In general, a reaction with a LARGE K, K > 103, is said to favor the products and thus forms more products than reactants SMALL K, K < 10-3, favors reactants and thus very. The equilibrium constant, K, reflects the ratio of the activities of the products versus the reactants, and represents the extent to which a reaction goes to completion.While it was designed for an honors-level Multiple choice, free-response, and calculation questions are included. This summative assessment covers all aspects of a traditional honors-level Chemistry unit on Equilibrium, including equilibrium constant expressions, Le Chatelier's Principle, and Ksp. It turns out, however, that the equilibrium constant expression has the same form even if the reaction is not elementary.

K sp = m * n The equilibrium constant (K C) expression (equation 9) that was derived in this section was based on the assumption that the equilibrium reaction was an elementary reaction. For ionic compounds with limited solubility in water, an equilibrium constant, K sp, can be defined from the ion concentration in water from the equation: M m A n (s) = mM n+ (aq) + nA m-(aq) where M m A n is the slightly soluble substance and M n+ and A m-are the ions produced in solution by dissosiation of M m A n. p” (pressure equilibrium constant) or simply “K”.

c” (concentration equilibrium constant) and “K. ) – a value which relates the concentration of products with the concentration of reactants in a chemical reaction (units depend on the reaction and are usually not used) Also known as “K.

Calculating k value