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- https://chem.libretexts.org/Courses/University_of_Florida/CHM2047%3A_One-Semester_General_Chemistry_(Kleiman)/09%3A_Gases/9.08%3A_Real_Gases_-_Deviations_from_Ideal_BehaviorNo real gas exhibits ideal gas behavior, although many real gases approximate it over a range of conditions. Gases most closely approximate ideal gas behavior at high temperatures and low pressures. D...No real gas exhibits ideal gas behavior, although many real gases approximate it over a range of conditions. Gases most closely approximate ideal gas behavior at high temperatures and low pressures. Deviations from ideal gas law behavior can be described by the van der Waals equation, which includes empirical constants to correct for the actual volume of the gaseous molecules and quantify the reduction in pressure due to intermolecular attractive forces.
- https://chem.libretexts.org/Courses/Bellarmine_University/BU%3A_Chem_104_(Christianson)/Phase_1%3A_The_Phases_of_Matter/1%3A_Gases/1.7%3A_Real_GasesNo real gas exhibits ideal gas behavior, although many real gases approximate it over a range of conditions. Gases most closely approximate ideal gas behavior at high temperatures and low pressures. D...No real gas exhibits ideal gas behavior, although many real gases approximate it over a range of conditions. Gases most closely approximate ideal gas behavior at high temperatures and low pressures. Deviations from ideal gas law behavior can be described by the van der Waals equation, which includes empirical constants to correct for the actual volume of the gaseous molecules and quantify the reduction in pressure due to intermolecular attractive forces.
- https://chem.libretexts.org/Courses/CSU_San_Bernardino/CHEM_2100%3A_General_Chemistry_I_(Mink)/09%3A_Gases/9.07%3A_Non-Ideal_Gas_BehaviorGas molecules possess a finite volume and experience forces of attraction for one another. Consequently, gas behavior is not necessarily described well by the ideal gas law. Under conditions of low pr...Gas molecules possess a finite volume and experience forces of attraction for one another. Consequently, gas behavior is not necessarily described well by the ideal gas law. Under conditions of low pressure and high temperature, these factors are negligible, the ideal gas equation is an accurate description of gas behavior, and the gas is said to exhibit ideal behavior. The van der Waals equation is a modified version of the ideal gas law that can be used to account for the non-ideal behavior.
- https://chem.libretexts.org/Courses/Widener_University/CHEM_176%3A_General_Chemistry_II_(Fischer-Drowos)/07%3A_Gases/7.07%3A_Non-Ideal_Gas_BehaviorGas molecules possess a finite volume and experience forces of attraction for one another. Consequently, gas behavior is not necessarily described well by the ideal gas law. Under conditions of low pr...Gas molecules possess a finite volume and experience forces of attraction for one another. Consequently, gas behavior is not necessarily described well by the ideal gas law. Under conditions of low pressure and high temperature, these factors are negligible, the ideal gas equation is an accurate description of gas behavior, and the gas is said to exhibit ideal behavior. The van der Waals equation is a modified version of the ideal gas law that can be used to account for the non-ideal behavior.
- https://chem.libretexts.org/Courses/Grinnell_College/CHM_363%3A_Physical_Chemistry_1_(Grinnell_College)/04%3A_Gases/4.03%3A_van_der_Waals_and_Redlich-Kwong_Equations_of_StateThe van der Waals Equation of State is an equation relating the density of gases and liquids to the pressure, volume, and temperature conditions. The Redlich–Kwong equation of state is an empirical, a...The van der Waals Equation of State is an equation relating the density of gases and liquids to the pressure, volume, and temperature conditions. The Redlich–Kwong equation of state is an empirical, algebraic equation that relates temperature, pressure, and volume of gases. It is generally more accurate than the van der Waals equation and the ideal gas equation at temperatures above the critical temperature.
- https://chem.libretexts.org/Courses/Thompson_Rivers_University/TRU%3A_Fundamentals_and_Principles_of_Chemistry_(CHEM_1510_and_CHEM_1520)/02%3A_Gases/2.07%3A_Non-Ideal_Gas_BehaviorGas molecules possess a finite volume and experience forces of attraction for one another. Consequently, gas behavior is not necessarily described well by the ideal gas law. Under conditions of low pr...Gas molecules possess a finite volume and experience forces of attraction for one another. Consequently, gas behavior is not necessarily described well by the ideal gas law. Under conditions of low pressure and high temperature, these factors are negligible, the ideal gas equation is an accurate description of gas behavior, and the gas is said to exhibit ideal behavior. The van der Waals equation is a modified version of the ideal gas law that can be used to account for the non-ideal behavior.
- https://chem.libretexts.org/Courses/University_of_Kentucky/UK%3A_General_Chemistry/09%3A_Gases/9.6%3A_Non-Ideal_Gas_BehaviorGas molecules possess a finite volume and experience forces of attraction for one another. Consequently, gas behavior is not necessarily described well by the ideal gas law. Under conditions of low pr...Gas molecules possess a finite volume and experience forces of attraction for one another. Consequently, gas behavior is not necessarily described well by the ideal gas law. Under conditions of low pressure and high temperature, these factors are negligible, the ideal gas equation is an accurate description of gas behavior, and the gas is said to exhibit ideal behavior. The van der Waals equation is a modified version of the ideal gas law that can be used to account for the non-ideal behavior.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Advanced_Statistical_Mechanics_(Tuckerman)/07%3A_Distribution_Functions_and_Liquid_Structure/7.07%3A_Derivation_of_the_Van_der_Waals_equationAs a specific example of the application of perturbation theory, we consider the Van der Waals equation of state.
- https://chem.libretexts.org/Courses/New_York_University/CHEM-UA_652%3A_Thermodynamics_and_Kinetics/01%3A_Lectures/1.05%3A_The_van_der_Waals_equation_of_state_and_radial_distribution_functionschosen so that the area above the line (between the line and the isotherm) and below the line (again between the line and the isotherm) is exactly the same. If we draw a curve through the isotherms jo...chosen so that the area above the line (between the line and the isotherm) and below the line (again between the line and the isotherm) is exactly the same. If we draw a curve through the isotherms joining all points of these isotherms at which the tie lines begin, continue the curve up to the critical isotherm, and down the other side where the tie lines end, this curve reaches a maximum at the critical point.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Chemical_Thermodynamics_(Supplement_to_Shepherd_et_al.)/03%3A_Extension_1.2_-_Microscopic_Gas_Models/3.01%3A_Van_der_Waals'_EquationWe often assume that gas molecules do not interact with one another, but simple arguments show that this can be only approximately true. Real gas molecules must interact with one another. At short dis...We often assume that gas molecules do not interact with one another, but simple arguments show that this can be only approximately true. Real gas molecules must interact with one another. At short distances they repel one another. At somewhat longer distances, they attract one another. Van der Waals’ equation fits pressure-volume-temperature data for a real gas better than the ideal gas equation does. The improved fit is obtained by introducing two experimentally determined parameters.
- https://chem.libretexts.org/Courses/DePaul_University/Thermodynamics_and_Introduction_to_Quantum_Mechanics_(Southern)/10%3A_Appendix-_Mathematics_for_Physical_Chemistry/10.03%3A_Calculus_in_More_than_One_Variable/10.3.05%3A_Real_GasesWe have already mentioned some thermodynamic variables, but in order to make more connections between chemistry and math we need to introduce some concepts that we need to start discussing real gases.
