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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 /), also called Chatelier's principle, Braun–Le Chatelier principle, Le Chatelier–Braun principle or the equilibrium law, [1] is a principle used to predict the effect of a change in conditions on chemical equilibrium.
Common-ion effect. In chemistry, the common-ion effect refers to the decrease in solubility of an ionic precipitate by the addition to the solution of a soluble compound with an ion in common with the precipitate. [1] This behaviour is a consequence of Le Chatelier's principle for the equilibrium reaction of the ionic association / dissociation.
By Le Chatelier's principle, the release of CO 2 from the lungs pushes the reaction above to the left, causing carbonic anhydrase to form CO 2 until all excess protons are removed. Bicarbonate concentration is also further regulated by renal compensation , the process by which the kidneys regulate the concentration of bicarbonate ions by ...
Henry Louis Le Chatelier[ 1 ] (French pronunciation: [ɑ̃ʁi lwi lə ʃɑtəlje]; 8 October 1850 – 17 September 1936) was a French chemist of the late 19th and early 20th centuries. He devised Le Chatelier's principle, used by chemists and chemical engineers to predict the effect a changing condition has on a system in chemical equilibrium.
Le Châtelier's principle (1884) predicts the behavior of an equilibrium system when changes to its reaction conditions occur. If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to partially reverse the change. For example, adding more S (to the chemical reaction above) from the outside will ...
Following Le Chatelier's principle, the chemical equilibrium of the Earth's carbon cycle will shift in response to anthropogenic CO 2 emissions. The primary driver of this is the ocean, which absorbs anthropogenic CO 2 via the so-called solubility pump.
According to Le Chatelier's principle, higher pressure favours ammonia. High pressure is necessary to ensure sufficient surface coverage of the catalyst with nitrogen. [ 54 ] For this reason, a ratio of nitrogen to hydrogen of 1 to 3, a pressure of 250 to 350 bar, a temperature of 450 to 550 °C and α iron are optimal.
In accordance with Le Chatelier's Principle, when the dissolution process is endothermic (heat is absorbed), solubility increases with rising temperature. This effect is the basis for the process of recrystallization , which can be used to purify a chemical compound.