Liquid pure saturated

FIG. 2-11 Enthalpy-concentration diagram for aqueous hydrogen chloride at 1 atm. Reference states enthalpy of liquid water at 0 C is zero enthalpy of pure saturated HCl vapor at 1 atm (—85.03 C) is 8000 kcal/moL NOTE It should he observed that the weight basis includes the vapor, which is particularly important in the two-phase region. Saturation values may be read at the ends of the tie lines. [Van Nuys, Trans. Am. Inst. Chem. Eng., 39, 663 (1943).]... 

Liquid Density Prediction Methods for the prediction of pure saturated hydrocarbons and nonhydrocarbon organics, compressed hydrocarbon hquids, and defined and undefined hydrocarbon mixtures were evaluated. Only the most accurate and convenient methods are included here. 

TABLE 2-396 The Modified Rockett Equation Input Parameters for Calculating Pure Saturated Liquid Densities... 

The physical properties of the liquid, rather than those of the vapor, are used For determining the film coefficient for condensation. Nus-selt [2. Ver. Dt.sch. Ing., 60, 541, 569 (1916)] derived theoretical relationships for predicting the film coefficient of heat transfer for condensation of a pure saturated vapor. A number of simplifying assumptions were used in the derivation. 

Quality of a Wet Vapor, in the vapor-liquid region of a pure substance, the composition of a two-phase system (at given T and P) varies from pure saturated liquid at the bubble jjoint M to pure saturated vapor at the dew point N along the line MQN on the P- V diagram (Figure 2-80). For a wet vapor represented by an intermediate... 

For the solvent (component 1),/° is the fugacity of pure saturated liquid 1 at the system temperature. However, the standard-state fugacity for the solute (component 2) is given by... 

Institute, New York 1955. (--) Calculated with ft, and ft from pure saturated liquid. 

The isothermal vaporization of pure liquid i represents its transition from saturated liquid to saturated vapor at temperature T and at saturation vapor pressure P8 6. The treatment of this transition is facilitated through use of property changes of vaporization defined by equation 139 ... 

Equation (11.17), which defines the fugacity of pure species i, may integrated for the change of state from saturated liquid to saturated vapor,1 at temperature T and at the vapor pressure PT -... 

Since coexisting phases of saturated liquid and saturated vapor are in < librium, the equality of fugacities as expressed by Eqs. (11.22) and (11.24) is criterion of vapor/liquid equilibrium for pure species. 

The third plane identified in Fig. 12.1 is the vertical one perpendicular to the composition axis and indicated by MNQRSLM. When projected on a parallel plane, the lines from several such planes present a diagram such as that shown by Fig. 12.4. This is the PT diagram lines t/C, and KC2 are vapor-pressure curves for the pure species, identified by the same letters as in Fig. 12.1. Each interior loop represents the PT behavior of saturated liquid and of saturated vapor for a mixture of fixed composition the different loops are for different compositions. Clearly, the PT relation for saturated liquid is different from that for saturated vapor of the same composition. This is in contrast with the behavior of a pure species, for which the bubble line and the dew line coincide. At points A and B in Fig. 12.4 saturated-liquid and saturated-vapor lines intersect. At such points a saturated liquid of one composition and a saturated vapor of another composition have the same T and P, and the two phases are therefore in equilibrium. The tie lines connecting the coinciding points at A and at B are perpendicular to the PT plane, as illustrated by the tie line VX in Fig. 12.1. 

The amount of heat required to convert 1 g. of a pure liquid into saturated vapour at any given temperature (or pressure, since the pressure of saturated vapour is a function only of temperature) is called the latent heat of evaporation (sometimes latent heat of vaporisation), denoted by 4. It is usually understood to apply to evaporation at the normal b.p. at 1 atm. pressure, and it varies rather considerably with temperature. For water ... 

Pure water may coexist as liquid and vapor only at temperature-pressure pairs that fall on the vapor-liquid equilibrium (VLE) curve. At points above the VLE curve (but to the right of the solid-liquid equilibrium curve), water is a subcooled liquid. At points on the VLE curve, water may be saturated liquid or saturated steam (vapor) or a mixture of both. At points below the VLE curve, water is superheated steam. 

A stirred tank with volume V t(L) is charged with V i(L) of a liquid, B. The space above the liquid (volume = Vi l/i) is filled with a pure gas, A, at an initial pressure Po(atm). The initial system temperature is ro(K). The stirrer in the lank is turned on, and A begins to dissolve in B. The dissolution continues until the liquid is saturated with A at the final system temperature (7 ) and pressure... 

H2O <0.4-0.5 wt.%, t5fpicaUy 0.1-0.2 wt.% enriched mid-ocean-ridge basalt (E-MORB) up to 1.5 wt.% CO2 50-400 ppm typically saturated at emption (gas phase almost pure CO2) leading to vesiculation S 800-1,500 ppm immiscible Fe-S-O liquids indicate saturation at emption... 

More intuitively the elevating effect of the attractive pore potential can be understood as follows. In a pore with strongly attractive potential, a liquid-like state can hold even with lower vapor pressure than the saturated one. When this system is equilibrated with pure liquid or saturated vapor, the excess potential must be balanced with the increase in density... 

The isothermal vaporization of a pure liquid results in a phase change from saturated liquid to saturated vapor at vapor pressure P . The... 

The amount of heat required to convert 1 g of a pure liquid into saturated vapor at any given temperature is called the latent heat of evaporation or latent heat of vaporization, It has been suggested that... 

In Equation 3 it is necessary to have reference-state values for component density, X pT, and fugacity (fi/xi)r. For pure-solvent components these are the pure saturated liquid density, p 0, and the fugacity of the saturated vapor, /i0sat, (which equals that of the saturated liquid) respectively, both at the temperature of interest. For mixed solvents, the density also requires volume of mixing data for the solvents, and the solvent fugacities are found from the vapor-liquid equilibrium data on the solute-free mixture. 

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