under which conditions do real gases most resemble ideal gases

Mostly under "normal" atmospheric pressure and "normal" temperature. That is about 1 atmosphere P and about 25 degrees C. At very low temperatures and very high pressures, gases deviate the most from ideal behavior.

Real gases resemble ideal gases under certain conditions, known as the conditions of low pressure and high temperature. Here are the specific conditions:

1. Low pressure: Real gases behave more like ideal gases at low pressure conditions. When the pressure is relatively low, the gas molecules are far apart from each other, causing the intermolecular forces between them to be relatively weak. As a result, the volume of gas particles becomes relatively insignificant compared to the total volume of the gas, resembling the behavior of ideal gases.

2. High temperature: Real gases also behave more like ideal gases at high temperature conditions. When the temperature is increased, the kinetic energy of gas molecules increases as well. As a result, the gas particles move more rapidly and have higher average velocities, causing the intermolecular forces to have less impact on the overall behavior of the gas. Therefore, at higher temperatures, real gases tend to resemble ideal gases.

It's important to note that as the pressure increases or the temperature decreases, the behavior of real gases diverges from ideal gas behavior due to the increased importance of intermolecular forces and decreased kinetic energy of the gas particles.

Real gases most closely resemble ideal gases under the following conditions:

1. High Temperatures: At high temperatures, the kinetic energy of gas particles increases, causing them to move faster. This increased kinetic energy helps overcome intermolecular forces, making the gas behave more like an ideal gas.
2. Low Pressures: At low pressures, the distance between gas particles increases, and the effect of intermolecular forces diminishes. As a result, the gas particles occupy a larger volume and exhibit less deviation from ideal gas behavior.
3. Large Volumes: When a gas occupies a large volume, the actual volume of the gas particles becomes a smaller fraction of the total volume. This reduces the influence of particle volume on the gas behavior, making it more similar to an ideal gas.
4. Non-Polar Gases: Real gases composed of non-polar molecules, where the electron distribution is symmetrically distributed, tend to exhibit properties closer to ideal gases. This is because non-polar molecules have weaker intermolecular forces compared to polar molecules.
5. Dilute Gases: When the gas is highly diluted, meaning it is present in small concentrations compared to the total volume, the effect of intermolecular forces becomes less significant and the gas behaves more like an ideal gas.

It's important to note that these conditions approximate ideal gas behavior, but real gases may still deviate from ideal behavior to varying degrees, depending on the specific gas and conditions.