Chemical equilibrium question, please answer 50 in detail

1) The time required to reach equilibrium is (less) in container A than in container B, and the conversion rate of SO2 in container A is greater than in container B (larger).

In the case of keeping the pressure constant, the number of moles of gas before and after the reaction is unequal, when the positive reaction occurs, the number of moles of gas decreases, in order to maintain the pressure, the volume will decrease, so the solubility of a will increase, the reaction rate will be accelerated, and it will take less time to reach equilibrium.

2) After the equilibration, if a small amount of the same amount of HE is introduced into the two containers

The chemical equilibrium in the avessel is shifted to the right.

When the same amount of HE is introduced, HE is an inert gas that will not participate in the reaction, but will increase the number of moles of the gas to increase the pressure, in order to keep the pressure unchanged, it can only increase the volume and reduce the solubility. It is equivalent to dilution, so the balance will shift to the right)

b. The chemical equilibrium movement in the vessel does not move (when the inert gas is added, it does not change when the volume is not impressed).

3) After reaching the equilibrium described in (1), if the same amount of original reaction gas is introduced into the two containers, the percentage content of SO3 in container A remains unchanged when the equilibrium is reached. The percentage content of SO3 in the B vessel decreases (when the original reaction gas is introduced in the same amount, the volume of A increases, resulting in no change in the reaction solubility of A, so the equilibrium does not change in peanuts.) bBecause the volume does not change, the solubility increases and the equilibrium shifts to the right, when there is no way to make the transformation to the previous state.

I hope you can give me my answer... If you have any questions, you can ask them.

1) Time A is less than B Conversion rate A is greater than B

2) A to the left B does not move.

3) A does not change, B z increases.

The balance shifted to the left

Because hydrochloric acid will react with ammonia gas to form ammonium salt solids, the concentration of ammonia gas is reduced, and the reaction rate is reduced, so the reverse reaction rate is greater than the positive one, so the equilibrium shifts to the left.

1. What are the conditions for the reaction? 2.The above reaction has reached equilibrium, is there anything left in 02?

Because the addition of 4molSO3 is equivalent to 4mol SO2 and 2molO2, adding these equilibrium does not move, and adding 2mol SOMOL O2 is equivalent to adding another 2mol SOMOL O2 and 1mol O2, adding 1mol more oxygen to the equilibrium system, and the equilibrium will move in the direction of positive reaction.

This is the equivalent equilibrium, and now the reactants are "one-sided", and they are very well analyzed in the analysis.

The answer is ab. Here's the answer:

Because A is constant pressure and B is constant temperature, this reaction is a reaction with decreasing pressure. As the reaction progresses, the pressure of B slowly decreases, and A is constant pressure, which is equivalent to the pressure of A to B (the pressure of A is higher than B), so the degree of reaction of A is relatively large, and the amount fraction of N2 in A is smaller, so N2 in A should be increased or N2 in B decreased.

a The addition of nitrogen is equivalent to increasing the volume of container A, although the total pressure remains unchanged, but the partial pressure of each gas is reduced (that is, nitrogen should also be divided into pressure), and the volume can also be increased according to the principle of Le Chatelier, and the reaction is carried out in the direction of reducing the volume, so the reverse reaction, that is, the amount of N2 in A is increased.

b is also possible, why, as you asked, to increase the concentration of the product, the reaction should proceed in the opposite direction. However, it should be noted that there is only one product in this reaction, and the increase of NH3 is equivalent to the increase of NH3 pressure, so the reaction should be carried out in the direction of decreasing pressure. What you're talking about is only applicable for multi-product reactions (at least 2).

The following example should be easier to understand:

2NO2=N2O4 In a container with constant temperature and capacity, the reaction is a reaction with reduced pressure, so no matter whether the product or product is increased, the reaction is always carried out in the direction of reducing pressure. That is, always think about the direction of the positive reaction, and be careful not to get confused. If you are interested, this knowledge can be expanded, which is also an advantage.

Because the volume is constant, the pressure of the system increases after NH3 is added, and the equilibrium moves to the direction of decreasing the number of molecules.

AB adds NH3, the pressure of the container increases, and the equilibrium moves to the side with the smaller coefficient in the chemical equation.

Increasing the amount of substance in B, the reaction moves in the direction of the positive reaction, because the positive reaction is a reaction with increased pressure, according to the principle of Le Châtea, the system will inhibit the continuation of the reaction, that is, the reaction of the increased gas B will not be as full as the original reaction, the conversion rate of B will decrease, and the conversion rate of A will increase.

So the question will move towards a positive response, but the conversion rate of B will decrease!

Equivalent equilibrium, the pressure increases, and the reaction moves in reverse.

The total pressure increases, and the seemingly balanced shift to the left;Then there is another situation, if you rush into some kind of inert gas that does not react, the total pressure also increases, why does the equilibrium not move to the left?

The effect of increasing or (decreasing) pressure on equilibrium in Le Chattle's principle is only applicable when the total pressure increases due to a decrease in the total volume (or a decrease in the total pressure due to an increase in the total volume).

So, only the amount of matter that increases b is increased, and the equilibrium shifts to the right. (constant capacity condition).

1 example, industrial synthesis of ammonia.

n2 + 3h2 <=2nh3

Add a lot of n2 to balance the positive movement.

The mass of the product, NH3, the amount of the substance must increase.

The conversion rate of reactant H2 must have increased, but the conversion rate of N2 decreased due to the increase of a lot.

Because N2 increases a lot, the whole mass increases, so even if NH3 increases, the mass fraction of NH3 is still downstream.