The correct answer is
The particles in a gas are attracted to each other.
:)
The following is NOT an assumption of the kinetic theory of gases : The particles in a gas are attracted to each other.
Kinetic Molecular Theory (KMT) states that a gas consists of molecules that move at a constant and random speed. The collisions between molecules are perfectly elastic so that no energy is wasted.
The molecules move in straight lines until they collide
Energy because this motion is expressed as Kinetic energy (KE) which can be formulated as:
[tex] \displaystyle KE = \frac {1} {2} mv ^ 2 [/tex]
The average kinetic energy value is only affected by temperature changes. The higher the temperature, the average kinetic energy of the molecule increases
This molecule is very small when compared to the distance between molecules, so the volume of gas contains mostly empty space
Gas particles move randomly (both speed and direction, as vector)
From the question :
Particle motion creates kinetic energy.
they collide between particles or the walls of its container
The volume of the individual particles is negligible
The motion of each particle is independent (no attraction or repulsion)
The collisions are elastic, so there is no loss of kinetic energy, only transferred from between particles
inertia affect during a collision
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Keywords: Kinetic Molecular Theory, Collisions, The average kinetic energy , gas molecule
