The Kinetic Molecular Theory (KMT) helps us understand how gases work, but it has some important limits. Here’s a simpler breakdown:

1. What KMT Assumes About Gases:

   • Gases are made up of tiny particles that are always moving around randomly.
   • The forces between these particles are very weak and don’t matter much.
   • When these particles bump into each other, the collisions don’t lose energy.

2. How Real Gases Act Differently:

   • Under high pressure and low temperature, real gases don’t follow KMT as expected.
   • Molecules take up space and can attract each other, which goes against what KMT says.

3. Using Equations:

   • The Ideal Gas Law ($PV = nRT$) is a formula used to describe how gases behave. However, it doesn’t give the right answers when conditions aren’t ideal.

4. Better Ways to Understand Real Gases:

   • One solution is to use the Van der Waals equation. This equation makes changes for the forces between molecules and their size, giving us a better picture of how real gases behave.