Real vs Ideal Gas: Pressure & Temperature Effects

[s.p.q.r]

If a sample of air had high pressure and high temperature, would it be a real or ideal gas?

 

[mgb_phys]

If it's air it is a real gas.
Generally at higher pressures gases become less 'real' as the molecules are closer together they interact - which ideal gases don't do.
In other words at low pressures the ideal gas laws are a better approximation.

Similairly at high temperatures the gas is moving around more so most of it's energy is kinetic rather than in any chemical properties of the molecules so it behaves more like an ideal gas.

 

[sir-pinski]

A gas can be classified as either a real or an ideal gas based on its behavior under certain conditions. In an ideal gas, the particles are assumed to have no volume and there are no intermolecular forces between them. This means that the gas follows the ideal gas law, which states that the pressure, volume, and temperature of a gas are directly proportional to each other.

On the other hand, a real gas deviates from the ideal gas behavior due to the presence of intermolecular forces and the finite volume of its particles. This results in a slight deviation from the ideal gas law, especially at high pressures and low temperatures.

In the given scenario, if a sample of air has high pressure and high temperature, it would exhibit characteristics of both a real and an ideal gas. At high pressure, the particles of the gas are closer together, resulting in stronger intermolecular forces and a deviation from ideal gas behavior. Similarly, at high temperatures, the particles have more kinetic energy and can overcome intermolecular forces, making the gas behave more like an ideal gas.

Therefore, it can be said that the sample of air would exhibit characteristics of both a real and an ideal gas at high pressure and high temperature. However, the extent of deviation from ideal gas behavior would depend on the exact values of pressure and temperature, as well as the composition of the gas.