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Sulfuric acid water systems

A tabulation of the partial pressures of sulfuric acid, water, and sulfur trioxide for sulfuric acid solutions can be found in Reference 80 from data reported in Reference 81. Figure 13 is a plot of total vapor pressure for 0—100% H2SO4 vs temperature. References 81 and 82 present thermodynamic modeling studies for vapor-phase chemical equilibrium and liquid-phase enthalpy concentration behavior for the sulfuric acid—water system. Vapor pressure, enthalpy, and dew poiat data are iacluded. An excellent study of vapor—liquid equilibrium data are available (79). [Pg.180]

Jaecker-Voirol, A., and P. Mirabel, Heteroniolecular Nucleation in the Sulfuric Acid-Water System," Atmos. Environ., 23, 2053-2057 (1989). [Pg.427]

The value of / for p-nitroaniline is measurable with adequate precision in sulfuric acid-water systems up to 24% [w/w] of acid. Within this range, Hammett defined the operational measure Hq of acidity of the solution by Eq. (29). [Pg.208]

T. Vermeulen and co-workers, Vapor-.Eiquid Equilibrium of the Sulfuric Acid/ Water System, AIChE meeting, Anaheim, Calif., (June 10, 1982). [Pg.194]

As the author points out, the sulfuric acid-water system is one of the few examples of a liquid binary system in which certain properties change discontinuously. In this case dsjdp, where s is the specific gravity and p the per cent concentration of H2S04, has discontinuities at certain values of p. The most pronounced correspond to the compositions H2S04—H20 and H2S04—2H20. Mendeleev (102) believes that these characteristic points are connected with the formation in the solutions of definite chemical compounds. The more stable the compound the sharper the discontinuity in the property versus composition. [Pg.247]

Figure 26. Variation of the fluorescent lifetime of Tb2(S04)3 in a sulfuric acid-water system as a function of water concentration [from Ref. (/0/)J. Figure 26. Variation of the fluorescent lifetime of Tb2(S04)3 in a sulfuric acid-water system as a function of water concentration [from Ref. (/0/)J.
Electrolysis yields only low amounts of ozone, 4 to 7 grams per kilowatt-hour, because the high current densities needed at the anode cause heavy losses of ozone by thermal destruction. Here, too, the yields can be improved by lowering the temperature. Thus, using sufficiently concentrated sulfuric acid solutions, it is possible to electrolyze at temperatures slightly above the eutectic point (—75° C.) of the sulfuric acid-water system, and so obtain yields close to 12 grams per kilowatt-hour (I, 6). [Pg.6]

Prepare an enthalpy-concentration chart for the sulfuric acid-water system, and compare your chart with the one in Appendix I. You will have to look up the necessary data in reference books or the literature. [Pg.530]

Figure 1.4 Enthalpy-concentration of sulfuric acid-water system relative to pure components. (Water and H2SO4 at 32°P and own vapor pressure.) (Data from International Critical Tables, 1943 O. A. Hougen and K. M. Watson.)... Figure 1.4 Enthalpy-concentration of sulfuric acid-water system relative to pure components. (Water and H2SO4 at 32°P and own vapor pressure.) (Data from International Critical Tables, 1943 O. A. Hougen and K. M. Watson.)...
At this point, we returned to the original nitration procedure (with 2 3 molar equivalents of sulfuric acid) to try to determine why the nitration was not safe upon scale up The AT for this original procedure could be calculated from the heat capacity (Cp) of the system and the heat of the reaction ( AH) by the equation Ah = Cp x AT. The heat capacity of nitric acid/sulfuric acid/ water systems are available ( 0 and found to be 678 cal/mole °C (assuming that the heat capacity of the CNP/CDMP component was negligible) Using the experimentally derived temperature rise, the heat of the nitration reaction was estimated to be ... [Pg.112]

Doyle, G. J. (1961). Self-nucleation in the sulfuric acid water system. J. Chem. Phys. 35,795-799. Drapcho, D. L., D. Sisterson, and R. Kumar (1983). Nitrogen fixation by lightning activity in a thunderstorm. Atmos. Environ. 17, 729-734. [Pg.651]

The sulfuric acid-water system reactions are shown in Table 10.7. Note that the reaction H2SC>4(g) — H2SC>4(aq) is not included as H2S04(aq) can be assumed to completely dissociate to HSO4 in the atmosphere for all practical purposes. [Pg.467]

The Ammonia-Nitric Acid-Sulfuric Acid-Water System... [Pg.478]

FIGURE 11.12 Composition of the critical H2S04-H20 nucleus, calculated for / = 1 cm-3 s, as a function of RH. The different curves correspond to the temperatures shown. (Reprinted from Atmos. Environ. 23, Jaecker-Voirol, A. and Mirabel, P., Heteromolecular nucleation in the sulfuric acid-water system, p. 2053, 1989, with kind permission from Elsevier Science Ltd, The Boulevard, Langford Lane, Kidlington OX5 1 GB, UK.)... [Pg.523]

Doyle, G. J. (1961) Self-nucleation in the sulfuric acid-water system, J. Chem. Phys. 35, 795-799. [Pg.533]

Nakajima, A., Hirai, T. Hayashi, T. (1978). Phase relationship of rodlike polymer, poly(p-phenyleneterephthalamide), in sulfuric acid-water system. Polymer Bulletin, Vol. 1, No. 2, pp. 143-147. [Pg.432]


See other pages where Sulfuric acid water systems is mentioned: [Pg.216]    [Pg.152]    [Pg.418]    [Pg.46]    [Pg.305]    [Pg.480]    [Pg.152]    [Pg.9]    [Pg.346]   
See also in sourсe #XX -- [ Pg.124 ]




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