for the system reported here. The calculation method used is similar to the one suggested by Prausnitz et al. ( 4 ) .Calculated values of yl based on 712 and ~2~ are given in Table 11 cy1 &d). The maximum percentage deviation between y1 expt~ and y1 calcd = (lOOAy/yl exptl) is less than 3.03%. Plots of log ( y l / y 2 ) us. x1 in accordance with the Redlich and Kister equation ( 5 ) showed the integrated value was 0.417 and the absolute value was 4.075. The small integrated value showed that the data were consistent. NOMENCLATURE g,, = energies of interaction between an i-j pair of molecules P = vapor pressure, mm of Hg x = mole fraction in liquid phase y = mole fraction in vapor phase CY,, = nonrandomness constant for binary i -j interactions AY = (Y1 exptl -y1 calcd) y = activity coefficient T = total pressure, mm of Hg T,, = coefficient defined in Equation 3Subscripts 1 = carbon disulfide 2 = methanol
A simple technique for the measurement of total and partial vapor pressures of the hydrochloric acid-ferrous chloride-water system and a method to correlate vaporliquid equilibrium data are described. The concentration ranges investigated were 2.95 to 8.18 and 0.73 to 1.28 moles per liter for HCI and FeCk, respectively. Experimental data obtained at 70°C. fit an equation relating the partial vapor pressures of the system and the mole fractions of the components. In the temperature range 50°to 90°C ., the total and partial vapor pressures obey the Clausius-Clapeyron equation.THE HCl-FeCl2-H20 system was studied because of its importance in regenerating hydrochloric acid from chloride solutions and the lack of experimental data in the literature.
partial difference equation such as Equation (15), (22), or (42), the memory requirement of the present approach should be about the same order of magnitude as the traditional methods. It should be noted that we encounter the dimensionality difficulty only when we solve Equation
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