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Which is an example of the kinetic-molecular theory not holding true for a gas? The average kinetic energy of particles depends only on the temperature. The particles in a gas travel in straight lines in a continuous, random motion. The attraction between particles causes a gas to condense at low temperatures. The particles in a gas make up a small portion of the total volume of the gas.

Kristi Hammond

in Physics

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Megan Page on February 16, 2019

Answer: the third option, the attraction between the particles causes a gas to condense in low temperaturesExplanation:1) The kinetic-molecular theory explains the behavior and properties of gases in terms of energy, the size and movement of its particles or molecules.2) Depending on the size, particles are considered to make a small portion of the total volume of the gas, to the point that their size is fully neglected (zero). The particles are considered not to occupy any space (volume) of the gas.3) The first and the second instructions are directly indicated by the molecular weight of the kinetic theory: (a) the average kinetic energy of particles depends only on the temperature, and (b) the particles in a gas travel in straight line in a continuous random motion.With regard to the assertion that the attraction between the particles causes a gas to condense at low temperatures, this is not true.First of all, the kinetic molecular theory of gases is not valid at low temperatures and high pressure.Second, depending on the gas and the force of intermolecular, in the low temperarures a gas which can condense or not. Depends on the attraction forces, which are neglected by the gas by the molecular weight of the kinetic theory.


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