it is co2 acctive
In the gas state, molecules have weak intermolecular forces of attraction. These forces are much weaker compared to the forces in the liquid or solid states, allowing gas molecules to move freely and independently of each other.
A gas is formed from molecules with intermolecular forces near zero.
higher molecular volumes and exhibit intermolecular forces, such as van der Waals forces, that cause deviations from ideal gas behavior. These intermolecular forces affect the compressibility, volume, and pressure of a real gas, making it different from the assumptions of an ideal gas.
No it is not true
the bonds between particles in a liquid are very weak
In the gas state, molecules have weak intermolecular forces of attraction. These forces are much weaker compared to the forces in the liquid or solid states, allowing gas molecules to move freely and independently of each other.
The gas molecules interact with one another
A gas is formed from molecules with intermolecular forces near zero.
A gas is formed from molecules with intermolecular forces near zero.
it is co2 acctive
In solid, the molecules r tightly packed by intermolecular forces, but in gas these forces r very loose.
higher molecular volumes and exhibit intermolecular forces, such as van der Waals forces, that cause deviations from ideal gas behavior. These intermolecular forces affect the compressibility, volume, and pressure of a real gas, making it different from the assumptions of an ideal gas.
An ideal gas is not a real thing, just an idea. The definition of an ideal gas is one where there are no forces between the particles. If there are no forces, there is nothing to bring the particles together into a liquid. In a real gas of course there are forces of attraction which keep the particles together when they are moving sufficiently slowly.
Van der Waals forces, specifically London dispersion forces, are the most important intermolecular forces that allow Ar gas to liquefy. These forces arise due to temporary dipoles induced in Ar atoms leading to attractive forces between neighboring atoms. At low temperatures and high pressures, these forces prevail, causing Ar gas to condense into a liquid state.
The correct order is: gas < liquid < solid. This is because in the gas phase, molecules are far apart and have weak intermolecular forces, in the liquid phase, molecules are closer together with moderate intermolecular forces, and in the solid phase, molecules are tightly packed with strong intermolecular forces.
Scientists can ignore intermolecular forces in a gas under ordinary conditions because gases have weak forces of attraction compared to liquids and solids. The particles in a gas are far apart and move freely, resulting in negligible interaction between individual particles. Hence, the effects of these weak forces are often minimal and can be disregarded for many practical purposes.
solid,liqiud,gas