Which of the following statements related to kinetic-molecular theory of gases is correct for an ideal gas? There are no attractive or repulsive forces between and among gas particles. Gas particles move slowly in a chaotic pattern until they collide with something. For a given amount of gas, the smaller the volume of the container, the fewer the collisions that occur with the container walls, since there is less surface area. The density of a gas is somewhat lower than that of a liquid. The more gas particles there are in a container, the more frequently they collide with one another, so the particles stick together, resulting in a lower pressure.
Which of the following statements related to kinetic-molecular theory of gases is correct for an ideal gas? There are no attractive or repulsive forces between and among gas particles. Gas particles move slowly in a chaotic pattern until they collide with something. For a given amount of gas, the smaller the volume of the container, the fewer the collisions that occur with the container walls, since there is less surface area. The density of a gas is somewhat lower than that of a liquid. The more gas particles there are in a container, the more frequently they collide with one another, so the particles stick together, resulting in a lower pressure.
ChapterU3: Weather: Phase Changes And Behaviour Of Gases
Section: Chapter Questions
Problem 7STP
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Question
Which of the following statements related to kinetic-molecular theory of gases is correct for an ideal gas?
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There are no attractive or repulsive forces between and among gas particles. |
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Gas particles move slowly in a chaotic pattern until they collide with something. |
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For a given amount of gas, the smaller the volume of the container, the fewer the collisions that occur with the container walls, since there is less surface area. |
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The density of a gas is somewhat lower than that of a liquid. |
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The more gas particles there are in a container, the more frequently they collide with one another, so the particles stick together, resulting in a lower pressure. |
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