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Which Of The Following Statements Is True Concerning Ideal Gases? written
An ideal gas is a theoretical gas that follows the kinetic theory of gases. It is a gas that is composed of molecules that are in constant random motion. The molecules of an ideal gas are assumed to be point masses that do not interact with each other except through perfectly elastic collisions. The volume occupied by these molecules is negligible. Ideal gases obey the ideal gas equation given by: PV = nRT. Ideal gas molecules themselves take up no volume, but the gas takes up volume since the molecules expand into a large region of space.
For an ideal gas, all of the following statements are true:
1. There are no intermolecular forces of attraction between the molecules of the gas.
2. The volume occupied by these molecules is negligible.
3. Ideal gases obey the ideal gas equation given by: PV = nRT.
The temperature of an ideal gas sample is directly related to the average kinetic energy of its particles. The temperature of a gas sample is directly related to the average velocity of its particles.
The pressure of an ideal gas sample is directly related to the number of particles in the sample and their average kinetic energy. The pressure of a gas sample is directly related to the number of particles in the sample and their average velocity.
The volume occupied by an ideal gas sample is directly related to the number of particles in the sample and their average kinetic energy. The volume occupied by a gas sample is directly related to the number of particles in the sample and their average velocity.
The molar volume of an ideal gas depends only on T and P, not the identity of the gas.
The root-mean-square speed (rms speed) of an ideal gas molecule is directly proportional to the square root of its absolute temperature.
The average kinetic energy per molecule for an ideal gas is proportional to its absolute temperature.
The speed distribution for an ideal gas molecule follows a Maxwell-Boltzmann distribution.
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