This value is proportional to an exponential of the negative columbic potential over RT in the Fuoss-Eigen equation. Along with stoichiometry and enthalpy changes, this value can be directly measured in isothermal titration calorimetry, and it is found from the slope of a Scatchard plot. In coordination complexes, the Irving-Williams series arranges metals by this property, which is equivalent to the stability constant. The change in (*) Gibbs free energy is equal to the negative RT times natural log of this value, which is actually a ratio of activities. First outlined by Guldberg and Waage in the law of mass action, this quantity is equal to the ratio to the forwar
This value is proportional to an exponential of the negative columbic potential over RT in the Fuoss-Eigen equation. Along with stoichiometry and enthalpy changes, this value can be directly measured in isothermal titration calorimetry, and it is found from the slope of a Scatchard plot. In coordination complexes, the Irving-Williams series arranges metals by this property, which is equivalent to the stability constant. The change in (*) Gibbs free energy is equal to the negative RT times natural log of this value, which is actually a ratio of activities. First outlined by Guldberg and Waage in the law of mass action, this quantity is equal to the ratio to the forward rate constant to the reverse rate constant. For 10 points, name this value which is a ratio of concentrations of reactants and products, symbolized K.
This value is proportional to an exponential of the negative columbic potential over RT in the Fuoss-Eigen equation.
equilibrium constant [or mass action constant or binding constant or stability constant or Ka or Keq before mention]