Industrial inorganic chemistry

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1. Industrial Inorganic Chemistry Presenter: Muhammad Saud Khalid Roll# 16103123-036

2. Inorganic Chemistry: It deals with the study of all elements and their compounds except those of compounds of carbon and hydrogen (hydrocarbons) and their derivatives.   Inorganic compounds are not covalently bonded they have more of ionic character than covalent character. Important classes of inorganic compounds are the  oxides , the  carbonates , the  sulphates , and the  halides etc. For example ZnO , Al 2 O 3 , HNO 3 , CaCO 3 , HCl etc.

3. Industrial Inorganic Chemistry Industrial inorganic chemistry includes subdivisions of the chemical industry that manufacture: a) Inorganic products on a large scale such as the heavy in-organics (  sulphuric acid, sulphates ) and fertilizers (potassium, nitrogen, and phosphorus products) b) Segments of fine chemicals that are used to produce high purity inorganics on a much smaller scale. Among these are  reagents  and raw materials used in high-tech industries, pharmaceuticals or electronics, for example, as well as in the preparation of inorganic specialties such as catalysts, pigments and medicines etc.

4. Inorganic chemistry is extremely important for many industries, but there are a handful of reactions which are of primary importance to the Chemical Industry. The natural sources for industrial manufacture of inorganic products, ranging from air to water via sulphur , phosphates, mineral salts and metal oxides.

5. Sources For Industrial Manufacture of Inorganic compounds Air contains molecular nitrogen and oxygen. They may be separated by  liquefaction  and  fractional distillation  along with  inert  gases, especially argon. Metals such as Fe, Cu, or P, K and Ca are obtained from mineral ores. Salt or  brine  can be used as sources of chlorine and sometimes NaOH , and Na 2 CO 3.

6. Sulphuric Acid Sulphuric acid H 2 SO 4 : 1) Generally it is produced by the contact process : a) Exothermic air oxidation of SO 2 (V 2 O 5 or Pt catalyst ). b) SO 3 is absorbed into 100% H 2 SO 4 to give a mixture disulphuric and sulphuric acids, known as Oleum . c) Oleum is hydrolyzed to H 2 SO 4.

7. Sulphuric Acid Uses Of Sulphuric acid as a source of raw material in some industries 1) 90% of the sulphur produced industrially is converted to H 2 SO 4 . 2 ) 2/3 of the H 2 SO 4 produced is consumed in fertilizer manufacture, to make ammonium sulphate : (NH 4 ) 2 SO 4 or superphosphate: 32% CaHPO 4 /Ca(H 2 PO 4 ) 2 •H 2 O 3% H 3 PO 4 50% CaSO 4 or potassium sulphate : K 2 SO 4 ( Mannheim process ) 3 ) H 2 SO 4 is also used to make chlorine dioxide ClO 2 for bleaching paper pulp and for sterilizing water. i ) Mathieson process : ii) Solvay process :

8. Nitrogen for Fertilizers Urea : 1 ) It is made by reaction of ammonia and the CO 2 by-product of the water-gas shift reaction . 2) It can be produced in forms that release nitrogen slowly to the soil: a) “SCU” fertilizers are urea pellets coated with ~2% paraffin wax containing S 8 that oxidizes away slowly in the soil. b) Urea-formaldehyde (UF) polymers decompose slowly in the ground. Ammonium sulphate : It is a safe form of ammonia for shipping, storage and use.

9. Nitrogen for Fertilizers Nitric Acid and Ammonium Nitrate : 1) The catalytic oxidation of ammonia by air over Pt gauze at ~900°C gives nitric oxide (NO 2 ) which is then converted to nitric acid by air and H 2 O ( l ) to give the net reaction : 2) Nitric acid is converted on-site to ammonium nitrate : 3) NH 4 NO 3 is potentially explosive!! 4) Calcium carbonate CaCO 3 (chalk, limestone) can be added to solid NH 4 NO 3 to form a non-explosive product. 5) NH 4 NO 3 can be stored safely as a dilute aqueous solution. 6) 3% clay can be added as a drying agent to prevent caking (34-0-0)

10. Ammonia (NH 3 ) Ammonia (NH 3 ) is prepared using the Haber process . Nitrogen and hydrogen will react together under these conditions: a high temperature - about 450ºC a high pressure - about 200 atmospheres (200 times normal pressure) an iron catalyst The Haber Process combines nitrogen from the air with hydrogen derived mainly from natural gas (methane) into ammonia. The reaction is reversible and the production of ammonia is exothermic.

11. Nitrogen for Explosives and Propellants Ammonium Nitrate : It is the most commonly used blasting explosive. 2) Gentle heating to its melting point (170°C) gives nitrous oxide : 3) @ T>250°C, or when shocked, violent decomposition to N 2 : 4) It is commonly mixed with an oxidizable substance (fuel oil) for legitimate use as a relatively safe and inexpensive explosive.

12. Nitrogen for Explosives and Propellants Potassium Nitrate, KNO 3 (Saltpeter) : Used for black powder : (41% KNO 3 , 29.5% C, 29.5% S): for firearms (before guncotton ) (75% KNO 3 15% C, 10% S): for fireworks, time fuses etc . Hydrazine, H 2 NNH 2 , Used for rocket propellants : The hydrazine is oxidized by H 2 O 2 , O 2( l ) , or F 2( l ) .

13. Chlorine Chlorate ion ClO 3 ¯ : 1 ) Cl 2 dissolved in hot, concentrated aqueous NaOH forms ClO 3 ¯ 2) Chlorate salts are strong oxidizing agents….KClO 3 can be used in place of KNO 3 as an oxidant for C and S in black powder . 3) Chlorate salts can be used as an unselective herbicide. 4) Chlorate salts are mainly used as a source of ClO 2 for bleaching paper pulp and for sterilizing water. Recall : Mathieson process and Solvay process

14. Chlorine Hypochlorite ion OCl ¯ and Hypochlorous acid HOCl : Cl 2 disproportionates when dissolved in water 2) HOCl decomposes slowly releasing oxygen Since HOCl is a powerful disinfectant, Cl 2 is used to treat water. 3) Cl 2 dissolved in cold, dilute aqueous NaOH generates kinetically stable solutions of OCl ¯…. HOUSEHOLD BLEACH !