Mole fraction, 462 table

From equations 10 and 11, values of the americium and plutonium distribution coefficient can be estimated for MgCl2 contents in the salt ranging from 0.02 to 1.0 mole fraction (Table II). 

The minimum value of (Q/A)j is 0.072 kW/(kg SWU/year) at a feed composition of 0.18 mole fraction UFj. This is to be contrasted with the optimum value of 0.31 kW/(kg SWU/year) reported by Geppert et al. [Gl] for experiments with a feed composition of 0.04 mole fraction UFfi, and a design value of 0.287 kW/(kg SWU/year) for a commercial plant with a feed composition of 0.042 mole fraction (Table 14.18). 

Root mean squared error (RMSE) of logarithmic solubility loglOOr), x in mole fractions. Table partially... 

Finally, Table 2 shows enthalpy calculations for the system nitrogen-water at 100 atm. in the range 313.5-584.7°K. [See also Figure (4-13).] The mole fraction of nitrogen in the liquid phase is small throughout, but that in the vapor phase varies from essentially unity at the low-temperature end to zero at the high-temperature end. In the liquid phase, the enthalpy is determined primarily by the temperature, but in the vapor phase it is determined by both temperature and composition. 

The data in Table III-2 have been determined for the surface tension of isooctane-benzene solutions at 30°C. Calculate Ff, F, F, and F for various concentrations and plot these quantities versus the mole fraction of the solution. Assume ideal solutions. 

The following data (for 25°C) were obtained at the pzc for the Hg-aqueous NaF interface. Estimate and plot it as a function of the mole fraction of salt in solution. In the table,/ is mean activity coefficient such that a = f m , where m is mean molality. 

The data in Table 7.6 list the mole fraction of methyl acrylate in the feedstock and in the copolymer for the methyl acrylate (Mi)-vinyl chloride (M2) system. Use Eq. (7.54) as the basis for the graphical determination of the reactivity ratios which describe this system. 

This result enables us to convert mole fractions to volume fractions. Table 8.1 lists the corresponding values of 0j and Xj for n = 50, 100, and 500 as needed for the evaluation of ASj . With Xj s and the corresponding 0- s available, the required values of are calculated by Eq. (8.38) ... 

Table 8.1 Values of 0 Corresponding to the Indicated Mole Fractions for Values of n = 50, 100, and 500 (These Quantities are Used in Example 8.1.)...

Returning to the bottoms of the first column containing myristic, palmitic, oleic, and stearic acids, the recomputed mole fractions and volatilities are given in Table 2. 

The special case involving the removal of a low (2—3 mol %) mole fraction impurity at high (>99 mol%) recovery is called purification separation. Purification separation typically results in one product of very high purity. It may or may not be desirable to recover the impurity in the other product. The separation methods appHcable to purification separation include equiUbrium adsorption, molecular sieve adsorption, chemical absorption, and catalytic conversion. Physical absorption is not included in this Hst as this method typically caimot achieve extremely high purities. Table 8 presents a Hst of the gas—vapor separation methods with their corresponding characteristic properties. The considerations for gas—vapor methods are as follows (26—44). 

The system of primary interest, then, is that of a condensable vapor moving between a Hquid phase, usually pure, and a vapor phase in which other components are present. Some of the gas-phase components may be noncondensable. A simple example would be water vapor moving through air to condense on a cold surface. Here the condensed phase, characterized by T and P, exists pure. The vapor-phase description requiresjy, the mole fraction, as weU as T and P. The nomenclature used in the description of vapor-inert gas systems is given in Table 1. 

The H in solubility tables (2-121 to 2-144) is the proportionahty constant for the expression of Henry s law, p = Hx, mere x = mole fraction of the solute in the liqiiid phase p = partial pressure of the solute in the gas phase, expressed in atmospheres and H = a. proportionality constant expressed in units of atmospheres of solute pressure in the gas phase per unit concentration of the solute in the hquid phase. (The unit of concentration of the solute in the liquid phase is moles solute per mole solution.)... 

As an example of the use of the nomograph, the line is shown which would be drawn to determine the solubility of n-hexane in water at 25°C. The coordinates given in Table 1 for normal paraffins have been used X = 15.0, Y = 20.0. The predicted solubility is 2 x 10 mole fraction The experimental value is 1.98 x 10as given by McAuliffe and Price. ... 

The computer results from Table 5-13 show the calculated compositions of benzene, diphenyl, triphenyl, and hydrogen. At a fixed feedrate, increasing V/F values correspond to movement through the plug flow reactor (i.e., increasing reactor volume). Thus, these results illustrate how the composition varies with position in the reactor. Here, the mole fraction of benzene decreases steadily as the reaction mixture progresses in the reactor, while the composition of diphenyl increases and reaches a maximum between 1,684 and 1,723 hr and thereafter decreases. This is often typical of an intermediate in consecutive reactions. 

All free energies are in kilocalories per mole on the mole fraction scale, relative to DMF. See Table 8-5 for rate data. 

On the basis of the values of AS° derived in this way it appears that the chelate effect is usually due to more favourable entropy changes associated with ring formation. However, the objection can be made that and /3l-l as just defined have different dimensions and so are not directly comparable. It has been suggested that to surmount this objection concentrations should be expressed in the dimensionless unit mole fraction instead of the more usual mol dm. Since the concentration of pure water at 25°C is approximately 55.5 moldm , the value of concentration expressed in mole fractions = cone in moldm /55.5 Thus, while is thereby increased by the factor (55.5), /3l-l is increased by the factor (55.5) so that the derived values of AG° and AS° will be quite different. The effect of this change in units is shown in Table 19.1 for the Cd complexes of L = methylamine and L-L = ethylenediamine. It appears that the entropy advantage of the chelate, and with it the chelate effect itself, virtually disappears when mole fractions replace moldm . ... 

Table 3 Dependence of Constants K and a of [T7] = KM° on Mole Fraction of Sodium Acrylate (Xsa) for Copolymer Acrylamide with Sodium Acrylate in 0.5 M NaCl at 25°C [9]...

Flow parameter (Norton Co.) = F = FP Concentration of solute in liquid, lb mol solute/lb mol solute free solvent (or stream) Concentration of solute in liquid, in equiUbri-um -with the gas, lb mol solute/lb mol solvent Concentration of solute in liquid, mole fraction, or mol fraction of more volatile component in liquid phase Curve fit coefficients for C2, Table 9-32 Curve fit coefficients for Cg, Table 9-32 Concentration of solute in liquid in equilibrium -with gas, mol fracdon Concentradon of solute in gas, lb mol solute/lb mol solute free (solvent) (stream) Capacity parameter (Norton)... 

The experimental results on poly(methacrylic acid) containing a small mole fraction of either 3-vinylperylene (PMAvPER, (30)) or lV-[12-(4-aminonaphthali-mide)]-2-methylacrylamide (PMAANI, (31)) show charge separation which is efficient for PMAvPER but not much for PMAANI. The quantum yields of charge separation for various chromophores covalently bound to PMA at pH 2.8 are summarized in Table 7. 

A comparison of the left-hand side (LHS) and the right-hand side (RHS) of Eq. (81) is given in Table IV. The comparison is made at three different values of x2, including the critical point. In order to assess their relative importance, values of all the individual terms in Eq. (81) are reported in the table. It is apparent that all the terms contribute significantly and that none may be neglected (except that In Kt must necessarily vanish at the critical mole fraction). 

P7.1 Vapor pressure data for ethanol (1) + 1,4-dioxane (2) at T = 323.15 K is given in the following table, where. vq is the mole fraction in the liquid phase and y is the mole fraction in the vapor phase. 

In the table,. Ys.min and. Y2.max give the mole fraction range over which the parameters a and a apply. 

The proton inventory technique was applied to this system in an attempt to verify further these suggestions. The rate constants for the reactions were evaluated in CH3OH/CH3OD, C2H5OH/C2H5OD, and H2O/D2O mixtures over the full range of deuterium mole fractions. The data for methanol and water are given in Table 9-8. 

Table I. Composition of Various Samples Studied Glass Samples Composition (mole fraction...

STRATEGY Expect a lower vapor pressure when the solute is present. Calculate the mole fraction of the solvent (water) in the solution and then apply Raoult s law. To use Raoult s law, we need the vapor pressure of the pure solvent (Table 8.2 or 8.3). 

Calculate the vapor pressure of the solvent in each of the following solutions. Use Table 8.3 to find the vapor pressure ot water in (a) an aqueous solution at 100.°C in which the mole fraction of sucrose is 0.100 (b) an aqueous solution at 10().°C in which the molality of sucrose is 0.100 mol-kg. ... 

The experimental results are summarized in Table 2. CO2 permeance (Rco2), selectivity (oicx)2/N2) and CO2 recovery (Y) increased with decreasing CO2 mole fraction in feed gas. CO2 in the feed gas was successfully concentrated to 97-99 % by the single-stage operation. CO2... 

C05-0035. What are the mole fractions of the three most abundant trace atmospheric constituents listed in Table... 

Table 8.3. Mole fractions of CO, H2 and CH3OH in the direct synthesis of methanol.

---