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About 14 results
  • 10.5: Some Special Types of Equilibria
    https://chem.libretexts.org/Courses/Mount_Aloysius_College/CHEM_100%3A_General_Chemistry_(O'Connor)/10%3A_Chemical_Equilibrium/10.05%3A_Some_Special_Types_of_Equilibria
    The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematic...The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematical relationship between K a and K b : The crystals precipitate in the wine or grow on the insides of the wine bottle and, if the bottle is stored on its side, on the bottom of the cork.
  • 9: Chemical Equilibria
    https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/09%3A_Chemical_Equilibria
    As was discussed in Chapter 6, the natural tendency of chemical systems is to seek a state of minimum Gibbs function. Once the minimum is achieved, movement in any chemical direction will not be spont...As was discussed in Chapter 6, the natural tendency of chemical systems is to seek a state of minimum Gibbs function. Once the minimum is achieved, movement in any chemical direction will not be spontaneous. It is at this point that the system achieves a state of equilibrium.
  • 13.6: Some Special Types of Equilibria
    https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Beginning_Chemistry_(Ball)/13%3A_Chemical_Equilibrium/13.06%3A_Some_Special_Types_of_Equilibria
    The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematic...The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematical relationship between K a and K b : The crystals precipitate in the wine or grow on the insides of the wine bottle and, if the bottle is stored on its side, on the bottom of the cork.
  • 11.6: Some Special Types of Equilibria
    https://chem.libretexts.org/Courses/SUNY_Adirondack/CHM_103%3A_Principles_of_Chemistry/11%3A_Chemical_Equilibrium/11.6%3A_Some_Special_Types_of_Equilibria
    In one sense, all chemical equilibria are treated the same. However, there are several classes of reactions that are noteworthy because of either the identities of the reactants and products or the fo...In one sense, all chemical equilibria are treated the same. However, there are several classes of reactions that are noteworthy because of either the identities of the reactants and products or the form of the K expression.
  • 9: Chemical Equilibria
    https://chem.libretexts.org/Courses/Millersville_University/CHEM_341-_Physical_Chemistry_I/09%3A_Chemical_Equilibria
    As was discussed in Chapter 6, the natural tendency of chemical systems is to seek a state of minimum Gibbs function. Once the minimum is achieved, movement in any chemical direction will not be spont...As was discussed in Chapter 6, the natural tendency of chemical systems is to seek a state of minimum Gibbs function. Once the minimum is achieved, movement in any chemical direction will not be spontaneous. It is at this point that the system achieves a state of equilibrium.
  • 13.5: Some Special Types of Equilibria
    https://chem.libretexts.org/Courses/Fresno_City_College/Introductory_Chemistry_Atoms_First_for_FCC/13%3A_Chemical_Equilibrium/13.5%3A_Some_Special_Types_of_Equilibria
    HC 2 H 3 O 2 is soluble in H 2 O (in fact, it is the acid in vinegar), so the reactant concentration will appear in the equilibrium constant expression. This is the same K w that was introduced in Cha...HC 2 H 3 O 2 is soluble in H 2 O (in fact, it is the acid in vinegar), so the reactant concentration will appear in the equilibrium constant expression. This is the same K w that was introduced in Chapter 12 and the same 1.0 × 10 −14 that appears in the relationship between the K a and the K b of a conjugate acid-base pair. The crystals precipitate in the wine or grow on the insides of the wine bottle and, if the bottle is stored on its side, on the bottom of the cork.
  • 13.5: Some Special Types of Equilibria
    https://chem.libretexts.org/Courses/Nassau_Community_College/Principles_of_Chemistry/13%3A_Chemical_Equilibrium/13.05%3A_Some_Special_Types_of_Equilibria
    The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematic...The conjugate acid of C 2 H 3 O 2 − is HC 2 H 3 O 2 . The K a for HC 2 H 3 O 2 is in Table \(\PageIndex{1}\) "Acid Dissociation Constants for Some Weak Acids" and is 1.8 × 10 −5 . Using the mathematical relationship between K a and K b : The crystals precipitate in the wine or grow on the insides of the wine bottle and, if the bottle is stored on its side, on the bottom of the cork.
  • Complex-Ion Equilibria
    https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Coordination_Chemistry/Complex_Ion_Equilibria/Complex-Ion_Equilibria
    In general, chemical equilibrium is reached when the forward reaction rate is equal to the reverse reaction rate and can be described using an equilibrium constant, K. Complex ion equilibria are no ex...In general, chemical equilibrium is reached when the forward reaction rate is equal to the reverse reaction rate and can be described using an equilibrium constant, K. Complex ion equilibria are no exception to this and have their own unique equilibrium constant. This formation constant, Kf , describes the formation of a complex ion from its central ion and attached ligands. This constant may be caled a stability constant or association constant.
  • 35.8: Standard Reduction Potentials & Polarographic Half-wave Potentials
    https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Instrumental_Analysis_(LibreTexts)/35%3A_Appendicies/35.08%3A_Standard_and_Formal_Electrode_Potentials
    \(\text{BaO}(s) + 2\text{H}^+ + 2e^- \rightleftharpoons \text{Ba}(s) + \text{H}_2\text{O}(l)\) \(\text{H}_2\text{O}(l) + e^- \rightleftharpoons \frac{1}{2} \text{H}_2(g) + \text{OH}^-\) \(\text{HgO}(s...\(\text{BaO}(s) + 2\text{H}^+ + 2e^- \rightleftharpoons \text{Ba}(s) + \text{H}_2\text{O}(l)\) \(\text{H}_2\text{O}(l) + e^- \rightleftharpoons \frac{1}{2} \text{H}_2(g) + \text{OH}^-\) \(\text{HgO}(s) + 2\text{H}^+ + 2e^- \rightleftharpoons \text{Hg}(l) + \text{H}_2\text{O}(l)\) \(\text{N}_2\text{O}(g) + 2\text{H}^+ + 2e^- \rightleftharpoons \text{N}_2(g) + \text{H}_2\text{O}(l)\) \(\text{SeO}_4^{3-} + 4\text{H}^+ + e^- \rightleftharpoons \text{H}_2\text{SeO}_3 + \text{H}_2\text{O}(l)\)
  • 16.13: Standard Reduction Potentials
    https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/16%3A_Appendix/16.13%3A_Standard_Reduction_Potentials
    This page provides standard electrode potentials (Eo) and formal potentials (Eo ??) for various reduction reactions involving different elements, as sourced from multiple references. Each entry includ...This page provides standard electrode potentials (Eo) and formal potentials (Eo ??) for various reduction reactions involving different elements, as sourced from multiple references. Each entry includes the specific reduction reaction and its corresponding potential values measured in volts. The information highlights discrepancies between sources for certain reactions, affecting the precision of potential calculations.
  • 1.17: Chemical Equilibria
    https://chem.libretexts.org/Courses/New_York_University/CHEM-UA_652%3A_Thermodynamics_and_Kinetics/01%3A_Lectures/1.17%3A_Chemical_Equilibria
    \[\begin{align} \Delta_\text{r} G &= \Delta_\text{r} G^\text{o} + RT \left[ d \: \text{ln} \left( \dfrac{P_\text{D}}{P^\text{o}} \right) + c \: \text{ln} \left( \dfrac{P_\text{C}}{P^\text{o}} \right) ...\[\begin{align} \Delta_\text{r} G &= \Delta_\text{r} G^\text{o} + RT \left[ d \: \text{ln} \left( \dfrac{P_\text{D}}{P^\text{o}} \right) + c \: \text{ln} \left( \dfrac{P_\text{C}}{P^\text{o}} \right) - a \: \text{ln} \left( \dfrac{P_\text{A}}{P^\text{o}} \right) - b \: \text{ln} \left( \dfrac{P_\text{B}}{P^\text{o}} \right) \right] \\ &= \Delta_\text{r} G^\text{o} + RT \left[ \text{ln} \left( \dfrac{P_\text{D}}{P^\text{o}} \right)^d + \: \text{ln} \left( \dfrac{P_\text{C}}{P^\text{o}} \right)^c…

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