United States Patent Office Patented Sept
Total Page：16
File Type：pdf, Size：1020Kb
3,149,913 United States Patent Office Patented Sept. 22, 1964 2 may vary over a wide range and may be as little as 1% 3,49,913 and as much as 50% and even higher. Particularly ad PROCESS FOR PRODUCING NETROSYL vantageous is the use of nitric acid in amounts such that SULFURECACE) d the resulting nitrosylsulfuric acid concentration approxi ALouis L. Ferstandig, El Cerrito, and Paul C. Condit, San 5 mates saturation values in order to afford maximum pro Asseino,poration, Calif.,San Francisco,assignors toCalif., California a corporation Research Cor of duction per unit reactor volume and yet avoid deposition Beavy are of solids. The solubility of nitrosylsulfuric acid in ap No Drawing. Fied June 14, 1961, Ser. No. 116,957 proximately 100% sulfuric acid ranges from about 48 3 (Caims. (CE. 23-39) grams per 100 grams of solution at 0° C. up to about 68 grams at 50 C. with, of course, a lesser solubility below This invention relates to a proces for the production of O 0 C. and a greater above 50° C. Although the presence nitrosylsulfuric acid. of the precipitated nitrosylsulfuric acid is usually a source Nitrosyisulfuric acid is particularly desirable for use of mechanical inconvenience, advantage may be taken of in the production of caprolactam from hexahydrobenzoic it by removal of the solid nitrosylsulfuric acid by filtra acid. Nitrosylsulfuric acid has long been known as an 5 tion and subsequent recycle of the mother liquor to the intermediate in connection with the lead-chamber sulfuric reaction Zone. acid process in which it is converted to Sulfuric acid with in general, the effective temperature range of the process concurrent liberation of nitric oxide in a reaction with is defined by the requirement that the reaction medium be sulfur dioxide. Several methods by which nitrosylsulfuric a liquid. At lower temperatures in the range about -20 acid may be prepared are known, but they all Suffer from 20 to -40 C., the reaction rate is, of course, slower than serious limitations. The usual method of choice in the art at temperatures appreciably higher, and in this range is the neat reaction of sulfur dioxide with fuming nitric whether there will be a liquid solution rather than a solid acid. The yields are poor, and there is a constant Safety Solution or solid depends upon the particular acid mix hazard. For unexplained reasons, violent autocatalytic ture used and the degree of conversion. While low tem temperature effects accompanied by explosive action are peratures favorably affect the solubility of sulfur dioxide frequently experienced in the synthesis. For reasonable 25 in the reaction mixture, faster rates and handling con safety, reaction temperatures must be kept below about veniences usually dictate operation at temperatures above 5° C. 0 C. At atmospheric pressure, the upper temperature It has now been found that nitrosylsulfuric acid may limit is defined by the reflux temperature of the mixture, be produced by reacting sulfur dioxide with a liquid Solti 30 and this is in the range of about 85-330° C. As the tion of nitric acid in sulfuric acid, the solution having conversion of the nitric acid proceeds this upper tempera an equivalent HO to SO3 ratio in the range of about ture limit increases due to depletion of the more volatile 1.7-0.17. Conversions and yields are excellent and the components. Pressure may be applied to the reaction sys reaction proceeds safely. term in order to make possible a higher liquid phase re Concentrated sulfuric acid is a very potent dehydrating action temperature, but in view of the nature of the mate medium, yet surprisingly in the present process dangerous 35 rials employed, corrosivity and the like, high pressure op concentrations of the unstable nitric acid anhydride, NCs, erations usually are not advantageous. However, tem do not appear to be formed. For reasons not clearly peratures as high as 200 C. are feasible at superatinos understood, when the reaction of sulfur dioxide with pheric pressures. A preferred temperature range is from nitric acid is carried out in very concentrated sulfuric 40 about -10° C. to about 150° C. acid, that is sulfuric acid having an equivalent H2O to The time required to complete the reaction will vary SOs ratio less than 1.7, there results a marked increase depending upon the temperature and concentration. Sui in the nitrosylsulfuric acid yield. Thus, the reaction of fur dioxide has a low solubility in the medium, and this sulfur dioxide with nitric acid in a Sulfuric acid solu limits the conversion rate; but it may be improved, as tion having an equivalent HO to SO3 ratio slightly larger 45 noted above, by carrying out the reaction under super than 1.7, results in substantially the same yield obtained atmospheric pressures. in the neat reaction. However, when the sulfuric acid Pressure equipment can be dispensed with, however, solution used is more concentrated, for example one in operations at atmospheric pressure by maintaining a having an equivalent HO to SO3 ratio of 1.7 or less, high flow rate of SO2 into a well-stirred reaction mixture. the yield is essentially quantitative and is merely dependent 50 Recycle of the exit gas stream, of course, increases the upon stopping the reaction at the equivalence point, i.e., efficiency of the process. At a temperature of about 20 where all the HNO has reacted. Fuming sulfuric acid 50 C., the reaction is complete in about seven and one solutions of nitric acid having H2O to SO3 ratios as half hours. At higher temperatures the time to com low as 0.7 and even lower are particularly desirable me pletion is much less. The contacting of the sulfur di diums for the present process. At ratios below about 0.17 55 oxide must be terminated at about the total nitric acid the fugacity of the sulfur trioxide introduces operational conversion point, else severe yield losses result due to problems, and some decrease in reaction rate is experi follow-up reactions in which nitrosylsulfuric acid is a enced. Particularly preferred solutions have an equivalent reactant. HO to SO ratio in the range 1.6-0.6. By equivalent The end point of the conversion may be determined ratio is meant the ratio of the sum of the mols of water 60 by several means. The most convenient is the develop present, that is, the mols of water combined in H2SO4 ment of a blue to blue-black coloration in the reaction plus uncombined, to the sum of the mols of SO3 present, medium. This appears to occur at the equivalence point also combined and uncombined. For example, 100% and is so pronounced as to be a generally reliable guide. HSO4 has an equivalent ratio of water to SO of 1:1; A second method is to follow the absorption of the ni and HSO4 having one mol of added water has an equiva 65 trosyl cation (NO+) in the ultraviolet spectrum using lent ratio of 2:1, e.g., 2. prepared standards, conventional techniques, and the The nitric acid employed in the process of the present known relevant wave lengths in order to stop the reac invention is desirably concentrated nitric acid, and by tion when a desired concentration of nitrosylsulfuric acid concentrated is meant that it should be of at least 50% is reached or the nitrosylsulfuric acid concentration has concentration. Red fuming nitric acid is an especially use reached a maximum. ful feed acid to the process. 70 The process of the present invention may be carried The weight percent of nitric acid in the acid mixture out in a batch or a continuous manner in a glass or a 3 4. corrosion-resistant alloy vessel fitted with a means for EXAMPLE II efficient stirring. Introduction of the sulfur dioxide into Example I was repeated, using a mixture of red fuming the reaction mixture in the process run at atmospheric nitric acid and 100% sulfuric acid. The time required pressure is desirably made at a point in the lower portion to maximum yield was 2.6 hours, and the yield at this of the reaction vessel, and in a manner whereby the gas 5 point was found to be 73.5% of theory. stream is broken up into very small bubbles. When su Temperature effects were also determined. When the peratmospheric pressures are used, the sulfur dioxide may equivalient ratio of water to SC was 1, e.g., 100% H2SO4, be introduced in a similar manner or in bulk, but care a spontaneous but controilable temperature rise of 80 must be taken not to add any appreciable amount of Sul C. occurred under the above experimental conditions. fur dioxide over the stoichiometric requirement. Simi O When the equivalent ratio is about 0.8, only a very minor larly, in adding sulfur dioxide in bulk to a pressure ves temperature effect is experienced, and at lesser equivalent sel, provision should be made for adequate removal of the ratios the temperature effect is not readily apparent. heat of reaction. When the end point of the reaction is reached, further EXAMPLE IV processing depends upon the ultimate objective. if it is 5 Example was repeated wherein the equivalent ratio desired to recover the nitrosylsulfuric acid, this is readily of H.G to SO was about 2.0. in order to minimize accomplished by cooling the reaction mixture to form the spontaneous temperature effect, the SO, flow rate crystalline nitrosylsulfuric acid which may be collected was maintained at only about one-third that normally em by filtraticin and the reconstituted mother liquid returned ployed, e.g., approximately 92 ml.