Pressure partial - diagrams

Figure B-1. Pressure impulse diagrams for damage to brick houses. Line 1 Threshold for light damage. Line 2 Threshold or moderate damage partial collapse of roof some bearing wall failures. Line 3 Threshold for severe damage 50 to 75 percent of bearing wall destruction. P, side-on overpressure. /, side-on impulse (Baker et al. 1983).

Fig. 2. (a) Sketch of the relations between defect concentrations and partial pressure (Brouwer diagram) of a pure oxide MO In regime II the intrinsic Schottky disorder determines the concentration, whereas in I and III non-stoichiometry prevails, (b) Dependence of the hole and electron concentration on the frozen-in oxygen vacancy concentration in a negatively (acceptor) doped oxide. 

The most convenient method for representation of enthalpy data for binary J solutions is by enthalpy/ concentration (Hx) diagrams. These diagrams are graphs T of the enthalpy plotted as a function of composition (mole fraction or mass fraction of one species) with temperature as parameter. The pressure is a constants and is usually 1 atmosphere. Figure 13.10 shows a partial diagram for the H2SO4/H2O system. 

A complimentary perspective of compositional variation in melting residues can be made from major-element oxide variation diagrams. Figure 6 shows the variation in major-element oxides versus FeO content as a function of pressure (1-7 GPa) and degree of batch melt extraction. FeO was chosen as the abscissa because of its large relative variation in partial melts and residues as a function of pressure. At 1 GPa the FeO content in the residue shows a mild increase with degree of melt extraction, but by 2 GPa FeO shows a mild decrease. This reflects the fact that low-pressure partial melts have FeO contents less than that of the bulk rock, but as pressure increases so does the FeO... 

The isotherms are plotted on pressure-composition diagrams (Figures 1.3a and b). The curves calculated by Raoult s law are the broken straight lines. They are obtained simply by joining the pure-component vapor pressure points to the zero pressure point on the opposite side to get the partial pressure curves and by joining the two vapor pressure points to get the total pressure curve. The solid lines are obtained by simulation and represent expected behavior of the mixtures. The... 

Figure 3.5 Defect concentrations as a function of the oxygen partial pressure (Brouwer diagrams) in binary MOi 5 oxide.

Fig. 51. (a) Temperature-pressure phase diagram of pure Zr02 [244] and (b) the zirconia-rich section of a Zr02-Y203 phase diagram [245]. Shaded areas indicate the ranges of compositions for partially stabilized zirconia (PSZ) and tetragonal zirconia polycrystals (TZP) [246]. 

The results for an equimolar CO -air mixture, obtained with several series of expansions, are presented in Fig.4. The pressure-temperature diagram in the upper part shows the experimental Wilson points and the dew line, which is extrapolated below the triple point For comparison, the frost line is plotted, too. The lower diagram shows the same Wilson points in a plot of the partial density of CO versus temperature. Here, the full curve represents the Wilson line for pure CO, obtained in the preceding investigation [1]. Obviously, spontaneous condensation of CO in the equimolar CO -air mixture begins nearly at the same partial density as with pure CO. ... 

Figure 1.10 Pressure/composition diagram for carbon dioxide//i-hexadecane (a Class B1 system) at 26.5°C, showing the very restricted range over which liquid CO2 is partially miscible with the -hexadecane. Vapour/liquid equilibria have not been investigated in detail in the immediate vicinity of the vapour pressure for pure CO2 but probably take the form shown in the inset, the mole fraction of CO2 at the point Q being about 0.98. The three phase pressure (P ") is probably about 2 bar less than the CO2 vapour pressure (P°). Subscripts 1 and 2 denote hexadecane-rich and...

Hochgesand (1968, 1970) and Kriebel (1989) present essentially identical flow diagrams for a selective Rectisol unit treating high-pressure partial oxidation gas. See Figure 14-18 for details. 

Phase relationships ia the system K O—B2O2—H2O have been described and a portion of the phase diagram is given ia Figure 8. The tetrahydrate, which can be dried at 65°C without loss of water of crystallisation, begias to dehydrate between 85 and 111°C, depending on the partial pressure of water vapor ia the atmosphere. This conversion is reversible and has a heat of dehydration of 86.6 kj/mol (20.7 kcal/mol) of H2O. Thermogravimetric curves iadicate that two moles of water are lost between 112 and 140°C, one more between 200 and 230°C and the last between 250 and 290°C (121). 

Carbon disulfide is completely miscible with many hydrocarbons, alcohols, and chlorinated hydrocarbons (9,13). Phosphoms (14) and sulfur are very soluble in carbon disulfide. Sulfur reaches a maximum solubiUty of 63% S at the 60°C atmospheric boiling point of the solution (15). SolubiUty data for carbon disulfide in Hquid sulfur at a CS2 partial pressure of 101 kPa (1 atm) and a phase diagram for the sulfur—carbon disulfide system have been published (16). Vapor—Hquid equiHbrium and freezing point data ate available for several binary mixtures containing carbon disulfide (9). 

FIG. 2-29 Enthalpy-concentration diagram for aqueous sodium hydroxide at 1 atm. Reference states enthalpy of liquid water at 32 F and vapor pressure is zero partial molal enthalpy of infinitely dilute NaOH solution at 64 F and 1 atm is zero. [McCahe, Trans. Am. Inst. Chem. Eng., 31, 129(1935).]... 

Background Indirect coal liquefaction differs fundamentally from direct coal hquefaction in that the coal is first converted to a synthesis gas (a mixture of H9 and CO) which is then converted over a catalyst to the final product. Figure 27-9 presents a simplified process flow diagram for a typical indirect coal hquefaction process. The synthesis gas is produced in a gasifier (see a description of coal gasifiers earlier in this section), where the coal is partially combusted at high temperature and moderate pressure with a mixture of oxygen and steam. In addition to H9 and CO, the raw synthesis gas contains other constituents (such as CO9, H9S, NH3, N9, and CHJ, as well as particulates. 

For any particular system, a graph can be constructed using the concentration of the solute in the liquid phase (Ca) and the concentration or partial pressure of the solute in the gas phase (Pa) as the abscissa and ordinate, respectively. A line indicating the equilibrium concentrations of the solute in the gas and solvent drawn on this graph, results in an equilibrium diagram. 

FIG. 4 Qualitative phase diagram close to a first-order irreversible phase transition. The solid line shows the dependence of the coverage of A species ( a) on the partial pressure (Ta). Just at the critical point F2a one has a discontinuity in (dashed line) which indicates coexistence between a reactive state with no large A clusters and an A rich phase (hkely a large A cluster). The dotted fine shows a metastability loop where Fas and F s are the upper and lower spinodal points, respectively. Between F2A and Fas the reactive state is unstable and is displaced by the A rich phase. In contrast, between F s and F2A the reactive state displaces the A rich phase. 

Vapor—Liquid Systems. The vapor-liquid region of a pure substance is contained within the phase or saturation envelope on a P-V diagram (see Figure 2-80), A vapor, whether it exists alone or in a mixture of gases, is said to be saturated if its partial pressure (P.) equals its equilibrium vapor pressure (P, ) at the system temperature T. This temperature is called the saturation temperature or dew point T ... 

Free-energy-concentration diagrams have been used in the study of the thermodynamic influence on the non-stoichiometry of the solid titanium carbide deposited from H2-CH4-TiCl4 gas mixtures at 1 900 K. The authors show how, from the partial pressure measurements of Ti vapour over a range of... 

The Phase Boundaries. Our interest in the phase diagram is solely to define the method by which the calculation of the partial pressures should be done. Because (1) there are only small... 

---