Chemical equilibria and redox equations GapFill

The equilibrium constant for a reversible reaction, written in terms of the concentrations of the reactants and products, is denoted by the symbol   KcPcQcEc. More specifically, it is the product of the concentrations of the products  plusdivided bytimesminus the product of the concentrations of the reactants, with each species' concentration raised to the power of its stoichiometric coefficient in the chemical equation. The concentration of a given species X is always written in units of mol dm⁻³, and is represented by  (X)[X]{X}<X>. You will only be expected to write expressions for the equilibrium constants of reactions where all the reactants and products are in the same phase, which are described as   heterogeneoushomogeneousanisogeneousisogeneous. The effect of a change in conditions on the position of an equilibrium can be predicted using  Curie'sLe Chatelier'sLaplace'sLavoisier's principle. The only factor that can affect the value of the equilibrium constant itself is   temperaturethe concentration of reagents in solutionpressurethe presence of a catalyst.

Oxidation and reduction reaction processes are often written in the form of  semi-demi-half-part-equations. The extent to which an element is oxidised in a particular substance is quantified by an oxidation number, also commonly known as an oxidation   gradestageclassstate.