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requal
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Just wondering, for van der waals equation, the real pressure is smaller than the ideal pressure and the real volume is smaller than the ideal volume?
requal said:Okay I found out that the real volume is indeed less than the ideal volume, but I don't get how the real volume is bigger than the ideal volume?
The Van der Waals gas equation is an equation that describes the behavior of real gases, taking into account the volume and attractive forces between gas molecules. It is an improvement upon the ideal gas law, which assumes that gas molecules have no volume and do not interact with each other.
The Van der Waals gas equation was developed by Dutch physicist Johannes Diderik van der Waals in 1873. He received the Nobel Prize in Physics in 1910 for his work on the equation and his other contributions to the study of gases.
The variables in the Van der Waals gas equation are pressure (P), volume (V), temperature (T), and the parameters a and b, which account for the attractive forces between gas molecules and the volume occupied by the gas molecules, respectively.
The ideal gas law assumes that gas molecules have no volume and do not interact with each other, whereas the Van der Waals gas equation takes into account the volume and attractive forces between gas molecules. This makes it more accurate for describing the behavior of real gases, especially at high pressures and low temperatures.
The Van der Waals gas equation is significant because it provides a more accurate description of the behavior of real gases, taking into account their volume and attractive forces. It is also a foundational equation in the study of thermodynamics and has applications in various fields such as chemistry, physics, and engineering.