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MindMap Gallery Chemical equilibrium states and chemical equilibrium shifts

Chemical equilibrium states and chemical equilibrium shifts

This is a mind map about chemical equilibrium states and chemical equilibrium movements. It introduces the factors that affect chemical equilibrium, Le Chatelier's principle, the establishment of chemical reaction equilibrium, Methods to determine the state of chemical equilibrium, etc.

Edited at 2024-02-10 22:29:15

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Chemical equilibrium states and chemical equilibrium shifts

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Chemical equilibrium states and chemical equilibrium shifts

chemical equilibrium state

Reversible reaction

Under the same conditions, there are both positive reactions and you reactions

Reactants and products exist simultaneously

The conversion rate of any component is less than "1"

Establishment of chemical reaction equilibrium

Markers "Forward reaction rate and reverse reaction"

Chemical equilibrium is a positive balance

Conditions change, the chemical equilibrium state may be changed, and a new equilibrium state is established by new conditions

How to determine the state of chemical equilibrium

most important sign

The rate of forward reaction is equal to the rate of reverse reaction

Judgment of different substances

Pay attention to judge the direction of reaction

The direction of the forward reaction is the production of products and the consumption of reactants

The reverse reaction direction is the consumption of products and the generation of reactants

Calculated from the ratio of stoichiometric numbers, the forward and reverse reaction rates of the same substance are equal

Static substance judgment

amount of matter

Percent content

amount of substance

Note that if the reactants of the reaction are liquid/solid and the product is gas, the reaction will start in the forward direction.

The percentage of gas is a fixed value

The reaction balance cannot be judged if the amount and fraction of the substance remain unchanged.

quantity concentration of substance

pressure

In a constant volume sealed container

For reactions in which the gas does not change before and after the reaction

Pressure is a fixed value, not a variable

If the pressure remains unchanged, it is impossible to determine whether it is balanced or not.

Response to increase or decrease in gas

Pressure is a variable

If the pressure remains unchanged, the reaction can be judged to have reached equilibrium.

Note that this pressure is also the partial pressure of the gas

density

The formula for calculating density is mass to volume

In a constant volume sealed container

The volume is a fixed value

For a reaction in which all reactants and products are gases, the mass of the gas is constant

It cannot be judged whether the reaction is balanced if the density remains unchanged.

For reactions that produce solids or liquids in the reactants and products, the mass of the gas will change

Density can be used as a marker to determine the equilibrium of a chemical reaction

In a constant pressure closed container

Volume is not a fixed value Therefore, many situations need to be considered

If the reactants and products are all gases, the mass of the object remains unchanged

For isovolumetric reactions, the pressure is constant and the volume remains constant.

Density is a fixed value and cannot be used as a symbol to judge balance.

For reactions involving gas changes, the pressure is constant and the volume changes

Density is a variable

The constant density can be used as a sign of whether the reaction is balanced.

If there is solid in the reactants or products, the mass change of the gas

If the reaction is isovolumetric, the volume remains constant and the mass of the gas is constant.

Density is the amount of change

Constant density can be used as a sign of equilibrium reaction

average molar mass of gas

The average molar mass of a gas is related to the amount of gas substance and the mass of the gas

In a closed container with constant volume, the volume is a constant value

If the reaction is an isovolumetric reaction involving all gases, the average molar mass of the gas does not change

The average molar mass of a gas is a fixed value and cannot be used as a symbol to judge equilibrium.

If the reaction is an all-gas reaction, there will be a gas change

The mass of the gas remains unchanged, but the amount of matter changes

The average molar mass of a gas is a variable

The average molar mass of the gas remains unchanged and can be used as a marker to determine whether the reaction is balanced.

If the reaction is an isovolumetric reaction involving solid and liquid

The volume of the gas remains unchanged, the amount of substance remains unchanged, and the mass changes

The change in the average molar mass of a gas can be used as a marker to determine whether the reaction is balanced.

color

The color is the same as the percentage content

shifts in chemical equilibrium

Factors affecting chemical equilibrium

temperature

For an exothermic reaction, as the temperature increases, the reaction proceeds in the reverse direction; as the temperature decreases, the reaction proceeds in the forward direction.

For endothermic reactions, as the temperature increases, the reaction proceeds in the forward direction; as the temperature decreases, the reaction proceeds in the reverse direction.

pressure

For a constant volume reaction, the pressure changes but the equilibrium does not move.

For a reaction in which gas increases, when the pressure increases, the reaction proceeds in the reverse direction; when the pressure decreases, the reaction proceeds in the forward direction.

For a reaction in which the gas decreases, the pressure increases and the reaction proceeds in the forward direction; the pressure decreases and the reaction proceeds in the reverse direction.

Note: This pressure should be the partial pressure of the reaction/generated gases rather than the total pressure.

Note: For inert gases, if they are in a constant-volume sealed container, they have no effect on the balance; if they are in a constant-pressure sealed container, they are considered to reduce the pressure.

concentration

For reactants, as the concentration of the reactant increases, the reaction proceeds forward

For products, as the product concentration increases, the reaction proceeds in reverse

Note: In an ion reaction, the increase in concentration must be the ions actually participating in the reaction. If they do not participate in the actual reaction, there will be no impact on the balance.

catalyst

Catalysts can change the forward and reverse reaction rates equally, but cannot change the equilibrium state.

Le Chatelier's Principle

Changing the conditions that affect chemical movement causes the equilibrium to shift in a direction that weakens this effect

For increasing reactants, increasing the reactant concentration can make the reaction proceed in the forward direction and consume the reactants, but the corresponding reactant concentration in the second equilibrium is greater than the concentration in the first reaction equilibrium.