eBook - ePub
Kinetic Theory of Gases
Walter Kauzmann
This is a test
- 272 pages
- English
- ePUB (adapté aux mobiles)
- Disponible sur iOS et Android
eBook - ePub
Kinetic Theory of Gases
Walter Kauzmann
DĂ©tails du livre
Aperçu du livre
Table des matiĂšres
Citations
Ă propos de ce livre
Written by a former Princeton University professor specializing in the thermal properties of matter, this monograph and text was designed for first-year students of physical chemistry who require further details of kinetic theory. The treatment focuses chiefly on the molecular basis of important thermodynamic properties of gases, including pressure, temperature, and thermal energy. Extended and often quite elementary presentations of abstract basic concepts offer students the opportunity to grasp the essentials of modern physical chemistry. Thermodynamic and molecular theories of heat are developed side by side, so that thermodynamic theory is constantly illuminated and enhanced by molecular theory.
Topics include equations of state of gases and empirical gases, the molecular explanation of the equations of state, and the molecular theory of the thermal energy and heat capacity of a gas. Additional subjects include the distribution of molecular velocities in a gas as well as molecular collisions and the transport properties of gases. Numerous exercises, many of them partially worked out, help students internalize concepts and illustrate practical uses and special applications. End-of-chapter problems offer further reinforcement.
Topics include equations of state of gases and empirical gases, the molecular explanation of the equations of state, and the molecular theory of the thermal energy and heat capacity of a gas. Additional subjects include the distribution of molecular velocities in a gas as well as molecular collisions and the transport properties of gases. Numerous exercises, many of them partially worked out, help students internalize concepts and illustrate practical uses and special applications. End-of-chapter problems offer further reinforcement.
Foire aux questions
Comment puis-je résilier mon abonnement ?
Il vous suffit de vous rendre dans la section compte dans paramĂštres et de cliquer sur « RĂ©silier lâabonnement ». Câest aussi simple que cela ! Une fois que vous aurez rĂ©siliĂ© votre abonnement, il restera actif pour le reste de la pĂ©riode pour laquelle vous avez payĂ©. DĂ©couvrez-en plus ici.
Puis-je / comment puis-je télécharger des livres ?
Pour le moment, tous nos livres en format ePub adaptĂ©s aux mobiles peuvent ĂȘtre tĂ©lĂ©chargĂ©s via lâapplication. La plupart de nos PDF sont Ă©galement disponibles en tĂ©lĂ©chargement et les autres seront tĂ©lĂ©chargeables trĂšs prochainement. DĂ©couvrez-en plus ici.
Quelle est la différence entre les formules tarifaires ?
Les deux abonnements vous donnent un accĂšs complet Ă la bibliothĂšque et Ă toutes les fonctionnalitĂ©s de Perlego. Les seules diffĂ©rences sont les tarifs ainsi que la pĂ©riode dâabonnement : avec lâabonnement annuel, vous Ă©conomiserez environ 30 % par rapport Ă 12 mois dâabonnement mensuel.
Quâest-ce que Perlego ?
Nous sommes un service dâabonnement Ă des ouvrages universitaires en ligne, oĂč vous pouvez accĂ©der Ă toute une bibliothĂšque pour un prix infĂ©rieur Ă celui dâun seul livre par mois. Avec plus dâun million de livres sur plus de 1 000 sujets, nous avons ce quâil vous faut ! DĂ©couvrez-en plus ici.
Prenez-vous en charge la synthÚse vocale ?
Recherchez le symbole Ăcouter sur votre prochain livre pour voir si vous pouvez lâĂ©couter. Lâoutil Ăcouter lit le texte Ă haute voix pour vous, en surlignant le passage qui est en cours de lecture. Vous pouvez le mettre sur pause, lâaccĂ©lĂ©rer ou le ralentir. DĂ©couvrez-en plus ici.
Est-ce que Kinetic Theory of Gases est un PDF/ePUB en ligne ?
Oui, vous pouvez accĂ©der Ă Kinetic Theory of Gases par Walter Kauzmann en format PDF et/ou ePUB ainsi quâĂ dâautres livres populaires dans Physical Sciences et Physical & Theoretical Chemistry. Nous disposons de plus dâun million dâouvrages Ă dĂ©couvrir dans notre catalogue.
Informations
Sujet
Physical SciencesSous-sujet
Physical & Theoretical ChemistryChapter 1
EQUATIONS OF STATE OF CASES;
EMPIRICAL RESULTS
1-1 The âprimary properties,â mass, volume, pressure, and temperature
Gases are substances which completely fill any container into which they are introduced. Let us suppose that standing before the student on his desk as he reads this chapter is a flask containing some gaseous substance such as air. The air in this flask has a great many propertiesâcolor, odor, density, velocity, viscosity, thermal conductivity, electrical conductivity, magnetic susceptibility, dielectric constant, chemical composition, and so on. In this chapter, however, we shall be concerned with four particularly important properties of a gaseous substance: mass, volume, pressure, and temperature. Because they are so important and are so frequently measured by chemists we shall call them the âprimary properties.â Before considering their relationship to each other, let us be sure that we understand what we mean by these four properties.
The properties in question are expressible as numbers, and can be best defined if we describe how one goes about determining these numbers. (This way of looking at scientific concepts is almost always the safest way of being sure that one knows exactly what a concept means, and deciding the circumstances under which the concept loses or changes its significance.)
The mass of a gas in a vessel can be determined by weighing the vessel when it contains the gas, and then weighing the vessel again after the gas has been pumped out. This procedure is straightforward, and although it is possible to imagine some subtle complications regarding the concept of mass, these complications play no role in physical chemistry, at least not under ordinary circumstances.
The volume of a gas can be most easily determined by weighing the water required to fill the vessel containing the gas, since the volume of a unit mass of water between 0°C and 100°C is very accurately known. The procedure is simple in principle, but a complication arises if the gas and the vessel are at an elevated temperature, where the mass of water per unit of volume may not be so well known. This complication can be overcome, of course, by using other liquids whose densities are known at the desired temperature. Furthermore, if the vessel has a simple geometry (a cube, sphere, cylinder, etc.), we may measure its dimensions and the volume may then be determined by means of a suitable geometric formula.
A more awkward complication arises in determining the mass of a given volume or the volume of a given mass of a gas when the gas is not in a containerâsay when it is flowing out of a nozzle or around the wing of an airplane. We shall avoid complications of this kind for the present, however, by considering only gases in closed vessels. On the other hand, we shall be very much concerned with vessels whose volumes can be alteredâparticularly with vessels in which one wall can be movedâfor instance, a gas contained in a piston chamber or a gas under compression by a liquid in a gas burette (Fig. 1-1). Clearly, each position of the piston or of the liquid corresponds to a volume which can be determined in principle in the manner described above.
The concept of pressure, although apparently simple in principle, is in practice subject to a good many qualifications. It may be measured by means of a manometer, with which one observes the height of a column of an inert liquid, such as mercury, that is balanced by the force exerted by the gas on the liquid surface. (This measurement will be described in more detail below, in Section 1-3.1). If a gas and its container are at rest, and if they are located in a region free of gravitational fields, then the pressure that the gas exerts on the container walls is the same at all points on all of the walls. Under these conditions one can speak of the pressure on the walls as âthe pressure of the gas,â and this pressure can be regarded as a property of the entire gas sample. On the other hand, if the system is located in a gravitational field, the pressure on the walls will not be uniform. A gas at the earthâs surface exerts a force on the bottom of its container which is greater by the weight of the gas than the force on the top of the container. Strictly speaking, such a gas sample as a whole does not have âa pressure.â If the box is small, however, and if the gas is not highly compressed, these pressure differences will be negligible so that one is in the habit of speaking of âthe pressureâ of the gas despite the fact that it cannot be precisely defined under these circumstances.
EXERCISE One liter of air at room temperature and at one atmosphere pressure (= about 1 kg/cm2 at the earthâs surface) has a mass of about 1 g. What is the percentage difference in pressure between the top and bottom of a column which is 1 m in height, filled with air at one atmosphere and located at the earthâs surface?
A more awkward complication arises if a gas moves relative to the walls of its containerâas will be the case if the gas is swirling about or if one of the walls (say the piston in Fig. 1-1) is in motion. The pressure may then be quite different on different walls, and again it is not possible to speak of âthe pressureâ of the whole gas sample. This complication will...
Table des matiĂšres
- Cover Page
- Title Page
- Copyright Page
- Editorâs Foreword
- Preface
- Contents
- Introduction
- Chapter 1: Equations of state of gases; empirical gases
- Chapter 2: The molecular explanation of the equations of state
- Chapter 3: The molecular theory of the thermal energy and heat capacity of a gas
- Chapter 4: The distribution of molecular velocities in a gas
- Chapter 5: Molecular collisions and the transport properties of gases
- Index of Symbols
- Index of Subjects
- Back Cover
Normes de citation pour Kinetic Theory of Gases
APA 6 Citation
Kauzmann, W. (2013). Kinetic Theory of Gases ([edition unavailable]). Dover Publications. Retrieved from https://www.perlego.com/book/112850/kinetic-theory-of-gases-pdf (Original work published 2013)
Chicago Citation
Kauzmann, Walter. (2013) 2013. Kinetic Theory of Gases. [Edition unavailable]. Dover Publications. https://www.perlego.com/book/112850/kinetic-theory-of-gases-pdf.
Harvard Citation
Kauzmann, W. (2013) Kinetic Theory of Gases. [edition unavailable]. Dover Publications. Available at: https://www.perlego.com/book/112850/kinetic-theory-of-gases-pdf (Accessed: 14 October 2022).
MLA 7 Citation
Kauzmann, Walter. Kinetic Theory of Gases. [edition unavailable]. Dover Publications, 2013. Web. 14 Oct. 2022.