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Why gases show high compressibility?
The intermolecular forces in gases are very weak.
Which matter has the minimum inter molecular force?
Intermolecular forces are weak in gases.
What are two characteristics of an ideal gas that are not true of a real gas?
they have no volume and their molecular force of attraction is negligible
How does the intermolecular forces between particles of matter in different states compare?
Intermolecular forces are very weak in gases. They are stronger in liquids, holding the molecules very close together, but still allowing motion around each other. They are strongest in solids, holding the molecules in a tight formation with only vibration about fixed positions.
Why are intermolecular force of attraction significant in solid and liquid but not in gases?
Intermolecular forces are significant in solids and liquids because the particles are in close proximity to each other, allowing the forces to have a strong influence on the arrangement and movement of the particles. In gases, the particles are further apart and have higher kinetic energy, which weakens the effect of intermolecular forces. As a result, gases are more influenced by factors such as temperature and pressure rather than intermolecular forces.
Why gases show high compressibility?
The intermolecular forces in gases are very weak.
What is the difference about the intermolecular forces of attraction between the phases that allows fluids and gases to flow but prevent solids from flowing?
Fluids and gases have weak intermolecular forces that allow particles to move past each other, enabling flow. In contrast, solids have stronger intermolecular forces that hold particles in fixed positions, preventing flow. This difference in intermolecular forces allows fluids and gases to flow easily, while solids maintain their rigid structure.
A description of gases and liquids are?
Gases have neither a definite shape nor a definite volume. Liquids do not have a definite shape, but they DO have a definite volume. Gases have no or little intermolecular forces holding them together, whereas liquids do have substantial intermolecular forces.
Which matter has the minimum inter molecular force?
Intermolecular forces are weak in gases.
Why does gas expend when heated and easy to compress?
The intermolecular forces in gases are weak.
What are two characteristics of an ideal gas that are not true of a real gas?
they have no volume and their molecular force of attraction is negligible
What does gases do to fill what ever space is available to them?
The intermolecular forces in gases are extremely small; gases easily diffuse in any space.
How does the intermolecular forces between particles of matter in different states compare?
Intermolecular forces are very weak in gases. They are stronger in liquids, holding the molecules very close together, but still allowing motion around each other. They are strongest in solids, holding the molecules in a tight formation with only vibration about fixed positions.
Do Gases have the strongest intermolecular bonds?
Gases don't form inter-molecular bonds, as the molecules are free floating. Solids would have the strongest, being held rigidly in a single shape, unlike liquids.
Why are intermolecular force of attraction significant in solid and liquid but not in gases?
Intermolecular forces are significant in solids and liquids because the particles are in close proximity to each other, allowing the forces to have a strong influence on the arrangement and movement of the particles. In gases, the particles are further apart and have higher kinetic energy, which weakens the effect of intermolecular forces. As a result, gases are more influenced by factors such as temperature and pressure rather than intermolecular forces.
What is intermolecular forces in Ar?
Intermolecular forces in argon involve London dispersion forces, which are weak attractive forces caused by temporary fluctuations in electron distribution. These forces are the primary intermolecular force in noble gases like argon, given their lack of permanent dipoles.
How does an ideal gas diff from a real gas?
Ideal gases are gases with negligible intermolecular forces and molecular volumes. Real gases have intermolecular forces and have definite volumes at room temperature and pressure (RTP).
