Download Metric conversion chart - Welcome to Chemistry At Central High

Advanced Chemistry useful handout #1
Metric conversion chart
109 g =
106 g =
1 Gg
giga
1 Mg
mega
103 g =
1 kg
kilo
1g
101 dg
BASE
deci
1 g = 10 dg
102 cg
103 mg
centi
1 g = 100 cg
milli
1 g = 1000 mg
micro
1g=
106 µg
109 ng
1g=
1012 pg
pico
1g=
1g=
1g=
1g=
1g=
1000 g = 1 kg
Additional conversion factors and constants:
Energy:
4.18 Joules = 1 calorie
1 Joule = 1 kg m2
sec2
Volume: 1 cm3 = 1 mL
1 dm3 = 1 L
1 m3 = 103 L
Density = __Mass___:
Volume
1 gram (water only)
mL
Avogadro’s number: N = 6.02 x 1023 particles
1 mole
nano
Kelvin = °Celsius + 273
1010 Å (Angstroms) = 1 meter (atomic size)
1 atm = 760 mm Hg
Linear to Volume: When converting between linear and volume measurements, you need to cube the
conversion factor! 10 cm = 1 dm : so (10 cm)3 = (1 dm)3 thus 1000 cm3 = 1 dm3 = 1 Liter
Some Helpful Formulas:
Gas Laws: Conversions: STP for gases = 0°C and 1 atm ; (or 273 K , 760 mm Hg)
Combined : P1 V1 = P2 V2
gas law
T1
T2
Ideal Gas Law: PV = nRT
Diffusion: rate A = √FW B
rate B √FW A
Molar volume of = 22.4 L
a gas at STP
mole
If you know P, V, T of a gas, you can calculate moles!
For PV = nRT: P in atm, V in L, n = moles, T in K, Ideal Gas Constant, R = 0.0821 L atm/mol K
(use Partial Pressure of a gas in PV = nRT to get mol of that particular gas)
Dalton’s law of Partial Pressures: Ptotal = Pa+ Pb + Pc + ....
Partial pressure = Pa = Xa Ptotal
where mol fraction= Xa =
Solutions: Molarity = moles solute or
L of solution
M = mol
L
Dilutions: V1M1 = V2M2 (can use mL for Volumes)
mol a
Total mol of gases
mol = V M
Or : can use millimoles and milliliters: M = mmol
mL
molality = m = mol solute
kg solvent
Pdry gas = Ptotal – Pwater vapor
V = mol (V must be in Liters)
M
mmol = mL M
mL = mmol
M
Acid Base Titration: VaMa(#H) = Vb Mb (#OH)
mol fraction= Xa =
mol a
total mol
Weight % =
g solute
100 g solution
More Helpful Formulas:
Solutions: More formulas
C gas = k Pgas : Solubility of a gas (Cgas) in a solution is proportional to the Partial Pressure of the gas
Colligative properties:
∆PA = XB PA° : V.P. decrease (∆PA) of a solvent = mol fraction of solute x V.P. of pure solvent (P A°)
Osmotic Pressure = π = MRT
Solution Freezing, Boiling pt. changes: ∆Tf = Kf m
∆Tb = Kb m
(For Water:Kf = 1.86°C/m, Kb = 0.52°C/m)
Heat and Thermochemistry: q = m Cp ∆T; Cp (in J/g°C) = 4.18 water, 2.09 ice, 1.84 steam
q = m ∆Hvap (boiling) ; ∆Hvap = 2257 J/g
q = m ∆Hfus (freezing) ; ∆Hfus = 334 J/g
(for water)
∆H°reaction = ∆Hf° (prod) – ∆Hf° (react)
Atoms Speed of light, c= 3.00 x 108 m/sec
Atomic Mass Unit: 1 amu = 1.66054 x 10–27 kg
Atomic scale energy unit (Million electron volt): 1 MeV = 1.60218 x 10–13 joules
mass of a proton = 1.00727650 amu,
neutron = 1.00866492 amu,
electron = 0.0005486 amu
Matter & Energy equivalence: E = m c2 ; (“large” units: use Joules, kg and m/sec)
1 amu = 931.494 MeV of energy (For atomic scale units)
Radioactive decay: ln N0 – ln Nt = 0.693 t
half-life;
Electrons: Planck’s constant, h= 6.63 x 10–34 J sec
c = λν
Energy of a photon: E = hν or E = h c
Wavelength of moving matter
(v = velocity)
λ
Bohr atom: E = hν = 2.18 x 10–18 J ( _ 1_ – _ 1_ )
ni2
n f2
λ = wavelength, ν = frequency
λ= h
mv
Energy of an electron transition in a
Hydrogen atom, ni, nf = initial and final
energy levels of the electron
Bonding: estimated ∆H reaction = Bond energy of bonds broken – bonds made
Bond order = 1/2 (# bonding electrons – # anti bonding electrons)
diamagnetic= all electrons paired; paramagnetic = has unpaired electrons