Document KR6weVDMgaj6YxDRme4ewZmOw

HEATING VENTILATINC AIR CONDITIONING GUIDE 1944 Table 4. Specific Enthalpy of Dry Air at 29.921 In. Hg . Temp F t Specific Enthalpy Btu per Lb ha Specific Heat Klo -96 -23.035 0.2399 -64 -15.356 0.2399 -320 -70.6.07080 0.2399 0.2400 Temp F t Specific Enthalpy Btu per Lb ha Specific Heat i. Temp F Mt Specific Enthalpy Btu per Lb ha Specific Heat K]1 32 7.680 0.2400 160 38.454 0.2403 64 15.363 0.2400 192 46.172 0.2405 96 23.053 0.2401 224 53.903 0.2406 128 30.749 0.2402 256 61.649 0.2408 Prepared by John A. Goff.' ture. In other words, the pressure effect may be much more important than the corresponding effect on specific volume. Values of the specific enthalpy of dry air at standard atmospheric pressure (29.921 in. Hg) as computed from Equation 6 are given in Table 4. Reference Point. It is desired to give some prominence to the choice of reference point. As energy, and therefore enthalpy, is purely relative, any convenient state can be selected at which to assign the value zero to specific enthalpy. The state chosen is 0 F, 29.921 in. Hg. Perhaps the only really valid argument for this particular choice is that, for ordinary calculations at, or near, atmospheric pressure, a- very simple equation can be used, namely, fta = 0.241 (7) WATER VAPOR Saturation Pressure. It is common knowledge that a substance like water can exist in at least three distinct phases, solid (ordinary ice), liquid and vapor; and that under certain conditions two or more phases can co-exist in stable equilibrium. For example, steam having a quality of 98 per cent is a mixture of two co-existing phases, vapor and liquid, 98 per cent by weight being vapor and 2 per cent by weight, liquid. When two phases call co-exist in stable equilibrium, each is said to be saturated with respect to the other. One of the important problems of thermodynamics is to formulate the conditions for saturation in mathematical terms. The answer to the problem can be. stated quite generally as equality, between the several ' co-existing phases, of (a) pressure, (b) temperature, (c) each component chemical potential. In the case of a-pure substance like water, containing a single com ponent, there is only one component chemical potential; and this becomes identical with a thermodynamic property called specific free enthalpy denoted by the letter g (Btu per pound) and defined by the equation: g = h -- Ts where A = specific enthalpy, Btu per pound. T = absolute temperature, degrees Fahrenheit, r = specific entropy, Btu per pound per degree Fahrenheit. '. To illustrate, liquid water at 212 F, 14.696 lb per square inch has a 1 specific free enthalpy of 180.07 -- 671.70 X 0.3120 = --25.90 Btu per . pound. At the same temperature-and pressure, water vapor has a specific 6 CHAPTER 1. THERMODYNAMICS OF AIR AND WATER MIXTURE free enthalpy of 1150.4 -- 671.70 X 1.7566 = --25.90 Btu per pound. The numerical data used in these calculations are to be found in the steam tables2. Since the two specific free enthalpies are equal at the same temperature and the same pressure, the two phases can co-exist in stable equilibrium to form a saturated mixture and are therefore saturated with respect to each other. But suppose that a different pressure had been assumed, the tempera ture being 212 F as before; for example, assume a pressure of 14 lb per square inch. The specific free enthalpy of the liquid phase will be practically the. same as before, but that of the vapor phase will change from --25.90 to --32.84 Btu per pound, most of this change being due .to change of entropy which, in the case of a vapor, depends markedly upon the pressure. Since the specific free enthalpies of the two phases are no longer equal, they cannot co-exist in stable equilibrium and neither is saturated. As a matter of fact the vapor is superheated while the liquid is supersaturated. From this analysis it will be seen that to a given temperature T there corresponds a definite saturation pressure ps. This is also called the vapor pressure of the liquid or solid as the case may be. It will also be seen that a working definition of saturation can only be arrived at by application of the fundamental laws of thermodynamics. Referring specifically to the vapor phase, if the actual pressure is less than the saturation pressure corresponding to the actual temperature, the vapor is said to be superheated; if it is greater, as it may well be under proper circumstances, the vapor is said to he supersaturated. Values of the saturation pressure of pure water are given in Table 6s. Specific Volume Accurate values of the specific volume of water vapor at pressures equal or near the saturation pressure (for the given temperature) can be' computed from Equation 1 since the second virial coefficient A(T) is known with satisfactory accuracy. Usually, however, the desired infor mation can be read directly from the steam tables. Values for the specific volume of the saturated vapor, t>g, are also listed in Table 8. Specific Enthalpy ^ The zero-pressure specific enthalpy, as calculated by A. R. Gordon from spectroscopic measurements, has. recently been corrected for dis tortion of the water molecules due to centrifugal forces. Best values at present available are listed in Table 5. From the numerical values of mean specific heat, it is clear that for ordinary calculations the following simple relation may be.used: j., = 0.4441 + 1061 (8) Reference Point. The reference point for water has been chosen as saturated liquid at 32 F in conformity with usual steam table practice. In order to refer the zero-pressure values of specific enthalpy to this Thermodynamic Properties of Steam, by J. H. Keenan and F. G. Keyes, published by John Wiley &, Sons, Inc., 1936. of which Table 8 is an abridgment. Strictly speaking the values listed in Table 6 are not values of Pt as labeled, but of p (Equation 13b) with the Dalton Factor (DF) taken to be unity. 7