equation sheet - exam 3

# equation sheet - exam 3 - ∆G = ∆H – T∆S Old stuff...

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

CEM 141 Exam 3 Lectures 20-33 Equations, not guaranteed to be complete! Drawing lewis structures, resonance, multiple bonds, bond orders Formal Charge VSEPR theory Valence bond theory, hybridization The stuff lecture 24 says about molecular orbital theory Gas laws Avogadro: V/n=V’/n’ Boyle: P 1 V 1 = P 2 V 2 Charels: V’/T’ = V/T Dalton law of partial pressures: P = sum of all partial pressures PV=nRT, for ideal gases Know how to generate temperature conversion function (know how to derive, not only use, for example, C to F conversion) In terms of density: density = m/v=PM/RT where M is a molar mass X i = n i / n Total (x is mole fraction, n is moles) Thermodynamics 2 nd law: for any spontaneous process, the entropy of the universe must increase
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: ∆G = ∆H – T∆S Old stuff: ∆ E = q + w W = -P∆V sign conventions At equilibrium: ∆G = 0 Therefore, ∆H = T∆S Trouton’s rule: 85 J/mol K = ∆S v = ∆H V /T B Solutions Molarity, M = moles/liter Molality, m = moles solute / kg solvent – temperature independent Mass percent: mass solute/total mass of solution * 100 Mole fraction: moles solute / total number of moles PPM: parts per million, mg solute/kg of solution = mg solute / volume in L (true for density = 1.00) Raoult’s law: P Total = X solvent P O solvent Van’t Hoff Equation: ∆T = k*m*I … k=solvent dependent constant, m is molality, i is the van’t hoff factor...
View Full Document

## This note was uploaded on 03/19/2008 for the course CEM 141 taught by Professor Hunter during the Fall '08 term at Michigan State University.

Ask a homework question - tutors are online