Law, of Boyle

The properties of hydrocarbon gases are relatively simple since the parameters of pressure, volume and temperature (PVT) can be related by a single equation. The basis for this equation is an adaptation of a combination of the classical laws of Boyle, Charles and Avogadro. 

Combining the laws of Boyle and Charles into one expression gives... 

The behavior of all gases that obey the laws of Boyle and Charles, and Avogadro s hypothesis, can be expressed by the ideal gas equation ... 

Kinetic theory A theory of matter based on the mathematical description of the relationship between pressures, volumes, and temperatures of gases (PVT phenomena). This relationship is summarized in the laws of Boyle s law, Charle s law, and Avogadro s law. 

Equation (5.1) can be derived from the empirical laws of Boyle and Charles by using the total differential. Boyle s law can be expressed by the relationship... 

Dilute gases obey the laws of Boyle and Gay-Lussac. PV = RT. lo a good approximation. Thus, it can readily be shown that the following relations hold for ihe compressibility ... 

If the gas is assumed 10 consist of molecules of negligible size and without interaction, then the gas can be shown to follow the laws of Boyle and Gay-Lussac therefore its isothermal and adiabatic compressibilities must be given by Equation (4). For a perfect gas, the percentage pressure rise is proportional to the percentage volume decrease if the change is small thus the compressibility is inversely proportional lo Ihe pressure. 

The equations for the laws of Boyle and Charles can be combined into one equation for use when pressure, volume, and temperature vary. 

In simple gases the molecular interactions are small. As a consequence some "model laws" may successfully be applied, e.g. the "laws" of Van der Waals, Trouton and Lennard-Jones. Van der Waals law is an extension of the law of Boyle-Gay Lussac, with corrections for the weak interaction and the proper volume of the gas molecules. For simple gases it is a fair approximation of the P-V-T-behaviour. It reads ... 

Law of Boyle. — The effect of pressure on gases was early discovered, but it was not until about 1662 that Boyle announced his Law —... 

The table shows that the theoretical deduction k = (p. 92) is only realised for the monatomic permanent gases, and also for mercury vapour, which is likewise monatomic. This also holds for certain metallic vapours not cited in the table. For all other gases k<% and the difference % — k is greater the more complicated the molecule and the more the gas in question deviates from the simple gas laws. Yet even where the laws of Boyle and Charles are followed with great exactness, as for... 

State the laws of Boyle, Charles, and Gay-Lussac as equations. (14.1)... 

As the vapour pressure curve shows, the boiling point of a compound can be lowered by reducing the total pressure this also has consequences on equipment design. According to the law of Boyle and Mariotte, p V = constant, the volume of gases increases under reduced pressure. These higher values have to be taken into account when calculating evaporation and condensation areas. 

From the kinetic theory of gases, without a knowledge of the law of distribution of velocities (i.e. of the way in which the number depends on v), we have found that the product of pressure and volume is a function only of the mean kinetic energy of the gas. But we have also an empirical law, the law of Boyle (1660) and Mariotte (1676), viz. at constant temperature the product of the pressure and volume of an ideal gas is constant. We must conclude from this that U, the mean kinetic energy per mole, depends only on the temperature of the gas. 

In my freshman course, I dealt with the ideal gas laws and the kinetic molecular theory that accounted for them. My organic chemistry classes explored the structural theory of organic chemistry developed in 1858byKekuleandCouper. Ineachofthose fields, I had to point out that the initial simple theory had to be amplified. Gases in fact were not ideal real gases did not exactly obey the simple laws of Boyle, Charles, and Gay-Lussac and the beautifully simple structural theory of 1858 could not account for all cases of isomerism. 

There are two delivery mechanisms used for these products. The first utilizes either a compressed or liquefied gas system and the second relies on Bernoulli s Principle. Compressed gases operate on the Laws of Boyles, Charles, and Guy Lussac over two sets of conditions to give ... 

The weights of gases as usually stated are those under standard conditions, 0°C. and 760 mm. pressure, and the necessary calculation must be made by the application of the laws of Boyle and of Charles to convert the results obtained in the experiment to those which would obtain under these conditions. 

As a general rule, the surface generated by three variables is not so simple as the one represented by a gas obeying the simple laws of Boyle and Charles. 

Avogadro s principle and the laws of Boyle, Charles, and Gay-Lussac can be combined into a single mathematical statement that describes the relationship among pressure, volume, temperature, and number of moles of a gas. This formula works best for gases that obey the assumptions of the kinetic-molecular theory. Known as ideal gases, their particles occupy a negligible volume and are far enough apart that they exert minimal attractive or repulsive forces on one another. 

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