Answer:
High temperatures and low pressures
Step-by-step explanation:
Ideal gas is a hypothetical state of gases that allows for easier calculations with gases.
Ideal Gas Assumptions
There are 5 assumptions that scientists make to apply ideal gas laws.
- Gases are constantly moving in linear motion
- There are no intermolecular forces (IMFs) between gas particles
- The volume of gas particles is negligible
- Particles have perfectly elastic collisions
- Kinetic energy is proportional to temperature.
Note that elastic collisions mean that no energy is lost through the collisions of particles. Additionally, very few gases actually follow these assumptions. However, sometimes the variation from these assumptions is small enough that the effects are negligible.
Most Ideal Behavior
Whilst ideal gases are not real, small gas particles at high temperatures and low pressures act mostly ideal. Gases at high temperatures move very quickly; this allows their motion to be mostly linear and for less energy to be lost in collisions.
Also, at low pressures, gas particles are further apart. The increased distance between the gas particles decreases the effect of IMFs, making gases more ideal. Additionally, the ratio of empty space to gas particles is larger when the volume is larger. This means that the volume of the particles is negligible.
Overall, high temperatures and low pressures help gases behave most ideally.