Partial pressure of acetone at different temperatures. Coefficients of dependences of pressures of saturated vapors of components on temperature
What is acetone? The formula of this ketone is considered in the school chemistry course. But not everyone has an idea of how dangerous the smell of this compound is and what properties this organic substance has.
Features of acetone
Technical acetone is the most common solvent used in modern construction. Since this compound has a low level of toxicity, it is also used in the pharmaceutical and food industries.
Technical acetone is used as a chemical raw material in the production of numerous organic compounds.
Doctors consider it a narcotic substance. When inhaling concentrated acetone vapors, serious poisoning and damage to the central nervous system are possible. This compound poses a serious threat to the younger generation. Drug users who use acetone vapor to induce a state of euphoria are at great risk. Doctors fear not only for the physical health of children, but also for their mental state.
A dose of 60 ml is considered lethal. When a significant amount of ketone enters the body, loss of consciousness occurs, and after 8-12 hours - death.
Physical properties
Under normal conditions, this compound is in a liquid state, has no color, and has a specific odor. Acetone, the formula of which is CH3CHNOCH3, has hygroscopic properties. This compound is miscible in unlimited quantities with water, ethyl alcohol, methanol, chloroform. It has a low melting point.
Features of use
Currently, the scope of acetone is quite wide. It is rightfully considered one of the most popular products used in the creation and production of paints and varnishes, in finishing works, in the chemical industry, and in construction. Increasingly, acetone is used to degrease fur and wool, to remove wax from lubricating oils. It is this organic substance that painters and plasterers use in their professional activities.
How to save acetone, whose formula is CH3COCH3? In order to protect this volatile substance from the negative effects of ultraviolet rays, it is placed in plastic, glass, metal bottles away from UV.
The room where a significant amount of acetone is supposed to be placed must be systematically ventilated and high-quality ventilation installed.
Features of chemical properties
This compound got its name from the Latin word "acetum", meaning "vinegar" in translation. The fact is that the chemical formula of acetone C3H6O appeared much later than the substance itself was synthesized. It was obtained from acetates and then used to make glacial synthetic acetic acid.
Andreas Libavius is considered the discoverer of the compound. At the end of the 16th century, by dry distillation of lead acetate, he managed to obtain a substance whose chemical composition was deciphered only in the 30s of the 19th century.
Acetone, whose formula is CH3COCH3, was obtained by coking wood until the beginning of the 20th century. After the increase in demand during the First World War for this organic compound, new methods of synthesis began to appear.
Acetone (GOST 2768-84) is a technical liquid. In terms of chemical activity, this compound is one of the most reactive in the class of ketones. Under the influence of alkalis, adol condensation is observed, as a result of which diacetone alcohol is formed.
During pyrolysis, ketene is obtained from it. In reaction with hydrogen cyanide, acetone cyanidanhydrin is formed. Propanone is characterized by the substitution of hydrogen atoms for halogens, which occurs at elevated temperatures (or in the presence of a catalyst).
How to get
At present, the majority of the oxygen-containing compound is obtained from propene. Technical acetone (GOST 2768-84) must have certain physical and operational characteristics.
The cumene method consists of three stages and involves the production of acetone from benzene. First, cumene is obtained by alkylating it with propene, then the resulting product is oxidized to hydroperoxide and split under the influence of sulfuric acid to acetone and phenol.
In addition, this carbonyl compound is obtained by the catalytic oxidation of isopropanol at a temperature of about 600 degrees Celsius. The accelerators of the process are metallic silver, copper, platinum, nickel.
Among the classical technologies for the production of acetone, the direct oxidation of propene is of particular interest. This process is carried out at elevated pressure and the presence of bivalent palladium chloride as a catalyst.
You can also get acetone by fermenting starch under the influence of the bacteria Clostridium acetobutylicum. In addition to the ketone, butanol will be present among the reaction products. Among the disadvantages of this option for obtaining acetone, we note an insignificant percentage yield.
Conclusion
Propanone is a typical representative of carbonyl compounds. Consumers are familiar with it as a solvent and degreaser. It is indispensable in the manufacture of varnishes, medicines, explosives. It is acetone that is part of the glue for film, is a means for cleaning surfaces from mounting foam and superglue, a means for washing injection engines and a way to increase the octane number of fuel, etc.
In practice, numerous solutions are widely used, consisting of two or more liquids that are readily soluble in each other. The simplest are mixtures (solutions) consisting of two liquids - binary mixtures. The patterns found for such mixtures can also be used for more complex ones. Such binary mixtures include: benzene-toluene, alcohol-ether, acetone-water, alcohol-water, etc. In this case, the vapor phase contains both components. The saturated vapor pressure of the mixture will be the sum of the partial pressures of the components. Since the transition of a solvent from a mixture to a vapor state, expressed by its partial pressure, is the more significant, the greater the content of its molecules in solution, Raoult found that “the partial pressure of a saturated vapor of a solvent over a solution is equal to the product of the pressure of saturated vapor over a pure solvent at the same temperature to its mole fraction in solution":
Where 
is the saturated vapor pressure of the solvent over the mixture; 
is the pressure of saturated vapor over a pure solvent; N is the mole fraction of the solvent in the mixture.
Equation (8.6) is a mathematical expression of Raoult's law. To describe the behavior of a volatile solute (the second component of a binary system), the same expression is used:
.
(8.7)
The total saturated vapor pressure over the solution will be (Dalton's law):
The dependence of the partial and total vapor pressure of the mixture on its composition is shown in fig. 8.3, where the pressure of saturated vapors is plotted on the ordinate axis, and the composition of the solution in mole fractions is plotted on the abscissa axis. At the same time, along the abscissa axis, the content of one substance (A) decreases from left to right from 1.0 to 0 mole fractions, and the content of the second component (B) simultaneously increases from 0 to 1.0 in the same direction. For any given composition, the total saturation vapor pressure is equal to the sum of the partial pressures. The total pressure of the mixture varies from the saturation vapor pressure of one individual liquid 
up to the saturated vapor pressure of the second pure liquid 
.
Raoult's and Dalton's laws are often used to evaluate the fire hazard of mixtures of liquids.
Mixture composition, mole fractions
Rice. 8.3 Diagram composition of the solution - saturation vapor pressure
Usually the composition of the vapor phase does not match the composition of the liquid phase and the vapor phase is enriched in the more volatile component. This difference can also be depicted graphically (the graph looks similar to the graph in Fig. 8.4, only the pressure is taken on the y-axis, not the temperature).
In diagrams representing the dependence of boiling points on composition (diagram composition - boiling point rice. 8.4), it is customary to build two curves, one of which relates these temperatures to the composition of the liquid phase, and the other to the composition of the vapor. The lower curve refers to liquid compositions (liquid curve) and the upper curve to vapor compositions (vapour curve).
The field enclosed between the two curves corresponds to a two-phase system. Any point in this field corresponds to the equilibrium of two phases - solution and saturated vapor. The composition of the equilibrium phases is determined by the coordinates of the points lying at the intersection of the isotherm passing through the curves and the given point.
At a temperature t 1 (at a given pressure), a liquid solution of composition x 1 will boil (point a 1 on the liquid curve), a vapor in equilibrium with this solution has a composition x 2 (point b 1 on the steam curve).
Those. liquid composition x 1 will correspond to vapor composition x 2 .
Based on the expressions: 
,
,
,
,
the relationship between the composition of the liquid and vapor phases can be expressed by the relationship:
.
(8.9)
Rice. 8.4. Composition-boiling point diagram for binary mixtures.
The real saturated vapor pressure of an individual liquid at a given temperature is a characteristic value. There are practically no liquids that would have the same saturation vapor pressure at the same temperature. That's why 
always more or less 
. If 
>
, That 
>
, i.e. the composition of the vapor phase is enriched with component A. Studying solutions, D.P. Konovalov (1881) made a generalization called Konovalov's first law.
In a binary system, vapor, in comparison with the liquid in equilibrium with it, is relatively richer in those of the components, the addition of which to the system increases the total vapor pressure, i.e. lowers the boiling point of the mixture at a given pressure.
Konovalov's first law is the theoretical basis for the separation of liquid solutions into their original components by fractional distillation. For example, a system characterized by point K consists of two equilibrium phases, the composition of which is determined by points a and b: point a characterizes the composition of saturated vapor, point b characterizes the composition of the solution.
According to the graph, it is possible to compare the compositions of the vapor and liquid phases for any point contained in the plane between the curves.
Real solutions. Raoult's law is not fulfilled for real solutions. There are two types of deviation from Raoult's law:
the partial pressure of solutions is greater than the pressures or vapor volatility of ideal solutions. The total vapor pressure is greater than the additive value. Such deviations are called positive, for example, for mixtures (Fig. 8.5 a, b) CH 3 COCH 3 -C 2 H 5 OH, CH 3 COCH 3 -CS 2, C 6 H 6 - CH 3 COCH 3, H 2 O- CH 3 OH, C 2 H 5 OH-CH 3 OCH 3 , CCl 4 -C 6 H 6 and others;
b
Rice. 8.5. The dependence of the total and partial vapor pressures on the composition:
a - for mixtures with a positive deviation from Raoult's law;
b - for mixtures with a negative deviation from Raoult's law.
the partial pressure of solutions is less than the vapor pressure of ideal solutions. The total vapor pressure is less than the additive value. Such deviations are called negative. For example, for a mixture: H 2 O-HNO 3 ; H 2 O-HCl; CHCl 3 -(CH 3) 2 CO; CHCl 3 -C 6 H 6 etc.
Positive deviations are observed in solutions in which heterogeneous molecules interact with less force than homogeneous ones.
This facilitates the transition of molecules from solution to the vapor phase. Solutions with a positive deviation are formed with the absorption of heat, i.e. the heat of mixing of pure components will be positive, there is an increase in volume, a decrease in association.
Negative deviations from Raoult's law occur in solutions in which there is an increase in the interaction of heterogeneous molecules, solvation, the formation of hydrogen bonds, and the formation of chemical compounds. This hinders the transition of molecules from solution to the gas phase.
|
Name component |
Antoine equation coefficients |
||
|
Butanol-1 | |||
|
Vinyl acetate | |||
|
Methyl acetate | |||
|
Morpholine | |||
|
Formic acid | |||
|
Acetic acid | |||
|
pyrrolidine | |||
|
benzyl alcohol | |||
|
Ethanthiol | |||
|
Chlorobenzene | |||
|
Trichlorethylene * | |||
|
Chloroform | |||
|
Trimethylborate * | |||
|
Methyl ethyl ketone | |||
|
ethylene glycol | |||
|
ethyl acetate | |||
|
2-methyl-2-propanol | |||
|
Dimethylformamide | |||
Notes: 1)
* data.
Main literature
Serafimov L.A., Frolkova A.K. The fundamental principle of the redistribution of concentration fields between areas of separation as the basis for the creation of technological complexes. -Theor. basics of chem. technol., 1997–T. 31, no. 2. pp.184–192.
Timofeev V.S., Serafimov L.A. Principles of technology of basic organic and petrochemical synthesis. - M.: Chemistry, 1992. - 432 p.
Kogan V. B. Azeotropic and extractive distillation. - L.: Chemistry, 1971. - 432 p.
Sventoslavsky V.V. Azeotropy and polyazeotropy. - M.: Chemistry, 1968. -244 p.
Serafimov L.A., Frolkova A.K. General laws and classification of binary liquid solutions in terms of excess thermodynamic functions. Methodical instructions. – M.: A/O Rosvuznauka, 1992. 40 p.
Wales S. Phase equilibrium in chemical technology. T.1. - M.: Mir, 1989. - 304 p.
Thermodynamics of liquid-vapor equilibrium. / Edited by Morachevsky A.G. - L.: Chemistry, 1989. - 344 p.
Ogorodnikov S.K., Lesteva T.M., Kogan V.B. Azeotropic mixtures. Handbook. - L .: Chemistry, 1971. - 848 p.
Kogan V.B., Fridman V.M., Kafarov V.V. Equilibrium between liquid and vapor. Reference manual, in 2 volumes. - M.-L.: Nauka, 1966.
Lyudmirskaya G.S., Barsukova T.V., Bogomolny A.M. Equilibrium liquid-steam. Directory. -L.: Chemistry, 1987.-336 p.
Reid R., Prausnitz J., Sherwood T. Properties of gases and liquids. - L .: Chemistry, 1982. -592 p.
Belousov V.P., Morachevsky A.G. Heats of mixing of liquids. Handbook. L .: Chemistry, 1970 256 p.
Belousov V.P., Morachevsky A.G., Panov M.Yu. Thermal properties of nonelectrolyte solutions. Directory. - L.: Chemistry, 1981. - 264 p.
Evaporation is the transition of a liquid to vapor from a free surface at temperatures below the boiling point of the liquid. Evaporation occurs as a result of the thermal movement of liquid molecules. The speed of movement of molecules varies widely, deviating strongly in both directions from its average value. Some of the molecules with a sufficiently large kinetic energy escape from the surface layer of the liquid into the gas (air) medium. The excess energy of the molecules lost by the liquid is expended on overcoming the forces of interaction between the molecules and the work of expansion (increase in volume) during the transition of the liquid into vapor.
Evaporation is an endothermic process. If heat is not supplied to the liquid from the outside, then as a result of evaporation, it cools. The evaporation rate is determined by the amount of vapor generated per unit of time per unit of liquid surface. This must be taken into account in industries related to the use, production or processing of flammable liquids. Increasing the evaporation rate with increasing temperature leads to a more rapid formation of explosive vapor concentrations. The maximum evaporation rate is observed during evaporation into vacuum and into an unlimited volume. This can be explained as follows. The observed rate of the evaporation process is the total rate of the process of transition of molecules from the liquid phase V 1 and condensation rate V 2 . The total process is equal to the difference between these two speeds: . At constant temperature V 1 does not change, but V 2 proportional to the vapor concentration. When evaporating into a vacuum in the limit V 2 = 0 , i.e. the total speed of the process is maximum.
The higher the vapor concentration, the higher the rate of condensation, hence the lower the total rate of evaporation. At the interface between the liquid and its saturated vapor, the evaporation rate (total) is close to zero. The liquid in a closed vessel, evaporating, forms a saturated vapor. A saturated vapor is a vapor that is in dynamic equilibrium with a liquid. Dynamic equilibrium at a given temperature occurs when the number of evaporating liquid molecules is equal to the number of condensing molecules. Saturated vapor, leaving an open vessel into the air, is diluted by it and becomes unsaturated. Therefore, in the air
In every room where containers with hot liquids are located, there is an unsaturated vapor of these liquids.
Saturated and unsaturated vapors exert pressure on vessel walls. Saturated vapor pressure is the pressure of vapor in equilibrium with a liquid at a given temperature. The pressure of saturated steam is always higher than that of unsaturated steam. It does not depend on the amount of liquid, the size of its surface, the shape of the vessel, but depends only on the temperature and nature of the liquid. As the temperature rises, the saturation vapor pressure of a liquid increases; At the boiling point, the vapor pressure is equal to atmospheric pressure. For each temperature value, the saturated vapor pressure of an individual (pure) liquid is constant. The saturation vapor pressure of mixtures of liquids (oil, gasoline, kerosene, etc.) at the same temperature depends on the composition of the mixture. It increases with an increase in the content of low-boiling products in the liquid.
For most liquids, the saturation vapor pressure at various temperatures is known. The values of saturated vapor pressure of some liquids at different temperatures are given in Table. 5.1.
Table 5.1
Saturated vapor pressure of substances at different temperatures
|
Substance |
Saturated vapor pressure, Pa, at temperature, K |
||||||
|
Butyl acetate Baku aviation gasoline Methyl alcohol carbon disulfide Turpentine Ethanol Ethyl ether ethyl acetate |
|||||||
Found in Table.
5.1 The saturation vapor pressure of a liquid is a component of the total pressure of the mixture of vapors with air.
Let us assume that the mixture of vapors with air formed above the surface of carbon disulphide in a vessel at 263 K has a pressure of 101080 Pa. Then the saturation vapor pressure of carbon disulfide at this temperature is 10773 Pa. Therefore, the air in this mixture has a pressure of 101080 - 10773 = 90307 Pa. With increasing temperature of carbon disulfide
its saturated vapor pressure increases, the air pressure decreases. The total pressure remains constant.
The part of the total pressure attributable to a given gas or vapor is called partial pressure. In this case, the vapor pressure of carbon disulfide (10773 Pa) can be called partial pressure. Thus, the total pressure of the vapor-air mixture is the sum of the partial vapor pressures of carbon disulfide, oxygen and nitrogen: P steam + + = P total. Since the pressure of saturated vapors is part of the total pressure of their mixture with air, it becomes possible to determine the vapor concentrations of liquids in air from the known total pressure of the mixture and the vapor pressure.
The saturation vapor pressure of liquids is determined by the number of molecules hitting the walls of the vessel, or by the concentration of vapor above the surface of the liquid. The higher the concentration of saturated steam, the greater its pressure. The relationship between the concentration of saturated vapor and its partial pressure can be found as follows.
Let us assume that it would be possible to separate the vapor from the air, and the pressure in both parts would remain equal to the total pressure Ptot. Then the volumes occupied by steam and air would decrease accordingly. According to the Boyle-Mariotte law, the product of the gas pressure and its volume at a constant temperature is a constant value, i.e. for our hypothetical case, we get:
.
n16.doc
Chapter 7. VAPOR PRESSURE, PHASE TEMPERATURESTRANSITIONS, SURFACE TENSION
Information about the vapor pressure of pure liquids and solutions, their boiling and solidification (melting) temperatures, as well as surface tension are necessary for calculating various technological processes: evaporation and condensation, evaporation and drying, distillation and rectification, etc.
7.1. Vapor pressure
One of the simplest equations for determining the saturation vapor pressure of a pure liquid as a function of temperature 
is the Antoine equation:
, (7.1)
Where A, IN, WITH- constants characteristic of individual substances. The values of the constants for some substances are given in Table. 7.1.
If two boiling points are known at the corresponding pressures, then, assuming WITH= 230, constants can be determined A And IN by jointly solving the following equations:
; (7.2)
. (7.3)
Equation (7.1) agrees quite satisfactorily with experimental data in a wide temperature range between the melting point and 
= 0.85 (i.e. 
= 0.85). This equation gives the greatest accuracy in those cases when all three constants can be calculated on the basis of experimental data. The calculation accuracy according to equations (7.2) and (7.3) is significantly reduced already at 
250 K, and for highly polar compounds at 0.65.
The change in the vapor pressure of a substance depending on temperature can be determined by the comparison method (according to the linearity rule), based on the known pressures of the reference liquid. If two temperatures of a liquid substance are known at the corresponding saturation vapor pressures, one can use the equation
, (7.4)
Where 
And 
– saturation vapor pressure of two liquids A And IN at the same temperature 
; 
And 
are the saturated vapor pressures of these liquids at a temperature 
; WITH- constant.
Table 7.1. The vapor pressure of some substances depending on
temperature
The table shows the values of the constants A, IN And WITH Antoine equations: , where is the pressure of saturated vapor, mm Hg. (1 mm Hg = 133.3 Pa); T– temperature, K.
| Substance name | Chemical formula | Temperature range, o C | A | IN | WITH |
|
| from | before |
|||||
| Nitrogen | N 2 | –221 | –210,1 | 7,65894 | 359,093 | 0 |
| nitrogen dioxide | N 2 O 4 (NO 2) | –71,7 | –11,2 | 12,65 | 2750 | 0 |
| –11,2 | 103 | 8,82 | 1746 | 0 |
||
| nitrogen oxide | NO | –200 | –161 | 10,048 | 851,8 | 0 |
| –164 | –148 | 8,440 | 681,1 | 0 |
||
| Acrylamide | C 3 H 5 ON | 7 | 77 | 12,34 | 4321 | 0 |
| 77 | 137 | 9,341 | 3250 | 0 |
||
| Acrolein | C 3 H 4 O | –3 | 140 | 7,655 | 1558 | 0 |
| Ammonia | NH3 | –97 | –78 | 10,0059 | 1630,7 | 0 |
| Aniline | C6H5NH2 | 15 | 90 | 7,63851 | 1913,8 | –53,15 |
| 90 | 250 | 7,24179 | 1675,3 | –73,15 |
||
| Argon | Ar | –208 | –189,4 | 7,5344 | 403,91 | 0 |
| –189,2 | –183 | 6,9605 | 356,52 | 0 |
||
| Acetylene | C 2 H 2 | –180 | –81,8 | 8,7371 | 1084,9 | –4,3 |
| –81,8 | 35,3 | 7,5716 | 925,59 | 9,9 |
||
| Acetone | C3H6O | –59,4 | 56,5 | 8,20 | 1750 | 0 |
| Benzene | C 6 H 6 | –20 | 5,5 | 6,48898 | 902,28 | –95,05 |
| 5,5 | 160 | 6,91210 | 1214,64 | –51,95 |
||
| Bromine | Br2 | 8,6 | 110 | 7,175 | 1233 | –43,15 |
| Hydrogen bromide | HBr | –99 | –87,5 | 8,306 | 1103 | 0 |
| –87,5 | –67 | 7,517 | 956,5 | 0 |
||
Continuation of the table. 7.1
| Substance name | Chemical formula | Temperature range, o C | A | IN | WITH |
|
| from | before |
|||||
| 1,3-Butadiene | C 4 H 6 | –66 | 46 | 6,85941 | 935,53 | –33,6 |
| 46 | 152 | 7,2971 | 1202,54 | 4,65 |
||
| n-Butane | C 4 H 10 | –60 | 45 | 6,83029 | 945,9 | –33,15 |
| 45 | 152 | 7,39949 | 1299 | 15,95 |
||
| Butyl alcohol | C4H10O | 75 | 117,5 | 9,136 | 2443 | 0 |
| Vinyl acetate | CH 3 COOCH=CH 2 | 0 | 72,5 | 8,091 | 1797,44 | 0 |
| Vinyl chloride | CH 2 \u003d CHCl | –100 | 20 | 6,49712 | 783,4 | –43,15 |
| –52,3 | 100 | 6,9459 | 926,215 | –31,55 |
||
| 50 | 156,5 | 10,7175 | 4927,2 | 378,85 |
||
| Water | H 2 O | 0 | 100 | 8,07353 | 1733,3 | –39,31 |
| Hexane | C 6 H 1 4 | –60 | 110 | 6,87776 | 1171,53 | –48,78 |
| 110 | 234,7 | 7,31938 | 1483,1 | –7,25 |
||
| Heptane | C 7 H 1 6 | –60 | 130 | 6,90027 | 1266,87 | –56,39 |
| 130 | 267 | 7,3270 | 1581,7 | –15,55 |
||
| Dean | C 10 H 22 | 25 | 75 | 7,33883 | 1719,86 | –59,35 |
| 75 | 210 | 6,95367 | 1501,27 | –78,67 |
||
| Diisopropyl ether | C6H14O | 8 | 90 | 7,821 | 1791,2 | 0 |
| N,N-Dimethylacetamide | C 4 H 9 ON | 0 | 44 | 7,71813 | 1745,8 | –38,15 |
| 44 | 170 | 7,1603 | 1447,7 | –63,15 |
||
| 1,4- Dioxane | C4H8O2 | 10 | 105 | 7,8642 | 1866,7 | 0 |
| 1,1-Dichloroethane | C 2 H 4 Cl 2 | 0 | 30 | 7,909 | 1656 | 0 |
| 1,2-Dichloroethane | C 2 H 4 Cl 2 | 6 | 161 | 7,18431 | 1358,5 | –41,15 |
| 161 | 288 | 7,6284 | 1730 | 9,85 |
||
| diethyl ether | (C 2 H 5) 2 O | –74 | 35 | 8,15 | 1619 | 0 |
| isobutyric acid | C4H8O2 | 30 | 155 | 8,819 | 2533 | 0 |
| Isoprene | C 5 H 8 | –50 | 84 | 6,90334 | 1081,0 | –38,48 |
| 84 | 202 | 7,33735 | 1374,92 | 2,19 |
||
| Isopropyl alcohol | C3H8O | –26,1 | 82,5 | 9,43 | 2325 | 0 |
| hydrogen iodide | HI | –50 | –34 | 7,630 | 1127 | 0 |
| Krypton | kr | –207 | –158 | 7,330 | 7103 | 0 |
| Xenon | Heh | –189 | –111 | 8,00 | 841,7 | 0 |
| n-Xylene | C 8 H 10 | 25 | 45 | 7,32611 | 1635,74 | –41,75 |
| 45 | 190 | 6,99052 | 1453,43 | –57,84 |
||
| O-Xylene | C 8 H 10 | 25 | 50 | 7,35638 | 1671,8 | –42,15 |
| 50 | 200 | 6,99891 | 1474,68 | –59,46 |
||
Continuation of the table. 7.1
| Substance name | Chemical formula | Temperature range, o C | A | IN | WITH |
|
| from | before |
|||||
| Butyric acid | C4H8O2 | 80 | 165 | 9,010 | 2669 | 0 |
| Methane | CH 4 | –161 | –118 | 6,81554 | 437,08 | –0,49 |
| –118 | –82,1 | 7,31603 | 600,17 | 25,27 |
||
| methylene chloride (dichloromethane) | CH2Cl2 | –28 | 121 | 7,07138 | 1134,6 | –42,15 |
| 127 | 237 | 7,50819 | 1462,59 | 5,45 |
||
| Methyl alcohol | CH 4 O | 7 | 153 | 8,349 | 1835 | 0 |
| -Methylstyrene | C 9 H 10 | 15 | 70 | 7,26679 | 1680,13 | –53,55 |
| 70 | 220 | 6,92366 | 1486,88 | –71,15 |
||
| methyl chloride | CH3Cl | –80 | 40 | 6,99445 | 902,45 | –29,55 |
| 40 | 143,1 | 7,81148 | 1433,6 | 44,35 |
||
| Methyl ethyl ketone | C4H8O | –15 | 85 | 7,764 | 1725,0 | 0 |
| Formic acid | CH2O2 | –5 | 8,2 | 12,486 | 3160 | 0 |
| 8,2 | 110 | 7,884 | 1860 | 0 |
||
| Neon | Ne | –268 | –253 | 7,0424 | 111,76 | 0 |
| Nitrobenzene | C 6 H 5 O 2 N | 15 | 108 | 7,55755 | 2026 | –48,15 |
| 108 | 300 | 7,08283 | 1722,2 | –74,15 |
||
| Nitromethane | CH 3 O 2 N | 55 | 136 | 7,28050 | 1446,19 | –45,63 |
| Octane | C 8 H 18 | 15 | 40 | 7,47176 | 1641,52 | –38,65 |
| 40 | 155 | 6,92377 | 1355,23 | –63,63 |
||
| Pentane | C 5 H 12 | –30 | 120 | 6,87372 | 1075,82 | –39,79 |
| 120 | 196,6 | 7,47480 | 1520,66 | 23,94 |
||
| Propane | C 3 H 8 | –130 | 5 | 6,82973 | 813,2 | –25,15 |
| 5 | 96,8 | 7,67290 | 1096,9 | 47,39 |
||
| propylene (propene) | C 3 H 6 | –47,7 | 0,0 | 6,64808 | 712,19 | –36,35 |
| 0,0 | 91,4 | 7,57958 | 1220,33 | 36,65 |
||
| propylene oxide | C3H6O | –74 | 35 | 6,96997 | 1065,27 | –46,87 |
| propylene glycol | C 3 H 8 O 2 | 80 | 130 | 9,5157 | 3039,0 | 0 |
| propyl alcohol | C3H8O | –45 | –10 | 9,5180 | 2469,1 | 0 |
| propionic acid | C 3 H 6 O 2 | 20 | 140 | 8,715 | 2410 | 0 |
| hydrogen sulfide | H 2 S | –110 | –83 | 7,880 | 1080,6 | 0 |
| carbon disulfide | CS2 | –74 | 46 | 7,66 | 1522 | 0 |
| Sulfur dioxide | SO2 | –112 | –75,5 | 10,45 | 1850 | 0 |
| Sulfur trioxide () | SO 3 | –58 | 17 | 11,44 | 2680 | 0 |
| Sulfur trioxide () | SO 3 | –52,5 | 13,9 | 11,96 | 2860 | 0 |
| Tetrachlorethylene | C 2 Cl 4 | 34 | 187 | 7,02003 | 1415,5 | –52,15 |
The end of the table. 7.1
| Substance name | Chemical formula | Temperature range, o C | A | IN | WITH |
|
| from | before |
|||||
| Thiophenol | C6H6S | 25 | 70 | 7,11854 | 1657,1 | –49,15 |
| 70 | 205 | 6,78419 | 1466,5 | –66,15 |
||
| Toluene | C 6 H 5 CH 3 | 20 | 200 | 6,95334 | 1343,94 | –53,77 |
| Trichlorethylene | C 2 HCl 3 | 7 | 155 | 7,02808 | 1315,0 | –43,15 |
| carbon dioxide | CO 2 | –35 | –56,7 | 9,9082 | 1367,3 | 0 |
| Carbon oxide | CO | –218 | –211,7 | 8,3509 | 424,94 | 0 |
| Acetic acid | C 2 H 4 O 2 | 16,4 | 118 | 7,55716 | 1642,5 | –39,76 |
| Acetic anhydride | C 4 H 6 O 3 | 2 | 139 | 7,12165 | 1427,77 | –75,11 |
| Phenol | C 6 H 6 O | 0 | 40 | 11,5638 | 3586,36 | 0 |
| 41 | 93 | 7,86819 | 2011,4 | –51,15 |
||
| Fluorine | F2 | –221,3 | –186,9 | 8,23 | 430,1 | 0 |
| Chlorine | Cl2 | –154 | –103 | 9,950 | 1530 | 0 |
| Chlorobenzene | C 6 H 5 Cl | 0 | 40 | 7,49823 | 1654 | –40,85 |
| 40 | 200 | 6,94504 | 1413,12 | –57,15 |
||
| hydrogen chloride | HCl | –158 | –110 | 8,4430 | 1023,1 | 0 |
| Chloroform | CHCl 3 | –15 | 135 | 6,90328 | 1163,0 | –46,15 |
| 135 | 263 | 7,3362 | 1458,0 | 2,85 |
||
| Cyclohexane | C 6 H 12 | –20 | 142 | 6,84498 | 1203,5 | –50,29 |
| 142 | 281 | 7,32217 | 1577,4 | 2,65 |
||
| Tetrachloride carbon | CCl 4 | –15 | 138 | 6,93390 | 1242,4 | –43,15 |
| 138 | 283 | 7,3703 | 1584 | 3,85 |
||
| Ethane | C 2 H 6 | –142 | –44 | 6,80266 | 636,4 | –17,15 |
| –44 | 32,3 | 7,6729 | 1096,9 | 47,39 |
||
| Ethylbenzene | C 8 H 10 | 20 | 45 | 7,32525 | 1628,0 | –42,45 |
| 45 | 190 | 6,95719 | 1424,26 | –59,94 |
||
| Ethylene | C 2 H 4 | –103,7 | –70 | 6,87477 | 624,24 | –13,14 |
| –70 | 9,5 | 7,2058 | 768,26 | 9,28 |
||
| Ethylene oxide | C 2 H 4 O | –91 | 10,5 | 7,2610 | 1115,10 | –29,01 |
| ethylene glycol | C 2 H 6 O 2 | 25 | 90 | 8,863 | 2694,7 | 0 |
| 90 | 130 | 9,7423 | 3193,6 | 0 |
||
| Ethanol | C 2 H 6 O | –20 | 120 | 6,2660 | 2196,5 | 0 |
| ethyl chloride | C 2 H 5 Cl | –50 | 70 | 6,94914 | 1012,77 | –36,48 |
When determining by the rule of linearity the pressure of saturated vapor of water-soluble substances, water is used as a reference liquid, and in the case of organic compounds that are insoluble in water, hexane is usually taken. The values of the pressure of saturated water vapor depending on the temperature are given in Table. P.11. The dependence of the saturated vapor pressure on the temperature of hexane is given in Fig. . 7.1.
Rice. 7.1. Temperature dependence of saturated vapor pressure of hexane
(1 mm Hg = 133.3 Pa)
Based on relation (7.4), a nomogram was constructed to determine the saturated vapor pressure depending on temperature (see Fig. 7.2 and Table 7.2).
Over solutions, the vapor pressure of the solvent is less than over a pure solvent. Moreover, the decrease in vapor pressure is the greater, the higher the concentration of the solute in the solution.
Allen
6
1,2-Dichloroethane
26
Propylene
4
Ammonia
49
diethyl ether
15
propionic
56
Aniline
40
Isoprene
14
acid
Acetylene
2
Iodobenzene
39
Mercury
61
Acetone
51
m-Cresol
44
Tetralin
42
Benzene
24
O-Cresol
41
Toluene
30
Bromobenzene
35
m-Xylene
34
Acetic acid
55
Ethyl bromide
18
iso-oily
57
Fluorobenzene
27
-Bromonaphthalene
46
acid
Chlorobenzene
33
1,3-Butadiene
10
methylamine
50
Chlorine vinyl
8
Butane
11
Methylmonosilane
3
methyl chloride
7
-Butylene
9
Methyl alcohol
52
Chloride
19
-Butylene
12
Methyl formate
16
methylene
Butylene glycol
58
Naphthalene
43
Ethyl chloride
13
Water
54
-Naphthol
47
Chloroform
21
Hexane
22
-Naphthol
48
Tetrachloride
23
Heptane
28
Nitrobenzene
37
carbon
Glycerol
60
Octane
31*
Ethane
1
Decalin
38
32*
ethyl acetate
25
Dean
36
Pentane
17
ethylene glycol
59
dioxane
29
Propane
5
Ethanol
53
Diphenyl
45
Ethyl formate
20
The chemical composition of the cell
Carbon - element characteristics and chemical properties
Verification work "basics of the doctrine of the biosphere"