Main Advanced Chemistry Formulas Cheat Sheet For Assignments

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 1g= 1g= 1g= 1g= 102 cg 103 mg Energy: 4.18 Joules = 1 calorie 1000 g = 1 kg deci 1 g = 10 dg centi 1 g = 100 cg milli 1 g = 1000 mg micro 1g= 106 µg 109 ng 1g= 1012 pg pico 1g= Additional conversion factors and constants: 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 solute kg solvent mol a Total mol of gases mol = V M Or : can use millimoles and milliliters: M = mmol mL molality = m = 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