Chlorides hydrogen

Hydrogen chloride may be conveniently prepared by heating sodium chloride with sulphuric acid NaCl + H2SO4 NaHS04 + HCl 

When this reaction has occuiTcd accidentally sufficient hydrogen chloride has been liberated to explosively burst the vessel. The purest form of hydrogen chloride is made by the action of water on silicon tetrachloride  

Commercially, hydrogen chloride is obtained either as a by-product in the manufacture of salt cake from sodium chloride, or by allowing chlorine produced as a by-product in electrolytic processes to react with hydrogen in the presence of activated charcoal. It is also formed as a byproduct in the manufacture of phenol. 

The gas is essentially inert to common materials of construction such as stainless steel under normal conditions of use. Platinum and gold are also not attacked by pure hydrogen chloride. 

In the presence of moisture, however, most metals are coiToded and it is advised that the proposed use and pressures are discussed with the supplier so that suitable construction materials are established prior to installation. Hydrogen chloride neither burns nor supports combustion. 

Hydrogen chloride. White atom is hydrogen and green atom is chlorine, publishers RESOURCE CROUP 

Hydrogen chloride was studied by the famous alchemist Basil Valentine (c. 1394- ), who gave it the name spiritus salis ( the spirit of salt ) by which it was known to most alchemists. 

Hydrochloric acid has traditionally been known as muriatic acid, a name that is still sometimes used by workers in fields in which it is used. 

ALCHEMY An ancient field of study from which the modern science of chemistry evolved. 

AQUEOUS A solution is one that consists of some material dissolved in water. 

The 2003 ACGIH ceiling-threshold limit value (C-TLV) for hydrogen bromide is 3 ppm (9.9mg/m ). 

ACGIH Hydrogen bromide. Documentation of the TLVs and BEIs, 7th ed, 2pp. Cincinnati, OH, American Conference of Governmental Industrial Hygienists, 2pp, 2001 

Basilico S, Garlanda T Criteria Document for Hydrogen Bromide, pp 1-16. 2985 Luxembourg, Grand Duchy of Luxembourg, Office for Official Publications of the European Communities, 1993 

Alexandrov DD Bromine and compounds. In International Labor Office Encyclopaedia of Occupational Health and Safety, 3rd ed, rev, Vol I, A-K. p 327. Geneva, 1983 

Public Health Service Registry of Toxic Effects of Chemical Substances (RTECS). Vol 3, p 2717. Department of Health and Human Services, Public Health Service, Washington, DC, US Gkjvemment Printing Office, April 1987 

DOT Proper Shipping Name Hydrogen chloride, anhydrous 

Hydrogen chloride, refrigerated liquid DOT Classification 2.3, Hazard Zone C (Gas poisonous by inhalation) 

Hydrogen chloride, refrigerated liquid TC Classification 2.3, 8 TC Label POISON GAS, CORROSIVE UN Number UN 1050 (for compressed gas) 

Anhydrous hydrogen chloride is a colorless gas that fumes strongly in moist air and has a highly irritating effect on body tissues. It has a sharp, suffocating odor and is shipped in cylinders as a liquefied compressed gas under its vapor pressure of 613 psig at 70°F (4230 kPa at 2LUC). 

Chemically, hydrogen chloride is relatively inactive and noncorrosive in the anhydrous state. However, it is readily absorbed by water to yield the highly corrosive hydrochloric (muriatic) acid. It also dissolves readily in alcohol and ether and reacts rapidly (violently, in some cases) with many organic substances. At high temperatures (3240°F or 1782°C and above), hydrogen chloride tends to dissociate into its constituent elements. 

The photochemical and thermal decompositions of this compound have received very little attention. Most kinetic data have come from studies of the synthesis and chlorine and hydrogen atom reactions. 

The hydrogen-chlorine chain reaction has proved to be one of the most controversial systems yet studied. After thirty years of investigation Bodenstein43 was able to say in 1931 that every worker on the photochemical synthesis of HC1 had produced his own mechanism even as late as 1940 little positive information had been obtained. However, the accumulated techniques and experience had firmly established the importance of atom chain reactions. The mechanism of photo-initiation and propagation is the same as for the hydrogen bromide photosynthesis, a non-branching chain reaction 

The complications which arose in the early photochemical work were due to the presence of impurities in the reactants, notably oxygen, NC13 and water which aided chain initiation or termination. In thermal reactions wall effects were in evidence. 

Ashmore and Chanmugam44 were the first workers to determine accurate Arrhenius parameters for the propagation reaction (21) in their study of the effects of NO and NOC1 as sensitiser of the H2-C12 chain reaction. They found k21 (250°) = 4.8 0.4 x 108 I.mole-1.sec 1 and E21 = 5.50 kcal.mole-1. 

Steiner and Rideal45 determined the Arrhenius parameters for (22), log k22 = 10.86 — 5200/4.58 T, from a study of the HCl-catalysed ortho-para hydrogen reaction in the temperature range 600-770°. When allowance is made for the better data for the hydrogen dissociation available to Steiner and Rideal, their results agree well with earlier work by Rodebush and Klingelhoefer46. 

Preparation. Perform the experiment in a fume cupboard]) Assemble an apparatus as shown in Fig. 53a, substituting a U-tube for tlie wash bottles. Place 10-15 g of sodium chloride into the reaction flask, and anhydrous calcium chloride in the U-tube. Pour 20-25 ml of a 70% sulphuric acid solution into the flask via the funnel, and see that the end of the funnel tube is submerged in the liquid. Fill a dry thick-walled 25-50-ml bottle with the evolving hydrogen chloride. How can you tell that the bottle is filled  

Dissolution in Water. Close the bottle containing hydrogen chloride with a stopper provided with a capillary facing inward. Invert the bottle with the gas and immerse its neck in a bath with water (see Fig. 53b). Explain what occurs. 

What is the solubility of hydrogen chloride in water What is the composition of an azeotropic mixture of hydrochloric acid with water What is called an azeotropic mixture of liquids and how does it differ from the pure liquids  

Why are dry sodium chloride and concentrated sulphuric acid taken when preparing hydrogen chloride How is hydrochloric acid produced in the industry  

What is the percent concentration of commercial hydrochloric acid  

Kirk-Othmer Encyclopedia of Chemical Technology (4th Edition) 

The entropy value of gaseous HCl is a sum of contributions from the various transitions summarized in Table 4. Independent calculations based on the spectroscopic data of H Cl and H Cl separately, show the entropy of HCl at 298 K to be 186.686 and 187.372 J/(mol K) (44.619 and 44.783 cal/(mol K), respectively. The low temperature (rhombic) phase is ferroelectric (6). SoHd hydrogen chloride consists of hydrogen-bonded molecular crystals consisting of zigzag chains having an angle of 93.5° (6). Proton nmr studies at low temperatures have also shown the existence of a dimer (HC1)2 (7). 

Temperature dependence of viscosity of the gas over a wide range of temperatures is given by equation 1 where Tis in Kelvin and T q is the value of Ti at 273 K. 

Gaseous diffusion and thermal diffusion data may be found in References 8 and 9. 

An increasing activation energy with decreasing temperature was noted in mixtures with mole fractions of HCl equal to 0.10 and 0.20 [118]. The linearity assumption was used to calculate values of ftnci Ar and 

These results conflict with measurements made of the dissociation rate in pure HCl at lower temperatures by recording the visible emission from the radiative recombination of chlorine atoms [119]. The rate coefficients were consistent with those calculated from the strict Arrhenius equation with a low activation energy of 70 kcal mole ,  

It was also concluded that the efficiency of HCl was no different than that of Ar with respect to the HCl decomposition process. 

The complexity introduced by including reactions (15)—(19) precludes the analysis of the entire density gradient oscillogram as was done for homonuclear dissociations. The determination of atomic efficiencies for heteronuclear decompositions is not possible using the laser-beam deflection technique. 

The large discrepancy between the bond dissociation and the activation energy has been attributed to the effect of vibration—vibration transfer [2]. According to one calculation, the absence of vibration—vibration transfer results in a calculated value of the activation energy close to 90 kcal mole . Inclusion of vibration—vibration transfer in the calculation yields values of fej that are in good agreement with the experimental data [1]. 

To obtain a precise value for the wave-number of the fundamental vibration of 

We use the same experimental data as in problem 28. These are given in table 1. 

We plot P (/) + J (7 — 1) against / in fig. 1 and draw a straight line through the points. From the intercept at / = 0 we deduce 

Chemical Name Synonyms Chemical Formula CAS number Molecular Weight Boiling point Melting point Triple point temperature Vapor pressure Absolute density Relative density Critical temperature Critical pressure Critical volume Critical density 

Critical compressibility factor 0.266 Latent heat of fusion (-114.2°C) 1991 J/gmole 

Refractive index (25°C, 1 atm) 1.000408 Dielectric constant (0°C, 1 atm) 1.0046 Free energy of formation  

Coughing, choking, pulmonary edema. Nas ulceration, bronchitis, pneumonia, and headache result from high concentrations. Higher concentrations may cause necrosis of the tracheal and bronchial epithelium, emphysema, and lesions of liver and other organs. 

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HYDROGEN CHLORIDE S TlSOE-t OI -6 6165E>02 9.7100E-03 -S.0306E400... 

The preference is for a process based on ethylene rather than the more expensive acetylene and chlorine rather than the more expensive hydrogen chloride. Electrolytic cells are a much more convenient and cheaper source of chlorine than hydrogen chloride. In addition, we prefer to produce no byproducts. 

In summary, path 2 from Example 2.1 is the most attractive reaction path if there is a large market for hydrogen chloride. In practice, it tends to be difficult to sell the large quantities of hydrogen chloride produced by such processes. Path 4 is the usual commercial route to vinyl chloride. 

The b3TJroduct, DCD, is not required for this project. Hydrogen chloride can be sold to a neighboring plant. Assume at this stage that all separations can be carried out by distillation. The normal boiling points are given in Table 4.1. 

Again, in practice, there is likely to be a trace of chlorine in the reactor effluent. This can be recycled to the reactor with the unreacted decane or allowed to leave with the hydrogen chloride byproduct (providing this meets with the byproduct specification). 

If the hydrogen chloride cannot be sold, it must be disposed of somehow. Alternatively, it could be converted back to chlorine via the reaction... 

Can the byproduct be subjected to further reaction and its value upgraded For example, most organic chlorination reactions produce hydrogen chloride as a byproduct. If this cannot be sold, it... 

Consider vinyl chloride production (see Example 2.1). In the oxychlorination reaction step of the process, ethylene, hydrogen chloride, and oxygen are reacted to form dichloroethane ... 

Present in citronella and valerian oils, tur penline, ginger, rosemary and spike oils. It is produced artificially by the elimination of hydrogen chloride from bornyl chloride (artifi cial camphor) or from isobornyl chloride, by the dehydrogenation of borneol and isobor-neol and by the action of elhanoic anhydride on bornylamine. Chiral. 

CaHjNCO, PhNCO. A pungent lachrymatory almost colourless liquid m.p. — 33 "C, b.p. 162°C. Used as a dehydrating agent and for characterization of alcohols. Prepared from aniline and phosgene in the presence of hydrogen chloride. 

By oxidation with permanganate it forms pinonic acid, C,oH,<503, a monobasic acid derived from cyclobutane. With strong sulphuric acid it forms a mixture of limonene, dipentene, terpinolene, terpinene, camphene and p-cymene. Hydrogen chloride reacts with turpentine oil to give CioHijCl, bomyl chloride, artificial camphor . 

Hydrogen chloride released dissolves in water during condensation in the crude oil distillation column overhead or in the condenser, which cause corrosion of materials at these locations. The action of hydrochloric acid is favored and accelerated by the presence of hydrogen sulfide which results in the decomposition of sulfur-containing hydrocarbons this forces the refiner to inject a basic material like ammonia at the point where water condenses in the atmospheric distillation column. 

Margottin-Maclou M, Doyennette L and Henry L 1971 Relaxation of vibrational energy in carbon monoxide, hydrogen chloride, carbon dioxide and nitrous oxide App/. Opt. 10 1768-80... 

Covalent bonding, in all the cases so far quoted, produces molecules not ions, and enables us to explain the inability of the compounds formed to conduct electricity. Covalently bonded groups of atoms can, however, also be ions. When ammonia and hydrogen chloride are brought together in the gaseous state proton transfer occurs as follows ... 

Bonds with characteristics intermediate between ionic and covalent can also be represented by, for example, two imaginary structures, I and II both of which contrihute to the true structure III. Consider gaseous hydrogen chloride ... 

A/13 twice the bond energy of hydrogen chloride (twice since two moles of hydrogen chloride are produced). 

A/14 the enthalpy of reaction, which is in this case twice the enthalpy of formation of hydrogen chloride. Clearly A/14 is the difference between the total bond energies of the products and the total bond energies ol the reactants, lhat is... 

Let us consider the formation of sodium chloride from its elements. An energy (enthalpy) diagram (called a Born-Haber cycle) for the reaction of sodium and chlorine is given in Figure 3.7. (As in the energy diagram for the formation of hydrogen chloride, an upward arrow represents an endothermic process and a downward arrow an exothermic process.)... 

An acid was once defined simply as a substance which produces hydrogen ions, or protons. However, the simple proton, H , is never found under ordinary conditions, and this definition required amendment. Bronsted and, independently, Lowry, therefore redefined an acid as a susbstance able to donate protons to other molecules or ions, and a base as a substance capable of accepting such protons. If we consider hydrogen chloride, HCl, as an example, the HCl molecule is essentially covalent, and hydrogen chloride (gas or liquid) contains no protons. But anhydrous hydrogen chloride in benzene will react with anhydrous ammonia ... 

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