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Would a gas whose molecules were true geometric points obey the ideal gas law?
Arooo2006
If gas molecules were true geometric points (ie had zero volume) AND had zero intermolecular interaction (such as attraction or repulsion), then the gas would obey the ideal gas law. Gases composed of small, non-interactive molecules (such as helium gas) obey the ideal gas law pretty well (as long as the gas is low density and temperature is rather high). For non-ideal gases, at least two correction factors are often used to modify the ideal gas law (correcting for non-zero volume of gas molecule and intermolecular attraction) such as in the Van der Waals equation for a real gas.
Wiki User
∙ 14y ago
Anonymous
Yes, a gas whose molecules are true geometric obey ideal gas law because molecules of ideal gas are also point particles.
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For ideal gas force of attraction between molecules?
In an ideal gas there is no attarcation between molecules. There is no such thing as an ideal gas it is a model that approximates the behaviour of real gases.
What gas would be most ideal if at STP?
Helium comes very close to ideal at STP since it is so small and monatomic. In reality most gases are pretty indistinguishable from ideal at STP because the molecules are so far apart that their individual volumes are negligible compared to the space they are in and the molecules are so far apart that they exert negligible force on each other.
What characteristic would make a gas non ideal?
The gas molecules interact with one another
Is ideal gas one whose particles take up space?
An ideal gas is a theoritical gas consisting of randomly moving particles.The kinetic theory of ideal gases makes 5 main assumptions:The size of molecules is negligible compared with the mean intermolecular distance (i.e. they are widely spaced molecules).Molecules move with different speeds and in random directions.Standard laws of motion apply.Collisions between molecules are elastic. Translational kinetic energy is not converted into other forms of energy.There are no attractive intermolecular forces between molecules except during collision.
What characteristics would make a gas non-ideal?
The gas molecules interact with one another
What is the geometric definition for point?
The intersection of two ideal lines
What would make gas non ideal?
The gas molecules interact with one another
For ideal gas force of attraction between molecules?
In an ideal gas there is no attarcation between molecules. There is no such thing as an ideal gas it is a model that approximates the behaviour of real gases.
The molar volume for CO2 and HCl are 22.262 Lmol and 22.244 Lmol Why are these molar volumes slightly less than the ideal molar volume of 22.4 Lmol?
Because neither is an ideal gas. Ideal gas molecules are assumed to be points with no spatial extensions, gas molecules have a finite size. The van der Waals equations of state need to be applied. This is the main reason.
Why does strong repulsion between molecules not represent an ideal gas behavior?
The ideal gas laws are based on a model in which the ideal gas is composed of molecules which neither attract nor repel each other. The pressure that the ideal gas exerts on its container is simply the result of the random thermal motion of the molecules and the continual collisions which result from that random thermal motion. If the molecules also repelled each other, then they would produce a gas with even higher pressure, and the pressure would also increase more rapidly, if the gas was compressed, than it does in the absence of such repulsion. The observed behavior of real gases is much closer to that of an ideal gas that does not include repulsion between molecules. No such repulsion has been observed.
Why real gases deaviat from ideal behaviou?
It is assumed that Ideal Gases have negligible intermolecular forces and that the molecules' actualphysical volume is negligible. Real Gases have the molecules closer together so that intermolecular forces and molecules' physical volumes are no longer negligible. High pressures and low temperatures tend to produce deviation from Ideal Gas Law and Ideal Gas behavior.
Explain what is the difference between real gas molecules and ideal gas molecules by kinetic theory?
In an ideal gas, molecules don't take up space, and don't have long-range interactions.
When can you safely assume any gas is ideal?
Characteristics of an ideal gas:- an extremely low concentration- molecules are in a permanent motion- Newton laws can be applied- all collisions are elastic- molecules are spherical- molecules are not compressible
Diff between real gas and ideal gas?
In an ideal gas molecules interact only elastically.
Why ammonia doesnt behave as an ideal gas?
NH3, as in Ammonia, like all real gases, are not ideal. Ideal gases follow the ideal gas laws, but ammonia does not adhere to a few of them. First of all, the volume of its molecules in a container is not negliggible. Next, NH3 molecules have intermolecular hydrogen bonding, which is a strong intermolecular bond. Thus, the forces of attaction between molecules is not neglible. All real gases have a certain degree of an ideal gas, but no real gas is actually ideal, with H2 being the closest to ideal.
What gas would be most ideal if at STP?
Helium comes very close to ideal at STP since it is so small and monatomic. In reality most gases are pretty indistinguishable from ideal at STP because the molecules are so far apart that their individual volumes are negligible compared to the space they are in and the molecules are so far apart that they exert negligible force on each other.
What is the molecules of an ideal gas?
Perfectly elastic collisions, point masses (no volume of individual molecules), no intermolecular attractions.
