Consider the following gases, all at STP: Ne, SF6, N2, CH4.(a) Which gas is most likely to depart from the assumptionof the kinetic-molecular theory that says there areno attractive or repulsive forces between molecules?(b) Which one is closest to an ideal gas in its behavior?(c) Which one has the highest root-mean-square molecularspeed at a given temperature? (d) Which one hasthe highest total molecular volume relative to the spaceoccupied by the gas? (e) Which has the highest averagekinetic-molecular energy? (f) Which one would effusemore rapidly than N2? (g) Which one would havethe largest van der Waals b parameter?

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Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.