Equilibrium Chemical reaction
Two-way reactions continue until equalibrium (the state at which there is balance between reactants and products) is reached. Discovering the equilibrium constant for a reaction is very helpful for understanding that reaction. Knowing the equilibrium constant of a reaction is important because it allows you to calculate how much product will ultimately be formed during a reaction.
Moreover, it also tells you how a particular mixture of chemicals will react. This is because chemical reactions always occur in the direction which will make the ratio of their products to reactants equal to the equilibrium constant.
In chemistry, Le Chatelier's principle, also called Chatelier's principle or "The Equilibrium Law", can be used to predict the effect of a change in conditions on a chemical equilibrium. The principle is named after Henry Louis Le Chatelier and sometimes Karl Ferdinand Braun who discovered it independently. It can be stated as:
If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established.
This principle has a variety of names, depending upon the discipline using it. See, for example, homeostasis. It is common to take Le Chatelier's principle to be a more general observation,[1] roughly stated:
Any change in status quo prompts an opposing reaction in the responding system.
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. In simultaneous equilibrium systems, phenomena that are in apparent
Moreover, it also tells you how a particular mixture of chemicals will react. This is because chemical reactions always occur in the direction which will make the ratio of their products to reactants equal to the equilibrium constant.
In chemistry, Le Chatelier's principle, also called Chatelier's principle or "The Equilibrium Law", can be used to predict the effect of a change in conditions on a chemical equilibrium. The principle is named after Henry Louis Le Chatelier and sometimes Karl Ferdinand Braun who discovered it independently. It can be stated as:
If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established.
This principle has a variety of names, depending upon the discipline using it. See, for example, homeostasis. It is common to take Le Chatelier's principle to be a more general observation,[1] roughly stated:
Any change in status quo prompts an opposing reaction in the responding system.
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. In simultaneous equilibrium systems, phenomena that are in apparent