According to kinetic molecular theory, how are gases compared with liquids and solids?
According to the kinetic theory of matter, molecules in gases move more in three dimensions—rotation, translation, and vibration—than molecules in solids and liquids.
Because of this, gases lack fixed volumes; instead, their molecules simply roam "carelessly" over available space, involving little to no intermolecular forces other than collisions.
Furthermore, we can observe that there are far more gas-molecule collisions than there are in liquids and none in solids.
It is also important to remember that a gas's pressure is determined by the collisions its molecules have with the container it is contained in as well as any other objects they come into contact with.
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The three distinct states of matter are explained by the Kinetic Theory of Matter.
Solid: The particles vibrate about fixed positions because of their low kinetic energy and well-organized, densely packed arrangement, which creates strong attractive forces between them.
Liquid: The arrangement of the particles is less dense and disorderly than in solids; the attractive forces between them are stronger in liquids than in solids, but they are still able to slide over one another because of the low kinetic energy of the particles.
Gas The particles are disorganized and widely spaced; their kinetic energy is high and their attractive forces are weak, causing them to travel at high speeds in a random manner.
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According to the kinetic molecular theory, gases differ from liquids and solids in the following ways:
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Particle Spacing: Gas particles are much farther apart than particles in liquids or solids. This large distance relative to their size means that intermolecular forces are significantly weaker in gases than in liquids or solids.
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Particle Movement: Gas particles move quickly and randomly, covering large distances relative to their size. In contrast, particles in liquids also move but are much closer together and slide past each other, while particles in solids vibrate in fixed positions due to very strong intermolecular forces that keep them tightly packed.
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Shape and Volume: Gases do not have a fixed shape or volume; they expand to fill the shape and volume of their container. Liquids have a fixed volume but take the shape of their container, whereas solids have both a fixed shape and volume.
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Compressibility: Gases are easily compressible due to the large amount of space between particles. Liquids and solids are virtually incompressible because their particles are already close together.
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Energy: Particles in gases have the highest kinetic energy compared to particles in liquids and solids, which is a direct consequence of their rapid, random motion.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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