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Vapor-pressure curve

In practice, however, it is recommended to adjust the coefficient m, in order to obtain either the experimental vapor pressure curve or the normal boiling point. The function f T ) proposed by Soave can be improved if accurate experimental values for vapor pressure are available or if it is desired that the Soave equation produce values estimated by another correlation. [Pg.156]

There are significant differences in various data sets pubtished for oleum vapor pressure. A review of existing vapor pressure data plus additional data from 10 to 8600 kPa (1.45 to 1247 psi) over the entire concentration range of oleum is available (93), including equations for vapor pressure versus temperature. Vapor pressure curves for oleum calculated from these equations are shown in Figure 19. Additional vapor pressure data from 0.06 to 14 kPa (0.5—110 torr) is given in the titerature (92). [Pg.182]

The Class I binary diagram is the simplest case (see Fig. 6a). The P—T diagram consists of a vapor—pressure curve (soHd line) for each pure component, ending at the pure component critical point. The loci of critical points for the binary mixtures (shown by the dashed curve) are continuous from the critical point of component one, C , to the critical point of component two,Cp . Additional binary mixtures that exhibit Class I behavior are CO2—/ -hexane and CO2—benzene. More compHcated behavior exists for other classes, including the appearance of upper critical solution temperature (UCST) lines, two-phase (Hquid—Hquid) immiscihility lines, and even three-phase (Hquid—Hquid—gas) immiscihility lines. More complete discussions are available (1,4,22). Additional simple binary system examples for Class III include CO2—hexadecane and CO2—H2O Class IV, CO2—nitrobenzene Class V, ethane—/ -propanol and Class VI, H2O—/ -butanol. [Pg.222]

It has good capacity and drying capabiHty as illustrated by the vapor pressure curves in Figure 5. At 25°C, the dew point attainable in gases dried with 95% sulfuric acid is less than —75°C. [Pg.510]

The Clapeyron equation is most often used to represent the relationship between the temperature dependence of a pure hquid s vapor pressure curve and its latent heat of vaporization. In this case, dT is the slope of the vapor pressure—temperature curve, ADis the difference between the... [Pg.233]

Liquid helium-4 can exist in two different liquid phases liquid helium I, the normal liquid, and liquid helium II, the superfluid, since under certain conditions the latter fluid ac4s as if it had no viscosity. The phase transition between the two hquid phases is identified as the lambda line and where this transition intersects the vapor-pressure curve is designated as the lambda point. Thus, there is no triple point for this fluia as for other fluids. In fact, sohd helium can only exist under a pressure of 2.5 MPa or more. [Pg.1126]

Figure 4 shows vapor pressure curves of rare-earth metals[24], clearly showing that there is a wide gap between Tm and Dy in the vapor pressure-temperature curves and that the rare-earth elements are classified into two groups according to their volatility (viz.. Sc, Y, La, Ce, Pr, Nd, Gd, Tb, Dy, Ho, Er, and Lu, non-volatile elements, and Sm, Eu, Tm, and Yb, volatile elements). Good correlation between the volatility and the encapsulation of metals was recently... [Pg.156]

Assume that a boiler feed water is being pumped at 180 °F. Read the chart in Figure 3-46 and the water vapor pressure curve, and follow over to read NPSH reduction = 0.45 feet. A pump selected for the sertice requires 6 feet cold water service NPSHr ... [Pg.194]

Vapor Pressure Curves. (Courtesy Ingersoll-Rand Co.)... [Pg.579]

A-6 Altitude and Atmospheric Pressures, 578 A-7 Vapor Pressure Curves, 579 A-8 Pressure Conversion Chart, 580 A-9 Vacuum Conversion, 581 A-10 Decimal and Millimeter Equivalents of Fractions, 582 A-11 Particle Size Measurement, 582 . A-12 Viscosity Conversions, 583 A-13 Viscosity Conversion, 584 A-14 Commercial Wrought Steel Pipe Data, 585 A-15 ... [Pg.643]

Overhead temperature for essentially pure products at 10 psig = 223°F from vapor pressure curve. [Pg.38]

Because trichlor is 99.9% overhead, use it only to select boiling point from vapor pressure curves at 10 psig overhead pressure = 223°F (1,280 mm Hg abs). [Pg.90]

Read aqua-ammonia vapor pressure curves at wt percent NH3 and corrected temperature (base temperature plus rise) (= 90 + 17.8 = 107.8°F, e.g., or 41.1°C). Read 29.5 mm Hg as vapor pressure of ammonia, Figure 9-76. [Pg.356]

At/Ap)j = slope of vapor pressure curve. This may be calculated from Antoine type vapor pressure equation or obtain from a plot. [Pg.190]

At pressures greater than about 100 psig, the slope of the vapor pressure curve, (At/Ap) is low enough not to influence the sensible heating zone equation, as most of the tube is in vaporization. However, at low pressures and vacuum service, a large portion of the tube is in sensible heat. [Pg.191]

Figure 11-26. Vapor pressure curve for ethylene refrigerant. (Used by permission Starling, K. E. Fluid Thermodynamic Properties for Light Petroleum Systems, 1973. Gulf Publishing Co., Houston, Texas. All rights reserved.)... Figure 11-26. Vapor pressure curve for ethylene refrigerant. (Used by permission Starling, K. E. Fluid Thermodynamic Properties for Light Petroleum Systems, 1973. Gulf Publishing Co., Houston, Texas. All rights reserved.)...
The vapor pressure (P ) of a pure liquid at a given temperature (T) is the pressure exerted by its vapor in equilibrium with the liquid phase in a closed system. All liquids and solids exhibit unique vapor pressure-temperature curves. For instance, in Figure 2-79, lines BA and AC represent the equilibrium vapor pressure curves of the solid and liquid phases, respectively. [Pg.342]

It is apparent from the vapor pressure curves that to obtain a gas supply from a storage vessel, or from a cylinder, it is only necessary to release it from the top vapor space. Propane can usually be supplied from storage to the plant by this natural vaporization, without any pumps or compressors, throughout the year. [Pg.302]

A glance at the vapor pressure curve for butane will, however, reveal that in winter there is a possibility of butane vapor liquefying after the vaporizer if the temperature is allowed to fall in the pipeline, even at moderate pressure. For this reason, such pipework is usually heated, either by electrical tapes or, if available, by steam or hot-water lines. [Pg.302]

Curve AC represents the vapor pressure curve of ice. At any point along this line, such as point A (0°C, 5 mm Hg) or point C, which might represent — 3°C and 3 mm Hg, ice and vapor are in equilibrium with each other. [Pg.233]

Consider the vapor pressure curves of molecules A, B, and C shown below. [Pg.257]

Fig. 4. The vapor pressure curves of pure water and of saturated aqueous... Fig. 4. The vapor pressure curves of pure water and of saturated aqueous...
The only parts of Fig. 5 which can meaningfully be described as solubility in a compressed gas are WX and XV. However, a very different situation arises if the saturated vapor pressure curve cuts the critical curve (M—N of Fig. 3). Figure 4 shows that this does not happen for the three sodium halides. The complete course of the critical curve is not known, but enough is known in the case of the sodium chloride system51 75 for it to be clear that it rises well above the maximum of the saturated vapor pressure curve. However, it is cut by the vapor pressure curves of less soluble salts such as sodium carbonate and sodium sulphate.40 87 The (p, T) projection of a system of the type water + sodium chloride is... [Pg.92]

Fig. 7. The (pt T) projection of a system in which the saturated vapor pressure curve does not cut the critical line, MN. Fig. 7. The (pt T) projection of a system in which the saturated vapor pressure curve does not cut the critical line, MN.
Systems in which the saturated vapor pressure curve cuts a three-phase line of liquid + liquid + gas at a second quaternary point (solid + liquid + liquid + gas). Such systems have the first (or normal) quaternary point (solid + solid + liquid + gas) at lower temperatures and pressures (Fig. 13). Examples, ethane +... [Pg.101]


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