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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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