CH-401 | Physical and Inorganic Chemistry
S.Y.B.Sc. | Sem IV | Chemistry
Dr A M Nemade, Dr H A Mahajan, Dr J U Patil, Dr V T PatilRs.70.00
S.Y.B.Sc. | Sem IV | CH-401
Chemistry
Physical and Inorganic Chemistry
We are very glad to present this book on “Physical and Inorganic Chemistry’’ of semester – II in the hands of S.Y.B.Sc. students. The book is strictly written according to the semester pattern syllabus framed by the board of studies in Chemistry, KBC NMU Jalgaon, for Second year B.Sc to be implemented from June 2019 and is written in very simple language giving exhaustive details. Questions of various types and numericals are included at the end of each chapter. This will help in generating interest and thorough understanding of the subject. We hope, this book will be useful for students and teachers.
Unit 1 Electrochemistry
1.1. Some Basic Terms Involved in Electrochemistry
1.2. Electromotive Force and its Measurement –
1.2.1 Measurement of EMF
1.3 Standard cell
1.4 Cell Reaction and EMF
1.5 Convention Regarding Sign of Emf
1.6 Single Electrode Potential –
1.6.1 Standard Electrode Potential
1.6.2 Reference electrodes
1.7 Calculation of Single Electrode Potentials –
1.7.1. Calculation of cell emf from single electrode potentials
1.8 Thermodynamics and EMF –
1.8.1 Free energy change (DG)
1.8.2 Enthalpy change (DH)
1.8.3 Entropy change (DS)
1.9 Nernst Equation
1.10 Standard Potentials and Equilibrium Constant
1.11 Classification of Electrodes
Unit 2 Chemical Thermodynamics
2.1 Helmholtz free Energy-
2.1.1 Physical Significance of DA
2.1.2 Variation of Helmholtz free energy (A) with temperature (T) and volume (V)
2.1.3 Variation of with respect to temperature at constant volume
2.1.4 DA for reaction
2.1.5 Variation of (DA/T) w.r. to Temperature at constant volume
2.2 The Gibbs free energy –
2.2.1 Physical Significance of Gibbs free energy
2.2.2 Relation between Gibbs free energy and Helmholtz free energy
2.2.3 Variation of Gibbs free energy (G) with temperature and pressure
2.2.4 Variation of w.r. to temperature at constant pressure
2.2.5 DA for chemical reaction – Gibbs–Helmholtz equation
2.2.6 Importance (application) of Gibbs Helmholtz equation
2.2.7 Variation of (DG/T) with temperature at constant pressure
2.2.8 Properties and Significance of DG
2.2.9 Sign of DG and spontaneity of Reaction
2.2.10 Calculation of free energy change
2.3 Fugacity and Activity –
2.3.1 Fugacity
2.3.2 Activity (a)
2.3.3 Determination of DG in terms of activity
2.4 Van’t Hoff Reaction Isotherm
2.5 Standard free energy of formation
2.6 Criteria of Equilibrium
2.7 Physical equilibria Involving Pure Substances –
2.7.1 Clapeyron Equation
2.7.2 Application of Clapeyron Equation
2.8 Vapour pressure of liquid –
2.8.1 Variation of vapour pressure with temperature
2.8.2 Clausius-Clapeyron Equation
Unit 3 Basic concepts of co-ordination chemistry
3.1 Introduction
3.2 Addition or Molecular Compounds
3.3 Definition and Terminology
3.4 Physical methods used in the study of complex
3.5 Writing the formula of the complex
Unit 4 Conductors, Insulators and Semiconductors
4.1 General properties of metals
4.2 Energy bands in solids
4.3. Classification of solids on the basis of band theory
4.4 Types of semiconductors
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