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- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Thermodynamics/Energies_and_Potentials/Free_EnergyFree energy is a composite function that balances the influence of energy vs. entropy.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Inorganic_Chemistry_(LibreTexts)/08%3A_Chemistry_of_the_Main_Group_Elements/8.13%3A_The_Halogens/8.13.02%3A_Chemical_Properties_of_the_Halogens/8.13.2.07%3A_The_Acidity_of_the_Hydrogen_HalidesThis page discusses the acidity of the hydrogen halides: hydrogen fluoride, hydrogen chloride, hydrogen bromide and hydrogen iodide. It begins by describing their physical properties and synthesis and...This page discusses the acidity of the hydrogen halides: hydrogen fluoride, hydrogen chloride, hydrogen bromide and hydrogen iodide. It begins by describing their physical properties and synthesis and then explains what happens when they react with water to make acids such as hydrofluoric acid and hydrochloric acid.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/16%3A_Entropy_and_Spontaneous_Reactions/16.15%3A_Maximum_Useful_WorkThe Gibbs free energy has another very useful property. When a spontaneous chemical reaction occurs, the decrease in free energy, corresponds to the maximum possible quantity of useful work which can ...The Gibbs free energy has another very useful property. When a spontaneous chemical reaction occurs, the decrease in free energy, corresponds to the maximum possible quantity of useful work which can be obtained.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Concept_Development_Studies_in_Chemistry_(Hutchinson)/17%3A_Equilibrium_and_the_Second_Law_of_ThermodynamicsWhen a mixture of reactants and products is not at equilibrium, the reaction will occur spontaneously in one direction or the other until the reaction achieves equilibrium. What determines the directi...When a mixture of reactants and products is not at equilibrium, the reaction will occur spontaneously in one direction or the other until the reaction achieves equilibrium. What determines the direction of spontaneity? What is the driving force towards equilibrium? How does the system know that equilibrium has been achieved? Our goal will be to understand the driving forces behind spontaneous processes and the determination of the equilibrium point.
- https://chem.libretexts.org/Courses/DePaul_University/Thermodynamics_and_Introduction_to_Quantum_Mechanics_(Southern)/03%3A_The_Second_and_Third_Laws_of_Thermodynamics/3.09%3A_Putting_the_Second_Law_to_Work/3.9.03%3A_A_G_and_Maximum_WorkThe functions A and G are oftentimes referred to as free energy functions. The reason for this is that they are a measure of the maximum work (in the case of ΔA ) or non p-V work (in the case of ΔG ...The functions A and G are oftentimes referred to as free energy functions. The reason for this is that they are a measure of the maximum work (in the case of ΔA ) or non p-V work (in the case of ΔG ) that is available from a process.
- https://chem.libretexts.org/Courses/Prince_Georges_Community_College/CHEM_2000%3A_Chemistry_for_Engineers_(Sinex)/Unit_6%3A_Thermo_and_Electrochemistry/Chapter_16%3A_Entropy_and_Free_Energy/Chapter_16.4%3A_Spontaneity_and_EquilibriumWe have identified three criteria for whether a given reaction will occur spontaneously: ΔS univ > 0, ΔG sys < 0, and the relative magnitude of the reaction quotient Q versus the equilibrium constant ...We have identified three criteria for whether a given reaction will occur spontaneously: ΔS univ > 0, ΔG sys < 0, and the relative magnitude of the reaction quotient Q versus the equilibrium constant K. (For more information on the reaction quotient and the equilibrium constant, see Chapter 15.) Recall that if Q < K, then the reaction proceeds spontaneously to the right as written, resulting in the net conversion of reactants to products.
- https://chem.libretexts.org/Courses/Lebanon_Valley_College/CHM_312%3A_Physical_Chemistry_II_(Lebanon_Valley_College)/04%3A_State_Functions_in_Thermodynamics/4.02%3A_A_G_and_Maximum_WorkThe functions A and G are oftentimes referred to as free energy functions. The reason for this is that they are a measure of the maximum work (in the case of ΔA ) or non p-V work (in the case of ΔG ...The functions A and G are oftentimes referred to as free energy functions. The reason for this is that they are a measure of the maximum work (in the case of ΔA ) or non p-V work (in the case of ΔG ) that is available from a process.
- https://chem.libretexts.org/Courses/University_of_Georgia/CHEM_3212%3A_Physical_Chemistry_II/08%3A_Gibbs_and_Helmholtz_Energies/8.03%3A_%CE%94A%2C_%CE%94G%2C_and_Maximum_WorkThe functions A and G are oftentimes referred to as free energy functions. The reason for this is that they are a measure of the maximum work (in the case of ΔA ) or non p-V work (in the case of ΔG ...The functions A and G are oftentimes referred to as free energy functions. The reason for this is that they are a measure of the maximum work (in the case of ΔA ) or non p-V work (in the case of ΔG ) that is available from a process.
- https://chem.libretexts.org/Courses/University_of_California_Davis/UCD_Chem_002C/UCD_Chem_2C_(Larsen)/Textbook/01%3A_Chemistry_Primer/1.03%3A_Free_Energy_and_Equilibrium_(quick)On the other hand, if free energy decreases over the course of the reaction, we show that by using a negative number for the value of the free energy. An number with a negative exponent, by the rules ...On the other hand, if free energy decreases over the course of the reaction, we show that by using a negative number for the value of the free energy. An number with a negative exponent, by the rules of exponents, is the same as the inverse of the number with a positive exponent of the same size. That's because the free energy is divided by the temperature and the gas constant; the resulting number becomes the exponent in the relationship.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Descriptive_Chemistry/Elements_Organized_by_Block/2_p-Block_Elements/Group_17%3A_The_Halogens/1Group_17%3A_General_Reactions/The_Acidity_of_the_Hydrogen_HalidesThis page discusses the acidity of the hydrogen halides: hydrogen fluoride, hydrogen chloride, hydrogen bromide and hydrogen iodide. It begins by describing their physical properties and synthesis and...This page discusses the acidity of the hydrogen halides: hydrogen fluoride, hydrogen chloride, hydrogen bromide and hydrogen iodide. It begins by describing their physical properties and synthesis and then explains what happens when they react with water to make acids such as hydrofluoric acid and hydrochloric acid.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/16%3A_Entropy_and_Spontaneous_Reactions/16.14%3A_The_Free_EnergyIf we assume, as we did previously, that neither ΔH m ° nor ΔS m ° varies much as the temperature changes from 298 K to the temperature in question, we can then use the values of ΔH m °(298 K) obtaine...If we assume, as we did previously, that neither ΔH m ° nor ΔS m ° varies much as the temperature changes from 298 K to the temperature in question, we can then use the values of ΔH m °(298 K) obtained from the Table of Some Standard Enthalpies of Formation at 25°C and ΔS m °(298 K) obtained from the Table of Standard Molar Entropies to calculate ΔG m ° for the temperature in question.
