Industrial Preparation and Manufacture of Sulphuric Acid (H₂SO₄)
The Manufacturing Process of Sulphuric Acid
Properties and Applications of Sulphuric Acid
- Physical and Chemical Properties
- Applications
Advanced Processes and Uses
- The Sulfur-Iodine Cycle
- Recycling in Industrial Use
Concentrated Sulphuric Acid Properties
The Significance of Sulphuric Acid in NEET Exams
Conclusion
FAQ’s

Sulphuric Acid: Industrial Process of Manufacture

Industrial Preparation and Manufacture of Sulphuric Acid (H₂SO₄)

Sulphuric acid (H₂SO₄), often known as oil of vitriol or hydrogen sulfate, is one of the most essential compounds in the chemical industry. Its industrial preparation of sulphuric acid involves a highly efficient and controlled process to meet the demands of various sectors.

The industrial manufacture of sulphuric acid primarily employs the Contact Process or Chamber Process, which combines sulfur dioxide and oxygen to produce sulfur trioxide, further reacted with water to yield H₂SO₄. This sulphuric acid manufacturing process is critical for producing fertilizers, detergents, pharmaceuticals, and other industrial chemicals.

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The Manufacturing Process of Sulphuric Acid

Step 1: Sulfur Dioxide Preparation

The industrial preparation of sulphur involves burning sulfur in the presence of oxygen, yielding sulfur dioxide (SO₂). This step is foundational in the industrial preparation of H₂SO₄ and ensures a consistent supply of SO₂ for further reactions.

Reaction: $S(s) + O₂(g) → SO₂(g)$ $S$ $($ $s$ $)$ $+$ $O$ $2$ $$ $($ $g$ $)$ $\to$ $SO$ $2$ $$ $($ $g$ $)$

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Step 2: Conversion to Sulfur Trioxide

Sulfur dioxide is then mixed with oxygen in the presence of a vanadium pentoxide (V₂O₅) catalyst at 400–450°C under 1–2 atm pressure to form sulfur trioxide (SO₃). This reaction, central to the H₂SO₄ manufacturing process, is highly exothermic and reversible.

Reaction: $2SO₂(g) + O₂(g) ⇌ 2SO₃(g)$ $2$ $SO$ $2$ $$ $($ $g$ $)$ $+$ $O$ $2$ $$ $($ $g$ $)$ $⇌$ $2$ $SO$ $3$ $$ $($ $g$ $)$

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Step 3: Production of Sulphuric Acid

Sulfur trioxide cannot be directly dissolved in water as it causes fog formation. Instead, SO₃ is absorbed into concentrated sulfuric acid to form oleum (H₂S₂O₇). The oleum is then diluted with water to produce concentrated sulfuric acid.

Reactions: $H₂SO₄ + SO₃(g) → H₂S₂O₇(l)$ $H$ $2$ $$ $SO$ $4$ $$ $+$ $SO$ $3$ $$ $($ $g$ $)$ $\to$ $H$ $2$ $$ $S$ $2$ $$ $O$ $7$ $$ $($ $l$ $)$ $H₂S₂O₇(l) + H₂O(l) → 2H₂SO₄$ $H$ $2$ $$ $S$ $2$ $$ $O$ $7$ $$ $($ $l$ $)$ $+$ $H$ $2$ $$ $O$ $($ $l$ $)$ $\to$ $2$ $H$ $2$ $$ $SO$ $4$ $$ This complete cycle forms the backbone of the manufacturing process of sulphuric acid used worldwide.

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Properties and Applications of Sulphuric Acid

Physical and Chemical Properties

Sulphuric acid is a colorless, oily liquid with a high affinity for water, making it an excellent dehydrating agent. It ionizes completely in aqueous solutions, forming hydronium (H₃O⁺), hydrogen sulfate (HSO₄⁻), and sulfate ions (SO₄²⁻). Its strong oxidizing nature allows it to react with metals, nonmetals, and organic substances at high temperatures.

Applications

The industrial production of sulphuric acid supports numerous sectors:

Fertilizer Manufacturing: Used in the “wet process” to produce phosphoric acid for phosphate fertilizers.
Chemical Synthesis: Essential in the production of detergents, dyes, pigments, and medicines.
Industrial Cleaning: Removes rust, scaling, and oxidation from metals in industries like automotive and steel manufacturing.
Energy Storage: Serves as an electrolyte in lead-acid batteries.
Water Treatment: Aids in wastewater management and purification.

Advanced Processes and Uses

The Sulfur-Iodine Cycle

The sulfur–iodine cycle utilizes thermochemical reactions to produce hydrogen from water. Though promising for hydrogen production, the process involves handling highly corrosive acids at extreme temperatures, posing safety challenges.

Recycling in Industrial Use

Spent sulfuric acid from processes like metal cleaning is recycled in Spent Acid Regeneration (SAR) facilities. The waste acid is burned, and the resulting SO₂ and SO₃ gases are used to produce fresh sulfuric acid.

Concentrated Sulphuric Acid Properties

Concentrated sulfuric acid (98-100%) is a weak electrolyte at ambient temperatures but reacts vigorously when heated. Its high affinity for water allows it to dehydrate organic materials, leaving a carbon residue, as seen in reactions with carbohydrates like sucrose.

The Significance of Sulphuric Acid in NEET Exams

For students preparing for NEET, the manufacturing process of sulphuric acid is a key topic. Understanding reactions, catalysts, and applications is crucial. Detailed notes, problem-solving techniques, and step-by-step explanations are provided by Infinity Learn experts to ensure clarity and better marks in the exams.

Conclusion

The industrial preparation of sulphuric acid is a cornerstone of modern chemical industries, driving advancements in fertilizers, energy storage, and materials processing. Its versatile nature and wide-ranging applications make it an indispensable compound in industrial chemistry.

FAQ’s

Is sulfuric acid molecular or ionic?

Between H2O and H3O+ and -OH, water forms a compromise. Nothing is ionic as a result of this. Because all of the bonds in sulfuric acid are covalent, it is a covalent chemical. The fact that it ionizes easily is beside the point.

What is the best way to neutralize sulfuric acid?

Pour baking soda immediately into an acid spill. Light acids like vinegar, as well as dangerous, powerful acids like muriatic and sulphuric acids, will be neutralized by this method. To neutralize the acid, cover the entire contaminated area with baking soda (sodium bicarbonate).

What is the purpose of sulfuric acid?

The most common use of sulfuric acid is in fertilizer production. It's used to make sulfate salts, synthetic detergents, and pigments, among other things.