Contents.Overview It is used to show how the point of of a system will move to oppose a change in the conditions of the system, following. This is most commonly seen in reversible reactions in chemistry, where a chemical reaction has reached a point where the formation of products happens at the same rate the products decay back into reactants.
This principle can then be used to increase the amount of desired products made by moving equilibrium towards that side in chemical industries.Concentration If the of reactants in a reaction increases, the point of equilibrium moves towards the products as this gets rid of the excess reactants and cancels the change.
Temperature: Temperature may be added to a system either externally or as a result of the chemical reaction. If a chemical reaction is exothermic (Δ H is negative or heat is released), heat is considered a product of the reaction. If the reaction is endothermic (Δ H is positive or heat is absorbed), heat is considered a reactant. So, increasing or decreasing temperature can be considered the same as increasing or decreasing the concentration of reactants or products. In the temperature is increased, the heat of the system increases, causing the equilibrium to shift to the left (reactants). If the temperature is decreased, the equilibrium shifts to the right (products). In other words, the system compensates for the reduction in temperature by favoring the reaction that generates heat.
To understand more about this subject, review the following lesson called Le Chatelier's Principle: Disruption and Re-Establishment of Equilibrium. The lesson features the following topics: Change. Le Chatelier's Principle. We learned in the previous lesson that Le Chatelier’s principle predicts that when a change is imposed upon a system at equilibrium, the equilibrium shifts in the direction that will counter the change. This principle is predicted nicely by the collision theory of reaction rates.
![Le chatelier Le chatelier](/uploads/1/2/5/6/125633785/524863413.jpg)
![Le Chatelier Le Chatelier](/uploads/1/2/5/6/125633785/163366089.jpg)
Pressure/Volume: Pressure and volume can change if one or more of the participants in a chemical reaction is a gas. Changing the partial pressure or volume of a gas acts the same as changing its concentration. If the volume of gas increases, pressure decreases (and vice versa). If the pressure or volume increase, the reaction shifts toward the side with lower pressure.
If the pressure is increased or volume decreases, equilibrium shifts toward the higher pressure side of the equation. Note, however, that adding an inert gas (e.g., argon or neon) increases the overall pressure of the system, yet does not change the partial pressure of the reactants or products, so no equilibrium shift occurs.