Sulfuric Acid Table

Sulfur recovery processes convert acid gases containing H2S and other sulfur compounds to elemental sulfur and sulfuric acid. Table II is a summary of many of the available sulfur recovery processes. 

Source Rieber, M. Okech, B. Fuller, R. "Sulfur Pollution Control The Disposal Problem" U.S. Bureau of Mines (Contract No. J0188144) Washington, D.C., July 1980 Volume 8, "Sulfuric Acid," Table 8.37, p. 8-89. 

The typical acids used in solution studies of carbenium ions are, by thermodynamically rigorous methodology, stronger than 100% sulfuric acid. Table I (19, 20) lists some of the common superacids as well as their approximate Hammett acidities. NMR studies of the products from organic... 

For samples with concentrations below 93.0%, expressed in degrees Baume, transfer about 200 mL of sample, previously cooled to a temperature below 15°, into a 250-mL hydrometer cylinder. Insert a suitable Baume hydrometer graduated at 0.1 °Be intervals, adjust the temperature of the sample to exactly 15.6°, and note the reading at the bottom of the meniscus, estimating it to the nearest 0.05 °Be. Determine the equivalent percentage of H2S04 from the Sulfuric Acid Table, Appendix nc. 

Dehydration with Strong Sulfuric Acid (Tables 6.3-6.5)... 

Anhydrous sulfuric acid (Table 10) has a very high dielectric constant and electrical conductivity as a consequence of autoionization (equations 22 and 23), which occurs via two different equilibria. 

There seems to be some indication that a-substituted 7-arylbutyric acids can be cyclized by sulfuric acid in better yields than the unsubstituted acids. Thus, whereas 7-phenylbutyric acid has not been cyclized in yields exceeding 50% with sulfuric acid (Table III), the a-methyl and a-ethyl homologs have been converted to the tetralones in 98% and 86% yields respectively. Similarly a-methyl-7-l-naphthylbutyric acid was cyclized in 91% yield, althou in the case of the unsubstituted acid yields over 75% could not be obtained. This peculiarity may be explained by the fact that ring closure of acids containing a substituent in the a-position gives rise to ketones lacking the usual reactive methyl-... 

The amount of intracrystalline complex present in the different catalyst samples was measured by UV spectroscopy after sample dissolution in concentrated sulfuric acid (Table 1). 

The elemental sulfur becomes colloidally stable in Sg molecules but can also add to sulfite and form thiosulfate S + S (0)3 S - S (0)3 (S203 ), which also loses the sulfur via disproportionation into H2S and SO4 . In hydrometeors and interfacial waters, however, sulfur reacts with oxygen (reactions 5.265 and 5.262) via SO2 to form hydrogen sulfite HSO3. Thiosulfate is an important intermediate in biological sulfur chemistry from both sulfate reduction and sulfide oxidation. Many hypothetical so-called lower sulfuric acids (Table 5.19) might appear as intermediates or in the form of radicals (such as SOH, HSO, HSO2, HSS and HS as seen from the structure formulas) in the oxidation chain from sulfide to sulfate ... 

Alkylation Mechanism with Zeolite Catalysts. The fact that the alkylate produced over a zeolite solid acid is quite similar in terms of product distribution to that obtained with sulfuric acid (Table 8) strongly points toward an alike general reaction mechanism occurring in both types of catalysts. The main catalytic cycles involved in the isobutane/butene alkylation mechanism are illustrated in Figure 6. 

Chlorinated and aromatic hydrocarbons, organic esters, aromatic hydroxy compounds, and certain ketones have an adverse effect on neoprene and consequently only Umited serviceability can be expected with them. Highly oxidizing acid and salt solutions also cause surface deterioration and loss of strength. Included in this category are nitric acid and concentrated sulfuric acid. Table 4.11 provides the compatibility of neoprene with selected corrodents. Reference 1 provides a more detailed listing. 

In contrast to nitration (Scheme 6.91) and bromination (Equation 6.103), the products of sulfonation of naphthalene (CioHg) with sulfuric acid (Table 6.13, example 4) (Equation 6.104) are different at different temperatures. Indeed, low temperature sulfonation has been demonstrated to be reversible and below 20°C only 1-naphthalenesulfonic acid is isolated (i.e., a-substitution). Above 160°C only 2-naphthalenesulfonic acid (P-substitution product) is isolable.The low-temperature product (1-naphthalenesulfonic acid) can be isomerized by heating to yield its isomer (2-naphthalenesulfonic acid). This is another case of kinetic and thermodynamic control providing different products (as discussed earlier for addition to conjugated alkenes [this chapter]). 

Among the parameters that are particularly affected by sensitization are ip and ice, as defined in Fig. 12.1. In this example, the ability to sustain passivity increases as the current density to maintain passivity Up) decreases and as the total film resistance increases, as indicated from measurements obtained with different metals exposed to 67% sulfuric acid (Table 12.3). The lower or more reducing the potential at which a passive metal becomes active, the greater the stability of passivity. The depassivation potential corresponding to the passive-active transition, called the Flade potential, can differ appreciably from Epp measured by going through the active-passive process of the same system. This technical distinction is important for the control aspect of anodic protection where Epp is the potential to traverse to obtain passivation, and the Flade potential is the potential to avoid traversing back into active corrosion. 

More than 90 percent of the elemental sulfur consumed in the United States is converted to sulfuric acid. Table 14.2 shows the pattern of U.S. sulfur consumption during the 1980s. ... 

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