What kind of gas is an ideal gas? Any examples?
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In studies, ideal gases are often encountered; in reality, however, it is actual gases that exist. It would be best to give a few examples of the types of gases that can be considered ideal gases in practical situations
The original poster suggests taking a look at physical chemistry. An ideal gas should be a gas that meets the following conditions: 1. The volume of its molecules is negligible compared to the volume of the gas itself； 2. There is no mutual attraction between molecules ； 3. Collisions between molecules and between molecules and the container walls do not result in a loss of kinetic energy. 4. In the container, the gas molecules are considered to be in uniform motion when there are no collisions; when collisions occur, velocity is exchanged without any loss of kinetic energy. 5. When solving thermodynamics problems, it is simply assumed that the molecular potential energy is zero while the molecular kinetic energy is not zero. 6. The internal energy of an ideal gas is the sum of the molecular kinetic energies. In practice, those that can approach the above conditions can be regarded as ideal gases
An ideal gas can be roughly considered as a gas at high temperature and low pressure, satisfying the conditions mentioned above.
Ideal gases do not exist; only situations that are similar to the properties of ideal gases exist. That is, the physical properties of gases at high temperatures and low pressures are similar to their ideal properties.
The correct answer is floor 4. In reality, gases are only infinitely close to ideal gases; when gases are at high temperatures and low pressures, they can be considered ideal gases~~
Ideal gases obey Dalton’s law of partial pressures. When the total pressure is not too high (usually not higher than 10,000 kPa), the gas phase can be considered an ideal gas
This post was last edited by caress7032 on 2010-4-10 22:57. For an ideal gas, at any temperature and pressure, Z = PVm/RT = 1. Z is known as the compressibility factor, and its value depends on temperature and pressure
Non-associated gases at low and normal pressures can generally be considered ideal gases.
An ideal gas should be in an ideal state; in reality, the situation can only be close to that. It is generally an approximate ideal state.
This post was last edited by El Niño on 2010-4-12 at 17:27. For an ideal gas, the key requirement is that 1, the size of the gas molecules can be ignored； 2. The mutual “independence” of individual molecules. Therefore, in general, at low pressures, the distance between molecules is large; the molecules can be treated as “points,” and their interactions can be ignored—making them ideal gases. Of course, some might argue: What if the temperature of the gas is extremely low? In this case, although the pressure is low, the molecules are still packed together; the distance between them is not large at all! To avoid objections, several brothers above mentioned that a certain temperature limit should also be set.
Gases that strictly obey the gas law (PV=(m/M)RT=nRT) are called ideal gases. In some books, this term refers to gases that satisfy the three laws of gases. ) From a microscopic perspective, a gas in which both the volume of the molecules themselves and the forces acting between them can be ignored is called an ideal gas.