Lakhasly

Chemical equilibrium can be shifted by changing the conditions that the system

experiences.Decreasing the temperature is equivalent to decreasing a reactant (for endothermic reactions) or a product (for exothermic reactions), and the equilibrium shifts accordingly.For example, if the temperature is increased for an endothermic reaction, essentially a reactant is being added, so the equilibrium shifts toward products.Le Chatelier's principle:

If an equilibrium is stressed, then the reaction shifts to reduce the stress.

Chemical equilibrium can be shifted by changing the conditions that the system

experiences. When we stress the equilibrium, the chemical reaction is no longer at

equilibrium, and the reaction starts to move back toward equilibrium in such a way

as to decrease the stress.

Le Chatelier's principle:

If an equilibrium is stressed, then the reaction shifts to reduce the stress.

There are several ways to stress an equilibrium. One way is to add or remove a

product or a reactant in a chemical reaction at equilibrium. When additional reactant

is added, the equilibrium shifts to reduce this stress: it makes more product. When

additional product is added, the equilibrium shifts to reactants to reduce the stress.

If reactant or product is removed, the equilibrium shifts to make more reactant or

product, respectively, to make up for the loss.

When reactants or products are added or removed, the value of the Ke does not

change. The chemical reaction simply shifts, in a predictable fashion, to reestablish

concentrations so that the keq expression reverts to the only one possible value in

given conditions.

Pressure changes do not markedly affect the solid or liquid phases. However, pressure strongly impacts the gas phase. Le Chatelier's principle implies that a pressure increase shifts an equilibrium to the side of the reaction with the fewer number of moles of gas, while a pressure decrease shifts an equilibrium to the side of the reaction with the greater number of moles of gas. If the number of moles of gas is the same on both sides of the reaction, pressure has no effect.

Because temperature is a measure of the energy of the system, increasing temperature can be thought of as adding energy. The reaction will react as if a reactant or a product is being added and will act accordingly by shifting to the other side. For example, if the temperature is increased for an endothermic reaction, essentially a reactant is being added, so the equilibrium shifts toward products. Decreasing the temperature is equivalent to decreasing a reactant (for endothermic reactions) or a product (for exothermic reactions), and the equilibrium shifts accordingly.