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Get Answers to all your Questions
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- #States of Matter : Gases and liquids
Which of the following claims concerning the kinetic molecular theory of gases is correct?
Gases consist of large, dense particles that are in constant motion.
Gas particles have a strong attraction to each other.
The volume of a gas particle is negligible compared to the volume of the container.
Gas particles move in straight lines and never collide with each other.
Answers (1)
The kinetic molecular theory of gases is a paradigm for explaining gas behaviour.
Gases, according to this hypothesis, are made up of microscopic particles that are constantly moving at random.
Option (3) is Correct - Because the kinetic molecular theory believes that gas particles are so minute that their volume is minimal in comparison to the volume of the container they occupy. This implies that gas particles may be thought of as point masses, and the overall volume of the gas can be assumed to be the container's volume.
The theory also makes some assumptions about how these particles behave:
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Gas particles are minuscule and have a minimal volume in comparison to the container's volume.
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Gas particles are always moving at random.
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There is no strong attraction or repulsion between gas particles.
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Gas particles clash with one another and the container's walls, but these collisions are fully elastic.
Option (1) is incorrect because the kinetic molecular theory expects tiny gas particles with minimal volume.
Option (2) is wrong because the kinetic molecular theory implies that there is no strong attraction or repulsion between gas particles.
Option (4) is wrong because the kinetic molecular theory assumes that gas particles move randomly and clash with each other and the container walls.
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