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Thermodynamic Properties Property Table -from direct measurement Equation of State -any equations that relates P,v, and T of a substance Ideal -Gas Equation of State Any relation among the pressure, temperature, and specific volume of a substance is called an equation of state. The simplest and best-known equation of state is the ideal-gas equation of state, given as where R is the gas constant. Caution should be exercised in using this relation since an ideal gas is a fictitious substance. Real gases exhibit ideal-gas behavior at relatively low pressures and high temperatures. Universal Gas Constant Universal gas constant is given on Ru = 8.31434 kJ/kmol-K = 8.31434 kPa-m3/kmol-k = 0.0831434 bar-m3/kmol-K = 82.05 L-atm/kmol-K = 1.9858 Btu/lbmol-R = 1545.35 ft-lbf/lbmol-R = 10.73 psia-ft3/lbmol-R Example Determine the particular gas constant for air and hydrogen. kJ 8.1417 kJ R kmol K u 0.287 Rair M kg kg K 28.97 kmol kJ 8.1417 kJ kmol K 4.124 Rhydrogen kg kg K 2.016 kmol Ideal Gas “Law” is a simple Equation of State PV mRT Pv RT PV NRuT P v RuT, v V/N P1V1 P2V2 T1 T2 Percent error for applying ideal gas equation of state to steam Question …... Under what conditions is it appropriate to apply the ideal gas equation of state? Ideal Gas Law Good approximation for P-v-T behaviors of real gases at low densities (low pressure and high temperature). Air, nitrogen, oxygen, hydrogen, helium, argon, neon, carbon dioxide, …. ( < 1% error). Compressibility Factor The deviation from ideal-gas behavior can be properly accounted for by using the compressibility factor Z, defined as Z represents the volume ratio or compressibility. Ideal Gas Real Gases Z=1 Z > 1 or Z<1 Real Gases Pv = ZRT or Pv = ZRuT, where v is volume per unit mole. Z is known as the compressibility factor. Real gases, Z < 1 or Z > 1. Compressibility factor What is it really doing? It accounts mainly for two things • Molecular structure • Intermolecular attractive forces Principle of corresponding states The compressibility factor Z is approximately the same for all gases at the same reduced temperature and reduced pressure. Z = Z(PR,TR) for all gases Reduced Pressure and Temperature P T PR ; TR Pcr Tcr where: PR and TR are reduced values. Pcr and Tcr are critical properties. Compressibility factor for ten substances (applicable for all gases Table A-3) Where do you find critical-point properties? Table A-7 Mol (kg-Mol) R (J/kg.K) Tcrit (K) Pcrit (MPa) Ar 28,97 287,0 (---) (---) O2 32,00 259,8 154,8 5,08 H2 2,016 4124,2 33,3 1,30 H2 O 18,016 461,5 647,1 22,09 CO2 44,01 188,9 304,2 7,39 Reduced Properties This works great if you are given a gas, a P and a T and asked to find the v. However, if you are given P and v and asked to find T (or T and v and asked to find P), trouble lies ahead. Use pseudo-reduced specific volume. Pseudo-Reduced Specific Volume When either P or T is unknown, Z can be determined from the compressibility chart with the help of the pseudoreduced specific volume, defined as not vcr ! Ideal-Gas Approximation The compressibility chart shows the conditions for which Z = 1 and the gas behaves as an ideal gas: (a) PR < 0.1 and TR > 1 Other Thermodynamic Properties: Isobaric (c. pressure) Coefficient v P 1 v 0 v T P v T P T Other Thermodynamic Properties: Isothermal (c. temp) Coefficient v v P T 1 v 0 v P T T P Other Thermodynamic Properties: We can think of the volume as being a function of pressure and temperature, v = v(P,T). Hence infinitesimal differences in volume are expressed as infinitesimal differences in P and T, using and coefficients v v dv dT dP vdT vdP T P P T If and are constant, we can integrate for v: v Ln T T0 P P0 v0 Other Thermodynamic Properties: Internal Energy, Enthalpy and Entropy u uT, v h hT, P u Pv s su, v Other Thermodynamic Properties: Specific Heat at Const. Volume u v u Cv 0 T v u T v T Other Thermodynamic Properties: Specific Heat at Const. Pressure h P h CP 0 T P h T P T Other Thermodynamic Properties: Ratio of Specific Heat Cp Cv Other Thermodynamic Properties: Temperature v s 1 s T 0 u v 1 T u Ideal Gases: u = u(T) 0 u u du dT dv T v v T Therefore, u du dT C v ( T )dT T v We can start with du and integrate to get the change in u: du C v dT, and u u 2 u1 T2 T1 C v (T) dT Note that Cv does change with temperature and cannot be automatically pulled from the integral. Let’s look at enthalpy for an ideal gas: h = u + Pv where Pv can be replaced by RT because Pv = RT. Therefore, h = u + RT => since u is only a function of T, R is a constant, then h is also only a function of T so h = h(T) Similarly, for a change in enthalpy for ideal gases: C p C p (T ) h 0 P & dh C p dT, and h h2 h1 T2 T1 C p (T)dT Summary: Ideal Gases For ideal gases u, h, Cv, and Cp are functions of temperature alone. For ideal gases, Cv and Cp are written in terms of ordinary differentials as du dh Cv ; Cp dT ideal gas dT ideal gas For an ideal gas, h = u + Pv = u + RT dh du R dT dT Cp = Cv + R kJ kg K Ratio of specific heats is given the symbol, Cp Cv Cp Cp (T) C v (T) (T) R 1 1 Cv Cv Other relations with the ratio of specific heats which can be easily developed: R R Cv and Cp -1 -1 For monatomic gases, 5 3 C p R , Cv R 2 2 and both are constants. Argon, Helium, and Neon For all other gases, Cp is a function of temperature and it may be calculated from equations such as those in Table A-5(c) in the Appendice Cv may be calculated from Cp=Cv+R. Next figure shows the temperature behavior …. specific heats go up with temperature. Specific Heats for Some Gases Cp = Cp(T) a function of temperature Three Ways to Calculate Δu and Δh Δu = u2 - u1 (table) 2 Δu = Δu = Cv,av ΔT 1 C v (T) dT Δh = h2 - h1 (table) 2 Δh = Δh = Cp,av ΔT 1 C p (T) dT Isothermal Process Ideal gas: PV = mRT For ideal gas, PV = mRT We substitute into the integral 2 Wb PdV 1 2 1 mRT dV V Collecting terms and integrating yields: Wb mRT 2 1 V2 dV mRTn V V1 Polytropic Process PVn = C Ideal Gas Adiabatic Process and Reversible Work 1. 2. 3. 4. 5. What is the path for process with expand or contract without heat flux? How P,v and T behavior when Q = 0? To develop an expression to the adiabatic process is necessary employ: Reversible work mode: dW = PdV Adiabatic hypothesis: dQ =0 Ideal Gas Law: Pv=RT Specific Heat Relationships First Law Thermodynamics: dQ-dW=dU Ideal Gas Adiabatic Process and Reversible Work (cont) First Law: Using P = MRT/V dQ dW 0 PdV dU MC vdT CV dT dV R T V 1 1 Integrating from (1) to (2) T2 V2 T1 V1 1 Ideal Gas Adiabatic Process and Reversible Work (cont) Using the gas law : Pv=RT, other relationship amid T, V and P are T2 V1 T1 V2 P2 V1 P1 V2 developed accordingly: T2 P2 T1 P1 1 1 Ideal Gas Adiabatic Process and Reversible Work (cont) An expression for work is developed using PV = constant. i and f represent the initial and final states W PdV PV i dV V PV i 1 1 V V W 1 f PV f PV i 1 i Ideal Gas Adiabatic Process and Reversible Work (cont) The path representation are lines where Pv = constant. For most of the gases, 1.4 The adiabatic lines are always at the righ of the isothermal lines. The former is Pv = constant (the exponent is unity) P f f i v Polytropic Process A frequently encountered process for gases is the polytropic process: PVn = c = constant Since this expression relates P & V, we can calculate the work for this path. Wb V2 V1 PdV Polytropic Process Process Constant pressure Constant volume Isothermal & ideal gas Adiabatic & ideal gas Exponent n 0 1 k=Cp/Cv Boundary work for a gas which obeys the polytropic equation Wb 2 1 PdV c v2 2 1 dV n V 1 n 1 n V V2 V1 c 1 n 1-n v1 1-n n 1 We can simplify it further n The constant c = P1V1 = n 2 P 2 V (V Wb n P2V2 ) P1V 1n V 11 n 1-n 1 n 2 P2V2 P1V1 , 1 n n 1 Polytropic Process Wb 2 1 PdV 2 1 c dV n V P2V2 P1V1 , n 1 1 n V 2 , n 1 PVn V1