Sulfuric acid production
“There is hardly another artificially produced substance so often used in technology as sulfuric acid...”
(D.I. Mendeleev)
FeS2- pyrite, sulfur pyrite, iron pyrite
S8 native rhombic sulfur
H2S – hydrogen sulfide
WITH u2S; ZnS; PbS – non-ferrous sulfides metals
CaSO4*2H2O – gypsum
Production technology
Production technology
Stage I: Pyrite firing
Kiln in
"fluidized bed"
1. Large pieces of pyrite are crushed, small pieces are sintered;
2. Enrich the air with oxygen;
3. Heat exchange, because temperature above 8000C;
4. The thick walls of the oven are lined with steel.
Stage II. Cyclone
Cleaning from
coarse dust.
Double cylinder, centrifugal force, gravitational attraction force.
Stage II. Electrostatic precipitator
Cleaning from
fine dust
The grid is positively charged
Wire negative
Stage II. Drying tower
Ceramic tubes - “nozzle”, increase the contact area.
Concentrated sulfuric acid on top, “furnace gas” on the bottom.
Cleaning the stove
gas"
Heat exchanger and contact apparatus
Heat exchange:
Stage III.
Oxidation of sulfur(IV) oxide to sulfur(VI) oxide
2 SO2(g) + O2(g) Û 2 SO3(g) +Q
1.Connections
2.Exothermic
3.Homogeneous
4.Catalytic
5.Reversible
6. Redox
Absorption
tower
Ceramic tubes - increasing the contact area.
Sulfuric acid on top, sulfur(VI) oxide on bottom.
Counterflow principle.
Preparation of oleum
SO3 + H2SO4 ® H2S2O7
Dispersion to-that
H2S2O7 + SO3 ® H2S3O10 OLEUM
Trisernaya to-that
H2S3O10 + SO3 ® H2S4O13
Tetrasulfur to-that
Stage IV.
Absorption of sulfur (VI) oxide by water
SO 3(g)+ N 2ABOUT(g) ® N 2SO4(l) + Q
1.Connections
2.Exothermic
3.Heterogeneous
4.Non-catalytic
5.Irreversible
6.No change in oxidation states
Complete H2SO4 production process
Application of sulfuric acid
Ø1. Production of mineral fertilizers.
Ø2. Production of sulfates (salts of sulfuric acid).
Ø3. Production of synthetic fibers.
Ø4. Ferrous and non-ferrous metallurgy.
Ø5. Production of organic dyes.
Ø6. Alcohols, acids, esters (organic substances).
Ø7. Food industry (molasses, glucose), emulsifier (thickener) E513.
Ø8. Petrochemicals (mineral oils).
Ø9. Production of explosives
Application of sulfuric acid
Technological principles for the production of sulfuric acid
1. The principle of continuity
2. The principle of integrated use of raw materials, the use of waste from other production
3. The principle of waste-free production
4. Heat transfer principle
5. Counterflow principle (“fluidized bed”)
6. The principle of automation and mechanization of production processes.
Transportation and storage of sulfuric acid
Transported in railway and road tankers made of acid-resistant steel
Store in hermetically sealed containers made of polymer or stainless steel, coated with an acid-resistant film.
Solving environmental problems
1. Use of technological schemes, minimizing air pollution
2. Improvement of technological
equipment, in particular various filters and absorbers
Sulfuric acid
Completed by a student of grade 9 “A” Smolyaninova Yulia.
- Sulfuric acid is a colorless oily liquid.
- It hardens into a crystalline mass at a temperature of +10°C.
- Sulfuric acid has a density of 1.84 g/cm3.
- 1 liter of such acid weighs 2 kg.
- The acid hardens at a temperature of -20°C.
- When this acid dissolves in water, a large amount of heat will be released due to the formation of hydrates.
- These hydrates can be isolated from solution at low temperatures in solid form.
Chemical properties
A dilute acid also exhibits oxidizing properties, so it reacts with metals that are in the activity series before hydrogen
H 2 SO 4 + Zn = H 2 + ZnSO 4
Reacts with basic oxides:
H 2 SO 4 + CuO = CuSO 4 + H 2 O
Chemical properties
With hydroxides:
Cu(OH) 2 + H 2 SO 4 = CuSO 4 + 2H 2 O
2NaOH + H 2 SO 4 = Na 2 SO 4 + 2H 2 O
- Cu(OH) 2 + H 2 SO 4 = CuSO 4 + 2H 2 O 2NaOH + H 2 SO 4 = Na 2 SO 4 + 2H 2 O
Interaction with salts during metabolic reactions:
H 2 SO 4 + BaCl 2 = 2HCl + BaSO 4
(in the cold)" width="640" Chemical properties
- Some metals (Al, Cr, Fe) do not react with concentrated acid.
- This occurs due to the formation of a protective film on the metal surface.
Fe + H2SO4 (conc.) = (cold)
- The production of mineral fertilizers is the largest area of application.
- Electrolyte in lead batteries
- Petroleum products purification
- Production of synthetic detergents, dyes, plastics, hydrogen fluoride and other reagents.
- Ore beneficiation in the mining industry
- Metalworking, textile, leather and other industries
- Production of medicinal products
- Sulfuric acid and oleum are very corrosive substances.
- They affect the skin, mucous membranes, and respiratory tract (cause chemical burns).
- When inhaling the vapors of these substances, they cause difficulty breathing, coughing, and often laryngitis, tracheitis, bronchitis, etc.
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Slide captions:
Center for Distance Education of Disabled Children at OSAOU "Belgorod Engineering Youth Boarding School" SULFURIC ACID Prepared by: chemistry teacher, Bykova O.S.
Sulfuric acid H2SO4 is a strong dibasic acid corresponding to the highest oxidation state of sulfur (+6). Under normal conditions, concentrated sulfuric acid is a heavy, oily liquid, colorless and odorless, with a sour “copper” taste. In technology, sulfuric acid is a mixture of both water and sulfuric anhydride SO3.
Molecules and ions of sulfuric acid have a tetrahedral structure.
FeS 2 S H 2 S SO 2 → SO 3 → H 2 SO 4 Pyrite Sulfur pyrite Production of sulfuric acid
General properties of acid solutions
Dilution of sulfuric acid
I. Chemical properties of dilute sulfuric acid 1. Dissociation: H 2 SO 4 H + + HSO 4 - HSO 4 - ↔ H + + SO 4 2 -
2. Interaction with metals (up to H) Zn + H 2 SO 4 → ZnSO 4 + H 2 Mg + H 2 SO 4 → MgSO 4 + H 2 Cu + H 2 SO 4 →
3. Interaction with basic and amphoteric oxides CuO + H 2 SO 4 → CuSO 4 + H 2 O CuO + 2 H + → Cu 2 + + H 2 O ZnO + H 2 SO 4 → ZnSO 4 + H 2 O ZnO + 2 H + → Zn 2+ + H 2 O
4 . Interaction with bases and amphoteric hydroxides 2NaOH + H 2 SO 4 → Na 2 SO 4 +2 H 2 O H + + OH - → H 2 O NaOH + H 2 SO 4 → Na H SO 4 +H 2 O Acid salt sodium hydrosulfate Zn(OH) 2 + H 2 SO 4 → ZnSO 4 +2H 2 O Zn(OH) 2 + 2 H + → Zn 2+ +2H 2 O
5. Interaction with salts H 2 SO 4 +BaCI 2 = BaSO 4 ↓ + 2HCI Ba 2+ +SO 4 2- = BaSO 4 ↓ K 2 CO 3 + H 2 SO 4 = K 2 SO 4 + CO 2 + H 2 O 2 H + + CO 3 2- = CO 2 + H 2 O
Qualitative reaction H 2 SO 4 +BaCI 2 = BaSO 4 ↓ + 2HCI Ba 2+ + SO 4 2- = BaSO 4 ↓
Sulfuric acid displaces more volatile acids NaCI + H 2 SO 4 → NaHSO4 + HCI
Properties of concentrated sulfuric acid Organic substances become carbonized!!! C12H22O11 (sucrose) → 12С (coal)
concentrated sulfuric acid oxidizes nonmetals HeMe + H2SO4(conc.) = H2O + SO2 + oxygen-containing acid HeMe, C + 2H2SO4 = 2H2O + CO2 + 2SO2 S + 2H2SO4 = 3SO2 + 2H2O 2P + 5H2SO4 = 2H3PO4 + 5SO2 + 2H2O
concentrated sulfuric acid oxidizes metals; concentrated H2+6SO4 is a strong oxidizing agent; when interacting with metals (except Au, Pt) it can be reduced to S+4O2, S0 or H2S-2 (Fe, Al, Cr also do not react without heating - they are passivated): 2Ag + 2H2SO4 → Ag2SO4 + SO2+ 2H2O 8Na + 5H2SO4 → 4Na2SO4 + H2S + 4H2O
Thank you for your attention!
If these statements are true in your opinion, then put a “+” sign opposite them, and if not, then a “-” sign.
1. The properties of concentrated sulfuric acid are due to the fact that the oxidation state of sulfur in it is +6 2. Concentrated sulfuric acid is a reducing agent. 3. Concentrated sulfuric acid cannot be transported in steel tanks, because steel contains iron 4. Concentrated sulfuric acid does not interact with metals after hydrogen. 5. Concentrated sulfuric acid reacts with non-metals 6. Concentrated sulfuric acid dissociates almost completely to form hydrogen ions and sulfate ions. 7. Products of sulfur reduction in sulfuric acid can have oxidation states +4, -2. 8. Aluminum is destroyed in concentrated sulfuric acid. 9. Concentrated sulfuric acid has no effect on organic substances 10. Concentrated sulfuric acid can displace other acids from their salts