Yes. We can treat diatomic gases as ideal gases also, if the pressure is low enough. The only difference is in their heat capacity.kelvin490 said:We know that one model for ideal gas is monoatomic gas with no attractive force between atoms, elastic collision and some other assumptions. I would like to ask if there exist a gas behave exactly the same but the only difference is it's a diatomic gas (or more complicated structure), should it be regarded as an ideal gas? (Note that the average KE for monoatomic and diatomic gas are different)
Chestermiller said:Yes. We can treat diatomic gases as ideal gases also, if the pressure is low enough. The only difference is in their heat capacity.
Chet
Yes.kelvin490 said:Thanks for the answer. For monoatomic ideal gas the cv is 3R/2 and cp is 5R/2, so γ=5/3 is for monoatomic ideal gas only?
An ideal gas is a theoretical gas that follows the ideal gas law, which states that it has no intermolecular forces, occupies no volume, and experiences no collisions between particles. It is a simplified model used to describe the behavior of real gases.
A diatomic gas is a gas composed of two atoms of the same element, such as oxygen (O2) or nitrogen (N2). These gases are considered to be simple molecules and can behave differently than monatomic gases (composed of single atoms).
Diatomic gases can deviate from ideal gas behavior due to their intermolecular forces, which can cause them to occupy a non-zero volume and experience collisions between particles. This can lead to deviations from the ideal gas law.
Diatomic gases can be considered ideal under certain conditions, such as at high temperatures and low pressures, where the effect of intermolecular forces is minimal. At these conditions, the gas particles behave similarly to an ideal gas and can be described by the ideal gas law.
If diatomic gas is regarded as an ideal gas, it can simplify calculations and make them more accurate as it follows a well-defined model. However, it may not accurately reflect the behavior of real gases under certain conditions, so it is important to consider the limitations of the ideal gas model when applying it to diatomic gases.