114. weaker than those in NF02. The W3O has good thermal <strong>and</strong> hydrolytic stability, but undergoes the fluoride abstraction reaction <strong>with</strong> strong Lewis acids, to give <strong>salt</strong>s such as E7?20+AsF6-, <strong>and</strong> adds to perfluoroolefins (under BF3 catalysis) to give stable RfONF2 compounds. It apparently reacts slowly <strong>with</strong> NO to give NOF. Difluoramine has an ammonia-like structure <strong>with</strong> the following parameters: N-H, 1.03-1.08; N-F, 1.38; FNF, 103', HNF, 102'; dipole moment, 1.93 D. It is best prepared from difluorourea (which is obtained by aqueous fluorination of urea) by treatment <strong>with</strong> H2SO4 at 90' or by the reaction of N2F4 <strong>with</strong> CgHgSH at 50'. The HNF2 is stable <strong>and</strong> can be stored, but the usual procedure is to generate it as needed <strong>and</strong> pass it directly into a reaction vessel, since it has a tendency to ex- plode when frozen. The reactions of HNF2 are usually complex, but it undergoes three general types of reactions as follows: oxidation, for example <strong>with</strong> aqueous &e+3 solution to give N2F4 (perhaps the NF2- ion is involved); reduction, as in the reaction <strong>with</strong> aqueous HI to give NH4F <strong>and</strong> HF; complex formation <strong>with</strong> ethers, Lewis acids, 2nd metal fluorides. Chlorodifluoramine ClNF2 is well known, C12NF <strong>and</strong> BrNF2 are known as unstable compounds, <strong>and</strong> the other halogen fluoramines appear to be very unstable. The CLNF2 (or BrNF2) can be prepared by the reaction of aqueous NaOCl (or NaOBr) <strong>with</strong> N,N-difluoroureas or N,N-dif!luorosulfuryl amide. The C 1 9 is prepared by the reaction of CLF <strong>with</strong> ClN3 at 25'C or <strong>with</strong> NaN3 at 0'. The CUW2 is stable but dissociates readily to give C1 atoms <strong>and</strong> NF2 radicals (which defines the reaction chemistry) while C12NF is explosively unstable in the liquid state. A few remaining N-F compounds such as NF2NO <strong>and</strong> N3F are of limited inter- est, but a number of inorganic compounds <strong>and</strong> a host of organic compounds have been prepared in recent years in which NF2 groups may be regarded as substituents, e.g., SF5NF2, C(NF2)4, C(NF)(NF2)2, CF3ONF2 <strong>and</strong> CFzN(O)=NF. Figure 3. A summary of the interconversions of the nitrogen fluorides is found in Chlorine Fluorides <strong>and</strong> Related Compounds The halogen fluorides of prime interest as propellant oxidizers have been C@,CLF5, C103F <strong>and</strong> BrF5, but a number of other halogen fluorides have been studied. Properties of halogen fluorides are summarized in Table 111. Chlorine monofluoride appears to have considerable ionic character as reflected in the The C1-F bond NMR chemical shift of @ = +441 ppm (vs. CFC13). distance is 1.63 d, the dipole moment, 0.88 D, the bnd dissociation energy, 60.4 kcal/mol, <strong>and</strong> the heat of formation, -13.5 kcal/mol. The CLF is an energetic fluorinating agent. It reacts <strong>with</strong> fluorides such as CsF or NOF to give Cs+CLF2- <strong>and</strong> NO+ClF2-, respectively, <strong>and</strong> has been reported to react <strong>with</strong> the Lewis acid AsF5 to give Cl+AsF6- but substantiating evidence is lacking. The high volatility of CLF (b.p. -1OOOC) suggests that little or no association or self-ionization (to Clf <strong>and</strong> CUP- ions or to C12F' <strong>and</strong> CLF2- ions) exists, but the electrical conductivity is higher than that of CLF3.' c12. Chlorine monofluoride is prepared by reaction of Cu3 ana ,
B I 3 m4*2 elect. I 11 115. Figure 3 - Interconversion of Nitrogen Fluorides
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Introduction 1. SECONDARY CELLS WIT
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I time curves at constant current d
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I 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11
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7. IV IV- Equivalent Weight, gr/ Eq
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1 3 9 SOYO FILLER,HQT PRESS Fig. 4.
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11. COAL PYROLYSIS USING LASER IRRA
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13. Macerals. Macerals from a singl
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i 1 I Photochemistry. A fundamental
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t P li. al ’ i ._ m LL
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' 19. PYROLYSIS OF COAL IN A MICROW
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I 21. In the third stage, the gas e
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.4 4 0 W 0 m .d m x .-( 0 x w M m s
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' 25. CONCLUSIONS The principal rea
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' .4 b s tract 28.
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30. the course of the experiment Ex
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d (Sulfur] dt m i trogenj dt 32. E
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34. Table 1, Properties of Feed Mat
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0 0 0 m 0 VI b N 0 c, VI N 0 v, N h
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- Literature Cited 38 1. Gordon, K
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40 z - B 30 w 6 20 yl w U 10 40. 10
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Z 0 In 80 CK W > 6 60- 0 I- 40- Z W
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44. 2.0 I 1.2 - 0 2 1.0- 0.8 i TIME
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- 2.81 1.NITROGEN 2. SULFUR 3. GASO
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48. The oil from the separator is v
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. 50 . Table I . Properties of Pitc
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52. Coke yield A - - - - 0 800 900
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FIGURE 8. 54. t 0.5 1 800 900 1,000
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Introduction 56. FLUORODINITROETUNO
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chloride extractant without other h
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60. identified (Reference 7) as the
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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
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- Page 98 and 99: Introduction 98. RFACTIONS OF OxYcm
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