After the reversible reaction is equilibrized, how to move the balance when the pressure increases?

When the reversible reaction reaches equilibrium, there are three types of pressure points: pressure decreases, pressure increases, and pressure does not change.

When other conditions are constant, increase the pressure, and the effect is different for each type.

The pressure decreases when the reversible reaction reaches equilibrium: the pressure is increased, the equilibrium moves in the positive direction, and the positive reaction is promoted;

When the pressure increases when the reversible reaction reaches equilibrium: increase the pressure, move the equilibrium in reverse, and inhibit the positive reaction;

When the pressure of the reversible reaction reaches equilibrium, the pressure does not change: the pressure is increased and decreased, and the equilibrium does not move, and the chemical reaction is not affected.

There are only a few ways to reduce the pressure:

1.Volume does not change: Lowering the temperature or reducing the amount of gas (i.e., the number of molecules per unit volume you mentioned) will do the trick.

2.The temperature does not change: either by reducing the amount of gas or by increasing the volume.

3.The amount of gas remains the same: increasing the volume or lowering the temperature can be achieved.

If the other two conditions remain the same, changing the remaining conditions can achieve the same goal.

Increase the pressure and move in the direction of volume reduction. They will eventually reach dynamic equilibrium.

There are many ways to reduce pressure, and reducing the number of molecules per unit volume is the essence of reducing pressure.

Increasing the volume is one of the methods, but as for reducing the pressure, reducing the volume depends on the temperature......

At the same temperature, the volume decreases, and the pressure seems to increase.

Specific reactions, specific treatments.

For example, if the reaction: m(g)+n(g)=p(g)+q(g) is the above reaction, and the sum of the coefficients of the left and right gaseous substances is the same, then the chemical equilibrium does not move.

For example, in the reaction: m(g)+n(g)=p(g)+q(l) as above, the pressure increases, and the chemical equilibrium moves in the direction of decreasing gas volume, that is, in the positive direction in the above chemical equation.

For example, the reaction: m(g)+n(s)=p(g)+q(g) As above, the pressure increases, and the chemical equilibrium moves in the direction of the decrease in the volume of the gas, that is, in the reverse direction of the chemical equation above.

In general, the positive reaction is to move to the right of the equation.

2so2+o2=2so3

In this reaction, the volume of the reactant gas is greater than the product, and the pressure increases, and the substance must be compressed, which will cause a tendency to decrease in volume, so it must move in the direction of SO3 formation.

For example, if the reaction: m(g)+n(g)=p(g)+q(g) is the above reaction, and the sum of the coefficients of the left and right gaseous substances is the same, then the chemical equilibrium does not move.

For example, in the reaction: m(g)+n(g)=p(g)+q(l) as above, the pressure increases, and the chemical equilibrium moves in the direction of decreasing gas volume, that is, in the positive direction in the above chemical equation.

For example, the reaction: m(g)+n(s)=p(g)+q(g) As above, the pressure increases, and the chemical equilibrium moves in the direction of the decrease in the volume of the gas, that is, in the reverse direction of the chemical equation above.

The relationship between pressure and reversible reaction equilibrium is only for the presence of gases involved in the reaction. If it is a liquid or a solid, the reaction is quiet, and the change and influence of pressure are not considered!

For a gas to participate in a reversible reaction of the balance slag, for example:

A+2B=2C+D (assuming that A, B, and C are all gases) If it is a container with a constant volume, and there are only A and B in it, when the reaction is carried out to equilibrium, since only C is a gas in the product, the amount of gas in the product is small, and the pressure will be smaller.

When the reversible reaction reaches equilibrium ():

a.The positive and negative reactions stopped.

b.The mass fraction of reactants and products no longer varies due to changes in temperature and pressure.

c.The mass fraction of reactants and products is the same.

d.The mass fraction of reaction carry-ons and products no longer changes over time.

Correct answer: d

1.If the positive reaction is a reaction with an increase in volume, the increased pressure equilibrium moves in the direction of the reverse reaction, and the decreasing pressure equilibrium moves in the direction of the positive reaction.

For example, N2O4<=>2NO2, the increase pressure equilibrium moves to the opposite reaction direction, and N2O4 increases. The balance of the reduced pressure moves in the direction of positive reaction, and the NO2 increases.

2.If the positive reaction is a reaction with a decrease in volume, the increasing pressure equilibrium moves in the direction of the positive reaction, and the decreasing pressure equilibrium moves in the direction of the reverse reaction.

For example, N2+3H2<=>2NH3, the increased pressure equilibrium moves to the direction of positive reaction, and NH3 increases. The decreasing pressure equilibrium shifted to the opposite reaction direction, and N2 and H2 increased.

To sum up, the increasing pressure equilibrium moves in the direction of volume increase, and the decreasing pressure equilibrium moves in the direction of volume decrease. If there is no change in the volume of gas in the equation, the equilibrium does not move.

Look at what the equation is. If the molar volume of the substance before and after the reaction is unchanged, the equilibrium does not move. After the reaction, the molar volume decreases, which shifts in the direction of the positive reaction, and the molar volume becomes larger, which moves in the direction of the reverse reaction.

As the pressure increases, the reaction moves in the direction of an increase in the total amount of gas generated.

Move to the side of the coefficient and the smaller.

What about the chemical formula? There's no chemical equation for what's going on.

Le Châteaure's principle.

If one of the conditions of the pure balance of the Pure Balance of the Flat Wheel is changed, the balance will move in a direction that can weaken the change.

Therefore, increasing the pressure results in chemical equilibrium.

Moves in the direction of the reduction in the volume of the gas.

At constant temperature and volume, the reaction a+b=2c+d, and then add a and b. after reaching equilibriumIf you put the added A and B into another container to react, and finally achieve the same equilibrium as the original, and then press it into the original vessel, the equilibrium mixture in the original container needs to occupy less space, which is equivalent to compression, and the equilibrium moves to the left.

In general, just move to a place where there is less stoichiometric time, remember this sentence.

Pressure reacts with reversibility.

The equilibrium relationship is only for the presence of gases involved in the reaction. If it is a reaction between a liquid and a solid, the nucleus does not consider the change and effect of pressure!

For a reversible reaction in which an air cavity excavation is involved, e.g.:

a+2b=2c+d (assuming a, b, c are all gases) If it is a container with a constant volume, there are only A and B in it, and when the reaction is in equilibrium, since only C is a gas in the product, the amount of gas in the product is the amount of substance.

If it is small, then the pressure will be smaller.