Calculate real gas properties accounting for molecular interactions and finite molecular volume.
The Van der Waals equation modifies the ideal gas law to account for molecular interactions and the finite volume of gas molecules, providing more accurate predictions for real gases.
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Standard conditions for carbon dioxide gas with its characteristic Van der Waals constants.
Pressure: 1.0 atm
Volume: 22.4 L
Temperature: 273.15 K
Moles: 1.0 mol
Van der Waals a: 3.59 L²·atm/mol²
Van der Waals b: 0.0427 L/mol
Nitrogen gas under standard temperature and pressure conditions.
Pressure: 1.0 atm
Volume: 22.4 L
Temperature: 273.15 K
Moles: 1.0 mol
Van der Waals a: 1.39 L²·atm/mol²
Van der Waals b: 0.0391 L/mol
Water vapor at elevated temperature showing significant deviation from ideal behavior.
Pressure: 2.0 atm
Volume: 15.0 L
Temperature: 373.15 K
Moles: 1.0 mol
Van der Waals a: 5.46 L²·atm/mol²
Van der Waals b: 0.0305 L/mol
Helium gas showing minimal deviation from ideal gas behavior due to weak intermolecular forces.
Pressure: 1.0 atm
Volume: 22.4 L
Temperature: 273.15 K
Moles: 1.0 mol
Van der Waals a: 0.034 L²·atm/mol²
Van der Waals b: 0.0237 L/mol