state and explain le chateliers principle with reference to (a) change in temperature (b) change in concentration
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Le Chatelier's principle (UK: /lə ʃæˈtɛljeɪ/, US: /ˈʃɑːtəljeɪ/), also called Chatelier's principle or "The Equilibrium Law", can be used to predict the effect of a change in conditions on some chemical equilibria. The principle is named after Henry Louis Le Chatelier and sometimes Karl Ferdinand Braun who discovered it independently. It can be stated as:
When any system at equilibrium for a long period of time is subjected to change in concentration, temperature, volume, or pressure, (1) the system changes to a new equilibrium and (2) this change partly counteracts the applied change.
It is common to treat the principle as a more general observation,[1] such as
When a settled system is disturbed, it will adjust to diminish the change that has been made to it,
or, "roughly stated",[1]
Any change in status quo prompts an opposing reaction in the responding system.
The principle has a variety of names, depending upon the discipline using it (see homeostasis(maintenance of steady state), a term commonly used in biology).
In chemistry, the principle is used to manipulate the outcomes of reversible reactions, often to increase the yield of reactions. In pharmacology, the binding of ligands to the receptor may shift the equilibrium according to Le Chatelier's principle, thereby explaining the diverse phenomena of receptor activation and desensitization.[2] In economics, the principle has been generalized to help explain the price equilibrium of efficient economic systems.
Phenomena in apparent contradiction to Le Chatelier's principle can arise in systems of simultaneous equilibrium: see the article on the theory of response reactions.
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