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According to kinetic molecular theory, which of the following statements are true about the behavior of gases?



The particles of a gas are in constant, random motion.



Gases consist of small particles that are separated from one another by empty space.



Collisions between gas particles are elastic.



All of the above statements explain the behavior of gases.

Verified Answer :

Oseni

Answer:

All of the above statements explain the behavior of gases.

Explanation:

The kinetic molecular theory is a model that seeks to explain the behaviour of gases. The model upon which the gas laws are derived is based on five hypotheses:

  • The molecules of gases are in constant random motion, colliding with themselves and the wall of the container holding the molecules
  • These molecules are small compared to the spaces that separate them
  • As the gas molecules collides with one another and the wall of the container, pressure is created within the container holding the gas
  • The collision of these gas molecules does not lead to loss of any energy. That is, the collision is elastic.
  • The average kinetic energy of the gas molecules is directly proportional to the temperature (in Kelvin) of the gas

Hence, all the statements in the options are correct.

The kinetic theory describes the gas behaviour. The gas molecules are small free-moving balls, in random motion and have elastic collisions.

What is the kinetic molecular theory?

According to the theory, the gas molecules are assumed small randomly free-moving balls.No energy is lost during the collisions between these particles.

The collisions of the particles of the gas in the system are elastic. The gas molecules are not bonded by any strong bond hence the space is huge compared to their size.  

Therefore, option D. all the given statements explain the behaviours of the gas.

Learn more about kinetic molecular theory here:

https://brainly.com/question/12064935

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