At which conditions do real gases behave most like ideal gases?

At which conditions do real gases behave most like ideal gases?

Step 1: Understand what an ideal gas is. An ideal gas is a theoretical gas that perfectly follows the gas laws without any exceptions.
Step 2: Know that real gases are different from ideal gases because they have intermolecular forces and occupy space.
Step 3: Learn that real gases behave more like ideal gases under certain conditions.
Step 4: Identify the conditions: low pressure means that gas particles are far apart, reducing the effect of intermolecular forces.
Step 5: Recognize that high temperature gives gas particles more energy, which also reduces the impact of intermolecular forces.
Step 6: Conclude that at low pressure and high temperature, real gases behave most like ideal gases.

Ideal Gas Behavior – Real gases approximate ideal gas behavior under conditions of low pressure and high temperature, where the effects of intermolecular forces and molecular volume are negligible.
Intermolecular Forces – At high temperatures, kinetic energy overcomes intermolecular attractions, allowing gases to behave more ideally.
Pressure Effects – At low pressures, gas molecules are far apart, reducing the impact of volume and intermolecular forces.