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Explain what is the difference between real gas molecules and ideal gas molecules by kinetic theory?
Real gas molecules have volume and experience intermolecular forces, while ideal gas molecules are treated as point particles with negligible volume and no intermolecular forces. In real gases, molecules have varying speeds and collision effects due to their volume and interactions, while ideal gases follow the assumptions of the kinetic theory perfectly due to their simplified behavior.
What would make gas non ideal?
The gas molecules interact with one another
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
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.
Helium is most likely to behave as an ideal gas when it is under?
Helium is most likely to behave as an ideal gas when it is under conditions of low pressure and high temperature. Ideal gases follow the ideal gas law, which assumes the gas molecules have negligible volume and there are no intermolecular forces between them. At low pressure and high temperature, the molecules are far apart and moving quickly, closer to the assumptions of an ideal gas.
Diff between real gas and ideal gas?
In an ideal gas molecules interact only elastically.
For ideal gas force of attraction between molecules?
For an ideal gas, there is assumed to be no force of attraction between molecules. This assumption allows for simplification of the gas behavior under certain conditions, such as low pressure and high temperature. In reality, real gases do experience weak forces of attraction between molecules, but these are considered negligible in the ideal gas model.
What aspects are not accounted for in the ideal gas law?
The ideal gas law does not account for the volume occupied by gas particles and the interactions between gas molecules.
What are the ideal conditions for a gas mixture containing propane to behave like an ideal gas when mixed with air?
The ideal conditions for a gas mixture containing propane to behave like an ideal gas when mixed with air are when the temperature is high, the pressure is low, and the molecules are far apart from each other. This allows the gas molecules to move freely and independently, similar to how an ideal gas behaves.
What happenes to the particels of a gas when there are fewer of them?
This is the ideal gas with no collisions between molecules..
What makes a gas non-ideal?
The gas molecules interact with one another
Would a gas whose molecules were true geometric points obey the ideal gas law?
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.
Explain what is the difference between real gas molecules and ideal gas molecules by kinetic theory?
Real gas molecules have volume and experience intermolecular forces, while ideal gas molecules are treated as point particles with negligible volume and no intermolecular forces. In real gases, molecules have varying speeds and collision effects due to their volume and interactions, while ideal gases follow the assumptions of the kinetic theory perfectly due to their simplified behavior.
What characteristic makes a gas non-ideal?
The gas molecules interact with one another
What would make gas non ideal?
The gas molecules interact with one another
What characteristics make a gas non-ideal?
The gas molecules interact with one another
What characteristic would make a gas non ideal?
The gas molecules interact with one another
