The chemical equilibrium constant is an indication of the degree of reaction, why is it only affecte

First of all, your understanding of the equilibrium constant is a bit one-sided, and the concentration quotient (i.e., the formula for calculating the equilibrium constant) when a reversible reaction reaches equilibrium at a certain temperature (usually the standard air pressure) is called the equilibrium constant of a reversible reaction But when you reach a new equilibrium, the value of the carboxylic acid in the equilibrium constant expression remains the same, and you notice that even though you change every value, the concentration quotient doesn't change, which is theoretically and practically proven.

The landlord does not understand the concept of equilibrium constants very clearly. The so-called degree of reaction refers to the relationship between the concentrations of reactants when chemical equilibrium is reached in a given chemical reaction system. The equilibrium constant is only a relational quantity, and the specific concentration can only be derived from other bars.

The equilibrium shift does not necessarily represent a change in the degree of reaction, when the pressure or concentration changes, the equilibrium shift means that the reactants still have to move in the direction of reaching the relationship expressed by the equilibrium constant, or the equilibrium constant does not change.

The equilibrium constant is the ratio of the concentration of the product to the concentration of the reactant (and how many powers) it does not necessarily change when the equilibrium moves k, because both the reactant and the product concentration change.

Please define it, balance the movement, and the length will not change.

Concentration equilibrium constant and pressure equilibrium constant. Due to the increase in total pressure. When equilibrium is reached again, the partial pressure of both reactants and products used to calculate the equilibrium constant increases, so this does not mean that k necessarily increases.

The equilibrium constant is only related to temperature, which is the result obtained by chemical thermodynamics δg=-rtlnk Gibbs free energy δg at a certain temperature is constant, therefore, the equilibrium constant k is only related to temperature.

When writing balance constant expressions, pay attention to the following questions:

When applying the equilibrium constant expression, the concentration of water molecules in a dilute solution can be omitted. Because the density of the dilute solution is close to 1 g ml. The amount concentration of the substance of water is mol l.

In the process of chemical change, the change of water quantity has little effect on the change of water concentration, so the concentration of water is a constant, which can be incorporated into the equilibrium constant.

For reactions in a solution that does not use water as a solvent, the concentration of the solvent is likewise constant.

When there are solid substances involved in the reaction, the intermolecular collision can only be carried out on the surface of the solid, and the amount and concentration of the solid substance has no effect on the reaction rate and equilibrium, therefore, the "concentration" of the solid is taken as a constant, and the concentration of the solid is not written in the equilibrium constant expression.

The expression of the chemical equilibrium constant is related to the way the chemical equation is written. For the same chemical reaction, due to the different ways of writing, the stoichiometric numbers of each reactant and product are different, and the equilibrium constant is different. But these equilibrium constants can be converted to each other.

Different chemical equilibrium systems have different equilibrium constants. A large equilibrium constant indicates that the equilibrium concentration of the product is larger, and the equilibrium concentration of the reactant is relatively small, indicating that the reaction is carried out more completely. Thus, the magnitude of the equilibrium constant can indicate how well the reaction is carried out.

The k>10 5 reaction is considered to be more complete (i.e., irreversible) and the k<10 (-5) reaction is difficult to proceed (i.e., no reaction).

The magnitude of the equilibrium constant can be used to determine how well the reaction is proceeding.

In secondary school, it is generally believed that the chemical equilibrium constant is only related to temperature, and that the equilibrium constant of endothermic reactions increases with increasing temperature, while the opposite is true for exothermic reactions. Strictly speaking, however, the equilibrium constant of a chemical reaction is a function of temperature and pressure, and the situation varies for different chemical equilibrium constants.

In gas-phase reactions, all standard equilibrium constants are simply a function of temperature. If the gas is ideal, then its empirical equilibrium constant is also only a function of temperature. But for non-ideal gases, the equilibrium constant is affected by a combination of temperature and pressure.

Theoretically, any reaction involving a condensed phase (solid or liquid) is a function of temperature and pressure. However, in the case that the pressure variation range is not large, the influence of pressure on the volume change of the condensed phase can be ignored, that is, the influence of pressure on the equilibrium constant can be ignored.

In fact, it is because when you measure the concentration of each state of matter, the concentration is only related to temperature (+ pressure).

It has been proved by thermodynamics that there is a certain relationship between it and the standard molar Gibbs free fiber attack energy change under constant temperature and pressure.

If it is an exothermic reaction, the enthalpy becomes less than zero, the temperature increases, the equilibrium shifts to the left, and the equilibrium constant decreases.

In the case of an endothermic reaction, the enthalpy becomes greater than zero, the temperature increases, the equilibrium shifts to the right, and the equilibrium constant increases.

RGM is a molar Gibbs free energy change in any state, which has been thermodynamically proved to have a certain relationship with the standard molar Gibbs free energy change at constant temperature and pressure. For gas reactions:

ma(g)＋nb(g)--pc(g)＋qd(g)

drgm＝drgm°＋rtln[(pc/p°)p(pd/p°)q/(pa/p°)m(pb/p°)n]

where PC, PD, PA, and PB are the partial pressures of each substance in any (non-equilibrium) state. When the chemical reaction reaches equilibrium:

drgm drgm° rtln[(pc p°)p(pd p°)q (pa p°)m(pb p°)n] balance 0

drgm° -rtln[(pc p°)p(pd p°)q (pa p°)m(pb p°)n] balance -rtlnk°

For reactions carried out in solution, drgm° -rtlnk°

This equation expresses the equilibrium constant as a relation to the standard molar Gibbs free energy variable. Thus, as long as the DRGM° at temperature t is known, the equilibrium constant of the reaction at temperature t can be obtained.

It can also be seen from this equation that at a certain temperature, for a reversible reaction, if the drgm° is more negative, the greater the k° value, and the more complete the positive reaction will be. Conversely, the more positive the drgm°, the smaller the k° value, and the less or practically impossible the positive reaction will be. [drgm° -rtlnk°] - This equation is the relationship between the standard molar Gibbs free energy variation, temperature, and equilibrium constant.

The specific relationship between the chemical equilibrium constant and temperature is shown in Huiyanxia:

1. The magnitude of the chemical equilibrium constant value indicates the degree of the reaction and the limit of the reaction when the equilibrium is reached at this temperature, the larger the chemical equilibrium constant value, the greater the degree of the reaction, and the smaller the vice versa;

2. The chemical eggplant equilibrium constant is only affected by temperature, which has nothing to do with the change of concentration of any reactant or product, and has nothing to do with the change of pressure;

3. If the positive reaction is an endothermic reaction, the constant value of chemical equilibrium increases or decreases due to the fact that the equilibrium moves in the direction of the forward or reverse reaction when the temperature is increased or decreased;

4. If the positive reaction is an exothermic reaction, the constant value of chemical equilibrium decreases or increases due to the increase or decrease of temperature, the equilibrium moves in the direction of the reverse or negative positive reaction.

The specific relationship between the chemical equilibrium constant and temperature is as follows:

1. The magnitude of the chemical equilibrium constant value indicates the degree of the reaction and the limit of the reaction when the equilibrium is reached at this temperature, the larger the chemical equilibrium constant value, the greater the degree of the reaction, and the smaller the vice versa;

2. The chemical equilibrium constant is only affected by temperature, and has nothing to do with the change of the concentration of any kind of reaction posture foci or products, nor is it related to the change of pressure traces.

3. If the positive reaction is an endothermic reaction, the constant value of chemical equilibrium increases or decreases due to the fact that the equilibrium moves in the direction of the forward or reverse reaction when the temperature is increased or decreased;

4. If the positive reaction is an exothermic wax deficiency reaction, the constant value of chemical equilibrium decreases or increases due to the increase or decrease of temperature, the equilibrium moves in the direction of reverse or positive reaction.