Thermodynamic properties/chlorine

R. Kapoor and J. J. Martin, Thermodynamic Properties of Chlorine, University of Michigan, 1957. 

Physical Properties. Thionyl chloride [7719-09-7], SOCI2, is a colorless fuming Hquid with a choking odor. Selected physical and thermodynamic properties are Hsted in Table 6. Thionyl chloride is miscible with many organic solvents including chlorinated hydrocarbons and aromatic hydrocarbons. It reacts quickly with water to form HCl and SO2. Thionyl chloride is stable at room temperature however, slight decomposition occurs just... 

Chlorine dioxide, CIO2, is a greenish yellow gas having a pungent odor that is distinctive from that of chlorine. Liquid chlorine dioxide has a deep red color and is explosive at temperatures above —40° C. Selected physical and thermodynamic properties of chlorine dioxide are given in Table 1. 

Table 1. Physical and Thermodynamic Properties of Chlorine Dioxide ...

Liu, K., Dickhut, R.M. (1994) Saturation vapor pressures and thermodynamic properties of benzene and selected chlorinated benzenes at environmental temperatures. Chemosphere 29, 581-589. 

Thermodynamic properties for explosion calculations are presented for major organic chemical compounds. The thermodynamic properties include enthalpy of formation, Gibbs free energy of formation, internal energy of formation and Helmholtz free energy of formation. The major chemicals include hydrocarbon, oxygen, nitrogen, sulfur, fluorine, chlorine, bromine, iodine and other compound types. 

IV. Appendix Tables of Thermodynamic Properties for Some Chlorine Oxyfluorides. ... 

In addition to a discussion of the individual compounds, a section was added correlating the physical and chemical properties of the chlorine oxyfluorides with their structure. In the Appendix, full tables of thermodynamic properties are given for each compound, where known. 

CC12FCC1F2. These compounds are non-toxic and non-flammable, and their thermodynamic properties are ideally suited for the compression/ expansion cycle in cooling and heat pump appliances. However, CFCs are chemically very inert, so when they are vented into the atmosphere, they do not react with atmospheric constituents. They diffuse unscathed first into the troposphere, then penetrate slowly into the stratosphere. There, the solar UV radiation photodissociates these compounds, liberating free chlorine atoms (the C-Cl bond is weaker than the C-F bond). The chlorine atoms react with atmospheric O3 to form chlorine oxide, which in turn reacts with atmospheric atomic oxygen regenerating chlorine atoms ... 

L. V. Gurvich, I. V. Veyts, and C. B. Alcock, Thermodynamic Properties of Individual Substances, Vol. 1 Elements Oxygen, Hydrogen (Deuterium, Tritium), Fluorine, Chlorine, Bromine, Iodine, Helium, Neon, Argon, Krypton, Xenon, Radon, Sulfur, Nitrogen, Phosphorus, and Their Compounds, Pt. 1 Methods and Computation, Hemisphere, New York, 1989. 

There are no reported experimental studies leading to the heat of formation of SlH2F(g). We estimate this value via a linear interpolation between the established A H°(298.15 K) values of SiH (g) and SiF (g) (1 ). The reasonableness of this approach has been demonstrated by Lapidus et al. (2 ), Hunt and Sirtl (3 ), and Seiter and Sirtl (4). Lapidus et al. (2 ) examined the trends in the thermodynamic properties of halogenated silanes and methanes. Hunt and Sirtl (3 ) and Seiter and Sirtl (4) studied the chlorinated silanes and proposed a linear relationship within the sequence SiH (g) to SiCl (g). 

Whereas the composition of dissolved main solid compounds in seawater is rather constant all over the oceans, the freshwater in the Baltic Sea outbalanced by river discharge is dominated by calcium bicarbonate. For this reason, significant anomalies are observed in Baltic waters from the standard composition of seawater (Nehring and Rohde, 1966), in particular in the brackish surface water, with amount increasing toward the eastern and northern margins of the Baltic Sea. Directly measured densities of Baltic water compared with density determined from the seawater equation of state with Baltic water salinity measured by chlorinity titration resulted in a deviation of up to 0.123 kg/m (Millero and Kremling, 1976). This may result in uncertainties in estimating the thermodynamic properties of Baltic water, for example, the vertical stability. 

Metallurgical, materials, ceramic and chemical engineers worldwide will welcome this new compilation of thermochemical data by Professor Barin. Here they will find the most comprehensive tables yet available for the thermodynamic properties of pure substances as a function of temperature at 100° intervals. Almost twenty-four hundred substances are included - the elements, and compounds of two, three, and four elements. The vast majority of substances are inorganic, but Dr. Barin has included a generous selection of the more common hydrocarbons, carbohydrates, and a few chlorinated hydrocarbons. The format of the tables conforms to that of the JANAF tables, and SI units are employed. 

Chlorofluorocarbons have unique chemical and thermodynamic properties that make them very attractive for a wide variety of applications, ranging from refrigeration and air conditioning to foam blowing and medical sterilants. Unfortunately, as mounting evidence shows, their inertness allows CFCs to be transported to the stratosphere, where their photolysis releases chlorine atoms that participate in catalytic ozone destruction. Consequently, the manufacture and use of these compounds is being phased out. 

The use of halogenated monomers or reactive intermediates can bring about a lowering of heat of combustion. For example, heat capacity and heat of combustion have been determined for copolymers of styrene with polyesters whose thermodynamic properties were known introduction of chlorine into the polyester molecule lowered the heat of combustion. The temperatures of self-ignition of polyesters containing 17.5% and 23.7% chlorine were 580 and 650 °C, respectively. 

FIGURE J5. Density of saturated liquid chlorine. (R.M. Kapoor and J.J. Martin, Thermodynamic Properties of Chlorine, Engineering Research Institute, University of Michigan, Ann Arbor, MI (1957).)... 

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