## Physical Chemistry and Its Biological ApplicationsPhysical Chemistry and Its Biological Applications presents the basic principles of physical chemistry and shows how the methods of physical chemistry are being applied to increase understanding of living systems. Chapters 1 and 2 of the book discuss states of matter and solutions of nonelectrolytes. Chapters 3 to 5 examine laws in thermodynamics and solutions of electrolytes. Chapters 6 to 8 look at acid-base equilibria and the link between electromagnetic radiation and the structure of atoms. Chapters 9 to 11 cover different types of bonding, the rates of chemical reactions, and the process of adsorption. Chapters 12 to 14 present molecular aggregates, magnetic resonance spectroscopy and photochemistry, and radiation. This book is useful to biological scientists for self-study and reference. With modest additions of mathematical material by the teacher, the book should also be suitable for a full-year major's course in physical chemistry. |

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Page 7

numerical multiplier times the second quantity; thus the gas

numerical multiplier times the second quantity; thus the gas

**equation**can be written with a constant of proportionality 0: V : g; or PV : cT (1-4) A further result of experiment is the conclusion that the numerical value of c varies ... Page 8

The ideal gas law, it must be remembered, is only a limiting law, in the sense that the volume variations of an actual gas approach those predicted by the

The ideal gas law, it must be remembered, is only a limiting law, in the sense that the volume variations of an actual gas approach those predicted by the

**equation**more and more closely as the pressure is lowered and as the temperature ... Page 11

Solution: The measured quantities can be substituted directly into the ideal gas

Solution: The measured quantities can be substituted directly into the ideal gas

**equation**. Then - 79.0 cm H z E I (76.0 cm/atm RT [(82.06 cm3 atm/(mol K)](306.0 K) I 9.40 X 10—4 mol )(22.7 cm“) KINETIC THEORY AND DERIVATION OF THE GAS ... Page 13

for the group of molecules if: P : —L (1-11) Since the motion of the molecules is entirely random, the components of velocity in the three directions are on the average equal, so that from

for the group of molecules if: P : —L (1-11) Since the motion of the molecules is entirely random, the components of velocity in the three directions are on the average equal, so that from

**Equation**(1-8), H F (1-12) c~'l W=Uzv= and PV ... Page 19

The observed volumetric behavior of many gases deviates from that predicted by the ideal gas

The observed volumetric behavior of many gases deviates from that predicted by the ideal gas

**equation**, and frequently it can be better represented by an**equation**containing additional arbitrary constants, such as the**equation**of van der ...### What people are saying - Write a review

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### Contents

1 | |

51 | |

89 | |

SECOND LAW AND EQUILIBRIUM | 115 |

CHAPTER 5 SOLUTIONS OF ELECTROLYTES | 152 |

CHAPTER 6 ACIDBASE EQUILIBRIA | 181 |

CHAPTER 7 OXIDATIONREDUCTION EQUILIBRIA | 213 |

CHAPTER 8 ELECTROMAGNETIC RADIATION AND THE STRUCTURE OF ATOMS | 244 |

CHAPTER 10 KINETICS OF CHEMICAL REACTIONS | 338 |

CHAPTER 11 ADSORPTION AND SURFACE EFFECTS | 403 |

CHAPTER 12 MACROMOLECULES AND MOLECULAR AGGREGATES | 436 |

CHAPTER 13 MAGNETIC RESONANCE SPECTROSCOPY | 494 |

CHAPTER 14 PHOTOCHEMISTRY AND RADIATION CHEMISTRY | 536 |

Table of Symbols and Abbreviations | 581 |

Index | 583 |

CHAPTER 9 BONDING AND MOLECULAR SPECTROSCOPY | 288 |

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### Common terms and phrases

absorption acid activity adsorbed adsorption amino amount applied benzene bond Calculate carbon carboxyl cell chain charge Chem chemical chemical shift chloride coefﬁcient colligative properties complex components concentration corresponding curve deﬁned described diagram dissociation effect electric electrolyte electron energy change enthalpy entropy enzyme equal equation equilibrium constant example ﬁlm ﬁrst ﬂow force fraction free energy frequency function heat hydrogen atom hydrogen ion increase ionic ionization kcal kinetic liquid magnetic ﬁeld material measured membrane mixture molar mole mole fraction molecules nucleus occurs orbital osmotic pressure oxidation oxygen particles phase polar potential protein proton quantum number radiation rate constant ratio reactant reaction resonance rotation sample shown in Figure signiﬁcant sodium solid solubility solvent species speciﬁc spectra spectrum spin structure substrate sucrose surface tension temperature tion titration transition triplet vapor pressure velocity vibrational volume wave wavelength zero