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Chlorine temperature dependencies

Chlorine, a member of the halogen family, is a greenish yellow gas having a pungent odor at ambient temperatures and pressures and a density 2.5 times that of air. In Hquid form it is clear amber SoHd chlorine forms pale yellow crystals. The principal properties of chlorine are presented in Table 15 additional details are available (77—79). The temperature dependence of the density of gaseous (Fig. 31) and Hquid (Fig. 32) chlorine, and vapor pressure (Fig. 33) are illustrated. Enthalpy pressure data can be found in ref. 78. The vapor pressure P can be calculated in the temperature (T) range of 172—417 K from the Martin-Shin-Kapoor equation (80) ... [Pg.505]

Membranes are commonly rated for their chlorine tolerance in ppm-hours, simply the product of the concentration and the contact time. Tolerance is temperature dependent. [Pg.2036]

Fig. 1. Examples of temperature dependence of the rate constant for the reactions in which the low-temperature rate-constant limit has been observed 1. hydrogen transfer in the excited singlet state of the molecule represented by (6.16) 2. molecular reorientation in methane crystal 3. internal rotation of CHj group in radical (6.25) 4. inversion of radical (6.40) 5. hydrogen transfer in halved molecule (6.16) 6. isomerization of molecule (6.17) in excited triplet state 7. tautomerization in the ground state of 7-azoindole dimer (6.1) 8. polymerization of formaldehyde in reaction (6.44) 9. limiting stage (6.45) of (a) chain hydrobromination, (b) chlorination and (c) bromination of ethylene 10. isomerization of radical (6.18) 11. abstraction of H atom by methyl radical from methanol matrix [reaction (6.19)] 12. radical pair isomerization in dimethylglyoxime crystals [Toriyama et al. 1977]. Fig. 1. Examples of temperature dependence of the rate constant for the reactions in which the low-temperature rate-constant limit has been observed 1. hydrogen transfer in the excited singlet state of the molecule represented by (6.16) 2. molecular reorientation in methane crystal 3. internal rotation of CHj group in radical (6.25) 4. inversion of radical (6.40) 5. hydrogen transfer in halved molecule (6.16) 6. isomerization of molecule (6.17) in excited triplet state 7. tautomerization in the ground state of 7-azoindole dimer (6.1) 8. polymerization of formaldehyde in reaction (6.44) 9. limiting stage (6.45) of (a) chain hydrobromination, (b) chlorination and (c) bromination of ethylene 10. isomerization of radical (6.18) 11. abstraction of H atom by methyl radical from methanol matrix [reaction (6.19)] 12. radical pair isomerization in dimethylglyoxime crystals [Toriyama et al. 1977].
The selectivity and product composition is different from that obtained for direct chlorination. The selectivity of the r-butoxy radical is intermediate between that of chlorine and bromine atoms. The selectivity is also solvent- and temperature-dependent. [Pg.706]

The reaction of volatile chlorinated hydrocarbons with hydroxyl radicals is temperature dependent and thus varies with the seasons, although such variation in the atmospheric concentration of trichloroethylene may be minimal because of its brief residence time (EPA 1985c). The degradation products of this reaction include phosgene, dichloroacetyl chloride, and formyl chloride (Atkinson 1985 Gay et al. 1976 Kirchner et al. 1990). Reaction of trichloroethylene with ozone in the atmosphere is too slow to be an effective agent in trichloroethylene removal (Atkinson and Carter 1984). [Pg.211]

The rate of volatilization will also increase with an increase in temperature, ten Hulscher et al. (1992) studied the temperature dependence of Henry s law constants for three chlorobenzenes, three chlorinated biphenyls, and six polynuclear aromatic hydrocarbons. They observed that within the temperature range of 10 to 55 °C, Henry s law corrstant doubled for every 10 °C increase in temperature. This temperature relationship should be corrsidered when assessing the role of chemical volatilization from large surface water bodies whose temperatines are generally higher than those typically observed in groimdwater. [Pg.16]

Friesen, K.J. and Webster, G.R.B. Temperature dependence of the aqueous solubility of highly chlorinated dibenzo-/>dioxins, Environ. Sci. Technol, 24(1) 97-101, 1990. [Pg.1658]

Wang, T., and D. W. Margerum, Kinetics of Reversible Chlorine Hydrolysis Temperature Dependence and General Acid/Base-Assisted Mechanisms, Inorg. Chem., 33, 1050-1055 (1994). [Pg.348]

Nickolaisen, S. L., R. R. Friedl, and S. P. Sander, Kinetics and Mechanism of the CIO + CIO Reaction Pressure and Temperature Dependences of the Bimolecular and Termolecular Channels and Thermal Decomposition of Chlorine Peroxide, J. Phys. Chem., 98, 155-169(1994). [Pg.719]

The molecular structure of (64) may be considered as a pentagonal bipyramid with the naphthalene, the chlorine and two phosphorus atoms in the pentagonal plane. It is structurally related to (53) by a 45° rotation of the naphthalene unit about the Ta—Cl vector. The temperature dependent 1H and 31PNMR spectra indicate that such a process is operative in solution. The structural parameters suggest that the jr-accepting interaction is substantial this is consistent with the inertness of the Ta-naphthalene unit toward substitution. [Pg.683]

The energy density of liquid cathode lithium cells can be further enhanced to over 500 Wh/kg (1000 Wh/dm3) by the use of halogen additives. BrCl, added to lithium-thionyl chloride cells, boosts the OCV to 3.9 V and prevents the formation of sulphur in the early stages of discharge. D-sized cells are manufactured, Addition of chlorine to lithium-sulphur yl chloride cells increases the energy density and improves the temperature-dependent electrical characteristics. [Pg.141]

Friesen, K. J., and G. R. B. Webster, Temperature Dependence of the Aqueous Solubilities of Highly Chlorinated Dibenzo-p- Dioxins. Environ. Sci. Technol., 1990 24, 97-101. [Pg.137]

In addition to the dependences of the reaction constants on the local environment examined above, the dependence of the activation energy of Zr-Cl bond hydrolysis on the chemical environment of the chlorine atom was taken into account. This effect was considered to be responsible for the increased introduction of chlorine atoms into the growing film and was used for the explanation of the temperature dependence of the chlorine concentration in the deposited film. [Pg.510]

Fig. 9.16. Temperature dependence of the residual chlorine concentration in the growing film triangles are experimental points and diamonds are simulation results. Fig. 9.16. Temperature dependence of the residual chlorine concentration in the growing film triangles are experimental points and diamonds are simulation results.
The second (intermediate) fraction containing phenyltrichlorosilane, diphenyl and diphenyldichlorosilane is separated when the temperature of the tower top is 198-207 °C (the temperature depends on the composition of the raw stock and the pressure in the system) and residual pressure is 50-80 GPa. At the end of the separation of the intermediate fraction its chlorine content should not be lower than 27.3%, the density should not be lower than 1.214 g/cm3, and the 301-308 °C fraction content (diphenyldichlorosilane as such) should not be lower than 90%. The intermediate fraction can be sent for repeated rectification. [Pg.51]

In the absence of catalysts phenylchlorosilanes do not chlorinate even at increased temperature (150-200 °C). It should be kept in mind, however, that the replacement chlorination of phenylchlorosilanes depending on the conditions of the reaction (the presence of a catalyst and its composition, the effect time of chlorine, temperature) is accompanied by breaking up the Si—Car bond ... [Pg.89]

Chlorination in shaft furnaces allows one to extract almost all of titanium (97-98%) out of the furnace charge. The extraction degree of other oxides depends on the chlorination temperature and properties of the extracted component. E.g., if silicon dioxide is in the mixture in the form of quartz, its chlorination degree is 10-20% if silicon dioxide is part of silicate, it is clorinated by 80% and more. Aluminum oxide in the form of corundum chlorinates only slightly alumosilicates chlorinate almost completely. [Pg.391]


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Chlorine temperature

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