ISBN: 0198541309
Godina izdanja: 1974
Oblast: Biologija
Jezik: Engleski
Autor: Strani

Nicholas C. Price, Raymond A. Dwek - Principles and problems in physical chemistry for biochemists
Clarendon Press, 1974
177 str.
meki povez
stanje: dobro, otpis iz biblioteke, Ex-library.

What use is physical chemistry to the student of biochemistry and biology? This central question is answered in this book mainly through the use of worked examples and problems. The text is brief and concise. It starts by introducing the laws of thermodynamics, and then uses these laws to derive the equations relevant to the student in dealing with chemical equilibria (including the binding of small molecules to proteins), properties of solutions, acids and bases, and oxidation-reduction processes. The student is thus shown how a knowledge of thermodynamic qualities makes it possible to predict whether, and how, a reaction will proceed. Thermodynamics, however, gives no information about how fast a reaction will happen. The study of the rates at which processes occur (kinetics) forms the second main theme of the book. This section poses and answers questions such as `how is the rate of a reaction affected by temperature, pH, ionic strength, and the nature of the reactants? These same ideas are then shown to be useful in the study of enzyme-catalysed reactions. This book is intended for all undergraduates interested in biology and biochemistry.

Biochemistry. | Chemistry, Physical and theoretical.

0198541309

(1) The First Law of Thermodynamics; (2) The Second Law of Thermodynamics; (3) Chemical Equilibrium; (4) Binding of Ligands to Macromolecules; (5) The Thermodynamics of Solutions; (6) Acids and Bases; and (7) Electrochemical Cells: Oxidation-Reduction Processes.

Contents
NOTE ON UNITS
1. THE FIRST LAW OF THERMODYNAMICS
What is thermodynamics? Basic definitions. Interactions of systems with their surroundings. Statement of the First Law of Thermodynamics. Appli-cations of the First Law. Worked examples. Thermochemistry. Bond energies. Worked examples. Problems.
2. THE SECOND LAW OF THERMODYNAMICS
Introduction. The meaning of entropy. Statement of the Second Law. Reversible and irreversible processes. The concept of free energy. Standard states. Worked example. The `biochemical` standard state. Problems.
3. CHEMICAL EQUILIBRIUM
Introduction. The relationship between Delta * G ^ 0 and equilibrium constant. Applications to solutions. Worked examples. Distinction between Delta*G and Delta * G ^ 0 The variation of the equilibrium constant with temperature. Worked examples. Measurements of thermodynamic functions of reaction. Problems.
4. BINDING OF LIGANDS TO MACROMOLECULES
Introduction. The binding equation treatment of binding data. Worked examples. Multiple binding site equilibria. Worked example. Non-equivalent ligand sites on a macromolecule. Experimental methods for obtaining binding data. Problems.
5. THE THERMODYNAMICS OF SOLUTIONS
Introduction. Equilibrium between phases. Raoult`s Law Ideal solutions. Alternative definition of an ideal solution. Properties of ideal solutions. Worked examples. `Anomalous` molecular weights. Non-ideal solutions-the concept of activity. Worked example. Electrolyte solutions. Worked example. Sparingly soluble salts. Worked example. Solutions of macro-molecules. Worked example. The Donnan effect. Worked example. Deter-mination of the molecular weights of macromolecules. Number average molecular weight. Weight average molecular weight. The concept of chemical potential. Problems.
6. ACIDS AND BASES
Introduction. The concept of pH. Acids and bases. Worked examples. Buffer solutions. Worked example. Dissociation of polyprotic acids. Worked example. The effect of ionic strength on acid-base equilibria. Problems.
7. ELECTROCHEMICAL CELLS: OXIDATION REDUCTION PROCESSES
Oxidation-reduction processes. The thermodynamics of reversible cells. Worked example. Types of half-cells. Half-cell electrode potentials. Electro-chemical cells. Worked examples. The sign convention for electrochemical cells. Worked examples. Calculation of thermodynamic parameters. The Nernst equation. Worked examples. Biochemical standard states. The Nernst equation and chemical equilibrium. The effect of non-ideality. Coupled oxidation reduction processes. Problems.
8. CHEMICAL KINETICS
The pathway of a reaction. The order and molecularity of a reaction. Types of rate processes. Worked examples. Determination of the order of a reaction. Worked example. A note on units. The kinetics of some other types of processes. Effect of temperature on the rate of a reaction. Worked example. Significance of the parameters in the Arrhenius equation. Transi-tion state theory. The effect of pH on the rate of a reaction. The effect of ionic strength on the rate of a reaction. The effect of isotope changes on reaction rates. Problems.
9. THE KINETICS OF ENZYME CATALYSED REACTIONS
Introduction. Steady-state kinetics. Treatment of kinetic data. Enzyme inhibition. Worked example. The effect of pH on enzyme reactions. Worked example. The effect of temperature on enzyme reactions. Summary. Problems.
10. SPECTROPHOTOMETRY
The electromagnetic spectrum. Worked example. The Beer-Lambert Law. Worked examples. Appropriate concentration ranges. Worked example. Two absorbing compounds. Worked example. Isosbestic points. Problems.
11. ISOTOPES IN BIOCHEMISTRY
The uses of isotopes. Problems.
APPENDIX 1: THE DEPENDENCE OF ENTHALPY AND ENTROPY ON PRESSURE AND TEMPERATURE
APPENDIX 2: THE EQUATION FOR MULTIPLE BINDING SITES
APPENDIX 3: THE HALF TIME METHOD FOR REACTION ORDER
APPENDIX 4: THE INTERACTION OF AN ENZYME WITH SUBSTRATE AND INHIBITOR
SOLUTIONS TO PROBLEMS
SOME USEFUL CONSTANTS
SOME SUGGESTIONS FOR FURTHER READING
INDEX