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Mike Blaber (Florida State University) 11.1: A Molecular Comparison of Gases, Liquids, and Solids is shared under a license and was authored, remixed, and/or curated by LibreTexts. The state of a substance depends on the balance between the kinetic energy of the individual particles (molecules or atoms) and the intermolecular forces.
- Intermolecular Forces
In contrast to intramolecular forces, such as the covalent...
- Kinetic Molecular Theory of Gases
Pressure and KMT. The macroscopic phenomena of pressure can...
- Chapter 10.7: The Kinetic Theory
At higher temperatures, therefore, the molecules of a gas...
- Intermolecular Forces
May 19, 2017 · Hope this helps :) Solids - vibrational (and rotational); moving very slowly. Liquids - vibrational, rotational, and translational; moving quickly. Gases - vibrational, rotational, and translational; moving very quickly. Particles are always moving. No matter what. There is a certain point where they move so slowly it is considered minuscule ...
Oct 10, 2023 · At higher temperatures, therefore, the molecules of a gas move more rapidly than at lower temperatures, and v p increases. The rms speed and the average speed do not differ greatly (typically by less than 10%). The distinction is important, however, because the rms speed is the speed of a gas particle that has average kinetic energy.
Jun 19, 2020 · Describe the behavior of an ideal gas. The kinetic-molecular theory is a theory that explains the states of matter and is based on the idea that matter is composed of tiny particles that are always in motion. The theory helps explain observable properties and behaviors of solids, liquids, and gases. However, the theory is most easily understood ...
The particles in a gas are moving very quickly in random directions. The speeds of the particles vary but, on average, they move quicker than they do in liquids and solids. This means that it does ...
Thus, the pressure of a gas becomes larger as the volume of the gas becomes smaller. Charles' Law (V T) The average kinetic energy of the particles in a gas is proportional to the temperature of the gas. Because the mass of these particles is constant, the particles must move faster as the gas becomes warmer.
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Heat causes the molecules to move faster, which means that the volume of a gas increases more than the volume of a solid or liquid. When you stop heating the flask it cools and contracts.
