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  2. Van 't Hoff equation - Wikipedia

    en.wikipedia.org/wiki/Van_'t_Hoff_equation

    The Van 't Hoff equation relates the change in the equilibrium constant, K eq, of a chemical reaction to the change in temperature, T, given the standard enthalpy change, Δ r H ⊖, for the process. The subscript r {\displaystyle r} means "reaction" and the superscript ⊖ {\displaystyle \ominus } means "standard".

  3. Determination of equilibrium constants - Wikipedia

    en.wikipedia.org/wiki/Determination_of...

    Equilibrium constants are determined in order to quantify chemical equilibria.When an equilibrium constant K is expressed as a concentration quotient, = [] [] [] [] it is implied that the activity quotient is constant.

  4. Job plot - Wikipedia

    en.wikipedia.org/wiki/Job_plot

    Within chemistry, a Job plot, otherwise known as the method of continuous variation or Job's method, is a method used in analytical chemistry to determine the stoichiometry of a binding event. The method is named after Paul Job and is also used in instrumental analysis and advanced chemical equilibrium texts and research articles.

  5. Equilibrium constant - Wikipedia

    en.wikipedia.org/wiki/Equilibrium_constant

    The decrease in zero-point energy due to deuterium substitution will then be more important for R'–H than for R–H, and R'–D will be stabilized more than R–D, so that the equilibrium constant K D for R' + D–R ⇌ R'–D + R is greater than K H. This is summarized in the rule the heavier atom favors the stronger bond. [19]

  6. Henderson–Hasselbalch equation - Wikipedia

    en.wikipedia.org/wiki/Henderson–Hasselbalch...

    In chemistry and biochemistry, the Henderson–Hasselbalch equation = + ⁡ ([] []) relates the pH of a chemical solution of a weak acid to the numerical value of the acid dissociation constant, K a, of acid and the ratio of the concentrations, [] [] of the acid and its conjugate base in an equilibrium.

  7. Reaction quotient - Wikipedia

    en.wikipedia.org/wiki/Reaction_quotient

    Equilibrium condition: At equilibrium, the reaction quotient (Q) is equal to the equilibrium constant (K) for the reaction. This condition is represented as Q = K, indicating that the forward and reverse reaction rates are equal. Predicting reaction direction: If Q < K, the reaction will proceed in the forward direction to establish equilibrium ...

  8. Free-energy relationship - Wikipedia

    en.wikipedia.org/wiki/Free-energy_relationship

    The lowercase letters (e, s, a, b, l) are system constants describing the contribution of the aerosol phase to the sorption process. [5] The capital letters (E, S, A, B, L) are solute descriptors representing the complementary properties of the compounds. Specifically, L is the gas–liquid partition constant on n-hexadecane at 298 K;

  9. Partition equilibrium - Wikipedia

    en.wikipedia.org/wiki/Partition_equilibrium

    K c = [NH 3 (CHCl3)]/[NH 3 (aq)] (where K c is the equilibrium constant) The equilibrium concentrations of ammonia in each layer can be established by titration with standard acid solution. It can thus be determined that K c remains constant, with a value of 0.4 in this case.