
Charge (Q)
1.60×10−19C
C = Coulomb
1 D =
3.335×10−30C⋅m
1 A =
10−10m
Formal charge
v.e. - lines - dots
6
octrahedral
Bond order
21 (bonding e - antibonding e)
Pressure (P)
AF
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
P1V1=P2V2
Charles’s law
T1V1=T2V2
Gay-Lussac’s law
T1P1=T2P2
Combined gas law
T1P1V1=T2P2V2
Avogadro’s law
n1V1=n2V2
STP 2
V = 22.4 L
T = 0°C = 273 K
P = 1 atm
Ideal gas law
PV=nRT
R constant
0.08206 mol⋅KL⋅atm
n
moles
M
molar mass
m
mass
Density of gases
d=RTMP
Dalton’s law of partial pressures
Pt=P1+P2+P3
Mole fraction
X1=ntn1
n1 = moles of compound (part)
nt = total mass (whole)
Pressure and mole fraction
Pt=X2Pt
X = mole fraction
Urms and molecular mass
urms=M3RT
R = 8.314 J/mol·K
R = 8.314 kg·m2/ s2·mol·K
Graham’s law describes diffusion and effusion
r2r1=M1M2