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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
The structure of liquid water is very similar, but in the...
- Kinetic Molecular Theory of Gases
Pressure and KMT. The macroscopic phenomena of pressure can...
- Intermolecular Forces
The substance changes from a gas to a liquid. When a liquid is cooled to even lower temperatures, it becomes a solid. The volume never reaches zero because of the finite volume of the molecules. Figure 13.5.1 13.5. 1: A sketch of volume versus temperature for a real gas at constant pressure.
- List of Phase Changes
- Phase Changes For States of Matter
- Examples of Phase Changes
- Why Phase Changes Occur
- References
Here is a list of the phase changes of matter. 1. Melting (Solid → Liquid) 2. Freezing (Liquid → Solid) 3. Vaporization or Evaporation (Liquid → Gas) 4. Condensation (Gas → Liquid) 5. Deposition (Gas → Solid) 6. Sublimation (Solid → Gas) 7. Ionization (Gas → Plasma) 8. Deionization or Recombination (Plasma → Gas)
Another way to learn phase changes is to associate them with the starting state of matter: 1. Solid: A solid can melt into liquid or sublimate into gas. 2. Liquid: A liquid can freeze into a solid or vaporize into a gas. 3. Gas: A gas can deposit into a solid, condense into a liquid, or ionize into plasma. 4. Plasma: Plasma can deionize or recombin...
Melting: Solid ice melts into liquid water.Freezing: Freezing waterchanges it from a liquid into solid ice.Vaporization: An example of vaporization is the evaporation of rubbing alcohol from skin into the air.Condensation: A good example of condensation is dew formation from water vapor in air.Most phase changes occur because of a change in the energy of the system. Increasing temperature gives atoms and molecules more kinetic energy, helping them break bonds and move further apart. Similarly, decreasing temperature slows down particles and makes it easier for them to gain rigid structure. Increasing pressure forces particle together, wh...
Blundell, Stephen J.; Katherine M. Blundell (2008). Concepts in Thermal Physics. Oxford University Press. ISBN 978-0-19-856770-7.IUPAC (1997). “Phase Transition”. Compendium of Chemical Terminology (2nd ed.) (the “Gold Book”). ISBN 0-9678550-9-8. doi:10.1351/goldbookJaeger, Gregg (1 May 1998). “The Ehrenfest Classification of Phase Transitions: Introduction and Evolution”. Archive for History of Exact Sciences. 53 (1): 51–81. doi:10.1007/s004070050021Oct 10, 2023 · A gas is composed of a large number of particles called molecules (whether monatomic or polyatomic) that are in constant random motion. Because the distance between gas molecules is much greater than the size of the molecules, the volume of the molecules is negligible.
Identify and describe the triple point of a gas from its phase diagram. Describe the state of equilibrium between a liquid and a gas, a liquid and a solid, and a gas and a solid. Up to now, we have considered the behavior of ideal gases. Real gases are like ideal gases at high temperatures.
A distinct boundary between the more dense liquid and the less dense gas is clearly observed. As we increase the temperature, the pressure of the water vapor increases, as described by the liquid-gas curve in the phase diagram for water (Figure 11.5.2), and a two-phase equilibrium of liquid and gaseous phases remains. At a temperature of 374 ...
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As you cool a liquid, removing energy from it, the movement of the particles gets slower. At some point they get slow enough that the attractive forces are strong enough to trap them and lock them into the solid structure. The liquid freezes. Changes of state between liquid and gas. Boiling.
