Chlorine and water

Phosphoms trichloride reacts readily with oxygen, sulfur, chlorine, and water. It serves as an intermediate in the production of phosphoms oxychloride, phosphoms sulfochloride, phosphoms pentachloride, and phosphonic (phosphorous) acids. PCl is also the raw material for the manufacture of dialkyl phosphonates,... 

Hypochlorous acid, preformed or generated in situ from chlorine and water, is employed in the manufacture of chlorohydrins (qv) from olefins, en route to epoxides, and in the production of chloramines (qv), especially chloroisocyanurates from cyanuric acid (see Cyanuric and isocyanuric acids). 

A chlorohydrin has been defined (1) as a compound containing both chloio and hydroxyl radicals, and chlorohydrins have been described as compounds having the chloro and the hydroxyl groups on adjacent carbon atoms (2). Common usage of the term appHes to aUphatic compounds and does not include aromatic compounds. Chlorohydrins are most easily prepared by the reaction of an alkene with chlorine and water, though other methods of preparation ate possible. The principal use of chlorohydrins has been as intermediates in the production of various oxitane compounds through dehydrochlorination. 

Ghlorohydrination in Chlorine and Water. The hypochlotination of propylene gives two isomers 90% l-chloro-2-propanol and 10% 2-chloro-1-propanol. 

From Allyl Alcohol. The reaction of allyl alcohol [107-18-6] with chlorine and water gives a mixture of glycerol m on ochl orohydrin s consisting of 73% 3-chloropropane-l,2-diol and 27% of 2-chloropropane-l,3-diol (57). In a recycle reaction system in which allyl alcohol is fed as a 4.5—5.5 wt % solution, chlorine is added at a rate of 7—9 moles per hour. The reaction time is about five seconds, the reaction temperature 50—60°C and the recycle ratio is 10—20 1. Under these conditions m on ochl orohydrin s have been obtained in 88% yield with 9% dichlorohydrins (58) (see Allyl ALCOHOL AND DERIVATIVES). 

Butyrchloral has been prepared by chlorination of acetaldehyde 2 and of paraldehyde. Butyrchloral hydrate has been prepared by treatment of a,j8-dichlorobutyraldehyde with chlorine and water.3 Butyrchloral has also been prepared4 by treatment of crotonaldehyde with hydrogen chloride followed by chlorination. Brown and Plump have used a procedure similar to the one described here.3... 

The statement that Mixtures of chlorine and water at certain concentrations are capable of explosion by spark ignition [1] should read Mixtures of chlorine and hydrogen [2],... 

Three equations describe the process. The first involves making the hypochlorous acid by reacting chlorine and water. In the second, the acid reacts with propylene to make chlorohydrin. The dehydirochlorination takes place in the third to give propylene oxide. 

Two of the reactions calce place in the same reactor in this plant. The formation of the hypochlorous acid (HOCl) from chlorine and water, and the reaction with propylene all occur simultaneously on the left in Figure 11—2. Propylene reacts readily with chlorine to form that unwanted by-product, propylene dichloride. To limit that, the HOCl and HCl are kept very dilute. But as a consequence, the concentration of the propylene leaving the reactor is very low—only 3—5% Ac any higher concentration, a separate phase or second layer in the reactor would form. It would preferentially suck up (dissolve) the propylene and chlorine coming in, leading to runaway dichloride yields. The low concentration levels of the propylene chlorohydrin and the need to recycle so many pounds of material is the reason the process is so energy intensive. It just takes a lot of electricity to pump all that stuff around. 

The epoxidation of propylene to propylene oxide is a high-volume process, using about 10% of the propylene produced in the world via one of two processes [127]. The oldest technology is called the chlorohydrin process and uses propylene, chlorine and water as its feedstocks. Due to the environmental costs of chlorine and the development of the more-efficient direct epoxidation over Ti02/Si02 catalysts, new plants all use the hydroperoxide route. The disadvantage here is the co-production of stoichiometric amounts of styrene or butyl alcohol, which means that the process economics are dependent on finding markets not only for the product of interest, but also for the co-product The hydroperoxide route has been practiced commercially since 1979 to co-produce propylene oxide and styrene [128], so when TS-1 was developed, epoxidation was looked at extensively [129]. 

What probably happens in the oxychlorination process is that chlorine is formed in situ. The reaction of hydrogen chloride and oxygen to give chlorine and water was discovered by Deacon in 1858. Once the chlorine is formed, it then adds to ethylene as in the direct chlorination mechanism. Cu ... 

Hydrogen chloride gas reacts with oxygen forming chlorine and water 4HC1 + 02 2CI2 + 2H2O A similar reaction occurs with hydrogen peroxide ... 

Nitrosyl chloride is oxidized by nitric acid to yield nitrogen dioxide, chlorine and water. 

Sodium inflow and acute excitotoxicity. Neurotoxicity of excitatory amino acids is a direct consequence of the excessive excitatory depolarization—may be related to a loss of the ionic homeostasis and/or to a depletion of the energetic stocks of the cell (Olney et al. 1986). Neuronal damage could depend on the extracellular presence of sodium accompanied by a passive flow of chlorine and water (Hablitz and Langmoen 1982). Some considerations suggest that the acute excitatory swelling does not explain completely the damages induced by excitatory amino acids (Pulsinelli et al. 1982). 

In the preparation of hypochlorous acid from chlorine and water, the yield is very low, on account of the small solubility of chlorine in water. The yield of HC10 can be increased either by adding an insoluble oxide or carbonate which forms a sparingly soluble chloride. 

In the system C12+H20, there are two components, just indicated two solid phases—ice and chlorine hydrate, C12.8H20 two soln.—one a soln. of water in an excess of chlorine, Sol. I, and a soln. of chlorine in an excess of water, Sol. II and a gas phase—a mixture of chlorine and water vapour in varying proportions. The system has not been completely studied, but sufficient is known to show that the equilibrium curves take the form shown diagrammatically in Fig. 20. The two invariant systems L and B have four coexisting phases—... 

Pour 2-3 ml of chlorine water into a test tube and add a sodium hydroxide solution dropwise. How can the vanishing of the colour and odour of the chlorine water be explained How does the alkali shift equilibrium in the reaction between chlorine and water State le Chatelier s principle. 

The first pentagonal bipyramidal complex of zinc, ZnLCl2 3H20, was reported in 1973, where L is the planar five-coordinate 2,6-diacetylpyridinebis(semicarbazone).346 The crystal structure determination shows the complex to contain the [LZnG(H2Q)]+ cation, with three bland two O-donor atoms forming a slightly distorted planar pentagon around the metal ion and the chlorine and water in axial positions. 

Hypoiodites. — The formation of hypoiodites is analogous to that of hypochlorites but the salts are known only in solution mixed with iodide. Again, like the hypochlorites, they change on heating they yield a mixture of iodide and iodate and from barium iodate iodic acid can be prepared. But it is more readily obtained by boiling iodine with nitric acid for iodine is more easily oxidised than either chlorine or bromine or chlorine and water may be used as an oxidising agent. 

Water. Some mixtures of chlorine and water can be ignited by a spark.31... 

Contrast the formation of chlorine hydrate with the action of chlorine and water in sunlight. 

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