Chem final - Constants and Equations M1V1 = M2V2 6.022 X...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Constants and Equations M1V1 = M2V2 6.022 X 10^23 – Avo’s # Charles Law T1V2 = T2V1 Boyle’s Law P1V1 = P2V2 K = 273 + C PV = nRT R = .08206 Latm / kmol d = P(MW) / RT Dalton’s Law P total = Pa +Pb + Pc + … Grahams Law Ua / Ub = √ (MWb / MWa) Heat evolved = (heat cap)(mass sol’n)(change in temp) Heat evolved = heat absorbed ΔH = nΣΔ Hf (products) - nΣΔ Hf (reactants) Wavelength X frequency = C (speed of light) C = 3.0 X 10^8 E = h X frequency E = HC / wavelengh H = planks constant 6.626 X 10^ -34 E = -2.178 X 10^-18 ( (1/n final^2) – (1/n initial^2) ) Formal charge = group # - ½ shared electrons – unshared electrons Molarity = moles solute / Liter soln Weight % = mass solute / mass solute + mass solvent Mole Fraction = moles solute / total moles Molality = moles solute / kg of solvent Raoult’s Law Psoln = X solvent ( P solvent) ; x = mole fraction ; P solvent = pres. of pure solvent ΔT = Kf (m) ; m = moles Ln ( N / No) = -kt T ½ = .693 / k K = A e ^ -Ea / RT
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 05/03/2008 for the course CHEM 103 taught by Professor Thompson during the Fall '05 term at William & Mary.

Ask a homework question - tutors are online