a chemical reaction is at equilibrium when
the composition is stationary and has no future tendancy to react
chemical equilibria are dynamic equilibria when
the forward and backward reactions continue but ther is NO net change
-> rates of movement in either direction are equal
Le chateliers principle
when a reaction at equilibrium is subjected to a change of conditions the composition of conditions adjusts so as to minimize the change
an increase of temperature in the case of endothermic reactions, shifts the position of equilibrium in favor of products
products
(and in exothermic reactions in favor of reactans)
a reaction at equilibrium is subjected to a change of concentration
increase of the reactant leads to the product and vice versa
a reaction at equilibrium is subjected to a change of pressure
increase of the total pressure leads to the products and vice versa
a reaction at equilibrium is subjected to a change of temperature
favors the endothermic reaction
the equilibrium is not affected by
the amount of solid state reaction participants
if a reaction involving gases is subjected to an increase in pressure
the reaction adjusts the composition so as to reduce the number of gas phase molecules and therby to minimize the increase in pressure
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