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  2. Equilibrium chemistry - Wikipedia

    en.wikipedia.org/wiki/Equilibrium_chemistry

    Equilibrium chemistry is concerned with systems in chemical equilibrium.The unifying principle is that the free energy of a system at equilibrium is the minimum possible, so that the slope of the free energy with respect to the reaction coordinate is zero.

  3. Gibbs–Helmholtz equation - Wikipedia

    en.wikipedia.org/wiki/Gibbs–Helmholtz_equation

    The definition of the Gibbs function is = + where H is the enthalpy defined by: = +. Taking differentials of each definition to find dH and dG, then using the fundamental thermodynamic relation (always true for reversible or irreversible processes): = where S is the entropy, V is volume, (minus sign due to reversibility, in which dU = 0: work other than pressure-volume may be done and is equal ...

  4. Thermodynamic equations - Wikipedia

    en.wikipedia.org/wiki/Thermodynamic_equations

    The equilibrium state of a thermodynamic system is described by specifying its "state". The state of a thermodynamic system is specified by a number of extensive quantities , the most familiar of which are volume , internal energy , and the amount of each constituent particle ( particle numbers ).

  5. Thermodynamic equilibrium - Wikipedia

    en.wikipedia.org/wiki/Thermodynamic_equilibrium

    Classical thermodynamics deals with states of dynamic equilibrium.The state of a system at thermodynamic equilibrium is the one for which some thermodynamic potential is minimized (in the absence of an applied voltage), [2] or for which the entropy (S) is maximized, for specified conditions.

  6. List of types of equilibrium - Wikipedia

    en.wikipedia.org/wiki/List_of_types_of_equilibrium

    Partial equilibrium, the equilibrium price and quantity which come from the cross of supply and demand in a competitive market; Radner equilibrium, an economic concept defined by economist Roy Radner in the context of general equilibrium; Recursive competitive equilibrium, an economic equilibrium concept associated with a dynamic program

  7. Van 't Hoff equation - Wikipedia

    en.wikipedia.org/wiki/Van_'t_Hoff_equation

    [11] Assume two products B and C form in a reaction: a A + d D → b B, a A + d D → c C. In this case, K eq can be defined as ratio of B to C rather than the equilibrium constant. When ⁠ B / C ⁠ > 1, B is the favored product, and the data on the Van 't Hoff plot will be in the positive region.

  8. Thermodynamic versus kinetic reaction control - Wikipedia

    en.wikipedia.org/wiki/Thermodynamic_versus...

    [11] [12] This time scale becomes shorter as the temperature is raised. In every reaction, the first product formed is that which is most easily formed. Thus, every reaction a priori starts under kinetic control. [13] A necessary condition for thermodynamic control is reversibility or a mechanism permitting the equilibration between products.

  9. First law of thermodynamics - Wikipedia

    en.wikipedia.org/wiki/First_law_of_thermodynamics

    The first law of thermodynamics is a formulation of the law of conservation of energy in the context of thermodynamic processes.The law distinguishes two principal forms of energy transfer, heat and thermodynamic work, that modify a thermodynamic system containing a constant amount of matter.