Chlorine liquid

CH3CHCICH2CI. Colourless liquid with a pleasant odour b.p. 96 C, Manufactured by treating liquid chlorine with an excess of liquid propene. It is very similar in properties to ethylene dichloride, and is used for similar purposes. 

Liquid chlorine dioxide, ClOj, boils at 284 K to give an orange-yellow gas. A very reactive compound, it decomposes readily and violently into its constituents. It is a powerful oxidising agent which has recently found favour as a commercial oxidising agent and as a bleach for wood pulp and flour. In addition, it is used in water sterilisation where, unlike chlorine, it does not produce an unpleasant taste. It is produced when potassium chlorate(V) is treated with concentrated sulphuric acid, the reaction being essentially a disproportionation of chloric(V) acid ... 

Chlorine is produced as a gas that is used captively, transferred to customers via pipeline, or Hquefied. Liquid chlorine, of higher purity than gaseous chlorine, is either used internally by the producers or marketed. The percentage of U.S. chlorine gas production subsequently Hquefied has increased over the past ten years reflecting higher demand for high purity chlorine. This percentage was 60.7% in 1978 and 81.1% in 1987 (5). The majority of this chlorine is consumed captively. 

Fig. 33. Vapor pressure of liquid chlorine as a function of temperature (78).

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. 

Caustic scrubber systems should be installed to control chlorine emissions from condensers and at storage and transfer points for liquid chlorine. 

As a liquid, chlorine is amber colored and is 1.44 times heavier than water. In solid form, it exists as rhombic crystals. Various properties of chlorine are given in Table 2. 

Chlorine dioxide is a yellow-green gas and soluble in water at room temperature to about 2.9 g/1 chlorine dioxide (at 30 mm mercury partial pressure) or more than 10 g/1 in chilled water. The boiling point of liquid chlorine dioxide is 11° C the melting point is - 59° C. Chlorine dioxide gas has a specific gravity of 2.4. The oxidant is used in a water solution and is five times more soluble in water than... 

Frank, W. L. (1995). Evaluation of a Containment Building for a Liquid Chlorine Unloading Facility. Proceedings of the 29th Annual Loss Prevention Symposium, July 30-August 2, 1995, Boston, MA, ed. E. D. Wixom and R. P. Benedetti, Paper 5b. New York American Institute of Chemical Engineers. 

A liquid chlorine tank was kept cool by a refrigeration system that used CFCs. In 1976 the local management decided to use ammonia instead. Management w as unaware that ammonia and chlorine react to form explosive nitrogen trichloride. Some of the armnonia leaked into the chlorine, and the nitrogen trichloride that was formed exploded in a pipeline... 

In one incident paraffin wax and chlorine were reacted at atmospheric pressure. Some paraffin traveled from the reactor back up the chlorine line and reacted with liquid chlorine in a catchpot, which exploded with great violence. Bits were found 30 m away [3]. 

The Rijnmond area is that part of the Rhine delta between Rotterdam and the North Sea. The Commission for the Safety of the Population at large (COVO) commissioned the study for six chemicals and the operations associated with them acrylonitrile, liquid ammonia, liquid chlorine, LNG, propylene, and part of a separation process (diethanolamine stripper of a hydrodesulfurizer). The study objectives were to evaluate methods of risk assessment and obtain experience with practical applications of these methods. The results were to be used to decide to what extent such methods can be used in formulating safety policy. The study was not concerned with the acceptability of risk or the acceptability of risk reducing measures. 

I2CI6 is readily made as a bright-yellow solid by reaction of I2 with an excess of liquid chlorine at —80° followed by the low-temperature evaporation of the CI2 care must be taken with this latter operation, however, because of the very ready dissociation of bClg into ICl and CI2. 

Calcium chloride solutions Sodium chloride solutions COj liquid Chlorine liquid Methanol solutions Ethanol solutions Ethylene glycol solutions... 

Standard materials for handling dry gases include for chlorine, UNS N10276 (type stainless steel is used for liquid chlorine) for bromine, UNS N10276 (below 60°C) ... 

Halogens Although tantalum is severely attacked by flourine at room temperature it does not react with liquid chlorine, bromine and iodine up to 150°C and the metal suffers no appreciable attack in wet or dry bromine, chlorine and iodine below 250°C. It is virtually uncorroded by hydrogen bromide and hydrogen chloride below 370°C, attack starting at about 375 and 410°C respectively. 

The mean value of k for a large number of liquids is 2 12 liquids containing hydroxyl groups, or those which have an enolic modification, liquid chlorine, fused salts, and metals, have much smaller values of k, and this is attributed to polymerisation, since if the actual molecular weight is larger than that assumed in calculating V , the latter value will also be smaller. Ramsay and Aston (1894) assumed that it will be proportionally smaller, but the values of the polymerisation coefficients thereby deduced obviously depend on the formula assumed for the polymerised molecule, and are therefore arbitrary. 

The heat flux measured during the reaction was integrated. The heat of reaction at - 10°C has thus been calculated as 2.84 kcal/gr-mol "product BrCl". Since for each mole of BrCl 0.5 moles chlorine needed to be condensed and cooled from room temperature, releasing a heat of 2.54 kcal/gr-mol, the heat of reaction from liquid chlorine at the same temperature would be 0.3 kcal/gr-mol "product BrCl". For the degree of dissociation quoted above, i.e. 48 %, the heat of reaction in the liquid phase is obtained as 0.6 kcal/gr-mol, in conformance with the data in (ref. 2). 

Due to the large contribution of the condensation of chlorine to the heat of the reaction, the heat of reaction and the kinetics may require further study under pressure, with liquid chlorine as one of the reagents. 

Chlorine has caused numerous accidents with metals. Beryllium becomes incandescent if it is heated in the presence of chlorine. Sodium, aluminium, aluminium/titanium alloy, magnesium (especially if water traces are present) combust in contact with chlorine, if they are in the form of powder. There was an explosion reported with molten aluminium and liquid chlorine. The same is true for boron (when it is heated to 400°C), active carbon and silicon. With white phosphorus there is a detonation even at -34°C (liquid chlorine). 

Liquid chlorine in contact with powdered vanadium causes the mixture to detonate. 

Tin burns in fluorine at 100°C whereas there was a spontaneous ignition of the metal when it was put in contact with liquid chlorine at -34 C. 

Liquid chlorine and glycerine were heated in a steel bomb at 70-80 C, which detonated. 

When dibutyl phthaiate is treated with liquid chlorine at 118°C in a steel bomb, it gives rise to an explosive reaction. 

STABREX Stabilized Liquid Bromine9 is far more stable than liquid chlorine bleach. For example, several tons of the new product were shipped to India and stored for one year above 90 °F. The product remained within specification (less than 10% degraded) for the entire year, after which it was successfully used to control fouling in an industrial water system. Chlorine would have completely degraded in this time under these conditions. Chemical wastage was eliminated. Accident risk in transporting oxidant was reduced because less volume was necessary. Table 2 shows the stability of the new product compared to industrial strength chlorine bleach in well-controlled laboratory tests. 

Liquid chlorine is unloaded from rail tankers into a storage vessel. To provide the necessary NPSH, the transfer pump is placed in a pit below ground level. Given the following information, calculate the NPSH available at the inlet to the pump, at a maximum flow-rate of 16,000 kg/h. 

A horizontal, cylindrical, storage tank, 3 m diameter, 12 m long, used for liquid chlorine at 10 bar, material carbon steel. 

A horizontal, cylindrical, tank, with hemispherical ends, is used to store liquid chlorine at 10 bar. The vessel is 4 m internal diameter and 20 m long. Estimate the minimum wall thickness required to resist this pressure, for the cylindrical section and the heads. Take the design pressure as 12 bar and the allowable design stress for the material as 110 MN/m2. 

Mixtures of aluminium powder with liquid chlorine, dinitrogen tetraoxide or tetran-itromethane are detonable explosives, but not as powerful as aluminium-liquid oxygen mixtures, some of which exceed TNT in effect by a factor of 3 to 4 [1], Mixtures of the powdered metal and various bromates may explode on impact, heating or friction. Iodates and chlorates act similarly [2], Detonation properties of gelled slurries of aluminium powder in aqueous nitrate or perchlorate salt solutions have been studied [3], Reactions of aluminium powder with potassium chlorate or potassium perchlorate have been studied by thermal analysis [4],... 

The finely powdered element inflames in gaseous chlorine or liquid chlorine at —33°C [1]. The latter is doubtful [2],... 

Combinations of liquid chlorine trifluoride with several halocarbons except perfluo-rohexane exploded immediately when suddenly mixed at all temperatures between 25° and — 70°C. Poly(chlorotrifluoroethylene), below See Carbon tetrachloride, Fluorinated solvents, both above... 

Interaction of liquid chlorine pentafluoride with ice at — 100°C [1], or of the vapour with water vapour above 0°C [2], is extremely vigorous. 

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