2012 Study-Guide-2

# Note t 0 for ideal gases du cv dt always true for any

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Unformatted text preview: aw formulations (ΔSuniv > 0 or ΔS + ΔSSurr > 0 for a spontaneous process under any conditions). Understand the third law. Know how to use the thermodynamic tables with values of standard enthalpy of formation, standard molar entropy and standard molar heat capacity. 1 Fundamental Equations You NEED to know from test #2: dU = δw + δq (First Law, ALWAYS TRUE) δw = - pext dV (Expansion, Compression Work, ALWAYS TRUE) dU = CV dT + πT dV (ALWAYS TRUE. Note πT = 0 for ideal gases) dU = CV dT (ALWAYS TRUE for any process on ideal gases or for isochoric processes on any materials). H = U + pV (definition of Enthalpy, ALWAYS TRUE) dH = CP dT + µT dP (ALWAYS TRUE. Note µT = 0 for ideal gases) dH = CP dT (ALWAYS TRUE for any process on ideal gases or for isobaric processes on any materials). CP - CV = nR (TRUE FOR IDEAL GASES ONLY) CVm = (3/2) R (TRUE FOR MONOATOMIC GASES) pext = p (TRUE FOR REVERSIBLE PROCESSES + PROCESSES AT CONSTANT P) δq = 0 (TRUE FOR ALL ADIABATIC PROCESSES dU = δqV (TRUE FOR ANY CONSTANT VOLUME (ISOCHORIC) PROCESS dH =...
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## This note was uploaded on 01/26/2014 for the course CHEM 3615 taught by Professor Aresker during the Spring '07 term at Virginia Tech.

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