Review: ΔE = q + w- primarily interested in chemistry with thermal energy transfer (heat) which can be easily measured, so. ... ΔE = q v (const v = no w) ΔH = ΔE + PΔV = q p (const p)- so if little PΔV, then ΔH ≈ ΔE- at const p, ΔH = q p (defined path) which is measurable- at const v, ΔE = q v (defined path) which is measurable (≈ ΔH) ΔH = 1) H final- H initial 2) H state2 – H state1 3) H products- H reactants 4) q p (defined path and measurable) ΔH = Change in Enthalpy ΔH – relative change, not absolute H Enthalpy (or “Heat”) of Fusion ΔH fusion (solid-liquid) Enthalpy (or “Heat”) of Vaporization ΔH vap (gas-liquid) Enthalpy (or “Heat”) of Sublimation ΔH subl (solid-gas) Enthalpy (or “Heat”) of Formation ΔH f º Enthalpy (or “Heat”) of Reaction ΔH rxn Enthalpy (or “Heat”) of Combustion ΔH
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This note was uploaded on 01/30/2011 for the course CHEM 2035 taught by Professor Brown during the Spring '10 term at University of Florida.