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Under what conditions will a gas be most likely to exhibit the ideal gas properties predicted by the ideal gas law? (3 points)

High pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction are weaker

High pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant

Low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker

Low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is less significant

Respuesta :

facundo3141592

The ideal gas approximation is used for high temperatures and low pressures:

"Low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker"

When we can use the ideal gas approximation?

Real gases behave like ideal gases when we have:

High temperature: This increases the kinetic energy of the molecules, so it allows the molecules to overcome the intermolecular forces. (At lowest temperatures the intermolecular forces are more relevant).

Low pressure: Low pressure means that there is "more space" between each molecule, and thus, there are fewer interactions between the molecules. If we increase the pressure, also does the number of interactions.

So the correct option is the third one:

"Low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker"

If you want to learn more about ideal gases, you can read:

https://brainly.com/question/25290815

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