2012 Study-Guide-1(1)

# Heat capacity at constant volume enthalpy h u pv heat

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Unformatted text preview: e or not. Heat capacity at constant volume Enthalpy H = U + PV Heat capacity at constant pressure Comparison of ΔH with ΔU 2) Fundamental Equations You NEED to Know to Obtain all other Equations: dU = δw + δq (First Law, ALWAYS TRUE) δw = - Pext dV (Expansion, Compression Work, ALWAYS TRUE) dU = CV dT (ALWAYS TRUE for any process on ideal gases or for any isochoric process). U and H are only a function of T for ideal gases. H = U + PV (definition of Enthalpy, ALWAYS TRUE) dH = CP dT (ALWAYS TRUE for any process on ideal gases or for any isobaric process). 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 ADIABATIC PROCESSES dU = δqV (TRUE FOR ANY CONSTANT VOLUME (ISOCHORIC) PROCESS dH = δqP (TRUE FOR ANY CONSTANT PRESSURE (ISOBARIC) PROCESS PV = nRT (TRUE FOR IDEAL/PERFECT GASES ONLY) (P + a/Vm2)(Vm - b) = RT (TRUE FOR VAN DER WAALS GASES ONLY) Z = PVm / RT (DEFINITION OF COMPRESSION FACTOR) Z = 1 + B’(T)...
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