BPH-201: PHARMACEUTICAL CHEMISTRY – III
Theory
(PHYSICAL CHEMISTRY)
Max. Marks: 80 Total Hours: 50 (2hrs/week)
Note: Examiner to set eight questions and the candidates are required to attempt any five.
1. States of Matter:(12)(a) Gaseous: Brief introduction to the behavior of gases, ideal and real gases, equations of state, Deviation from ideal behavior, critical phenomena, critical constant and its determination, coefficient of thermal expansion and compressibility.(b) Liquids: Intensive and extensive properties, Additive and constitutive properties, molar volume, molar refraction, surface tension, parachor, optical activity and their importance in structure elucidation.
(c) Solids: Amorphous and crystalline solids, geometry and symmetry of crystals, point defects, Miller indices, types of crystals, physical properties of crystals, Crystal diffraction, Bragg’s equation, application in mol. wt. determination, liquid crystalline state, smectic and nematic liquid crystals. Swarm theory of liquid crystals.2. Solutions:(8)(a) Non- Electrolyte Solutions: Concentrationscales, ideal and real solutions, colligative properties, Mol. wt. determination, Donnan- Membrane Equilibrium and drug absorption, Solution of gases in liquids, solutes distributing in immiscible solvents, partition- coefficient and its importance.(b) Electrolyte Solutions: Arrhenius theory of electrolytic dissociation, Debye-Huckel theory and its use in protein purification, Ionic equilibrium in blood, applications.3. Thermodynamics:(13)(a) Energy and First Law of Thermodynamics: Preliminaries and definitions, reversibility, energy and enthalpy changes, heat capacities and their relationship for ideal gas, isothermal and adiabatic processes involving ideal gases. Applications, Thermo- chemical equations. Heats of reaction, effect of temperature, state etc. Kirchhoff’s equation and numericals for exercises.(b) Second and Third Law of Thermodynamics: Carnot Cycle, irreversible process, molecular interpretation of entropy, entropy calculations for ideal gas systems, absolute entropy, entropy changes for phase changes and chemical reactions.(c) Free Energy and Equilibrium: Helmholtz and Gibb’s free energy, concept of spontaneity, chemical equilibrium, expressions for equilibrium constant, effect of volume, temperature and pressure.
4. Phase Equilibrium:(6)
Phase component, degrees of freedom, deduction of phase rule, equilibrium between phases and cooling curves. Phase diagrams for one component system, for two component systems involving eutectics. Three-component systems, triangular plots and partially miscible three liquid systems (formation of one, two and three miscible pairs).
5. Kinetics and Adsorption:(11)
a) Reaction Rates: Rate and rate constant, order and molecularity, zero, first, second and third order reactions, half- life time, determination of rate and order, consecutive, parallel and opposing reactions, ionic and free-radical reactions. Theories and reaction Kinetics, (Collision, Lindman and Transition state Theory)
b) Catalysis: Characteristics of catalyzsed reactions, homogeneous and heterogeneous catalysis, acid base catalysis, enzyme catalysis, theory of catalysis.
c) Adsorption: Physiosorption and Chemisorptions, adsorption isotherms, Freundlich and Langmuir adsorption isotherms, Gibbs adsorption isotherm, BET equation and its use in surface area determination.
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