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Gas four basic states of matter (including solids, liquids, and plasma) is one. Pure will be able to make a gas atoms (eg a noble gas or atomic gas like neon), the basic molecule atom (oxygen, for example), or the type of atoms in molecules (eg, carbon dioxide), a type of compound has been made. A gas mixture would contain a variety of pure gases much like the air. What distinguishes the individual gas particles in gas-liquid and solid separation is large. This distribution is usually colorless gas invisible to the human observer. Gas particles and the gravitational interaction of the electric field vectors are considered negligible figure represents a constant speed.
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State of matter, gaseous, liquid, and plasma is one of the states, [1] and the second, on the other hand, provides an upper limit on the gas temperature. Lower limit of the temperature scale lie degenerative quantum gases [2] is gaining increasing attention in these days. [3] High-density atomic gases super cooled to very low temperatures are classified by their statistical behavior of the Bose gas or a Fermi gas. , Material For a complete list of these exotic states of matter see list of states.
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Observing a gas, it is typical to specify a frame of reference or length scale. Macroscopic or global point of a gas in a larger scale. This region (referred to as a volume) must be of sufficient size to have a large sample of the gas particles. As a result of the sample size, the statistical analysis of the "average") of the behavior of gas particles (ie, speed, temperature or pressure is generated. Contrast, the length of the smaller scale of the microscopic point of view, or particles.
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Macroscopically, the characteristics of the gas to be measured and the gas particles (velocity, pressure, or temperature) or their surroundings (volume) terms. For example, Robert Boyle studied pneumatic chemistry for a small portion of his career. The macroscopic properties of an experiment related to the pressure and volume of a gas. The J-tube manometer experiment, J. Boyle trapped an inert gas in the closed end of the tube with a column of mercury in the form of letters used in a test tube, and, therefore, the number of particles and the temperature constant. Gas pressure was increased, adding more mercury column, gas' trapped volume is decreased (ie, as the well-known inverse relationship) was observed. In addition, Boyle multiplied the pressure and volume of each observation, the product continuously. This relationship held every gas Boyle observed leading to the law, (PV = k), named in honor of his work in this field.
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There are many tools available to study the mathematical properties of the gas. Gases as the extreme conditions, and these tools become a bit more complex, Euler and Navier-Stokes equations of inviscid flow equations [9] to account for viscous effects. These equations are adapted to the conditions of the gas system in question. Using the results of the analytical Algebra Boyle's lab equipment. His results were not possible in the relatively low pressure of the gas in a way where the behavior of the "ideal" is to learn. Ideal relations applies to the calculation of the safety requirements of various materials used in flight. Was designed to explore the use of today's high-tech equipment operating safely for more exotic environments where the gas is not an "ideal" way to play. Advanced math, including statistics and Multivariable calculus, in order to, for example, to resolve the situation is complex, dynamic space reentry vehicles. An example of the image space shuttle reentry to ensure the appropriate material properties under this loading condition is recognition. In this regime of flight, their behavior is not gas.

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