Gay - Lussac experiment

Near the beginning of the nineteenth century, Joseph Gay-Lussac experimented with the volumes of gases. He found that adding two volumes of gas to one volume of gas produced only two volumes of gas. Puzzled, Gay-Lussac tried adding three volumes of gas to one volume. The result was still two When he tried adding one volume of gas to a second volume of gas, again the result was two. What was going on ... 

Let, in compliance with the solution of Gibbs Paradox, the integration constant S0 be the (change of) entropy AS which is added to the entropy a to figure out the measured entropy Sclaus of the equilibrium state of the system A (the final state of Gay-Lussac experiment) at a temperature 0. We have shown that without such correction, the less entropy o is evidenced,... 

After the fumes had condensed on the cold surface of the tank, Courtois noticed a residue of dark purple, metallic-looking crystals. A sample of this made its way into the hands of French chemist Joseph Gay-Lussac. He d heard that Sir Humphrey Davy also had a sample, and he didn t want an Englishman to make a big discovery based on a Frenchman s shrewd observation, so he got to work. Gay-Lussac experimented feverishly and discovered that the purple material was a new element. He named it iode, from the Greek for violet. Davy suggested iodine, echoing chlorine, an element that iodine resembles. 

At the maximum, the first term approaches zero because pjT 0, if the other terms remain finite. So we have to inspect the second term. We emphasize once more that we are dealing at constant energy. For an ideal gas, it is known that at the Gay - Lussac experiment, the temperature remains constant at isodynamic expansion. Therefore, we could directly obtain an expression for the second term. 

Equation (5.25) is the condition of the Gay - Lussac experiment. The isodynamic lines must be at the same time isotherms. Conversely, an isothermal process of an ideal gas is an isodynamic process. Such a process is taking place in the Carnot cycle. This means that the amount of energy is taken up from a thermal reservoir as thermal energy is released as expansion energy and vice versa. The situation is different in the Gay - Lussac experiment. Here the gas itself converts internally. When we write the energy as... 

Assuming the indicated values for the carbon molecular masses and its gas density, the carbonic oxide will be consisting, in conformity with the Gay-Lussac experiments, from equal volume parts of carbon and oxygen, and its volume will be equal with the sum of their constituents volumes. The resulted molecule will be formedfrom carbon and oxygen units, molecule to molecule, with an analog behavior to the nitrous gas. The mass of the carbonic acid molecule will be (11.36+2xl5.074)/2=20.75=1.5196/0.07321 and the one of the carbonic oxide will be given by (11.36+15.074)72=13.22=0.96782. 

Let us explore the entropy Sgoitz during the Gay-Lussac experiment. 

The procedure may be illustrated by the following simple experiment, which is a modification of the Gay Lussac-Stas method. The sodium chloride solution is added to the silver solution in the presence of free nitric acid and a small quantity of pure barium nitrate (the latter to assist coagulation of the precipitate). 

Charles and Gay-Lussac carried out a number of experiments with the hope of improving the performance of their balloons. They found that, provided the pressure is kept constant, the volume of a gas increases as its temperature is raised. In this case, a straight-line graph is obtained when the volume is plotted against the temperature (Fig. 4.10). This result implies... 

After some debate between the two, in which Dalton cast doubt on Gay-Lussac s experiments, the conclusion was reached that equal volumes of gas (when measured under the same conditions of temperature and pressure) must contain equal numbers of molecules. This statement (Avogadro 1811), attributable to another great scientist, Amedeo Avogadro (1776-1856), from 1820 Professor of Physics at Turin, was consistent with observation, if it is assumed that simple gases such as oxygen and nitrogen are composed of molecules made up of two atoms, and is now known as Avogadro s... 

In 1808 two French chemists, Joseph Louis Gay-Lussac (1778-1850) and Louis-Jacques Thenard (1777-1857), experimented along the same lines as Davy and should also be given some credit for the discovery of these elements. The Frenchmen named the new element bore, and Davy called it boracium. ... 

As new experiments were performed, the results sometimes seemed to contradict Berzelius s atomic weight determinations. Different chemists began to make different assumptions about how the weights should be calculated. There was confusion also about the terms atom and molecule themselves. At mid-century these two words were still used interchangeably. Even the discovery of simplicity sometimes proved to be confusing. In 1808 the French chemist and physicist Joseph Louis Gay-Lussac discovered a simple chemical law and chemists did not know how to explain it. 

Gay-Lussac announced the results of his experiments in 1808. The reaction was mixed. Although Berzelius accepted the results and used them in his atomic-weight research, Dalton maintained that they couldn t possibly be correct. The truth is, he said, that gases do not unite in equal or exact measures in any one instance when they... 

Gay-Lussac and Thenard then gave a detailed description of the experiment, saying ... 

His paper on the reactions that take place in the Gay-Lussac towers of sulfuric acid plants resulted from his successful experiments on the absorption of obnoxious sulfur dioxide fumes from an ultramarine plant In order to analyze the gases, he invented the Winkler gas buret with a three-way stopcock, and perfected his own methods. In the meantime he made his living by producing nickel and cobalt on a commercial scale. 

The investigation of Davy was afterwards prosecuted by Gay-Lussac and TmSnard, who, however, for some.timc still regarded the metn] to be a compound of the alkali with hydrogen. Berzelius, on the contrary, repeating Davy s experiments, satisfied himself of the correctness of the theory of the latter chemist. 

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