njit-etd1961-002 - New Jersey Institute of Technology

Al [ (¹ - Tr1)- 1.-2 = T1 - TTr2)0.38Equation (8)(J) The enthalpy of the saturated vapor, H sv , at¹ atm. and -¹9 ° C. was determined by adding thelatent heat of vaporization to the enthalpy ofthe saturated liquid.(K) The molal enthalpy of the ideal gas at -¹9°C.was obtained by adding to Hsv the enthalpy correctioncorresponding to -¹9 ° C. and ¹ atm. Thus,H*3 = HSV + (H* 3 - HSV)(L) The values of ideal enthalpy from -¹0 to 400 ° C.were obtained by adding T1to H*3 the value 2 Cp*dTj Twhere Cp* is the molel heat capacity for ideal-gasbehavior as a function of temperature, and is givenby Walker ¹6 as (9.48 -F 0.009¹4T - 6.4 x ¹0 -7 T 2 )calorie per gram mole per degree Kelvin.(M) The enthalpies of the saturated vapor from -¹0 ° C.to the critical point were evaluated by correctingtheir enthalpy departures from ideal gas usingTable 47 of Watson and et al. ³ .(N) The values of enthalpy in the superheated regionfrom -¹0 ° C. to 400°C. and from ² to ¹50 atmosphereswere determined by subtracting from the values ofideal enthalpy the values of enthalpy deviationsfrom ideality obtained from Table 50 of Watson andet al. 5 .(0) The enthalpies of the saturated liquid from-¹0 °C. to the critical point were obtained directlyby subtracting the latent heat of vaporizationcalculated in (1) from the values of the saturatedvapor enthalpy.5