At high pressures how does the volume of a real gas compare with the volume of an ideal gas under the same conditions and why

At high pressure, volume of a real gas is lower than volume of an ideal gas under the same condition

Explanation:

At high pressure, total volume of gas molecules are no longer negligible as compared to volume of gas or more precisely volume of gas container.

For ideal gases, gas molecules are assumed to be point masses. That means, ideal gas molecules do not have measurable volumes.

But, in real gases, gas molecules have small but measurable volume.

At low pressure, volume a gas is so high that volume of gas molecules are neglected. Hence real gases behaves ideally at low pressure.

But, at high pressure, actual volume of a gas should be volume of gas container minus volume of gas molecules.

hence volume of a real gas is lower than ideal gas at high pressure

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.