Kinetic-Molecular Theory

Question 1

According to Kinetic-Molecular Theory (KMT), are there attractive forces between gas particles?

Answer 1

No

Question 2

According to KMT, how are gas particles moving?

Answer 2

In random, constant motion

Question 3

According to KMT, how does the size of gas particles compare to the size of the space between them?

Answer 3

The gas particles are much smaller than the space between them

Question 4

According to KMT, how is the average kinetic energy of gas particles related to gas temperature?

Answer 4

Average kinetic energy is directly proportional to temperature

Question 5

Are gas particle collisions elastic or inelastic? What does this mean?

Answer 5

They are elastic, meaning that the total kinetic energy of the particles is constant

Question 6

What is the name for a gas obeying the assumptions of KMT?

Answer 6

An ideal gas

Question 7

According to KMT, how does gas pressure arise?

Answer 7

From gas particles colliding with the container wall

Question 8

How does KMT explain Charles’ Law?

Answer 8

As temperature rises, volume increases to spread gas collisions over a greater area to keep pressure constant

Question 9

How does KMT explain Avogadro’s Law?

Answer 9

More moles causes more particles to collide with their container. Volume increases to keep pressure constant

Question 10

Is the kinetic energy of gas particles directly or inversely related to their speed?

Answer 10

Directly related to speed

Question 11

Is the kinetic energy of gas particles directly or inversely related to their mass?

Answer 11

Inversely related to mass
Greater particle mass at constant speed = lower energy