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The volume occupied by gas molecules is negligible when compared to volume occupied by the gas.The collisions between gas molecules-gas molecules and gas molecules-walls of the container are perfectly elastic.
the negligible volume of a gas means that gas has a volume which is too little
they have no volume and their molecular force of attraction is negligible
Because no matter how big or small the gas particle itself is they are so spread apart that its size becomes negligible
a solid in gas and liquid in gas solutions are diffiuclt to obtain because it is difficult for these solute particles to be individually dispersed in a gas medium. the particles are usually in clusters of collodial size.
The volume occupied by gas molecules is negligible when compared to volume occupied by the gas.The collisions between gas molecules-gas molecules and gas molecules-walls of the container are perfectly elastic.
the negligible volume of a gas means that gas has a volume which is too little
they have no volume and their molecular force of attraction is negligible
gas particles have little to no attraction for each other and have a negligible (insignificant) volume that needs not to be accounted for
Because no matter how big or small the gas particle itself is they are so spread apart that its size becomes negligible
5.62 atm
As the volume of a given gas sample is dependent on its temperature and pressure; to find a volume of any gas which does exist, the temperature and the pressure of the system/vessel should be given directly or could be calculated.
a solid in gas and liquid in gas solutions are diffiuclt to obtain because it is difficult for these solute particles to be individually dispersed in a gas medium. the particles are usually in clusters of collodial size.
gasses take up the entire volume of their containers regardless of their molecular size. The intermolecular space is so huge that their molecular mass is negligible in comparison.
A 'real' gas would occupy a higher volume as compared to the same amount of gas would have when 'idealistically' calculated by the 'ideal' gas law. The 'eigen' volume (its own molecular dimension) is to be taken in account at high pressure.
kinetic theory of matter states that1.gas is made of a large number of small molecules.2.the molecules of the gas move randomly in all directions . During their motionthey hit the walls of the container which is responsible for the pressure.3. the volume occupied by the gas molecules is very small when compared to thetotal volume of the gas.(volume of the container in which the gas is kept)4. the force of attraction between the molecules of the gas is negligible.
Real gases behave most like ideal gases at high temperatures and low pressures.CASE 1 :- (At Higher Temperatures)when the temperature is high the kinetic energy of molecules increases and the intermolecular attractions among the atoms decreases.The volume of the gas molecules become negligible compared to volume of the vessel. therefore the real gases act like ideal At Higher Temperatures.CASE 2 :- (At Lower Temperatures)At low temperatures volume of the container is larger. therefore intermolecular attractive forces are negligible and the volume of the particles also become negligible compared with the volume of the vessel.therefore the real gases act like ideal At Lower Temperatures.