By Ya. A. Smorodinsky
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Additional resources for Temperature (Science for Everyone)
Sample text
III. Now that the temperature of the gas is equal to that of the heat sink, move the cylinder into the heat sink and start compressing the gas, watching that at all times its temperature is constant and equal to T2. This will consume a work 52 Temperature A2 and transfer a heat Q2 to the heat sink. Stop the compression when the pressure and volume of the gas correspond to the third vertex of the curvilinear quadrangle (Fig. 7). IV Move the cylinder back into the thermos and, continuing to compress the gas, make it return to the initial state, that is, make it reach the pressure and temperature it had at the start of the first stage (Fig.
In chemistry the burning and oxidation of matter could be explained by the release of caloric. The caloric theory became generally accepted in the last quarter of the 18th century. light was ascribed two properties: its ability to illuminate and its ability to heat. Those who considered light to represent vibrations of ether believed that heat also consisted of similar vibrations and of motions generated by the ether in the particles of a body. " The caloric theory (nowadays we would say "the caloric model") explained a wealth of facts.
Walther Hermann Nernst had started along the correct way even before Planck’s discovery. He was the first to realize that some types of motion do not have "equal rights" in the partitioning of energy, being "frozen out" at low temperatures and entering the picture only at high temperatures. These ideas enabled Nernst to predict the behavior of things in the vicinity of absolute zero, although the actual meaning of his prediction became clearer much later in quantum mechanics. We shall see later how these ideas of N ernst have transformed the concept of the "number of degrees of freedom", which looks so trivial in classical mechanics.