General Chemistry detailed syllabus for Chemical Engineering (CH) for 2015 revision curriculum has been taken from the SITTTRs official website and presented for the CH students. For course code, course name, number of credits for a course and other scheme related information, do visit full semester subjects post given below.
For Chemical Engineering 3rd Sem scheme and its subjects, do visit CH 3rd Sem 2015 revision scheme. The detailed syllabus of general chemistry is as follows.
Course Outcomes:
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SPECIFIC OUTCOMES
MODULE I
- Apply the laws of chemical combination.
- Illustrate each of the following laws of chemical combination with two examples each: Law of conservation of mass, Law of definite proportions ,Law of multiple proportions, Law of reciprocal proportions, Gay lussac’s law of gaseous volumes, Avagadro’s law and mention its applications.
- Solve problems based on the above laws of chemical combination
- State Dulong and Petit’s Law
- Calculate atomic weight of an element from its equivalent weight
- State the relationship between vapour density and molecular weight.
- Narrate the periodicity in properties.
- State modern periodic law and briefly discuss the modern periodic table. Explain the periodicity in the properties of elements in terms of the following: Atomic and ionic radii, Ionisation enthalpy, Electron gain enthalpy and electro negativity
- Explain the concept of hybridization (sp3,sp2,sp) with one example each (methane ethene , ethyne)
MODULE II
- Understand the classification of organic compounds
- Classify the given organic compounds on the basis of functional group
- Illustrate ‘Homologous series with examples
- Name any five homologous series
- Understand the methods of purification of organic compounds.
- State the criteria of purity of an organic compound
- Describe the purification of organic solids by crystallization and sublimation with examples.
- Describe the purification of organic liquids by distillation (Simple distillation, Fractional distillation, Distillation under reduced pressure and steam distillation) and chromatography(Column chromatography, Thin layer chromatography and paper chromatography)
- Comprehend the methods of analysis of organic compounds
- Describe any one test that can be used for detection of the following elements
- Hydrogen
- Carbon
- Nitrogen
- Halogens
- Sulphur
- Phosphorus
- Describe the following experiments used for the estimation of the following elements: Hydrogen and Carbon by combustion method (Liebig’ method) Nitrogen by Dumas method , Halogen by Carius method, Sulphur by Carius method
- Solve problems based on the above methods of estimation
- Describe any one test that can be used for detection of the following elements
- Elucidate the molecular formula of organic compounds
- Define empirical formulae
- Find the empirical formulae from the given percentage composition
- Define the molecular formulae
- Define structural formulae- dash formula, complete formula condensed formula and bond line formula
- Describe the shape of the following molecules using hybridization
- Methane
- Ethane
- Ethene
- ethyne
- Benzene
- Comprehend the different types of Isomerism
- Name the first 5 members of alkane, alkene and alkyne series using I.U.P.A.C System
- Define Isomerism
- Illustrate the following classes of structural isomerism with an example for each
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- Chain isomerism
- Functional group isomerism
- Position isomerism
- Metamerism
- Illustrate stereoisomerism
- Geometrical isomerism exhibited by Maleic acid and fumaric acid
- Optical isomerism exhibited by lactic acid.
- Understand the methods of preparation of Hydrocarbons
- Describe one method for the preparation of the following hydrocarbons- Methane (decarboxylation method), ethane (Wurtz reaction) ,ethene(by dehydrohalogenation),Ethyne (action of water on calcium carbide) ,Benzene (cyclic polymerization of ethyne)
- Describe chemical reaction of the following hydrocarbons methane,ethylene,Acetylene and benzene with chlorine under different conditions
- List the uses of the following hydrocarbons methane, ethane, ethylene, Acetylene and Benzene.
- Explain
- Addition reaction of bromine in CCl4 and HBr to symmetrical and unsymmetrical alkenes -Markovnikov’s rule and Anti Markovnikov’s rule
- Acidity of ethyne -reaction with sodium and sodamide
- Friedel craft’s alkylation of benzene.
MODULE III
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- Explain the methods of preparation, of ethyl alcohol (fermentation and using Grignard reagent),Esterification, Chlorination and oxidation reactions and uses of Ethylalcohol.
- Explain the method of preparation of formaldehyde(from methanol),acetaldehyde(from ethanol) and acetone (from isopropyl alcohol), Describe nucleophilic addition reaction (addition of HCN), Cannizaro’s reaction and aldol condensation reaction of formaldehyde and acetaldehyde,oxidation reaction of acetaldehyde and acetone using strong and mild oxidising agents (test of aldehyde and ketone)
- Explain method of preparation of acetic acid(from Grignard reagent) .Chemical properties of acetic acid -reduction and Hell-Volhard-Zelinsky (HVZ reaction)
- Explain Williamson’s Method for preparing Ether and to know the important precautions and uses of ether
- Explain the method of preparation of aniline(from nitrobenzene) and diazotisation of aniline
- Explain the method of conversion of aniline to phenol.chlorobenene and benzene
- Describe the method of preparation of phenol by Dow’s process and Cumene process.Electrophilic substituition reaction (nitration and bromination)and special reactions (Kolbe reaction and Reimer-Tiemann reactions) of Phenol
- Describe the structure of glucose (open chain and Ring structure)
- Explain the chemical reactions of glucose -reduction,oxidation .acetylation and reaction with phenyl hydrazine
- Comprehend the chemistry of Amino Acids and Proteins
- Classification of aminoacids (essential and nonessential amino acid with 2 example each)
- Explain the properties of amino acids(zwitter ion and isoelectric point) and concept of peptide bond
- Describe the 10,2,0 30 structure of protein.
- List the biological functions and test for proteins.
MODULE IV PHYSICAL CHEMISTRY
- Understand the conditions of chemical equilibrium
- Illustrate with example
- Reversible
- Irreversible reactions
- State the law of mass action
- Derive expression for the equilibrium constant Kp and Kc
- Derive the relation between Kp and Kc and solve problems based on this
- Derive an expression for equilibrium constant for each of the following reactions H2+I2 = 2HI N2+3H2=2NH3 N2O4 = 2 NO2
- State Le-Chatlier’s principle
- Predict the optimum conditions for getting maximum yield of the product by Applying the Le-Chatlier’s principle in each of the following process
- Manufacture of NH3 by Haber process
- Manufacture of SO3 by contact process
- Illustrate with example
- Understand the kinetics of chemical reactions
- Define rate or velocity of a chemical reaction
- Distinguish between order and molecularity of a chemical reaction
- Illustrate first order reaction with two examples(acid catalyzed hydrolysis of ester and inversion of cane sugar)
- Derive an equation for 1st order reaction
- Explain half-life period–derive an expression to determine the half-life period
- Solve problems based on 1st order reactions
- Illustrate second order reactions with two examples (saponification reaction and H2-I2 reaction)
- Illustrate third order reaction with one example: (2NO2+O2^ 2NO3)
- Explain the effect of temperature on reaction rate and define the terms threshold energy . and activation energy ,state Arrhenius equation (exponential and logarithmic forms)
- Comprehend the behaviour of Gaseous state
- List the characteristics of Gaseous state and their physical properties- pressure, volume and temperature.
- State Boyle’s law, Charle’s law and Avogadro’s law and solve simple problems based on these laws.
- Derive ideal gas equation (PV=nRT)
- Know the significance of universal gas constant and calculate its value in different units.
- State the postulates of kinetic theory
- Distinguish between real gas and ideal gas and give the conditions and the reasons of deviations from ideal behaviour.
- Explain the van der Walls equation of state of real gases and the significance of van der Waals constants.
MODULE I: INORGANIC CHEMISTRY
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MODULE II: ORGANIC CHEMISTRY
CLASSIFICATION OF ORGANIC COMPOUNDS Introduction to organic chemistry-functional groups-Homologous series-classification of organic compounds on the basis of functional group-Give any 5 examples of homologous series PURIFICATION OF ORGANIC COMPOUNDS Criteria of purity-melting point, boiling point and mixed melting point- Purification of solid organic compounds by crystallization and sublimation-Give the principle and two Examples Purification of liquid organic compounds by distillation-principle and two examples of simple distillation, fractional distillation-distillation under reduced pressure and steam distillation Chromatography- theory- Types of chromatography -Adsorption and partition chromatography -Adsorption chromatography- Column chromatography and thin layer chromatography Partition chromatography-paper chromatography QUALITATIVE AND QUANTITATIVE ANALYSIS OF ORGANIC COMPOUNDS Give one method of detection of following elements along with the chemistry of reactions – carbon and hydrogen by combustion test , Nitrogen ,sulphur, and halogen by Lassaigne’s test )and phosphorus by ammonium molybdate test . Estimation of elements carbon and hydrogen by Liebig’s method -Nitrogen by Dumas method-halogens by Carius method- Sulphur by Carius method-solve simple problems based on these methods of estimation. MOLECULAR FORMULA OF ORGANIC COMPOUNDS Definition of empirical formula-deduction of empirical formula from percentage composition of elements-definition of molecular formula, calculation of molecular formula from empirical formula-Structural formulae of compounds- dash formula, complete formula, condensed formula and bond line formula. Shape of molecules using hybridization-methane and ethane by sp3, ethene and benzene by sp2 and ethyne by sp hybridization PREPARATION OF HYDROCARBON IUPAC names of first five members of alkanes alkenes and alkynes(straight chain and branched chain) Preparation of hydrocarbons – methane by decarboxylation of carboxylic acid using sodalime distillation-ethane by Wurtz reaction of chloromethane – ethene by dehydrohalogenation of chloroethane using alcoholic KOH – ethyne by action of water on calcium carbide and benzene by cyclic polymerization of ethynes. Chemical properties of hydrocarbons – chlorination of methane, ethane and ethyne, Benzene -substitution and addition reactions of chlorine under different conditions, Addition reaction of Br2 in CCl4 to alkenes (test of unsaturation) – Addition of HBr to symmetrical and unsymmetrical alkenes -Markovnikov’s and AntiMarkovnikov’s addition – Acidity of ehynes – reaction with sodium and sodamide (test of alkynes) – Friedel – Craft’s methylation of benzene, Any three uses of methane, ethane, ethene, ethyne and benzene.
MODULE III: ORGANIC CHEMISTRY
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MODULE IV PHYSICAL CHEMISTRY
CHEMICAL EQUILIBRIUM Reversible and Irreversible reactions with two examples for each-Statement of Law of mass action-Equilibrium constants-Equilibrium concentration of reactants and products-molar concentration and partial pressure-Derivation of expressions for equilibrium constants-Kc and Kp-Law of chemical equilibrium-Derivation of relation between Kc and Kp-Application of the relation to three chemical equilibria H2 + I2 <-^2HI, N2 + 3H2 2NH3 and N2O4^^ 2NO2 and simple problems using this relation Lechateleir’s principle-Statement and application of Le – Chateleir’s principle to synthesis of ammonia by Haber process and manufacture of sulphuric acid by contact process. CHEMICAL KINETICS Rate of chemical reaction- definition and unit-Factors affecting rate of chemical reaction -rate law and rate constant-order and molecularity -examples of first order, second order and third order reactions-examples of Unimolecular,bimolecular and termolecular reactions-Difference between order and molecularity of reaction- Derivation of an expression of rate constant of first order reactions-Definition of half life period and derivation of expression of half life period from expression of first order rate constantproblems using these expressions-Effect of temperature on reaction rate-Definition of Threshold energy and Activation energy- Arrhenius equation- Exponential forms and logarithmic forms- Explanation of terms- Arrhenius frequency factor and activation energy. GASEOUS STATE Characteristics of gaseous state- Properties of gases like pressure,volume and temperature -Behaviour of gases -Gas Laws -Boyles Law, Charles Law and Avagadro’s law (Qualitative and Quantitative statements )-Problems based on these laws -Derivation of ideal gas equation of states -explanation of significance of universal gas constant -Derivation of values of universal gas constant in different units-Postulates of kinetic theory of gases -Deviation of behaviour of gas from ideal gas – conditions and reasons -Differences between ideal gas and real gas – Van Der Waal’s equation of state of a real gas – Explanation of different terms and significance of Van Der Waal’s constants along with their units.
Reference Books:
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For detailed syllabus of all other subjects of Chemical Engineering, 2015 revision curriculum do visit CH 3rd Sem subject syllabuses for 2015 revision.
To see the syllabus of all other branches of diploma 2015 revision curriculum do visit all branches of SITTTR diploma 2015 revision.