Gases can act like ideal gases or real gases depending on different conditions.

Here are two important situations that affect how gases behave:

• High Pressure: When the pressure is really high, gas molecules get close together. This makes them stop acting like ideal gases.

• Low Temperature: At low temperatures, real gases start to stick together. The forces between the particles become strong enough to change their behavior.

To understand real gases better, we can use something called the Van der Waals equation.

It looks like this:

$(P + a(n/V)^2)(V - nb) = nRT$

In this equation:

• $a$ and $b$ help us account for the forces between gas particles and the space they take up.

But be careful! Working with these numbers can be tricky. It takes time to get it right.