When we think about how temperature and pressure affect gases, it's important to know the difference between ideal and real gases.

Ideal gases are like a perfect situation. In this perfect world, nothing sticks together, and there is no space taken up. However, real gases don't always follow these rules.

Here's a simple breakdown of how temperature and pressure play a role:

1. Temperature:

   • When the temperature goes up, gas particles move around faster.
   • This usually means they spread out more. Because of this, the ideal gas laws seem to work better.
   • But at really high temperatures, real gases start to behave more like ideal gases. This happens because the energy from the movement of particles is stronger than the forces that pull them together.

2. Pressure:

   • When the pressure increases, the gas molecules get pushed closer together.
   • For real gases, this can change how they behave because they have forces attracting them and take up space. This is especially true at high pressures.
   • At low pressures, the space (or volume) that the gas molecules take up becomes less important. This makes it easier for them to follow the ideal gas laws.

In summary, the extreme temperatures and pressures make real gases act differently from our ideal gases. It all comes down to those tricky attractions between particles and the space they use!