Chemistry
Explore all chapters, materials, and resources below
Unit 1: Foundation and Fundamentals
Unit 2: Stoichiometry
Unit 3: Atomic Structure
Unit 4: Classification of Elements and Periodic Table
Unit 5: Chemical Bonding and Shapes of Molecules
Unit 6: Oxidation and Reduction
Unit 7: States of Matter
Unit 8: Chemical Equilibrium
9.1. Hydrogen, Oxygen and ozone : 4 teaching hours
9.2 Nitrogen
9.3 Halogens
9.4 Carbon and Phosphorus
9.5 Sulphur :
10.1 Metals and Metallurgical Principles
10.2 Alkali and Alkaline earth Metals
Unit- 11. Bio-inorganic Chemistry : 3 teaching hours
Unit- 12. Basic Concept of Organic Chemistry : 6 teaching hours
Unit 13. Fundamental Principles of Organic Chemistry : 10 teaching hours
Unit 14. Hydrocarbons : 8 teaching hours
Unit 15. Aromatic Hydrocarbons : 6 teaching hours
Unit: 16 Fundamentals of Applied Chemistry : 4 teaching hours
Unit: 17 Modern Chemical Manufactures
Syllabus
General and Physical Chemistry : 48 teaching hours.
Unit -1 . Foundation and Fundamentals : 2 teaching hours
General introduction of chemistry, Importance and scope of chemistry, Basic concepts of chemistry (atoms, molecules, relative masses of atoms and molecules, atomic mass unit ( amu), radicals, molecular formula, empirical formula ), Percentage composition from molecular formula.
Unit -2 . Stoichiometry : 8 teaching hours
Dalton’s atomic theory and its postulates , Laws of stoichiometry, Avogadro’s law and some deductions ( Molecular mass and vapour density , Molecular mass and volume of gas, Molecular mass and no. of particles) , Mole and its relation with mass, volume and number of particles; Calculations based on mole concept ; Limiting reactant and excess reactant ;Theoretical yield, experimental yield and % yield ; Calculation of empirical and molecular formula from % composition (Solving related numerical problems)
Unit -3 . Atomic Structure : 8 teaching hours
Rutherford’s atomic model ; Limitations of Rutherford’s atomic model; Postulates of Bohr’s atomic model and its application ; Spectrum of hydrogen atom ; Defects of Bohr’s theory; Elementary idea of quantum mechanical model: de Broglie’s wave equation; Heisenberg’s Uncertainty Principle ; Concept of probability; Quantum Numbers ; Orbitals and shape of s and p orbitals only; Aufbau Principle; Pauli’s exclusion principle; Hund’s rule and electronic configurations of atoms and ions (up to atomic no. 30)
Unit-4. Classification of elements and Periodic Table: 5 teaching hours
Modern periodic law and modern periodic table; Classification of elements into different groups, periods and blocks ; IUPAC classification of elements; Nuclear charge and effective nuclear charge ;Periodic trend and periodicity : Atomic radii ,Ionic radii , Ionization energy , Electron affinity ,Electronegativity , Metallic characters (General trend and explanation only)
Unit-5. Chemical Bonding and Shapes of Molecules : 9 teaching hours
Valence shell, valence electron and octet theory ; Ionic bond and its properties ; Covalent bond and coordinate covalent bond ;Properties of covalent compounds ; Lewis dot structure of some common compounds of s and p block elements ; Resonance ;VSEPR theory and shapes of some simple molecules (BeF2, BF3, CH4, CH3Cl, PCl5, SF6, H2O,NH3,CO2,H2S, PH3); Elementary idea of Valence Bond Theory; Hybridization involving s and p orbitals only ; Bond characteristics: Bond length, Ionic character, Dipole moment; Vander Waal’s force and molecular solids ; Hydrogen bonding and its application; Metallic bonding and properties of metallic solids
Unit-6. Oxidation and Reduction : 5 teaching hours
General and electronic concept of oxidation and reduction; Oxidation number and rules for assigning oxidation number ; Balancing redox reactions by oxidation number and ion-electron (half reaction) method ; Electrolysis : Qualitative aspect and Quantitative aspect(Faradays laws of electrolysis)
Unit-7. States of Matter : 8 teaching hours
7.1 Gaseous state : Kinetic theory of gas and its postulates ;Gas laws -Boyle’s law and Charles’ law, Avogadro’s law ;Combined gas equation ;Dalton’s law of partial pressure ;Graham’s law of diffusion; Ideal gas and ideal gas equation ; Universal gas constant and its significance; Deviation of real gas from ideality (Solving related numerical problems based on gas laws)
7.2 Liquid state : Physical properties of liquids- Evaporation and condensation ,Vapour pressure and boiling point ,Surface tension and viscosity (qualitative idea only) ; Liquid crystals and their applications
7.3 Solid state : Types of solids -Amorphous and crystalline solids, Efflorescent, Deliquescent and Hygroscopic solids ; Crystallization and crystal growth; Water of crystallization; Introduction to unit crystal lattice and unit cell .
Unit-8. Chemical equilibrium: 3 teaching hours
Physical and chemical equilibrium; Dynamic nature of chemical equilibrium; Law of mass action; Expression for equilibrium constant and its importance; Relationship between Kp and Kc ; Le Chatelier’s Principle (Numericals not required)
Unit -1 . Foundation and Fundamentals : 2 teaching hours
General introduction of chemistry, Importance and scope of chemistry, Basic concepts of chemistry (atoms, molecules, relative masses of atoms and molecules, atomic mass unit ( amu), radicals, molecular formula, empirical formula ), Percentage composition from molecular formula.
Unit -2 . Stoichiometry : 8 teaching hours
Dalton’s atomic theory and its postulates , Laws of stoichiometry, Avogadro’s law and some deductions ( Molecular mass and vapour density , Molecular mass and volume of gas, Molecular mass and no. of particles) , Mole and its relation with mass, volume and number of particles; Calculations based on mole concept ; Limiting reactant and excess reactant ;Theoretical yield, experimental yield and % yield ; Calculation of empirical and molecular formula from % composition (Solving related numerical problems)
Unit -3 . Atomic Structure : 8 teaching hours
Rutherford’s atomic model ; Limitations of Rutherford’s atomic model; Postulates of Bohr’s atomic model and its application ; Spectrum of hydrogen atom ; Defects of Bohr’s theory; Elementary idea of quantum mechanical model: de Broglie’s wave equation; Heisenberg’s Uncertainty Principle ; Concept of probability; Quantum Numbers ; Orbitals and shape of s and p orbitals only; Aufbau Principle; Pauli’s exclusion principle; Hund’s rule and electronic configurations of atoms and ions (up to atomic no. 30)
Unit-4. Classification of elements and Periodic Table: 5 teaching hours
Modern periodic law and modern periodic table; Classification of elements into different groups, periods and blocks ; IUPAC classification of elements; Nuclear charge and effective nuclear charge ;Periodic trend and periodicity : Atomic radii ,Ionic radii , Ionization energy , Electron affinity ,Electronegativity , Metallic characters (General trend and explanation only)
Unit-5. Chemical Bonding and Shapes of Molecules : 9 teaching hours
Valence shell, valence electron and octet theory ; Ionic bond and its properties ; Covalent bond and coordinate covalent bond ;Properties of covalent compounds ; Lewis dot structure of some common compounds of s and p block elements ; Resonance ;VSEPR theory and shapes of some simple molecules (BeF2, BF3, CH4, CH3Cl, PCl5, SF6, H2O,NH3,CO2,H2S, PH3); Elementary idea of Valence Bond Theory; Hybridization involving s and p orbitals only ; Bond characteristics: Bond length, Ionic character, Dipole moment; Vander Waal’s force and molecular solids ; Hydrogen bonding and its application; Metallic bonding and properties of metallic solids
Unit-6. Oxidation and Reduction : 5 teaching hours
General and electronic concept of oxidation and reduction; Oxidation number and rules for assigning oxidation number ; Balancing redox reactions by oxidation number and ion-electron (half reaction) method ; Electrolysis : Qualitative aspect and Quantitative aspect(Faradays laws of electrolysis)
Unit-7. States of Matter : 8 teaching hours
7.1 Gaseous state : Kinetic theory of gas and its postulates ;Gas laws -Boyle’s law and Charles’ law, Avogadro’s law ;Combined gas equation ;Dalton’s law of partial pressure ;Graham’s law of diffusion; Ideal gas and ideal gas equation ; Universal gas constant and its significance; Deviation of real gas from ideality (Solving related numerical problems based on gas laws)
7.2 Liquid state : Physical properties of liquids- Evaporation and condensation ,Vapour pressure and boiling point ,Surface tension and viscosity (qualitative idea only) ; Liquid crystals and their applications
7.3 Solid state : Types of solids -Amorphous and crystalline solids, Efflorescent, Deliquescent and Hygroscopic solids ; Crystallization and crystal growth; Water of crystallization; Introduction to unit crystal lattice and unit cell .
Unit-8. Chemical equilibrium: 3 teaching hours
Physical and chemical equilibrium; Dynamic nature of chemical equilibrium; Law of mass action; Expression for equilibrium constant and its importance; Relationship between Kp and Kc ; Le Chatelier’s Principle (Numericals not required)
Inorganic Chemistry : 35 teaching hours
Unit-9. Chemistry of Non-metal :
9.1. Hydrogen, Oxygen and ozone : 4 teaching hours
9.1.1 Hydrogen : Chemistry of atomic and nascent hydrogen ; Isotopes of hydrogen and their uses; Application of hydrogen as fuel ; Heavy water and its applications
9.1.2 Oxygen : Allotropes of Oxygen – Definition of allotropy and examples; Types of oxides (acidic, basic, neutral, amphoteric, peroxide and mixed oxides) ; Applications of hydrogen peroxide; Medical and industrial application of oxygen
9.1.3 Ozone: Occurrence ; Preparation of ozone from oxygen; Structure of ozone; Test for ozone; Ozone layer depletion (causes, effects and control measures) ; Uses of ozone
9.2 Nitrogen : 5 teaching hours
Reason for inertness of nitrogen and active nitrogen ; Chemical properties of ammonia [ Action with CuSO4 solution, water, FeCl3 solution, Conc. HCl, Mercurous nitrate paper, O2 ]; Applications of ammonia; Harmful effects of ammonia ; Oxy-acids of nitrogen (name andformula); Chemical properties of nitric acid [HNO3 as an acid and oxidizing agent (action with zinc, magnesium, iron, copper, sulphur, carbon, SO2 and H2S) ; Ring test for nitrate ion.
9.3 Halogens: 5 teaching hours
General characteristics of halogens; Comparative study on preparation (no diagram and description is required); Chemical properties [with water, alkali, ammonia, oxidizing character, bleaching action] and uses of halogens (Cl2, Br2 and I2); Test for Cl2, Br2 and I2 ; Comparative study on preparation (no diagram and description is required), properties ( reducing strength, acidic nature and solubility) and uses of haloacids (HCl, HBr and HI)
9.4 Carbon and Phosphorus : 3 teaching hours
9.4.1 Carbon : Allotropes of carbon (crystalline and amorphous) including fullerenes (structure, general properties and uses only) ; Properties (reducing action, reaction with metals and nonmetals) and uses of carbon monoxide
9.4.2 Phosphorus : Allotropes of phosphorus (name only); Preparation (no diagram and description is required), properties ( basic nature ,reducing nature , action with halogens and oxygen) and uses of phosphine.
9.5 Sulphur : 5 teaching hours
Allotropes of sulphur (name only) and uses of sulphur ; Hydrogen sulphide (preparation from Kipp’s apparatus with diagram,) properties (Acidic nature, reducing nature, analytical reagent) and uses ; Sulphur dioxide its properties (acidic nature, reducing nature, oxidising nature and bleaching action) and uses ; Sulphuric acid and its properties (acidic nature, oxidising nature, dehydrating nature) and uses ; Sodium thiosulphate (formula and uses) .
Unit-10. Chemistry of Metals
10.1 Metals and Metallurgical Principles : 5 teaching hours
Definition of metallurgy and its types (hydrometallurgy, pyrometallurgy, electrometallurgy) ; Introduction of ores ; Gangue or matrix, flux and slag, alloy and amalgam ; General principles of extraction of metals (different processes involved in metallurgy) – concentration, calcination and roasting, smelting, carbon reduction, thermite and electrochemical reduction ; Refining of metals (poling and electro-refinement)
10.2 Alkali and Alkaline earth Metals : 5 teaching hours
10.2.1 Alkali Metals : General characteristics of alkali metals ; Sodium [extraction from Down’s process, properties (action with Oxygen, water, acids nonmetals and ammonia) and uses] ; Properties (precipitation reaction and action with carbon monooxide) and uses of sodium hydroxide ; Properties (action with CO2, SO2, water, precipitation reactions) and uses of sodium carbonate
10.2.2 Alkaline Earth Metals : General characteristics of alkaline earth metals ; Molecular formula and uses of (quick lime, bleaching powder, magnesia, plaster of paris and epsom salt); Solubility of hydroxides, carbonates and sulphates of alkaline earth metals (general trend with explanation) ; Stability of carbonate and nitrate of alkaline earth metals (general trend with explanation).
Unit- 11. Bio-inorganic Chemistry : 3 teaching hours
Introduction to Bio-inorganic Chemistry ; Introduction of Micro and macro nutrients ; Importance of metal ions in biological systems (ions of Na, K, Mg, Ca, Fe, Cu, Zn, Ni, Co, Cr) ; Ion pumps (sodium-potassium and sodium-glucose pump) 11.5 Metal toxicity (toxicity due to iron, arsenic, mercury, lead and cadmium)
Unit-9. Chemistry of Non-metal :
9.1. Hydrogen, Oxygen and ozone : 4 teaching hours
9.1.1 Hydrogen : Chemistry of atomic and nascent hydrogen ; Isotopes of hydrogen and their uses; Application of hydrogen as fuel ; Heavy water and its applications
9.1.2 Oxygen : Allotropes of Oxygen – Definition of allotropy and examples; Types of oxides (acidic, basic, neutral, amphoteric, peroxide and mixed oxides) ; Applications of hydrogen peroxide; Medical and industrial application of oxygen
9.1.3 Ozone: Occurrence ; Preparation of ozone from oxygen; Structure of ozone; Test for ozone; Ozone layer depletion (causes, effects and control measures) ; Uses of ozone
9.2 Nitrogen : 5 teaching hours
Reason for inertness of nitrogen and active nitrogen ; Chemical properties of ammonia [ Action with CuSO4 solution, water, FeCl3 solution, Conc. HCl, Mercurous nitrate paper, O2 ]; Applications of ammonia; Harmful effects of ammonia ; Oxy-acids of nitrogen (name andformula); Chemical properties of nitric acid [HNO3 as an acid and oxidizing agent (action with zinc, magnesium, iron, copper, sulphur, carbon, SO2 and H2S) ; Ring test for nitrate ion.
9.3 Halogens: 5 teaching hours
General characteristics of halogens; Comparative study on preparation (no diagram and description is required); Chemical properties [with water, alkali, ammonia, oxidizing character, bleaching action] and uses of halogens (Cl2, Br2 and I2); Test for Cl2, Br2 and I2 ; Comparative study on preparation (no diagram and description is required), properties ( reducing strength, acidic nature and solubility) and uses of haloacids (HCl, HBr and HI)
9.4 Carbon and Phosphorus : 3 teaching hours
9.4.1 Carbon : Allotropes of carbon (crystalline and amorphous) including fullerenes (structure, general properties and uses only) ; Properties (reducing action, reaction with metals and nonmetals) and uses of carbon monoxide
9.4.2 Phosphorus : Allotropes of phosphorus (name only); Preparation (no diagram and description is required), properties ( basic nature ,reducing nature , action with halogens and oxygen) and uses of phosphine.
9.5 Sulphur : 5 teaching hours
Allotropes of sulphur (name only) and uses of sulphur ; Hydrogen sulphide (preparation from Kipp’s apparatus with diagram,) properties (Acidic nature, reducing nature, analytical reagent) and uses ; Sulphur dioxide its properties (acidic nature, reducing nature, oxidising nature and bleaching action) and uses ; Sulphuric acid and its properties (acidic nature, oxidising nature, dehydrating nature) and uses ; Sodium thiosulphate (formula and uses) .
Unit-10. Chemistry of Metals
10.1 Metals and Metallurgical Principles : 5 teaching hours
Definition of metallurgy and its types (hydrometallurgy, pyrometallurgy, electrometallurgy) ; Introduction of ores ; Gangue or matrix, flux and slag, alloy and amalgam ; General principles of extraction of metals (different processes involved in metallurgy) – concentration, calcination and roasting, smelting, carbon reduction, thermite and electrochemical reduction ; Refining of metals (poling and electro-refinement)
10.2 Alkali and Alkaline earth Metals : 5 teaching hours
10.2.1 Alkali Metals : General characteristics of alkali metals ; Sodium [extraction from Down’s process, properties (action with Oxygen, water, acids nonmetals and ammonia) and uses] ; Properties (precipitation reaction and action with carbon monooxide) and uses of sodium hydroxide ; Properties (action with CO2, SO2, water, precipitation reactions) and uses of sodium carbonate
10.2.2 Alkaline Earth Metals : General characteristics of alkaline earth metals ; Molecular formula and uses of (quick lime, bleaching powder, magnesia, plaster of paris and epsom salt); Solubility of hydroxides, carbonates and sulphates of alkaline earth metals (general trend with explanation) ; Stability of carbonate and nitrate of alkaline earth metals (general trend with explanation).
Unit- 11. Bio-inorganic Chemistry : 3 teaching hours
Introduction to Bio-inorganic Chemistry ; Introduction of Micro and macro nutrients ; Importance of metal ions in biological systems (ions of Na, K, Mg, Ca, Fe, Cu, Zn, Ni, Co, Cr) ; Ion pumps (sodium-potassium and sodium-glucose pump) 11.5 Metal toxicity (toxicity due to iron, arsenic, mercury, lead and cadmium)
Organic Chemistry : 30 teaching hours
Unit- 12. Basic Concept of Organic Chemistry : 6 teaching hours
Introduction to organic chemistry and organic compounds ; Reasons for the separate study of organic compounds from inorganic compounds ; Tetra-covalency and catenation properties of carbon ; Classification of organic compounds ; Alkyl groups, functional groups and homologous series ; Idea of structural formula, contracted formula and bond line structural formula ; Preliminary idea of cracking and reforming, quality of gasoline, octane number, cetane number and gasoline additive
Unit 13. Fundamental Principles of Organic Chemistry : 10 teaching hours
IUPAC Nomenclature of Organic Compounds (upto chain having 6 carbon atoms) ; Qualitative analysis of organic compounds (detection of N, S and halogens by Lassaigne’s test) ; Isomerism in Organic Compounds ; Definition and classification of isomerism ; Structural isomerism and its types: chain isomerism, position isomerism, functional isomerism, metamerism and tautomerism ; Concept of geometrical isomerism (cis & trans) & optical isomerism (d & l form)
Preliminary Idea of Reaction Mechanism : Homolytic and heterolytic fission ; Electrophiles, nucleophiles and free- radicals ; Inductive effect: +I and –I effect ; Resonance effect: +R and –R effect .
Unit 14. Hydrocarbons : 8 teaching hours
14.1 Saturated Hydrocarbons (Alkanes): Preparation from haloalkanes (Reduction and Wurtz reaction), Decarboxylation, Catalytic hydrogenation of alkene and alkyne ; Chemical properties: Substitution reactions (halogenation, nitration & sulphonation only), oxidation of ethane ; Unsaturated hydrocarbons (Alkenes & Alkynes) .
14.2 Alkenes: Preparation by Dehydration of alcohol, Dehydrohalogenation, Catalytic hydrogenation of alkyne ; Chemical properties: Addition reaction with HX (Markovnikov’s addition and peroxide effect), H2O, O3, H2SO4 only
14.3 Alkynes: Preparation from carbon and hydrogen, 1,2 dibromoethane, chloroform/iodoform only ; Chemical properties: Addition reaction with (H2, HX, H2O), Acidic nature (action with Sodium, ammoniacal AgNO3 and ammoniacal Cu2Cl2) ; Test of unsaturation (ethene & ethyne): bromine water test and Baeyer’s test ;
14.4 Comparative studies of physical properties of alkane, alkene and alkyne; Kolbe’s electrolysis methods for the preparation of alkane, alkene and alkynes
Unit 15. Aromatic Hydrocarbons : 6 teaching hours
Introduction and characteristics of aromatic compounds : Huckel’s rule of aromaticity : Kekule structure of benzene : Resonance and isomerism : Preparation of benzene from decarboxylation of sodium benzoate, phenol, and ethyne only ; Physical properties of benzene ; Chemical properties of benzene: Addition reaction: hydrogen, halogen, Electrophilic substitution reactions: orientation of benzene derivatives (o, m & p), nitration, sulphonation, halogenations, Friedal-Craft’s reaction (alkylation and acylation), combustion of benzene ( free combustion only) and uses.
Unit- 12. Basic Concept of Organic Chemistry : 6 teaching hours
Introduction to organic chemistry and organic compounds ; Reasons for the separate study of organic compounds from inorganic compounds ; Tetra-covalency and catenation properties of carbon ; Classification of organic compounds ; Alkyl groups, functional groups and homologous series ; Idea of structural formula, contracted formula and bond line structural formula ; Preliminary idea of cracking and reforming, quality of gasoline, octane number, cetane number and gasoline additive
Unit 13. Fundamental Principles of Organic Chemistry : 10 teaching hours
IUPAC Nomenclature of Organic Compounds (upto chain having 6 carbon atoms) ; Qualitative analysis of organic compounds (detection of N, S and halogens by Lassaigne’s test) ; Isomerism in Organic Compounds ; Definition and classification of isomerism ; Structural isomerism and its types: chain isomerism, position isomerism, functional isomerism, metamerism and tautomerism ; Concept of geometrical isomerism (cis & trans) & optical isomerism (d & l form)
Preliminary Idea of Reaction Mechanism : Homolytic and heterolytic fission ; Electrophiles, nucleophiles and free- radicals ; Inductive effect: +I and –I effect ; Resonance effect: +R and –R effect .
Unit 14. Hydrocarbons : 8 teaching hours
14.1 Saturated Hydrocarbons (Alkanes): Preparation from haloalkanes (Reduction and Wurtz reaction), Decarboxylation, Catalytic hydrogenation of alkene and alkyne ; Chemical properties: Substitution reactions (halogenation, nitration & sulphonation only), oxidation of ethane ; Unsaturated hydrocarbons (Alkenes & Alkynes) .
14.2 Alkenes: Preparation by Dehydration of alcohol, Dehydrohalogenation, Catalytic hydrogenation of alkyne ; Chemical properties: Addition reaction with HX (Markovnikov’s addition and peroxide effect), H2O, O3, H2SO4 only
14.3 Alkynes: Preparation from carbon and hydrogen, 1,2 dibromoethane, chloroform/iodoform only ; Chemical properties: Addition reaction with (H2, HX, H2O), Acidic nature (action with Sodium, ammoniacal AgNO3 and ammoniacal Cu2Cl2) ; Test of unsaturation (ethene & ethyne): bromine water test and Baeyer’s test ;
14.4 Comparative studies of physical properties of alkane, alkene and alkyne; Kolbe’s electrolysis methods for the preparation of alkane, alkene and alkynes
Unit 15. Aromatic Hydrocarbons : 6 teaching hours
Introduction and characteristics of aromatic compounds : Huckel’s rule of aromaticity : Kekule structure of benzene : Resonance and isomerism : Preparation of benzene from decarboxylation of sodium benzoate, phenol, and ethyne only ; Physical properties of benzene ; Chemical properties of benzene: Addition reaction: hydrogen, halogen, Electrophilic substitution reactions: orientation of benzene derivatives (o, m & p), nitration, sulphonation, halogenations, Friedal-Craft’s reaction (alkylation and acylation), combustion of benzene ( free combustion only) and uses.
Applied Chemistry : 15 teaching hours
Unit: 16 Fundamentals of Applied Chemistry : 4 teaching hours
Fundamentals of Applied Chemistry ; Chemical industry and its importance ; Stages in producing a new product ; Economics of production ; Cash flow in the production cycle ; Running a chemical plant; Designing a chemical plant ; Continuous and batch processing ; Environmental impact of the chemical industry.
Unit: 17 Modern Chemical Manufactures : 11 teaching hours
Modern Chemical Manufactures (principle and flow sheet diagram only) ; Manufacture of ammonia by Haber’s process ; Manufacture of nitric acid by Ostwald’s process ; Manufacture of sulphuric acid by contact process ; Manufacture of sodium hydroxide by Diaphragm Cell ; Manufacture of sodium carbonate by ammonia soda or Solvay process ; Fertilizers (Chemical fertilizers, types of chemical fertilizers, production of urea with flow-sheet diagram)
Unit: 16 Fundamentals of Applied Chemistry : 4 teaching hours
Fundamentals of Applied Chemistry ; Chemical industry and its importance ; Stages in producing a new product ; Economics of production ; Cash flow in the production cycle ; Running a chemical plant; Designing a chemical plant ; Continuous and batch processing ; Environmental impact of the chemical industry.
Unit: 17 Modern Chemical Manufactures : 11 teaching hours
Modern Chemical Manufactures (principle and flow sheet diagram only) ; Manufacture of ammonia by Haber’s process ; Manufacture of nitric acid by Ostwald’s process ; Manufacture of sulphuric acid by contact process ; Manufacture of sodium hydroxide by Diaphragm Cell ; Manufacture of sodium carbonate by ammonia soda or Solvay process ; Fertilizers (Chemical fertilizers, types of chemical fertilizers, production of urea with flow-sheet diagram)