Using the kinetic molecular theory, explain what the difference is between a gas that exerts a pressure of 1.0 atm and one that exerts a pressure of 1.5 atm. *

In the kinetic molecular theory, the molecules of an ideal gas are in constant random motion inside the container of the gas, and the pressure of the gas (which is the pressure exerted by the molecules in their collisions with the walls of the container) arise from this random motion of the molecules.

The main assumptions of the kinetic theory of gases are:

In particular, the pressure of the gas is directly proportional to the average kinetic energy of the molecules, according to the equation:

where

p is the pressure of the gas

V is the volume of the container

K is the average kinetic energy of the molecules in the gas

We see that as the pressure is higher, the higher the kinetic energy of the particles: this means that the molecules will move faster, on average.

Therefore in this problem, the gas that exerts a pressure of 1.5 atm will have molecules moving faster than the molecules of the gas exerting a pressure of only 1.0 atm.

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.