Course Code:2852, Course Title: Fundamentals of Physical Chemistry Marks 100, 4 Credits, 60 Lectures
1.State of Matter: Microscopic and macroscopic system; properties of molecules; potential and kinetic energy of molecules; Degrees of freedom of motion; transnational rotational and vibrational energy of systems; principle of equipartition of energy; State of aggregation of matter.
2.Gaseous State: Properties of gases; The gas laws; ideal and real gases; ideal gas equation; Kinetic theory and its application to ideal gases; Pressure of ideal gases; Boltzmann distribution of molecular energies; Deviation from ideal behaviour; Vander walls equation, Critical constants; Principle of corresponding states; Collision number, Mean free path; Dalton’s law of partial pressure.
3.Liquids and Solutions: Physical properties and molecular structure; Surface tension measurement of surface tension, Visocosity, Poisculies equation, measurement Visocosity, Molar refractivity and dipole moment, measurement Vapour pressure; Dependence of Vapour pressure on temperature variation, Solution; solubility, solubility prodruct, molecular solution, ionic solution, units of concentration, Raoult’s law; Ideal and nonideal solutions; Colligative
properties of solution, Effect of electrolytes on Colligative properties. Henry’s law determination of molecular weight by measuring colligative properties.
4.Chemical Equilibrium: Equilibrium in chemical reactions and the equilibrium law; Kp, kc, and kx measurements; Degree of dissociation; Effects of temperature, pressure and concentration changes of equilibrium; Principle of Le Chatelier and Braun; Ostwald dilution law; Dissociation of solid; Solubility product; common ion effect, pH and buffer solution;
5.Energetics in Chemistry: Work and heat; internal energy; The first law of thermodynamics; State function and exact differentials; Enthalpy; Work of expansions reversible and adiabatic expansions; Joule-Thomson effect; Heat capacities at constant pressure and constant volume; Enthalpy changes in various chemical and physical processes; Measurements; Second law of thermodynamics; Spontaneity and reversibility of chemical reactions; Hess’s law and its application; Born-Haber cycle; Bond enthalpy.
6.Electrochemistry: Oxidation-reduction equilibria, concept of reduction potential, Galvanic cell, electrolytes, non-electronic conduction measurements of electrolytic conductance, application of conductance measurements, transport numbers and their determination.
7.Rates of Chemical reaction: Rate of reaction, rate equation, order and rate constant, Measurement of reaction rates, Determination of order and rate constant, Elementary and complex reaction, Molecularity, Effect of temperature on the rate of reaction. Activation energy, Catalysis.
Book Recommended: 1.Physical chemistry, PW atkins 2.Physical Chemistry, G W Castellan 3.A text Book of Physical Chemistry, S Glasstone 4.Principles of Physical Chemistry, S H Maroon and C F Pruttons 5.General Chemistry, D Ebbing
1.State of Matter: Microscopic and macroscopic system; properties of molecules; potential and kinetic energy of molecules; Degrees of freedom of motion; transnational rotational and vibrational energy of systems; principle of equipartition of energy; State of aggregation of matter.
2.Gaseous State: Properties of gases; The gas laws; ideal and real gases; ideal gas equation; Kinetic theory and its application to ideal gases; Pressure of ideal gases; Boltzmann distribution of molecular energies; Deviation from ideal behaviour; Vander walls equation, Critical constants; Principle of corresponding states; Collision number, Mean free path; Dalton’s law of partial pressure.
3.Liquids and Solutions: Physical properties and molecular structure; Surface tension measurement of surface tension, Visocosity, Poisculies equation, measurement Visocosity, Molar refractivity and dipole moment, measurement Vapour pressure; Dependence of Vapour pressure on temperature variation, Solution; solubility, solubility prodruct, molecular solution, ionic solution, units of concentration, Raoult’s law; Ideal and nonideal solutions; Colligative
properties of solution, Effect of electrolytes on Colligative properties. Henry’s law determination of molecular weight by measuring colligative properties.
4.Chemical Equilibrium: Equilibrium in chemical reactions and the equilibrium law; Kp, kc, and kx measurements; Degree of dissociation; Effects of temperature, pressure and concentration changes of equilibrium; Principle of Le Chatelier and Braun; Ostwald dilution law; Dissociation of solid; Solubility product; common ion effect, pH and buffer solution;
5.Energetics in Chemistry: Work and heat; internal energy; The first law of thermodynamics; State function and exact differentials; Enthalpy; Work of expansions reversible and adiabatic expansions; Joule-Thomson effect; Heat capacities at constant pressure and constant volume; Enthalpy changes in various chemical and physical processes; Measurements; Second law of thermodynamics; Spontaneity and reversibility of chemical reactions; Hess’s law and its application; Born-Haber cycle; Bond enthalpy.
6.Electrochemistry: Oxidation-reduction equilibria, concept of reduction potential, Galvanic cell, electrolytes, non-electronic conduction measurements of electrolytic conductance, application of conductance measurements, transport numbers and their determination.
7.Rates of Chemical reaction: Rate of reaction, rate equation, order and rate constant, Measurement of reaction rates, Determination of order and rate constant, Elementary and complex reaction, Molecularity, Effect of temperature on the rate of reaction. Activation energy, Catalysis.
Book Recommended: 1.Physical chemistry, PW atkins 2.Physical Chemistry, G W Castellan 3.A text Book of Physical Chemistry, S Glasstone 4.Principles of Physical Chemistry, S H Maroon and C F Pruttons 5.General Chemistry, D Ebbing
Fundamentals of Physical Chemistry
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September 07, 2019
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