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  2. Chemical equilibrium - Wikipedia

    en.wikipedia.org/wiki/Chemical_equilibrium

    Chemical equilibrium. In a chemical reaction, chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system. [1] This state results when the forward reaction proceeds at the same ...

  3. 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. [1][2] This principle, applied to mixtures at equilibrium provides a definition of an ...

  4. Le Chatelier's principle - Wikipedia

    en.wikipedia.org/wiki/Le_Chatelier's_principle

    Le Chatelier's principle. In chemistry, Le Chatelier's principle (pronounced UK: / lə ʃæˈtɛljeɪ / or US: / ˈʃɑːtəljeɪ /), also called Chatelier's principle, Braun–Le Chatelier principle, Le Chatelier–Braun principle or the equilibrium law, [1] is a principle used to predict the effect of a change in conditions on chemical ...

  5. 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, Keq, of a chemical reaction to the change in temperature, T, given the standard enthalpy change, ΔrH⊖, for the process. The subscript means "reaction" and the superscript means "standard". It was proposed by Dutch chemist Jacobus Henricus van 't Hoff in 1884 in his book ...

  6. Dynamic equilibrium - Wikipedia

    en.wikipedia.org/wiki/Dynamic_equilibrium

    Dynamic equilibrium. In chemistry, a dynamic equilibrium exists once a reversible reaction occurs. Substances transition between the reactants and products at equal rates, meaning there is no net change. Reactants and products are formed at such a rate that the concentration of neither changes. It is a particular example of a system in a steady ...

  7. Equilibrium constant - Wikipedia

    en.wikipedia.org/wiki/Equilibrium_constant

    a thermodynamic equilibrium constant, denoted by , is defined to be the value of the reaction quotient Qt when forward and reverse reactions occur at the same rate. At chemical equilibrium, the chemical composition of the mixture does not change with time, and the Gibbs free energy change for the reaction is zero.

  8. Phase rule - Wikipedia

    en.wikipedia.org/wiki/Phase_rule

    Phase rule. In thermodynamics, the phase rule is a general principle governing "pVT" systems, whose thermodynamic states are completely described by the variables pressure (p), volume (V) and temperature (T), in thermodynamic equilibrium. If F is the number of degrees of freedom, C is the number of components and P is the number of phases, then.

  9. Reversible reaction - Wikipedia

    en.wikipedia.org/wiki/Reversible_reaction

    Reversible reaction. A reversible reaction is a reaction in which the conversion of reactants to products and the conversion of products to reactants occur simultaneously. [1] A and B can react to form C and D or, in the reverse reaction, C and D can react to form A and B. This is distinct from a reversible process in thermodynamics.