The chemical equilibrium moves, what is the shift of the chemical equilibrium

Le Chatelier's Principle's principle), also known as the equilibrium movement principle, is a qualitative ** chemical equilibrium point principle, the content of which is:

Chemical equilibrium is a dynamic equilibrium in which if one of the factors affecting the equilibrium is changed, the equilibrium moves in a direction that can attenuate the change to counteract the change.

Le Chatle's principle (also known as the principle of equilibrium movement) is a qualitative principle of chemical equilibrium points,[1] the main contents are:

In a reaction where equilibrium has been reached, if one of the conditions that affect the equilibrium is changed (such as temperature, pressure, and the concentration of chemicals participating in the reaction), the equilibrium will move in a direction that can attenuate the change.

For example, in a reversible reaction, when the concentration of reactants is increased, the equilibrium will move in the direction of the positive reaction, and the balance will gradually decrease the concentration of the increased reactants. However, this weakening is not possible to eliminate the effect of increasing the concentration of reactants on the reactants themselves, and increases them compared to those in the old equilibrium system.

In reversible reactions with the participation or generation of gases, the equilibrium always shifts in the direction of volume reduction when the pressure is increased, e.g. at n2+3h2

In the reversible reaction of 2NH3, after reaching an equilibrium, the system is pressurized, for example, the pressure is increased to twice the original, then the old equilibrium is broken, and the equilibrium moves in the direction of volume reduction, that is, in the direction of the positive reaction in this reaction, when a new equilibrium is established, the increased pressure is weakened, and it is no longer twice the original equilibrium, but this increased pressure cannot be completely eliminated, nor is it the same as the original equilibrium, but in between.

The application of Le Chatelier's principle can make the conversion rate of some industrial production processes reach or close to the theoretical value, and at the same time, it can also avoid some ineffective solutions (such as blast furnace carbonization schemes), which are very widely used.

You can divide the details.

Let's start by looking at the reaction.

2no2(g)=n2o4(g)

The positive direction of the reaction is the direction in which the number of molecules decreases.

After reaching equilibrium, 1Increase the amount of reactant NO2, and the balance is shifted to the right, to reach a new equilibrium, and the conversion rate will increase.

2.If the amount of NO2 is increased under constant temperature and constant capacitance, the pressure will inevitably increase, and the equilibrium will definitely move to the right in the direction of the decrease in the number of gas molecules, and the conversion rate will increase.

Chemical equilibrium shift refers to the change of reaction conditions (such as temperature, pressure, and the amount and concentration of the chemical substances participating in the reaction) after a reversible reaction has reached equilibrium under certain conditionsThe original equilibrium is disrupted, and the percentage of each component in the equilibrium mixture is changed, so that a new equilibrium is reached under new conditions, which is called a chemical equilibrium shift.

When other conditions remain unchanged, the concentration of reactants is increased or decreased, and the equilibrium shifts to the direction of positive reaction. Decrease the concentration of reactants or increase the concentration of products, and the equilibrium moves in the direction of the reverse reaction.

Effect of pressure on chemical equilibrium.

Pressure has two meanings: partial pressure and total pressure. Therefore, the influence of pressure on chemical equilibrium should be divided into two aspects: the influence of component gas partial pressure on chemical equilibrium and the influence of total system pressure on equilibrium.

The effect of the concentration on equilibrium discussed is fully applicable to the effect of partial pressure on equilibrium, because the variant of p=crt can be derived from the ideal gas equation, which shows that the partial pressure is proportional to the concentration, and whether the total pressure has an effect on the equilibrium depends on whether the total number of gas molecules before and after the reaction changes.

Reversible reactions are divided into forward and reverse, if the forward reaction rate is greater than the reverse rate, it is said to be forward movement; And vice versa. When other conditions remain unchanged, the concentration of reactants is increased or decreased, and the equilibrium moves to the direction of positive reaction, that is, to the direction of reactants. Decreasing the concentration of reactants or increasing the concentration of products, the equilibrium moves in the direction of the reverse reaction, that is, in the direction of the generated reactants.

Increase the concentration of reactants or decrease the concentration of the products, and the equilibrium moves in the direction of the products, and increase the concentration of the products or decrease the concentration of the reactants, and the balance moves in the direction of the reactants.

For reversible reactions, the forward reaction and the reverse reaction are carried out at the same time, but the instant mold rate will change due to external conditions.

When v is positive = v inverse, the reaction reaches equilibrium (i.e., dynamic equilibrium).

Then, after the equilibrium is reached, by changing the external conditions (such as temperature, pressure, etc.), the V forward and V inverse will change.

If you make v just as you say yes, it's right in terms of phenomena, but there are some problems with the narrative, the forward and reverse reactions are always going on, but because the equilibrium moves backwards (i.e., to the left), the phenomenon occurs (and only if the equilibrium is balanced before the chloride ions are added).

Equilibrium is a state of dynamic equilibrium.

The reaction between chlorine and water is converted into hydrochloric acid and hypochlorous acid, and some hydrochloric acid and hypochlorous acid are also converted into chlorine and water. Shifting left means that the reaction proceeds to the left. The same goes for shifting right.

The equilibrium will be broken, for example, hydrogenation ions or something.

If you don't understand, you can simply count them and discuss them online.

Equilibrium establishment is reversible and is a dynamic equilibrium, where the reaction moves backwards only to indicate a decrease in the formation of hydrochloric acid and hypochlorous acid.

Left and right actually mean positive and negative.

Like what. A+B is invertible with the symbol C+D

Moving to the left is not an inverse reaction.

This equation represents the forward and reverse reactions at the same time, rather than referring to a single reaction.

Moving to the left, the balance is changed.

Originally, the reaction rate of A+B to C+D is the same as the rate at which C+D produces A+B.

Due to the change of some local land pieces (depending on the situation), the rate of the two is not the same.

Moving to the left, the C+D reaction rate becomes larger, which is greater than the A+B reaction rate.

Move to the right, it's the other way around.

I don't know if I understand this explanation. —w

First of all, you have to understand a concept, all reactions in the chemical equilibrium dust circle are reversible reactions, and reversible reactions are reactions all the time, and the chemical equilibrium movement is to move towards the positive reaction (generally from left to right) or the pie collapse to the reverse reaction. For example, if the balance of chlorine gas reacts with water to form hydrochloric acid and hypochlorous acid, if the equilibrium is to the right, it means that the positive reaction is more intense, and the proportion of hydrochloric acid and hypochlorous acid is larger. But that doesn't mean you don't react to the left, remember that both the left and right are reacting, and moving is just a matter of which reaction is more intense.