Key Differences

• Real Gases: These gases don’t always behave the way we expect. They can change because of forces between their molecules and how much space the molecules take up.

• Ideal Gases: These gases follow a rule called the ideal gas law ($PV=nRT$). They behave this way well when pressure is low and temperature is high.

Challenges in Engineering:

• Engineers face problems when trying to predict how gases will act.

• The way real gases behave can change a lot, making it hard to do calculations.

Potential Solution:

• One way to fix this is by using the Van der Waals equation:
  $\left(P + a\frac{n^2}{V^2}\right)(V - nb) = nRT$
  This helps us understand how real gases behave better.