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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.
The relation between the Gibbs free energy and the equilibrium constant can be found by considering chemical potentials. [ 1 ] At constant temperature and pressure in the absence of an applied voltage, the Gibbs free energy , G , for the reaction depends only on the extent of reaction : ξ (Greek letter xi ), and can only decrease according to ...
The equilibrium state is represented by the equation: + + If α is the fraction of dissociated electrolyte, then αc 0 is the concentration of each ionic species. (1 - α) must, therefore be the fraction of undissociated electrolyte, and (1 - α)c 0 the concentration of same. The dissociation constant may therefore be given as
In chemistry, Le Chatelier's principle (pronounced UK: / l ə ʃ æ ˈ t ɛ l j eɪ / or US: / ˈ ʃ ɑː t əl j eɪ /) [1] is a principle used to predict the effect of a change in conditions on chemical equilibrium. [2] Other names include Chatelier's principle, Braun–Le Chatelier principle, Le Chatelier–Braun principle or the equilibrium ...
If possible, a species will move from areas with higher electrochemical potential to areas with lower electrochemical potential; in equilibrium, the electrochemical potential will be constant everywhere for each species (it may have a different value for different species).
In chemistry, the lever rule is a formula used to determine the mole fraction (x i) or the mass fraction (w i) of each phase of a binary equilibrium phase diagram.It can be used to determine the fraction of liquid and solid phases for a given binary composition and temperature that is between the liquidus and solidus line.
An ICE table or RICE box or RICE chart is a tabular system of keeping track of changing concentrations in an equilibrium reaction. ICE stands for initial, change, equilibrium . It is used in chemistry to keep track of the changes in amount of substance of the reactants and also organize a set of conditions that one wants to solve with. [ 1 ]
The equilibrium in water solution may be shifted towards either compound. For example, the equilibrium constant for the conversion of acetone (H 3 C) 2 C =O to propane-2,2-diol (H 3 C) 2 C(OH) 2 is about 10 −3, [1] while that of formaldehyde H 2 C =O to methanediol H 2 C(OH) 2 is 10 3. [2] For conversion of hexafluoroacetone (F 3 C) 2 C =O to ...