Manual Introduction to thermodynamics and kinetic theory of matter

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Applications of the theory developed for irreversible processes will be deferred to a later chapter. We will assume that the substance does not have an intrinsic angular momentum. We also assume that the system consists of an r -component non-reactive mixture. Therefore the case of chemical reactions is excluded, but it is easy to modify the theory to include the case of chemical reactions. After completing the formulation of the theory under the assumptions taken, we will point out where the necessary modifications must be made to include chemical reactions.

Since the kinetic theory part of this work does not deal with fluids with an angular momentum, we will not consider the irreversible thermodynamics of such fluids. Unable to display preview. Download preview PDF. Skip to main content. Advertisement Hide. Thermodynamics of Irreversible Processes. This process is experimental and the keywords may be updated as the learning algorithm improves.


This is a preview of subscription content, log in to check access. Kirkwood and I. Google Scholar. Callen, Thermodynamics Wiley, New York, Schooley, ed. Lindsay, ed. Clausius, Ann. Leipzig , Planck, Thermodynamics Dover, New York, Eringen, ed. Barnes, J.

Physics Kinetic Theory part 1 (Introduction) CBSE class 11

Hutton, and K. Maxwell, Phil. London , 49 Chapman, Proc. London A 93, 1 — Clausius, Phil. Onsager, Phys. Meixner, Ann. Meixner and H. Springer, Berlin, , Vol.

Understanding heat

Landau and E. Lifshitz, Fluid Mechanics Pergamon, London, Stuart, B. Gal-Or, and A. Brainard, eds.

Introduction to thermodynamics and kinetic theory of matter - CERN Document Server

Mono Book, Baltimore, , p. Acta 12 , Nettleton, Phys. Fluids 4 , Lebon, Bull. Lebon, D. Jou, and J. In Daniel Bernoulli published Hydrodynamica , which laid the basis for the kinetic theory of gases. In this work, Bernoulli posited the argument, still used to this day, that gases consist of great numbers of molecules moving in all directions, that their impact on a surface causes the gas pressure that we feel, and that what we experience as heat is simply the kinetic energy of their motion.

Bernoulli also surmised that temperature was the effect of the kinetic energy of the molecules, and thus correlated with the ideal gas law. The theory was not immediately accepted, in part because conservation of energy had not yet been established, and it was not obvious to physicists how the collisions between molecules could be perfectly elastic. Other pioneers of the kinetic theory which were neglected by their contemporaries were Mikhail Lomonosov , [5] Georges-Louis Le Sage ca. In this same work he introduced the concept of mean free path of a particle.

Also the logarithmic connection between entropy and probability was first stated by him. In the beginning of the twentieth century, however, atoms were considered by many physicists to be purely hypothetical constructs, rather than real objects. An important turning point was Albert Einstein 's [15] and Marian Smoluchowski 's [16] papers on Brownian motion , which succeeded in making certain accurate quantitative predictions based on the kinetic theory.

More modern developments relax these assumptions and are based on the Boltzmann equation. These can accurately describe the properties of dense gases, because they include the volume of the molecules. The necessary assumptions are the absence of quantum effects, molecular chaos and small gradients in bulk properties. Expansions to higher orders in the density are known as virial expansions. An important book on kinetic theory is that by Chapman and Cowling. This is known as the Knudsen regime and expansions can be performed in the Knudsen number.

In kinetic model of gases, the pressure is equal to the force exerted by the atoms hitting and rebounding from a unit area of the gas container surface. When a gas molecule collides with the wall of the container perpendicular to the x axis and bounces off in the opposite direction with the same speed an elastic collision , the change in momentum is given by:.

Since the motion of the particles is random and there is no bias applied in any direction, the average squared speed in each direction is identical:. By Pythagorean theorem in three dimensions the total squared speed v is given by.

ME 6765: Kinetics and Thermodynamics of Gases

From Eq. Thus, the product of pressure and volume per mole is proportional to the average translational molecular kinetic energy.

In addition to this, the temperature will decrease when the pressure drops to a certain point. As noted in the article on heat capacity , diatomic gases should have 7 degrees of freedom, but the lighter diatomic gases act as if they have only 5. Monatomic gases have 3 degrees of freedom.

At standard temperature The total number and velocity distribution of particles hitting the container wall can be calculated [21] based on naive kinetic theory, and the result can be used for analyzing effusion into vacuum :. Note that only the particles within the following constraint are actually heading to hit the wall:. Integrating over all appropriate velocities within the constraint yields the number of atomic or molecular collisions with a wall of a container per unit area per unit time:. The last line makes use of ideal gas law. This quantity is also known as the impingement rate in vacuum physics.

The kinetic theory of gases deals not only with gases in thermodynamic equilibrium, but also very importantly with gases not in thermodynamic equilibrium. This means using kinetic theory to consider what are known as "transport properties", such as mass diffusivity , viscosity and thermal conductivity.

History of thermodynamics

The diffusion constant is related to viscosity by the Einstein relation kinetic theory. In books on elementary kinetic theory [22] one can find results for dilute gas modeling that have widespread use. The derivation of the kinetic model for shear viscosity usually starts by considering a Couette flow , where two parallel plates are separated by a gas layer. The lower plate is stationary, and an equal and opposite force must therefore be acting on it to keep it at rest. The non-equilibrium flow is superimposed on a Maxwell—Boltzmann equilibrium distribution of molecular motions.

The mean free path is the average distance traveled by a molecule, or a number of molecules per volume, before they make their first collision. On the average, a molecule that crosses the surface makes its last collision before crossing at a distance equal to two-thirds of the mean free path i.

At this distance above and below the surface, the forward momentum of the molecule is respectively. The incoming molecules are coming from all directions at the one side of the surface and with all speeds. This molecular flux i. Next we multiply by the total flux to get the change of momentum per unit time and per unit area, that is carried by the molecules crossing from either above or below the surface area.

This gives the equation. From statistical thermodynamics for gases we have equations relating average molecular speed to most likely speed and further to temperature.