what are the main drawbacks of the van der waals equation of state for real gases and how are they corrected?
The Van Der Waals equation of state is a thermodynamic equation that describes the behavior of real gases, taking into account their size and intermolecular forces. It predicts the relationship between pressure, volume, and temperature for a gas at a given state.
The Van Der Waals equation of state does not accurately describe the behavior of gases at high pressures or low temperatures, as it does not take into account the non-ideal behavior of real gases. It also assumes that the gas molecules have no volume and do not interact with each other, which is not the case in reality.
The Van Der Waals equation of state can be corrected by introducing correction factors to account for the size of the gas molecules and the attractive forces between them. These corrections can be made by incorporating the compressibility factor and the reduced temperature and pressure into the equation.
The compressibility factor, also known as the Z-factor, is a correction factor that takes into account the deviation of gases from ideal behavior. It is defined as the ratio of the actual volume of a gas to the volume predicted by the ideal gas law. As the compressibility factor deviates from 1, the Van Der Waals equation of state becomes less accurate.
Several other equations of state have been developed to improve upon the Van Der Waals equation, such as the Redlich-Kwong equation, the Peng-Robinson equation, and the Soave-Redlich-Kwong equation. These equations incorporate additional parameters to better account for the non-ideal behavior of real gases.