a theoretical idea, an ideal gas is one that obeys perfectly the ideal gas law, PV = nRT, at all temperature and pressure conditions. Real gases (nitrogen, oxygen, etc.) behave almost exactly like ideal gases when the temperature and pressure are close to room conditions. An ideal gas would have no attractive forces between its molecules, and its molecules would take up no space (they would be mathematical points). This is not really true, since: all gases do have attractive forces between their molecules (they can all be condensed to liquids by cooling them enough that the attractive forces are able to make the molecules clump together as liquids) all gases molecules have some size, or you would be able to infinitely compress them (and you cannot) The ideal gas law can be derived from the assumptions that are made in the kinetic-molecular theory. When the temperature is quite a way above the molecule's boiling point, then attractive forces are almost meaningless. When the pressure is not too high, molecules have so much space between them that their small size is not relevant. Under these conditions, real gases obey the ideal gas law very closely.
follows the perfect gas laws without deviation. Practically, there are no ideal gases, but it is the basis from which calculations are made and corrections applied.
A gas that obeys all the postulates of the kinetic molecular theory. Real gases differ from the expected behavior of an ideal gas for two reasons: (1) the force of attraction between the particles in a gas is not quite zero, and (2) the volume of the particles in a gas is not quite zero.
ideal gases; perfect gas; ideal gas law. A gas whose pressure P, volume V, and temperature T are related by PV = nRT, where n is the number of moles of gas and R is the ideal gas law constant. Ideal gases have molecules with negligible size, and the average molar kinetic energy of an ideal gas depends only on its temperature. Most gases behave ideally at sufficiently low pressures.
Ideal gas is a gas in which there is complete absence of cohesive forces between the component molecules; the behavior of such a gas can be predicted accurately by the ideal gas equation through all ranges of temperature and pressure. The concept is theoretical, since no actual gas meets the ideal requirement.
An ideal gas is a theoretical gas which follows the Ideal Gas Law: PV = [a constant]T P = pressure V = volume T = temperature
a collection of identical, infinitesimally small particles that interact only by elastic collisions.
Is a gas that follows the perfect gas laws without deviation. There is no such thing, however it is the basis from which calculations are made and corrections applied. ( 030)
One which obeys the ideal gas law. At low pressures, real gases behave like ideas gases.
a model in which gas molecules are treated as though they were geometric points exerting no force on each other; gas that behaves as predicted by kinetic molecular theory. Ideal Gas Law Equation PV = nRT
is a gas that obeys the ideal-gas equation of state.
a hypothetical gas with molecules of negligible size that exert no intermolecular forces
a gas consisting of point-like particles which do not interact with each other (ie, they do not stick together or repel each other)
a gas that conforms, in physical behavior, to a particular, idealized relatio
a gas that conforms in physical behavior to aparticular idealized relation between pressure volume and temperature
a hypothetical (imaginary) gas, which has no existence
an assembly of atoms or molecules which interact with each other only via occasional collisions
an exceptionally simple case, where the phenomenlogical law can be obtained from the partical-based model using judicious assumptions of randomness, due to the lack of any significant interaction between its parts
a gas made up of a large number of small spherical molecules, in random motion , that have only elastic collisions
One that obeys the gas laws at all temperatures and pressures. In reality no such gas exists.
a gas that obeys Boyle's law and Charles's law and satisfies the equation of state, has internal energy that depends on temperature only, and has specific heat that is independent of temperature
A hypothetical gas that obeys exactly all postulates of the kinetic-molecular theory.
(Also called perfect gas.) A gas for which the potential energy of interaction between molecules is independent of their separation and hence is independent of gas volume. Thus, the internal energy of an ideal gas depends only on its temperature. To a very good approximation, atmospheric gases at normal terrestrial temperatures and pressures are ideal.
a hypothetical gas that exactly obeys the ideal gas law. A real gas approaches ideal behavior at high temperature and/or low pressure.
An ideal gas or perfect gas is a hypothetical gas consisting of identical particles of zero volume, with no intermolecular forces. Additionally, the constituent atoms or molecules undergo perfectly elastic collisions with the walls of the container. Real gases do not exhibit these exact properties, although the approximation is often good enough to describe real gases.