Under standard temperature and pressure, which would be 100 kPa (1.0 bar) and 273.15 K (0 oC). This is not correct. The answer is at high temperature and low pressure, according to my college prof.
Nitrogen (N2) behaves more ideally at 1 ATM rather than at 500 ATM. At higher pressures, deviations from ideal gas behavior become more significant due to the increased intermolecular interactions and molecular volume effects, causing the gas to behave less ideally.
Oxygen (O2) would be expected to behave more ideally at high pressures compared to methanol (CH3OH). This is because oxygen is a diatomic gas with weak intermolecular forces, making it behave closer to an ideal gas at high pressures. Methanol, on the other hand, is a polar molecule with stronger intermolecular forces, which can cause deviations from ideal behavior.
The ideal gas law describes how gases should ideally behave under certain conditions. It relates the pressure, volume, temperature, and amount of a gas together: PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature.
A real gas behaves most like an ideal gas when it is at low pressure and high temperature.
A real gas behaves most like an ideal gas at high temperatures and low pressures.
Helium
Water vapor will behave most ideally at low pressures and high temperatures. This is because at these conditions, water molecules are far apart and have higher kinetic energy, resulting in less intermolecular interactions.
ideal gasses have two properties 1. a low pressure 2. high temperatures
Nitrogen (N2) behaves more ideally at 1 ATM rather than at 500 ATM. At higher pressures, deviations from ideal gas behavior become more significant due to the increased intermolecular interactions and molecular volume effects, causing the gas to behave less ideally.
Oxygen (O2) would be expected to behave more ideally at high pressures compared to methanol (CH3OH). This is because oxygen is a diatomic gas with weak intermolecular forces, making it behave closer to an ideal gas at high pressures. Methanol, on the other hand, is a polar molecule with stronger intermolecular forces, which can cause deviations from ideal behavior.
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The ideal gas law describes how gases should ideally behave under certain conditions. It relates the pressure, volume, temperature, and amount of a gas together: PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature.
P waves travel through solids, liquids, and gasses.
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Gases behave most ideally at low pressure and high temperatures. At low pressures, the average distance of separation among atoms or molecules is greatest, minimizing interactive forces. At high temperatures, the atoms and molecules are in rapid motion and are able to overcome interactive forces more easily.
[P + a(n/V)2] (V - nb) = nRT As you see this is a correction method for gasses other than ideal. Gasses at high pressure and high/low temperature. The ideal gas equation makes assumptions that are not always applicable to real word conditions as to gasses.