Which of the following statements about the kinetic molecular theory are not correct?
a. the combined volume of all the molecules of the gas is negligible relative to the total volume in which the gas is contained
b. gases consist of molecules that are in continuous, random motion
c. the average kinetic energy of the molecules is not related to the absolute temperature
d. attractive and repulsive forces between gas molecules are negligible

The false statement is: (C) The average kinetic energy of the molecules is not related to the absolute temperature

Explanation:

According to the Kinetic Theory of Gases, gases are composed of small fast moving particles that are in constant random motion. These gaseous particles are known as molecules.

It is assumed that the mass of all the gaseous molecules is the same and the intermolecular interactions (attractive or repulsive) are negligible.

Also, the total volume of all the gaseous molecules is considered to be negligible as compared to the volume of the container.

According to this theory, average kinetic energy (K) of the gaseous particles is directly proportional to the absolute temperature (T) of the gas, by the equation:

Here, is the Boltzmann constant

Therefore, the false statement about the kinetic molecular theory is (C)

hey there!

mass = 6.75 g

volume =   9 cm³

therefore:

d = mass / volume

d   = 6.75 / 9

d = 0.7 g/cm³

answer b