The observation which indicates that the kinetic-molecular theory has limited use for describing a certain gas is: D. Increasing collisions of gas molecules will increase energy between them.
The kinetic-molecular theory of gas states that gas molecules (particles) exhibit a perfectly elastic collision and are always in a state of continuous
(constant) random motion.
According to the kinetic-molecular theory, the average kinetic energy of gas molecules (particles) is highly dependent on temperature.
This ultimately implies that, the average kinetic energy of gas molecules (particles) is directly proportional to the absolute temperature of an ideal gas.
The collisions of gas particles are perfectly elastic because there are no forces of attraction between gas particles and as such no energy is lost.
Additionally, gas molecules (particles) move in a straight line until they collide with another body.
In conclusion, there is no net loss of energy from the collisions of gas particles because it is perfectly elastic.
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