By James Jeans

ISBN-10: 0521092329

ISBN-13: 9780521092326

This publication might be defined as a student's variation of the author's Dynamical idea of Gases. it's written, despite the fact that, with the wishes of the coed of physics and actual chemistry in brain, and people components of which the curiosity was once almost always mathematical were discarded. this doesn't suggest that the publication includes no severe mathematical dialogue; the dialogue particularly of the distribution legislation is kind of targeted; yet commonly the maths is worried with the dialogue of specific phenomena instead of with the dialogue of basics.

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**Extra resources for An Introduction to the Kinetic Theory of Gases (Cambridge Science Classics)**

**Sample text**

So far we have been concerned only with the average kinetic energy, and the average speeds of molecules; we have had no occasion to think of the energies or speeds of individual molecules. And it is obvious that the speeds of motion of the various molecules cannot be all equal; even if they started equal, a few collisions would soon abolish their equality. For the solution of many problems, it is necessary to know how the velocities of motion are arranged round the mean, after so many collisions have occurred that the gas has reached its final steady state in which the distribution of velocities is no longer changed by collisions.

The number of molecules in this group will of course be proportional not only to the volume dxdydz, but also to the product of the small ranges dudvdw. Thus it is proportional to the product of differentials dudvdw dxdydz. It is also proportional to another factor of the nature of a "density", which specifies the number of molecules per unit range lying within the range in question. This factor naturally depends on the particular values of x, y, z and of u, v9 w. Let us suppose that, whatever these values are, it is f(u,v,w,x,y,z)y so that the number of molecules in the group under consideration is f(u,v,w,x,y,z) dudvdw dxdydz.

For a collision between two molecules does not of itself produce any pressure on the boundary, and neither does it affect the value of expression (2), since energy is conserved at a collision. It may at first seem strange that the pressure should depend on the state of things throughout the whole of the gas in a vessel, and not only on the state of things close to the boundary on which the pressure is exerted. One molecule, for instance, in the far interior of the gas may be moving with immense velocity.

### An Introduction to the Kinetic Theory of Gases (Cambridge Science Classics) by James Jeans

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