COMPAIRING OF PERFECT GASES AND REAL GASES

In brief, we may state that Ideal gases have molecular interactions, with the mass of the molecules receiving more attention. However, the factors are altered by an unusually low temperature and high pressure. The Bayel Maryot rule states that for Ideal gases, the effect of pressure on the bulk at constant temperature has a constant magnitude, hence in this instance, PV is equal to CONST (PV = constant). The attractive force between molecules and the majority of molecules in actual gases (gases seen in nature) should be investigated under high pressure and low temperature (relatively). Actual gases in environments similar to Ideal gases must be very dependent on the rule for Ideal gases. And it should be distinct from the circumstances of ethylene gas. This indicates that gases differ from the principles of Normal gases to the extent that their gravity increases as a result of high pressure and a lower temperature. The distance between molecules decreases when pressure is high enough and temperature is low enough. However, the strength of molecular interactions has greatly increased, which has the effect of changing a substance from a gas to a liquid. As this method was once used to turn gases into liquids. Compressor is the term used to describe the process by which gases are changed into liquids. The compression factor of all perfect gases is z=1, and under any pressure, it neither drops nor increases from 1. This is another contrast between the behavior of perfect gases and real gases. However, this behavior differs in real gases because they can have compression factors that are diametrically opposed to 1, or (z≠1). Keywords: Ideal gas, Real gas, Carbon dioxide, compression factor, compressor.

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