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- https://chem.libretexts.org/Courses/Prince_Georges_Community_College/CHEM_1020%3A_General_Chemistry_II_(S.N._Yasapala)/05%3A_Thermochemistry/5.04%3A_Gibbs_Free_Energy/5.4.02%3A_Free_Energy_and_the_Equilibrium_ConstantFor a reversible process (with no external work), the change in free energy can be expressed in terms of volume, pressure, entropy, and temperature. If the products and reactants are in their standard...For a reversible process (with no external work), the change in free energy can be expressed in terms of volume, pressure, entropy, and temperature. If the products and reactants are in their standard states and ΔG° < 0, then K > 1, and products are favored over reactants at equilibrium. If ΔG° > 0, then K < 1, and reactants are favored over products at equilibrium. If ΔG° = 0, then K=1, and neither reactants nor products are favored at equilibrium. We can use the measured equilibrium constant
- https://chem.libretexts.org/Courses/Bellarmine_University/BU%3A_Chem_104_(Christianson)/Phase_2%3A_Understanding_Chemical_Reactions/5%3A_Equilibrium%3A_How_Far_Reactions_Go/5.2%3A_The_Equilibrium_ConstantThe law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of ...The law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of the gases or their partial pressures can be used. The equilibrium constant can be defined in terms of forward and reverse rate constants via the law of mass action.
- https://chem.libretexts.org/Courses/Saint_Marys_College_Notre_Dame_IN/CHEM_122-02_(Under_Construction)/2%3A_Equilibrium/2.1%3A_Chemical_Equilibrium/The_Equilibrium_ConstantThe law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of ...The law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of the gases or their partial pressures can be used. The equilibrium constant can be defined in terms of forward and reverse rate constants via the law of mass action.
- https://chem.libretexts.org/Courses/Lebanon_Valley_College/CHM_312%3A_Physical_Chemistry_II_(Lebanon_Valley_College)/05%3A_Single_Component_Phase_Equilibrium/5.02%3A_Chemical_Potential_and_FugacityLet μ′ be the chemical potential and \fug′ be the fugacity at the pressure p′ of interest; let μ″ be the chemical potential and \fug″ be the fugacity of the same gas at some ...Let μ′ be the chemical potential and \fug′ be the fugacity at the pressure p′ of interest; let μ″ be the chemical potential and \fug″ be the fugacity of the same gas at some low pressure p″ (all at the same temperature).
- https://chem.libretexts.org/Courses/College_of_the_Canyons/CHEM_202%3A_General_Chemistry_II_OER/04%3A_Chemical_Equilibrium/4.03%3A_Gas_Phase_Equilibria_and_Heterogeneous_SystemsThe law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of ...The law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of the gases or their partial pressures can be used. The equilibrium constant can be defined in terms of forward and reverse rate constants via the law of mass action.
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_IIA/04%3A_Chemical_Equilibrium/4.02%3A_The_Equilibrium_ConstantThe law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of ...The law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of the gases or their partial pressures can be used. The equilibrium constant can be defined in terms of forward and reverse rate constants via the law of mass action.
- https://chem.libretexts.org/Courses/Lebanon_Valley_College/CHM_312%3A_Physical_Chemistry_II_(Lebanon_Valley_College)/06%3A_Multiple_Component_Phase_Equilibrium/6.04%3A_Non-ideality_in_Gases_-_FugacityThe relationship for chemical potential was derived assuming ideal gas behavior. But for real gases that deviate widely from ideal behavior, the expression has only limited applicability. In order to ...The relationship for chemical potential was derived assuming ideal gas behavior. But for real gases that deviate widely from ideal behavior, the expression has only limited applicability. In order to use the simple expression on real gases, a “fudge” factor is introduced called fugacity. Fugacity is used instead of pressure.
- https://chem.libretexts.org/Courses/University_of_Kansas/CHEM_130%3A_General_Chemistry_I_(Sharpe_Elles)/16%3A_Chemical_Thermodynamics/16.06%3A_Free_Energy_and_the_Equilibrium_ConstantFor a reversible process (with no external work), the change in free energy can be expressed in terms of volume, pressure, entropy, and temperature. If the products and reactants are in their standard...For a reversible process (with no external work), the change in free energy can be expressed in terms of volume, pressure, entropy, and temperature. If the products and reactants are in their standard states and ΔG° < 0, then K > 1, and products are favored over reactants at equilibrium. If ΔG° > 0, then K < 1, and reactants are favored over products at equilibrium. If ΔG° = 0, then K=1, and neither reactants nor products are favored at equilibrium. We can use the measured equilibrium constant
- https://chem.libretexts.org/Courses/City_College_of_San_Francisco/Chemistry_101A/Topic_G%3A_Chemical_Equilibrium/11%3A_Chemical_Equilibrium/11.2%3A_The_Equilibrium_ConstantThe law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of ...The law of mass action describes a system at equilibrium in terms of the concentrations of the products and the reactants. For a system involving one or more gases, either the molar concentrations of the gases or their partial pressures can be used. The equilibrium constant can be defined in terms of forward and reverse rate constants via the law of mass action.
- https://chem.libretexts.org/Courses/Millersville_University/CHEM_341-_Physical_Chemistry_I/07%3A_Mixtures_and_Solutions/7.05%3A_Non-ideality_in_Gases_-_FugacityThe relationship for chemical potential was derived assuming ideal gas behavior. But for real gases that deviate widely from ideal behavior, the expression has only limited applicability. In order to ...The relationship for chemical potential was derived assuming ideal gas behavior. But for real gases that deviate widely from ideal behavior, the expression has only limited applicability. In order to use the simple expression on real gases, a “fudge” factor is introduced called fugacity. Fugacity is used instead of pressure.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Thermodynamics_and_Chemical_Equilibrium_(Ellgen)/11%3A_The_Third_Law_Absolute_Entropy_and_the_Gibbs_Free_Energy_of_Formation/11.07%3A_The_Fugacity_of_a_GasFor an ideal gas, the Gibbs free energy is a simple function of its pressure. It turns out to be useful to view the integral as a contribution to a “corrected pressure.” The “correction” is an adjustm...For an ideal gas, the Gibbs free energy is a simple function of its pressure. It turns out to be useful to view the integral as a contribution to a “corrected pressure.” The “correction” is an adjustment to the pressure that, in our calculations, makes the real gas behave as an ideal gas. The idea is that we can express the Gibbs free energy as a function of this corrected pressure, which we call the fugacity. Fugacity is therefore a function of pressure.
