Formula of sulfur hydroxide and its nature. Sulfur oxide. Detailed analysis of the higher oxide

1) For the reaction with the hydroxide formed by some element of the 1 (A) - group, weighing 4.08 g, 1.46 g of hydrochloric acid is required. This element: rubidium; to

aly; lithium; sodium;
2) The sum of the coefficients in the equation for the reaction of higher sulfur hydroxide with potassium hydroxide is: 4; 6; 5; 8;

1. Lithium hydroxide reacts with; 1) calcium hydroxide 2) hydrochloric acid 3) magnesium oxide 4) barium 2. most pronounced

ene non-metallic properties of a simple substance:

1) chlorine 2) sulfur 3) silicon 4) calcium

3.group number in the periodic table is:

1) the higher valency of the atom 2) the number of electrons in the atom 3) the number of protons in the nucleus 4) the number of electron layers

4. Higher nitrogen hydroxide reacts with:

1) calcium hydroxide 2) hydrochloric acid 3) barium sulfate 4) silicon oxide

5. The most pronounced metallic properties of a simple substance: 1) sodium 2) magnesium 3) calcium 4) potassium

For all reactions it will be necessary to write down the full and short ionic equations. 1. Potassium → potassium hydroxide → potassium sulfate →

barium sulfate

2. Phosphorus → phosphorus (III) oxide → phosphorus (V) oxide → phosphoric acid → calcium phosphate

3. Zinc → zinc chloride → zinc hydroxide → zinc oxide

4. Sulfur → sulfur dioxide → higher sulfur oxide → sulfuric acid → aluminum sulfate.

5. Lithium → lithium hydroxide → lithium chloride → silver chloride

6. Nitrogen → nitric oxide (II) → nitric oxide (IV) → nitric acid → sodium nitrate

7. Sulfur → calcium sulfide → calcium oxide → calcium carbonate → carbon dioxide

8. Carbon dioxide→ sodium carbonate → calcium carbonate → calcium oxide

9. Iron → iron (II) oxide → iron (III) oxide → iron (III) sulfate

10. Barium → barium oxide → barium chloride → barium sulfate

1) The simple substance copper is referred to in the expression: A) the wire is made of copper B) copper is part of copper oxide C) copper is part of malachite D) m

nothing is a part of bronze 2) In the periods of the periodic system, with an increase in the charge of the nuclei, it does not change: A) the mass of the atom B) the number of energy levels C) total number electrons D) the number of electrons in the external energy level 3) Formulas of higher oxides of sulfur, nitrogen, chlorine, respectively: A) SO3, N2O5, Cl2O7 B) SO2, N2O5, Cl2O7 C) SO3, N2O3, ClO2 D) SO2, NO2, Cl2O5 4) Ionic bond type and crystal lattice has: A) sodium fluoride B) water C) silver D) bromine 5) Formulas of soluble base and amphoteric hydroxide, respectively: A) BaO, Cu(OH)2 B) Ba(OH)2, Al(OH)3 C) Zn (OH) 2, Ca (OH) 2 D) Fe (OH) 3, KOH 6) The coefficient in front of the oxygen formula in the reaction of thermal decomposition of potassium permanganate: A) 1 B) 2 C) 3 D) 4 copper oxide (II) refers to the reactions: A) decomposition B) compounds C) substitution D) exchange 8) The amount of heat released during the combustion of 2 g of coal (thermochemical reaction equation C + O2 \u003d CO2 + 393 kJ), is equal to: A) 24 kJ B) 32.75 kJ C) 65.5 kJ D) 393 kJ 9) At elevated temperatures, oxygen reacts with all substances of the group: A) CuO, H2, Fe B) P, H2, Mg C) Cu, H2, Au D) S, CH4, H2O 10) Reacts with both hydrogen and oxygen at elevated temperatures: A) copper (II) oxide B) gold C) sulfur D) nitric acid 11) Dilute sulfuric acid can react with: A) Mg and Cu(OH)2 B) CO2 and NaOH C) FeO and H2S D) P and CuCl2 12) Sulfur oxide (IV) does not react with: A) O2 B) HCl C) H2O D) NaOH 13) Formulas of substances "X" and "Y" in the transformation scheme CaO Y - HCl B) X - H2O; Y - HCl B) X - H2; Y – Cl2 D) X – H2O; Y - Cl2 14) The mass fraction of sulfur in sulfur oxide (IV) is: a) 20% b) 25% c) 33% d) 50% 15) A solution containing 19.6 g of sulfuric acid was neutralized with an excess of magnesium oxide. The amount of substance of the formed salt is: a) 0.2 mol b) 2 mol c) 0.1 mol d) 1 mol 16) The number of completely filled energy levels in the sodium atom: A) 2 B) 3 C) 4 D) 5 17 ) The ratio of the chemical activity of the elements in the pair is correctly indicated: A) Li  Na B) Na  K C) Li  K D) Na  Li 18) Metallic properties in the series Li  Na  K  Cs A) increase B) decrease C ) do not change D) change periodically 19) The electronic formula of the external energy level of the bromine atom: A) 2s22p5 B) 3s13p6 C) 4s14p7 D) 4s24p5 20) The atom has the electronic formula 1s22s22p63s23p5: A) iodine B) bromine C) chlorine D) fluorine 21 ) The metallic properties of chemical elements in the series I  Br  Cl  F A) increase B) decrease C) change periodically D) do not change 22) The formula of a substance with a covalent non-polar bond: A) SO3 B) Br2 C) H2O D) NaCl 23 ) The crystal lattice of solid carbon monoxide (IV): A) ionic B) atomic C) molecular D) metallic 24) A substance with an ionic bond: A) sulfur oxide (VI) B) chlorine C) hydrogen sulfide D) sodium chloride 25) A series of numbers 2, 8, 5 corresponds to the distribution of electrons over the energy levels of the atom: A) aluminum B) nitrogen C) phosphorus D) chlorine 26) Electronic formula of the external energy level 2s22p4 corresponds to the atom: a) sulfur B) carbon C) silicon D) oxygen 27) The atom has four electrons at the external energy level: A) helium B) beryllium C) carbon D) oxygen

Characteristic of sulfur: 1) The position of the element in the Periodic system D.I Characteristic of sulfur: 1) The position of the element in the Periodic system

D.I. Mendeleev and the structure of its atoms 2) The nature of a simple substance (metal, non-metal) 3) Comparison of the properties of a simple substance with the properties simple substances, formed by elements neighboring in a subgroup 4) Comparison of the properties of a simple substance with the properties of simple substances formed by elements adjacent in a period 5) The composition of the higher oxide, its character (basic, acidic, amphoteric) amphoteric hydroxide) 7) composition of a volatile hydrogen compound (for non-metals)

colorless liquid Molar mass 80.06 g/mol Density 1.92 g/cm³ Thermal properties T. melt. 16.83°C T. kip. 44.9°C Enthalpy of formation -395.8 kJ/mol Classification Reg. CAS number Security LD 50 510 mg/kg Toxicity Data is based on standard conditions (25 °C, 100 kPa) unless otherwise noted.

Sulfur oxide (VI) (sulfuric anhydride, sulfur trioxide, sulfuric gas) SO 3 - the highest oxide of sulfur. Under normal conditions, a highly volatile, colorless liquid with a suffocating odor. At temperatures below 16.9 ° C, it solidifies with the formation of a mixture of various crystalline modifications of solid SO 3.

Receipt

Can be obtained by thermal decomposition of sulfates:

$\backslash mathsf(Fe\_2(SO\_4)\_3\; \backslash xrightarrow(^ot)\; Fe\_2O\_3\; +\; 3SO\_3)$

or the interaction of SO 2 with ozone:

$\backslash mathsf(SO\_2\; +\; O\_3\; \backslash rightarrow\; SO\_3\; +\; O\_2)$

For the oxidation of SO 2, NO 2 is also used:

$\backslash mathsf(SO\_2\; +\; NO\_2\; \backslash rightarrow\; SO\_3\; +\; NO)$

This reaction underlies the historically first, nitrous method for the production of sulfuric acid.

Physical properties

Sulfur oxide (VI) - under normal conditions, a highly volatile, colorless liquid with a suffocating odor.

The SO 3 molecules in the gas phase have a flat trigonal structure with D 3h symmetry (OSO angle = 120°, d(S-O) = 141 pm). Upon transition to the liquid and crystalline states, a cyclic trimer and zigzag chains are formed. Type chemical bond in a molecule: a covalent polar chemical bond.

Solid SO 3 exists in α-, β-, γ- and δ-forms, with melting points of 16.8, 32.5, 62.3 and 95 ° C, respectively, and differing in the shape of crystals and the degree of polymerization of SO 3. The α-form of SO 3 consists mainly of trimer molecules. Other crystalline forms of sulfuric anhydride consist of zigzag chains: isolated at β-SO 3 , connected into flat networks at γ-SO 3 or into three-dimensional structures at δ-SO 3 . When cooled, the vapor first forms a colorless, ice-like, unstable α-form, which gradually passes in the presence of moisture into a stable β-form - white "silky" crystals, similar to asbestos. The reverse transition of the β-form to the α-form is possible only through the gaseous state of SO 3 . Both modifications "smoke" in air (droplets of H 2 SO 4 are formed) due to the high hygroscopicity of SO 3. Mutual transition to other modifications proceeds very slowly. The variety of forms of sulfur trioxide is associated with the ability of SO 3 molecules to polymerize due to the formation of donor-acceptor bonds. Polymeric structures of SO 3 easily transform into each other, and solid SO 3 usually consists of a mixture of various forms, the relative content of which depends on the conditions for obtaining sulfuric anhydride.

Chemical properties

$\backslash mathsf(2KOH\; +\; SO\_3\; \backslash rightarrow\; K\_2SO\_4\; +\; H\_2O)$

and oxides:

$\backslash mathsf(CaO\; +\; SO\_3\; \backslash rightarrow\; CaSO\_4)$

SO 3 is characterized by strong oxidizing properties, usually reduced to sulfur dioxide:

$\backslash mathsf(5SO\_3\; +\; 2P\; \backslash rightarrow\; P\_2O\_5\; +\; 5SO\_2)$ $\backslash mathsf(3SO\_3\; +\; H\_2S\; \backslash rightarrow\; 4SO\_2\; +\; H\_2O)$ $\backslash mathsf(2SO\_3\; +\; 2KI\; \backslash rightarrow\; SO\_2\; +\; I\_2\; +\; K\_2SO\_4)$

When interacting with hydrogen chloride, chlorosulfonic acid is formed:

$\backslash mathsf(SO\_3\; +\; HCl\; \backslash rightarrow\; HSO\_3Cl)$

It also reacts with sulfur dichloride and chlorine to form thionyl chloride:

$\backslash mathsf(SO\_3\; +\; Cl\_2\; +\; 2SCl\_2\; \backslash rightarrow\; 3SOCl\_2)$

Application

Sulfuric anhydride is used primarily in the production of sulfuric acid.

Sulfuric anhydride is also released into the air when sulfur pellets are burned, which are used in the disinfection of premises. Upon contact with wet surfaces, sulfuric anhydride turns into sulfuric acid, which already destroys fungus and other harmful organisms.

Write a review on the article "Sulfur(VI) oxide"

Literature

• Akhmetov N. S. "General and inorganic chemistry» M.: graduate School, 2001
• Karapetyants M. Kh., Drakin S. I. "General and inorganic chemistry" M .: Chemistry 1994

An excerpt characterizing Sulfur oxide (VI)

Natasha flushed. - I don't want to marry anyone. I'll tell him the same when I see him.
– That's how! Rostov said.
“Well, yes, it’s all nonsense,” Natasha continued to chat. - And why is Denisov good? she asked.
- Good.
- Well, goodbye, get dressed. Is he scary, Denisov?
- Why is it scary? Nicholas asked. - Not. Vaska is nice.
- You call him Vaska - strange. And that he is very good?
- Very good.
“Well, come and drink some tea.” Together.
And Natasha stood up on tiptoe and walked out of the room the way dancers do, but smiling the way happy 15-year-old girls smile. Having met Sonya in the living room, Rostov blushed. He didn't know how to deal with her. Yesterday they kissed in the first moment of the joy of meeting, but today they felt that it was impossible to do this; he felt that everyone, both mother and sisters, looked at him inquiringly and expected from him how he would behave with her. He kissed her hand and called her you - Sonya. But their eyes, having met, said “you” to each other and kissed tenderly. With her eyes, she asked him for forgiveness for the fact that at Natasha's embassy she dared to remind him of his promise and thanked him for his love. He thanked her with his eyes for the offer of freedom and said that one way or another, he would never stop loving her, because it was impossible not to love her.
“How strange, however,” said Vera, choosing a general moment of silence, “that Sonya and Nikolenka now met like strangers. - Vera's remark was just, like all her remarks; but, like most of her remarks, everyone became embarrassed, and not only Sonya, Nikolai and Natasha, but also the old countess, who was afraid of her son’s love for Sonya, which could deprive him of a brilliant party, also blushed like a girl. Denisov, to Rostov's surprise, in a new uniform, pomaded and perfumed, appeared in the living room as dandy as he was in battles, and so amiable with ladies and gentlemen, which Rostov did not expect to see him.

Returning to Moscow from the army, Nikolai Rostov was adopted by his family as the best son, hero and beloved Nikolushka; relatives - as a sweet, pleasant and respectful young man; acquaintances - as a handsome hussar lieutenant, a clever dancer and one of the best grooms in Moscow.
The Rostovs knew all of Moscow; the old count had enough money this year, because all the estates were mortgaged, and therefore Nikolushka, having got his own trotter and the most fashionable trousers, special ones that no one else in Moscow had, and boots, the most fashionable, with the most pointed socks and little silver spurs, had a lot of fun. Rostov, returning home, experienced a pleasant feeling after a certain period of time trying on himself for the old conditions of life. It seemed to him that he had matured and grown very much. Despair for an examination that was not consistent with the law of God, borrowing money from Gavrila for a cab, secret kisses with Sonya, he recalled all this as about childishness, from which he was immeasurably far away now. Now he is a hussar lieutenant in a silver cape, with soldier George, preparing his trotter for a run, along with well-known hunters, elderly, respectable. He has a familiar lady on the boulevard, to whom he goes in the evening. He conducted a mazurka at a ball at the Arkharovs, talked about the war with Field Marshal Kamensky, visited an English club, and was on you with one forty-year-old colonel, whom Denisov introduced him to.
His passion for the sovereign somewhat weakened in Moscow, since during this time he did not see him. But he often talked about the sovereign, about his love for him, making it feel that he still did not tell everything, that there was something else in his feeling for the sovereign that could not be understood by everyone; and wholeheartedly shared the feeling of adoration common at that time in Moscow for Emperor Alexander Pavlovich, who at that time in Moscow was given the name of an angel in the flesh.
During this short stay of Rostov in Moscow, before leaving for the army, he did not get close, but, on the contrary, parted ways with Sonya. She was very pretty, sweet, and obviously passionately in love with him; but he was in that time of his youth, when it seems there is so much to do that there is no time to do it, and the young man is afraid to get involved - he values ​​\u200b\u200bhis freedom, which he needs for many other things. When he thought of Sonya during this new sojourn in Moscow, he said to himself: Eh! there are still many, many of these will be and are there, somewhere, still unknown to me. I still have time, when I want, to make love, but now there is no time. In addition, it seemed to him that something humiliating for his courage in women's society. He went to balls and sororities, pretending to do so against his will. running, English club, revelry with Denisov, a trip there - that was another matter: it was decent for a young hussar.

Sulfur is common in earth's crust, ranks sixteenth among other elements. It occurs both in the free state and in bound form. Non-metallic properties are characteristic of this chemical element. Its Latin name "Sulfur", denoted by the symbol S. The element is part of various ions of compounds containing oxygen and / or hydrogen, forms many substances belonging to the classes of acids, salts and several oxides, each of which can be called sulfur oxide with the addition symbols denoting valency. The oxidation states it exhibits in various compounds+6, +4, +2, 0, -1, -2. Sulfur oxides with various degrees of oxidation are known. The most common are sulfur dioxide and trioxide. Less well known are sulfur monoxide, as well as higher (except SO3) and lower oxides of this element.

Sulfur monoxide

An inorganic compound called sulfur oxide II, SO, after appearance this substance is a colorless gas. When in contact with water, it does not dissolve, but reacts with it. This is a very rare compound that occurs only in a rarefied gaseous environment. The SO molecule is thermodynamically unstable, it initially turns into S2O2, (called disulfur gas or sulfur peroxide). Due to the rare occurrence of sulfur monoxide in our atmosphere and the low stability of the molecule, it is difficult to fully determine the dangers of this substance. But in a condensed or more concentrated form, the oxide turns into peroxide, which is relatively toxic and caustic. This compound is also highly flammable (reminiscent of methane in this property), and when burned, sulfur dioxide is produced - a poisonous gas. Sulfur oxide 2 was found near Io (one of the Venusian atmosphere and in the interstellar medium. It is assumed that on Io it is produced as a result of volcanic and photochemical processes. The main photochemical reactions are as follows: O + S2 → S + SO and SO2 → SO +O.

Sulphur dioxide

Sulfur oxide IV, or sulfur dioxide (SO2), is a colorless gas with a suffocating, pungent odor. At a temperature of minus 10 C, it passes into a liquid state, and at a temperature of minus 73 C, it solidifies. At 20C, about 40 volumes of SO2 dissolve in 1 liter of water.

This sulfur oxide, dissolving in water, forms sulfurous acid, as it is its anhydride: SO2 + H2O ↔ H2SO3.

It interacts with bases and 2NaOH + SO2 → Na2SO3 + H2O and SO2 + CaO → CaSO3.

Sulfur dioxide has the properties of both an oxidizing agent and a reducing agent. It is oxidized by atmospheric oxygen to sulfuric anhydride in the presence of a catalyst: SO2 + O2 → 2SO3. With strong reducing agents, such as hydrogen sulfide, it plays the role of an oxidizing agent: H2S + SO2 → S + H2O.

Sulfur dioxide is mainly used in industry to produce sulfuric acid. Sulfur dioxide is obtained by burning sulfur or iron pyrite: 11O2 + 4FeS2 → 2Fe2O3 + 8SO2.

Sulfuric anhydride

Sulfur oxide VI, or sulfur trioxide (SO3) is an intermediate product and has no independent value. It is a colorless liquid in appearance. It boils at a temperature of 45 C, and below 17 C it turns into a white crystalline mass. This sulfur (with the oxidation state of the sulfur atom + 6) is extremely hygroscopic. With water, it forms sulfuric acid: SO3 + H2O ↔ H2SO4. Dissolving in water, it releases a large amount of heat, and if a large amount of oxide is added at once, not gradually, then an explosion can occur. Sulfur trioxide dissolves well in concentrated sulfuric acid to form oleum. The content of SO3 in oleum reaches 60%. This sulfur compound is characterized by all the properties

Higher and lower oxides of sulfur

Sulfurs are a group of chemical compounds with the formula SO3 + x, where x can be 0 or 1. The monomeric oxide SO4 contains a peroxo group (O-O) and is characterized, like the oxide SO3, by the oxidation state of sulfur +6. This sulfur oxide can be produced at low temperatures (below 78 K) by reaction of SO3 and or by photolysis of SO3 mixed with ozone.

Lower sulfur oxides are a group of chemical compounds, which include:

• SO (sulfur oxide and its dimer S2O2);
• sulfur monoxides SnO (are cyclic compounds consisting of rings formed by sulfur atoms, while n can be from 5 to 10);
• S7O2;
• polymer oxides of sulfur.

Interest in lower sulfur oxides has increased. This is due to the need to study their content in the terrestrial and extraterrestrial atmospheres.

In redox processes, sulfur dioxide can be both an oxidizing agent and a reducing agent because the atom in this compound has an intermediate oxidation state of +4.

How does the oxidizing agent SO 2 react with stronger reducing agents, for example with:

SO 2 + 2H 2 S \u003d 3S ↓ + 2H 2 O

How does the reducing agent SO 2 react with stronger oxidizing agents, for example with in the presence of a catalyst, with, etc.:

2SO 2 + O 2 \u003d 2SO 3

SO 2 + Cl 2 + 2H 2 O \u003d H 2 SO 3 + 2HCl

Receipt

1) Sulfur dioxide is formed during the combustion of sulfur:

2) In industry, it is obtained by firing pyrite:

3) In the laboratory, sulfur dioxide can be obtained:

Cu + 2H 2 SO 4 \u003d CuSO 4 + SO 2 + 2H 2 O

Application

Sulfur dioxide is widely used in the textile industry for bleaching various products. Moreover, it is used in agriculture for the destruction of harmful microorganisms in greenhouses and cellars. In large quantities, SO 2 is used to produce sulfuric acid.

Sulfur oxide (VI) – SO 3 (sulfuric anhydride)

Sulfuric anhydride SO 3 is a colorless liquid, which at temperatures below 17 ° C turns into a white crystalline mass. It absorbs moisture very well (hygroscopic).

Chemical properties

Acid-base properties

How a typical acid oxide sulfuric anhydride interacts:

SO 3 + CaO = CaSO 4

c) with water:

SO 3 + H 2 O \u003d H 2 SO 4

A special property of SO 3 is its ability to dissolve well in sulfuric acid. A solution of SO 3 in sulfuric acid is called oleum.

Oleum formation: H 2 SO 4 + n SO 3 \u003d H 2 SO 4 ∙ n SO 3

redox properties

Sulfur oxide (VI) is characterized by strong oxidizing properties (usually reduced to SO 2):

3SO 3 + H 2 S \u003d 4SO 2 + H 2 O

Getting and using

Sulfuric anhydride is formed during the oxidation of sulfur dioxide:

2SO 2 + O 2 \u003d 2SO 3

In its pure form, sulfuric anhydride has no practical value. It is obtained as an intermediate in the production of sulfuric acid.

H2SO4

Mention of sulfuric acid is first found among Arab and European alchemists. It was obtained by calcining iron sulfate (FeSO 4 ∙ 7H 2 O) in air: 2FeSO 4 \u003d Fe 2 O 3 + SO 3 + SO 2 or a mixture with: 6KNO 3 + 5S \u003d 3K 2 SO 4 + 2SO 3 + 3N 2, and the emitted vapors of sulfuric anhydride were condensed. Absorbing moisture, they turned into oleum. Depending on the method of preparation, H 2 SO 4 was called vitriol oil or sulfur oil. In 1595, the alchemist Andreas Libavius ​​established the identity of both substances.

For a long time, vitriol oil was not widely used. Interest in it greatly increased after the 18th century. Indigo carmine, a stable blue dye, was discovered. The first factory for the production of sulfuric acid was founded near London in 1736. The process was carried out in lead chambers, at the bottom of which water was poured. A molten mixture of saltpeter with sulfur was burned in the upper part of the chamber, then air was let in there. The procedure was repeated until an acid of the required concentration was formed at the bottom of the container.

In the 19th century the method was improved: instead of saltpeter, nitric acid was used (it gives when decomposed in the chamber). To return nitrous gases to the system, special towers were designed, which gave the name to the whole process - the tower process. Factories operating according to the tower method still exist today.

Sulfuric acid- it is a heavy oily liquid, colorless and odorless, hygroscopic; dissolves well in water. When concentrated sulfuric acid is dissolved in water, a large amount of heat is released, so it must be carefully poured into water (and not vice versa!) And mix the solution.

A solution of sulfuric acid in water with an H2SO4 content of less than 70% is usually called dilute sulfuric acid, and a solution of more than 70% is called concentrated sulfuric acid.

Chemical properties

Acid-base properties

Dilute sulfuric acid exhibits all the characteristic properties of strong acids. She reacts:

H 2 SO 4 + NaOH \u003d Na 2 SO 4 + 2H 2 O

H 2 SO 4 + BaCl 2 \u003d BaSO 4 ↓ + 2HCl

The process of interaction of Ba 2+ ions with sulfate ions SO 4 2+ leads to the formation of a white insoluble precipitate BaSO 4 . This is qualitative reaction to sulfate ion.

Redox properties

In dilute H 2 SO 4 , H + ions are oxidizing agents, and in concentrated H 2 SO 4 sulfate ions are SO 4 2+ . SO 4 2+ ions are stronger oxidizing agents than H + ions (see diagram).

AT dilute sulfuric acid dissolve metals that are in the electrochemical series of voltages to hydrogen. In this case, metal sulfates are formed and released:

Zn + H 2 SO 4 \u003d ZnSO 4 + H 2

Metals that are in the electrochemical series of voltages after hydrogen do not react with dilute sulfuric acid:

Cu + H 2 SO 4 ≠

concentrated sulfuric acid is a strong oxidizing agent, especially when heated. It oxidizes many, and some organic substances.

When concentrated sulfuric acid interacts with metals that are in the electrochemical series of voltages after hydrogen (Cu, Ag, Hg), metal sulfates are formed, as well as the product of sulfuric acid reduction - SO 2.

Reaction of sulfuric acid with zinc

With more active metals (Zn, Al, Mg), concentrated sulfuric acid can be reduced to free. For example, when sulfuric acid interacts with, depending on the acid concentration, various products of sulfuric acid reduction can be formed simultaneously - SO 2, S, H 2 S:

Zn + 2H 2 SO 4 \u003d ZnSO 4 + SO 2 + 2H 2 O

3Zn + 4H 2 SO 4 = 3ZnSO 4 + S↓ + 4H 2 O

4Zn + 5H 2 SO 4 = 4ZnSO 4 + H 2 S + 4H 2 O

In the cold, concentrated sulfuric acid passivates some metals, for example, and therefore it is transported in iron tanks:

Fe + H 2 SO 4 ≠

Concentrated sulfuric acid oxidizes some non-metals (, etc.), recovering to sulfur oxide (IV) SO 2:

S + 2H 2 SO 4 \u003d 3SO 2 + 2H 2 O

C + 2H 2 SO 4 \u003d 2SO 2 + CO 2 + 2H 2 O

Getting and using

In industry, sulfuric acid is obtained by contact. The acquisition process takes place in three stages:

1. Obtaining SO 2 by roasting pyrite:

4FeS 2 + 11O 2 = 2Fe 2 O 3 + 8SO 2

1. Oxidation of SO 2 to SO 3 in the presence of a catalyst - vanadium (V) oxide:

2SO 2 + O 2 \u003d 2SO 3

1. Dissolution of SO 3 in sulfuric acid:

H2SO4+ n SO 3 \u003d H 2 SO 4 ∙ n SO 3

The resulting oleum is transported in iron tanks. Sulfuric acid of the required concentration is obtained from oleum by pouring it into water. This can be expressed in a diagram:

H 2 SO 4 ∙ n SO 3 + H 2 O \u003d H 2 SO 4

Sulfuric acid finds a variety of uses in the most various areas National economy. It is used for drying gases, in the production of other acids, for the production of fertilizers, various dyes and medicines.

Salts of sulfuric acid

Most sulfates are highly soluble in water (slightly soluble CaSO 4 , even less PbSO 4 and practically insoluble BaSO 4). Some sulfates containing water of crystallization are called vitriol:

CuSO 4 ∙ 5H 2 O copper sulfate

FeSO 4 ∙ 7H 2 O ferrous sulfate

Salts of sulfuric acid have everything. Their relation to heating is special.

sulfates active metals( , ) do not decompose even at 1000 ° C, while others (Cu, Al, Fe) - decompose upon slight heating into metal oxide and SO 3:

CuSO 4 \u003d CuO + SO 3

Download:

Download free abstract on the topic: "Production of sulfuric acid by contact method"

You can download essays on other topics

*on the image of the record is a photograph of copper sulphate

The +4 oxidation state for sulfur is quite stable and manifests itself in SHal 4 tetrahalides, SOHal 2 oxodihalides, SO 2 dioxide, and their corresponding anions. We will get acquainted with the properties of sulfur dioxide and sulfurous acid.

1.11.1. Sulfur oxide (IV) The structure of the so2 molecule

The structure of the SO 2 molecule is similar to the structure of the ozone molecule. The sulfur atom is in a state of sp 2 hybridization, the shape of the orbitals is a regular triangle, the shape of the molecule is angular. The sulfur atom has an unshared electron pair. The S-O bond length is 0.143 nm, the bond angle is 119.5°.

The structure corresponds to the following resonant structures:

Unlike ozone, the multiplicity of the S-O bond is 2, i.e., the main contribution is made by the first resonant structure. The molecule is characterized by high thermal stability.

Physical properties

Under normal conditions, sulfur dioxide or sulfur dioxide is a colorless gas with a pungent suffocating odor, melting point -75 °C, boiling point -10 °C. Let's well dissolve in water, at 20 °C in 1 volume of water 40 volumes of sulfur dioxide are dissolved. Toxic gas.

Chemical properties of sulfur oxide (IV)

Sulfur dioxide is highly reactive. Sulfur dioxide is an acid oxide. It is quite soluble in water with the formation of hydrates. It also partially interacts with water, forming a weak sulfurous acid, which is not isolated individually:

SO 2 + H 2 O \u003d H 2 SO 3 \u003d H + + HSO 3 - \u003d 2H + + SO 3 2-.

As a result of dissociation, protons are formed, so the solution has an acidic environment.

When sulfur dioxide gas is passed through a sodium hydroxide solution, sodium sulfite is formed. Sodium sulfite reacts with excess sulfur dioxide to form sodium hydrosulfite:

2NaOH + SO 2 = Na 2 SO 3 + H 2 O;

Na 2 SO 3 + SO 2 \u003d 2NaHSO 3.

Sulfur dioxide is characterized by redox duality, for example, it, showing reducing properties, discolors bromine water:

SO 2 + Br 2 + 2H 2 O \u003d H 2 SO 4 + 2HBr

and potassium permanganate solution:

5SO 2 + 2KMnO 4 + 2H 2 O \u003d 2KНSO 4 + 2MnSO 4 + H 2 SO 4.

oxidized by oxygen to sulfuric anhydride:

2SO 2 + O 2 \u003d 2SO 3.

It exhibits oxidizing properties when interacting with strong reducing agents, for example:

SO 2 + 2CO \u003d S + 2CO 2 (at 500 ° C, in the presence of Al 2 O 3);

SO 2 + 2H 2 \u003d S + 2H 2 O.

Production of sulfur oxide (IV)

Burning sulfur in air

S + O 2 \u003d SO 2.

Sulfide oxidation

4FeS 2 + 11O 2 \u003d 2Fe 2 O 3 + 8SO 2.

The action of strong acids on metal sulfites

Na 2 SO 3 + 2H 2 SO 4 \u003d 2NaHSO 4 + H 2 O + SO 2.

1.11.2. Sulfuric acid and its salts

When sulfur dioxide is dissolved in water, weak sulfurous acid is formed, the bulk of the dissolved SO 2 is in the form of a hydrated form of SO 2 H 2 O, upon cooling, a crystalline hydrate is also released, only a small part of the sulfurous acid molecules dissociates into sulfite and hydrosulfite ions. In the free state, the acid is not isolated.

Being dibasic, it forms two types of salts: medium - sulfites and acidic - hydrosulfites. Only alkali metal sulfites and hydrosulfites of alkali and alkaline earth metals dissolve in water.