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3310501
Code: 3310501
Credits: 5
Semester 1
MECHANICAL
Physical Analytical & Inorganic Chemistry
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Physical Analytical & Inorganic Chemistry Syllabus — Unit-wise Content
The official GTU curriculum for Physical Analytical & Inorganic Chemistry (subject code 3310501) as prescribed for MECHANICAL · Semester 1 divides the course into 8 units, covering 116 listed topics. The unit-wise breakdown below is read from the GTU syllabus document for this subject code, so you can check what the course actually covers before deciding which papers to attempt.
Download the official syllabus PDF (3310501)Unit 1 PROPERTIES OF LIQUID
- 1.1. Explain the different Physical properties of liquids.
- 1.2. Describe the properties of liquids.
- 1.3. Different use to determine the properties of liquids
- 1.1. Physical properties of liquid
- 1.2. Types of physical properties and Characteristics of each property.
- 1.3. Definition of the Surface tension, Parachor, Refractive index, Molar refraction, Specific refraction, Viscosity.
- 1.4. Surface tension and viscosity
- 1.5. Drop pipette method (Stalagmometer) to determine the Surface tension.
- 1.6. Ostwald's viscometer to determine viscosity of liquids.
- 1.7. Refractometer to determine refractive Index of liquid.
Unit 2 CHEMICAL KINETICS
- 2.1. Explain the different reactions & kinetics of reaction.
- 2.2. Describe about order of reaction
- 2.3. List the of factors affecting the rate of reaction.
- 2.4. Solve problems
- 2.1. Define the terms :
- 2.1.1. Rate of reaction
- 2.1.2. Specific reaction rate
- 2.1.3. Velocity constant
- 2.2. Molecularity and order of reaction
- 2.3. Definition the terms : 2.3.1First order reaction
- 2.3.2. Half concentration period
- 2.4. Derivation equation for first order reaction.
- 2.5. Derivation of equation for second order reaction.
- 2.6. Half life period for first & second order reaction.
- 2.7. Problems related chemical kinetics.
Unit 3 CHEMICAL THERMO DYNAMICS
- 3.1. Explain the different types of processes. 3.2Explain thermodynamic terms like- System, Surrounding etc.
- 3.3. Explain the laws of Chemical Thermodynamics.
- 3.4. State Hess’s law & its application.
- 3.5. Differentiate between Exothermic & endothermic of reactions
- 3.1. System and surroundings, Types of System and suitable illustrations
- 3.2. Thermodynamic property- extensive and intensive
- 3.3. First law of thermodynamics.
- 3.4. Function ,Internal energy, Enthalpy
- 3.5. Rule of assigning sign to work done(W) and heat transferred (Q) as positive and negative.
- 3.6. Molar heat capacity- at constant volume (Cv) and at Constant pressure (Cp). the relationship Cp - Cv = R
- 3.7. Adiabatic change, Isothermal change , Reversible process, Irreversible process
- 3.8. Derivation equation for Adiabatic Expansion of an Ideal gas. PVγ = Constant
- 3.9. Second law of thermodynamics
- 3.10. Aspects of thermo-chemistry & Phenomenon of heat of reaction.
- 3.11. Types of heat of reactions – Exothermic and endothermic processes with examples Physical, Analytical & Inorganic Chemistry Course Code: 3310501 GTU/ NITTTR Bhopal/12 Gujarat State Unit Major Learning Outcomes Topics and Sub-topics
- 3.12. State Hess's law of constant heat Summation.
- 3.13. Problems applying Hess's law.
Unit 4 BASIC CONCEPTS OF CHEMICAL ANALYSIS
- 4.1. Explain the concept of solubility product and ionic product and its application in inorganic analysis.
- 4. . 2 Explain the basic concepts of volumetric analysis.
- 4. . 3 Describe basic concepts of chromatography.
- 4.4. Use chromatograph analysis.
- 4.1. Basic Concepts: Common ion Effect, Solubility Product, Ionic product, Salt hydrolysis
- 4.2. State conditions for precipitation Considering Ip and Ksp
- 4.3. Application of H2S and NH4CL in inorganic qualitative analysis
- 4.4. Volumetric analysis
- 4.4.1. Acid-base titration
- 4.4.2. Complex metric titration
- 4.4.3. Oxidation-reduction titration
- 4.4.4. Precipitation titration
- 4.5.1. Classification of chromatography
- 4.5.2. (a) Paper chromatography (b) Gas Chromatography
Unit 5 SURFACE CHEMISTRY
- 5.1. Explain basic concepts of colloidal
- 5.2. Describe the preparation, properties of sol.
- 5.3. Describe about the purification of sol solutions.
- 5.4. Explain of Emulsion & its types.
- 5.5. Explain the Concepts of Adsorption & related terms.
- 5.6. Use basis concepts of colloids in different application such as smoke precipitation etc.
- 5.1. Adsorption, Adsorbate, Definition of Adsorbent
- 5.2. Classification of adsorption: Physical adsorption and Chemisorption
- 5.3. Types of solution: True solution, Suspension and colloidal solution
- 5.4. Classification of colloidal solution 5.5Lyophobic and Lyophilic sol.
- 5.6. Methods of preparing colloidal Solutions.
- 5.6.1. Condensation methods
- 5.6.2. Dispersion methods
- 5.7. Purification of colloidal solutions
- 5.7.2. Ultra filtration
- 5.8. Important properties of colloidal solution and explain the following in details
- 5.8.1. Scattering of light (Tyndall effect)
- 5.8.2. Brownian movement
- 5.8.4. Electro osmosis
- 5.9. Emulsion & Gels.
- 5.7.1. Types of emulsion
- 5.7.2. Cleansing action of soap
- 5.10. Application of colloids Smoke precipitation, Purification of water, Sewage treatment, Leather tanning etc. Physical, Analytical & Inorganic Chemistry Course Code: 3310501 GTU/ NITTTR Bhopal/12 Gujarat State Unit Major Learning Outcomes Topics and Sub-topics
Unit 6 ELECTROMETRIC METHODS OF ANALYSIS
- 6.1. Explain basic concepts of electrometric
- 6.2. Explain of construction & Working of electrochemical cells.
- 6.3. Describe about pH metry & Potentiometry titrations.
- 6.4. Describe Various aspects of conductometery & Kohlrausch Law of independent Migration of ions.
- 6.1. Defintion the term ` Electrode ' the Types of Electrodes
- 6.2. Distinction among the : Inert electrode, Working electrode & Reference electrode; with suitable Illustrations.
- 6.3. Construction & Working of reference electrode:
- 6.3.1. Hydrogen electrode
- 6.3.2. Calomel electrode
- 6.3.3. Quinhydrone electrode
- 6.3.4. Glass electrode
- 6.3.5. Ag/ Agcl/ Kcl electrode
- 6.4. pH & pOH, give their relationship
- 6.4.1. Methods used to determine pH of given solution by— - pH paper, - pH meter & - Universal indicator methods.
- 6.4.2. Problem to ascertain pH and pOH.
- 6.5. pH metry titration
- 6.6. Potentiometry titration.
- 6.7. Various aspects of conductometric titration
- 6.8. Kohlrausch Law of independent Migration of ions.
Unit 7 PREPARATION OF STANDARD SOLUTION
- 7.1. Define the terms: Solute, Solvent and Solution.
- 7.2. Explain different methods of expressing concentration with examples.
- 7.3. List the types of chemicals & its uses.
- 7.4. Describe about primary & secondary standard solutions.
- 7.5. Describe the
- 7.1. Different methods of expressing concentration. i) Weight/Weight method (W /W) ii) Weight/Volume method (W/V)
- 7.1.1. Types of W/W methods -Molality (M), -Mole fraction (X), -Parts per million (PPM)
- 7.1.2. Different types of W/V Methods. i) gms/liter ii) Normality (N) iii) Molarity (M) iv) Formality (F) v) P.P.M. / mg/liter
- 7.1.3. Problems on them.
- 7.2. Types of different standards i) Primary standards ii) Secondary standards
- 7.2.1. Conditions for primary standard
- 7.2.2. Procedure for preparing primary standard Solution. Physical, Analytical & Inorganic Chemistry Course Code: 3310501 GTU/ NITTTR Bhopal/12 Gujarat State Unit Major Learning Outcomes Topics and Sub-topics methods of preparation of standard solutions.
- 7.2.3. Primary standard for standardization of i) Acids ii) Bases iii) FeSo4 7H2O iv) KMnO4 & v) AgNO3.
Unit 8 INDUSTRIALLY IMPORTANT COMPOUNDS
- 8.1. Describe the manufacture and uses of important compounds
- 8.1. Caustic soda-Manufacture and uses
- 8.2. Ammonia- Manufacture and uses
- 8.3. Suphuric Acid- Manufacture and uses
- 8.4. Potassium Dichromate- Manufacture and uses
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