The Gaseous State - We have a pretty good understanding of...

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We have a pretty good understanding of the gaseous state in terms of the link between the variables describing  the microscopic (atomic-scale) realm, and the variables describing the macroscopic realm. In the microscopic world we can talk about position, velocity, and mass of the individual atoms, all of which are  governed by Newton's laws of motion. By the use of statistical mechanics and averages we can then relate these  variables to the macroscopic world by talking about such quantities as pressure, volume, temperature, and  moles. For now, though, let's focus on the macroscopic world and search for an equation of state that will tell us  the relationships between all these macroscopic world quantities. Boyle's Law We start with the experimental observations of Robert Boyle, who showed that the quantities of pressure times  volume are a constant. This is called Boyle's Law. This is shown in the diagrams below. Each line on the graph is a line of constant temperature, and is called an isotherm. In a plot of P versus 1/V, we  see that the isotherms are straight lines with constant slopes. For an ideal gas the pressure times the volume is constant, but for real-world gases this is not always true.
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This note was uploaded on 10/13/2011 for the course CHEMISTRY 121 taught by Professor Staff during the Fall '10 term at Bangladesh University of Eng and Tech.

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The Gaseous State - We have a pretty good understanding of...

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