secondary cells with lithium anodes and immobilized fused_salt
secondary cells with lithium anodes and immobilized fused_salt secondary cells with lithium anodes and immobilized fused_salt
vapor Pressure (psia) Figure 4. Vapor Pressure of MlqQ 0 1 *2 3 4 5 6 7 Weight Percent Carbon in Ehaust (1000/14-7) Plgurc 5. Temperature VS. Carbon Content of Q SgiesIIBO-AP RopdhYlt COnlpoSiti~ - .. ._-
, 73. THE SYIVl?HESIS OF FLUORAMMONIUM SALTS’ Vytautas Grakauskas, Allen H. Remanick, and Kurt Baum Contribution from Chemical & Biological Processes, Aerojet.-General Corporation, Azusa, California 91703. Of the four possible fluorine-substituted ammonium ions, only the tetrafluoro derivative has been reported as a stable salt.*,3 Difluoramine and trifluoramine have been reported to form reversible complexes with Lewis acids at low Lenperatures. Fluoramin was claimed to be a by-product of the electrolysis of ammonium bifluoride5~‘ but the results have been shown to be in error.7 Xnethylfluoramihe was synthesized by the fluorination of unsymmetrical dimethylsulfamide and the compound was sufficiently basic to form a stable hydrochloride. Fluorimonium salts prepared by the rearrangement of aikyldifluoraainesg can also be considered as alkylidene derivatives of substituted fluoramines. 8 Simple salts of fluoramine have now been prepared by the reaction of alkyl N-fluorocarbamates with strong acids. The starting materials are synt’iesized readily by the fluorination .of alkyl carbamates.1° Fluoraomonim Bisulfate. Fluorimonium salts have been prepared and cnaracterizea in sulfuric acid. Under these conditions, the hydrolysis of N- fluorocarbamates in sulfuric acid would be expected to give the fluorammonium ion, which also should be stable. !;%en a solition of ethyl N-fiuorocarbamate in concentrated sulfuric acid bas heated at 65 to 4G0, carbon dioxide and ethylene were evolved. The F13 nm spectrum of the sulfuric acid solution consisted of a quartet at 36.8 ppm relative to SLternai trifluoroacetic acid, with a coupling constant of 38 cps. ?nus, the flmrine was coupled to three equivalent hydrogens, and it is notexorthy that tne hydrogens did not exchange rapidly with the solvent. By contrast, the F19 spectrum of an unheded solution of ethyl N-fluorocarbamate in sulPaic acid consisted of a single broadened signal at 27.5 ppm; the NH protons of the starting material thus exchanged with the solvent rapidly by the nmr time scale.
- Page 21 and 22: I 21. In the third stage, the gas e
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- Page 25 and 26: ' 25. CONCLUSIONS The principal rea
- Page 28 and 29: ' .4 b s tract 28.
- Page 30 and 31: 30. the course of the experiment Ex
- Page 32 and 33: d (Sulfur] dt m i trogenj dt 32. E
- Page 34 and 35: 34. Table 1, Properties of Feed Mat
- Page 36 and 37: 0 0 0 m 0 VI b N 0 c, VI N 0 v, N h
- Page 38 and 39: - Literature Cited 38 1. Gordon, K
- Page 40 and 41: 40 z - B 30 w 6 20 yl w U 10 40. 10
- Page 42 and 43: Z 0 In 80 CK W > 6 60- 0 I- 40- Z W
- Page 44 and 45: 44. 2.0 I 1.2 - 0 2 1.0- 0.8 i TIME
- Page 46 and 47: - 2.81 1.NITROGEN 2. SULFUR 3. GASO
- Page 48 and 49: 48. The oil from the separator is v
- Page 50 and 51: . 50 . Table I . Properties of Pitc
- Page 52 and 53: 52. Coke yield A - - - - 0 800 900
- Page 54 and 55: FIGURE 8. 54. t 0.5 1 800 900 1,000
- Page 56 and 57: Introduction 56. FLUORODINITROETUNO
- Page 58 and 59: chloride extractant without other h
- Page 60 and 61: 60. identified (Reference 7) as the
- Page 62 and 63: 62. to FEFO -e quite high (80 to 85
- Page 64 and 65: 64. RECENT CHEMISTRY OF THE OXYGEN
- Page 66 and 67: polymers for the conventional fuel
- Page 68 and 69: 68. In summary, two general methods
- Page 70 and 71: 70. Table XI1 Differential Thermal
- Page 74 and 75: C H -0-C-NHF, - 2 5 II 0 74. H 9304
- Page 76 and 77: 76. The infrared spectrum is descri
- Page 78 and 79: , 78. PREPARATION AND POLYMERIZATIO
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- Page 82 and 83: If it ~ 3 ~ o~t 7 s Y'2t the therm1
- Page 84 and 85: Chlorine Fentafluaride T q D OC 252
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- Page 90 and 91: 90. DENSITY, VISCOSITY AND SURFACE
- Page 92 and 93: 92. If it is assumed that the syste
- Page 94 and 95: 94. After condensation of oxidizer
- Page 96 and 97: Stirring Solenoid LHe 7. Cryostat 9
- Page 98 and 99: Introduction 98. RFACTIONS OF OxYcm
- Page 100 and 101: , Acknowledgement 100. This work wa
- Page 102 and 103: 102. volume and then by pumping to
- Page 104 and 105: 104. The x-ray powder pattern (Tabl
- Page 106 and 107: Irredie tion Time, mi&) 106. Table
- Page 108 and 109: I. Introduction 108. RE7IIEw OF ADV
- Page 110 and 111: 1.40 w F O/) 103-4O 'F 110. /H 0 21
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- Page 116 and 117: Compound C102F ~ 1 , 0 ~ -146 ~ 116
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- Page 120 and 121: 120. DETONABILITY TESTING AT NONAMB
,<br />
73.<br />
THE SYIVl?HESIS OF FLUORAMMONIUM SALTS’<br />
Vytautas Grakauskas, Allen H. Remanick, <strong>and</strong> Kurt Baum<br />
Contribution from Chemical & Biological Processes,<br />
Aerojet.-General Corporation, Azusa, California 91703.<br />
Of the four possible fluorine-substituted ammonium ions, only the tetrafluoro<br />
derivative has been reported as a stable <strong>salt</strong>.*,3 Difluoramine <strong>and</strong> trifluoramine<br />
have been reported to form reversible complexes <strong>with</strong> Lewis acids at<br />
low Lenperatures. Fluoramin was claimed to be a by-product of the electrolysis<br />
of ammonium bifluoride5~‘ but the results have been shown to be in error.7<br />
Xnethylfluoramihe was synthesized by the fluorination of unsymmetrical dimethylsulfamide<br />
<strong>and</strong> the compound was sufficiently basic to form a stable hydrochloride.<br />
Fluorimonium <strong>salt</strong>s prepared by the rearrangement of aikyldifluoraainesg<br />
can also be considered as alkylidene derivatives of substituted fluoramines.<br />
8 Simple <strong>salt</strong>s of fluoramine have now been prepared by the reaction of<br />
alkyl N-fluorocarbamates <strong>with</strong> strong acids. The starting materials are synt’iesized<br />
readily by the fluorination .of alkyl carbamates.1°<br />
Fluoraomonim Bisulfate. Fluorimonium <strong>salt</strong>s have been prepared <strong>and</strong><br />
cnaracterizea in sulfuric acid. Under these conditions, the hydrolysis of N-<br />
fluorocarbamates in sulfuric acid would be expected to give the fluorammonium<br />
ion, which also should be stable.<br />
!;%en a solition of ethyl N-fiuorocarbamate in concentrated sulfuric acid<br />
bas heated at 65 to 4G0, carbon dioxide <strong>and</strong> ethylene were evolved. The F13<br />
nm spectrum of the sulfuric acid solution consisted of a quartet at 36.8 ppm<br />
relative to SLternai trifluoroacetic acid, <strong>with</strong> a coupling constant of 38 cps.<br />
?nus, the flmrine was coupled to three equivalent hydrogens, <strong>and</strong> it is notexorthy<br />
that tne hydrogens did not exchange rapidly <strong>with</strong> the solvent. By contrast,<br />
the F19 spectrum of an unheded solution of ethyl N-fluorocarbamate in<br />
sulPaic acid consisted of a single broadened signal at 27.5 ppm; the NH protons<br />
of the starting material thus exchanged <strong>with</strong> the solvent rapidly by the<br />
nmr time scale.