1. ∆H = H final - H initial The stoichiometric coefficients in thermochemical equations must be interpreted as numbers of moles. 1 mol of C 5 H 12 reacts with 8 mol of O 2 to produce 5 mol of CO 2, 6 mol of H 2 O, and releasing 3523 kJ is referred to as one mole of reactions. ∆H o rxn =  ∆H f o (prod) -  ∆H f o (react) Specific heat capacity (J/(g∙K)= heat lost or gained by system (Joules) mass(grams)  T (Kelvins) m  T f –T i ) q c P = VariableSystem 1System 2 CpCp TfTf TiTi m q

2. heat transfer out (exothermic), -q heat transfer in (endothermic), +q SYSTEM ∆E = q + w w transfer in (+w) w transfer out (-w)

3. Heat Energy Internal energy Kinetic Energy Potential Energy Endothermic Exothermic Thermodynamics Thermal Equilibrium System Surroundings Law of Conservation of Energy Heat Capacity Specific Heat Capacity First Law of Thermodynamics Melting Freezing Deposition Sublimation Evaporation Condensation State Function Standard state temperature Standard state pressure Standard states matter Enthalpy Hess’s Law Thermochemical Equation Enthalpy of Formation Intramolecular forces Intermolecular forces Hydrogen Bonding Polarization Polarizability Vapor Pressure Equilibrium Heat of Vaporization Phase Diagram Solid Liquid Gas Triple Point Critical Point Super Critical Fluid