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This is actually because this chemical equation is unique to chemical equilibrium. It can be understood in this way: because the reaction of 2 volumes of Hi produces one volume of H2 and one volume of I2, it can be regarded as the volume of the gas before the reaction is 2 volumes, and the volume of the gas after the reaction is also two volumes, so the pressure does not change before and after the reaction.

Therefore, at this time, whether it is an increase in pressure, the equilibrium does not change in any direction, so considering the influence of concentration, filling Hi, it is obvious that the concentration of Hi increases, so the equilibrium moves in the direction of positive reflection.

For reactions where the volume of gas does not change before and after the reaction, the effect of concentration is generally considered.

Changing the concentration of reactants or products must change the chemical equilibrium. Changing the pressure affects the chemical equilibrium by changing the concentration of the substance, so it is not useful for reactants and products that are solid and the volume does not change after the pressure change. So the above reaction changes the pressure and does not work.

Can you tell me how many pages?

This equilibrium reaction does not move under pressure, changing the equilibrium shift of the concentration of a substance, which are two different cases. It is necessary to consider a single factor, and there is no need to consider the superposition of factors, otherwise it will be confusing.

This should be done in a constant-capacity container.

When the reactants are increased, the concentration of the reactants increases, and the reaction moves forward.

There is no effect on the increase in pressure, so you don't need to look at this.

Both aspects should be considered.

I waited from late summer night to autumn dawn. Life is a lifetime, grass and trees are autumn, and the days ahead are not too bitter.

The answer is C analysis: according to the meaning of the question, it should be a question of exactly the same equivalent equilibrium before and after the reaction of constant temperature and closing, constant volume, that is, in order to achieve the percentage content of each component at the equilibrium time and the same as the above equilibrium, the amount of ammonia filled must be equivalent to the amount of 10molN2 and 30molH2 filled, that is, the amount of ammonia substance produced by the complete conversion of 10molN2 and 30molH2 is 20mol, Therefore, the ammonia filled is 20mol wide permeability.

The conversion rate of H2 is 25%, then the hydrogen of the reaction is 30mol 25%=, calculated according to the equation, N2 + 3H2 = 2NH3

3mol 2mol

xx=5mol

That is, the equilibrium is 5mol of ammonia.

Because it is the same equilibrium, when 20mol ammonia is charged, the ammonia is still 5mol when the equilibrium state is reached, the ammonia reacted is 15mol, and the conversion rate of ammonia is 15 20=

So for c

Because it's a closed container, it's constant volume, and because the temperature doesn't change, it's constant temperature.

Constant temperature and constant volume require the same balance.

Assuming that the nitrogen and hydrogen that are starting to rush in are completely converted, then ammonia is twenty moles.

Choose between B and Netoc C.

The crude conversion rate of H2 is 25 percent, so the ammonia produced is 5 moles.

When you fill it with 20 moles of ammonia, because it's the same equilibrium, you're only going to have 5 moles left.

There are 15 moles converted into nitrogen and hydrogen 15 20 = so the answer is c

n2 3h2 ==2nh3 n2 3h2 ==2nh3 start: 10 30 0 0 0 20

Conversions: 5 to 15

Balance 5 5

The above starting grip is the equivalent of the lifting and dismantling balance.

The answer is c

First, the volume. This reaction is a reaction with a decrease in volume, increasing the reactants, and the equilibrium shifts to the right, so the amount of NH3 should be more than the equilibrium, if it does not move, it should be; It is also not possible to react completely, and should be less than 4mol l).

P.S. equilibrium constant k=[nh3]2 (product of the coefficients of the concentrations of all products, there is only one product of this reaction) [n2][h2]3 (product of the coefficients of the concentrations of all reactants).

When 1molN2, 3molH2 reaches equilibrium, assuming that the container volume is 1L, then [NH3]=,[N2]=,[H2]=,K=

If 2molN2,6molH2 reaches equilibrium, assuming [NH3]=xmol l,[n2]=(,[H2]=(,k=x 2 (, then solving the equation can get a specific value, and you can't calculate it, don't say so much, in short, between and 4; Set the body destruction stool product to other values, the calculation result is different, but it is also between and 4, and you can complete the following by yourself.

Second, constant pressure. In this state, the reaction equilibrium does not move, and NH3 is.

It can be understood that if a closed movable baffle is added to the middle of the closed container, then either side of the baffle is exactly the same as in the first case (1moln2, 3molh2), so the essence of this state is the sum of the two first states.

For pure gas reactions, the intuitive conditions that affect the equilibrium of the reaction are: the amount (or concentration) of the substance, the pressure, and the temperature.

1. You did not mention whether the reaction is endothermic or exothermic here, so the temperature factor is not analyzed.

2. Analysis from the amount (or concentration) of the substance: increasing a, b, a and b is to increase the amount of reactants, and the equilibrium will move to the positive direction of the reaction (that is, to the right). Collapse of the survey.

3. From the pressure analysis: no matter whether a, b, a and b are added here, the total amount of substances in the system is increased, and the pressure is increased under the same volume.

For a+b=c, increase the pressure and shift the balance to the right.

For a+b=2c, the pressure is increased and the balance does not move.

For a+b=3c, increase the pressure and shift the balance to the left.

Just see your question added, continue to give you an explanation:

For the case of A+B=2C, the pressure does not affect the equilibrium of the reaction, it can be understood that when A+B is added, this part of the newly added A and B will react to generate a certain amount of C, but the proportional relationship between the newly generated C and the added A+B is the same as the proportional relationship of the original equilibrium, that is, after the new addition of A+B, the system will have a positive reaction rate increase, but this is only a temporary state, not an equilibrium state, after reaching equilibrium, it is still the same as the original equilibrium state.

In fact, if you ask this, it means that you do not fundamentally understand the concept of "equilibrium", there is a blind spot, equilibrium indicates a state, in this state, the reaction rate of the product generated by the reaction of the reactant is equal to the reaction rate of the product re-becoming the reactant, which is a final state, not a temporary state, and does not mean that the reaction occurs in the forward or reverse direction, and the corresponding product or reactant is generated, I don't know if you understand this.

Under the condition that other conditions remain unchanged, increasing the concentration of reactants or decreasing the concentration of products can make the equilibrium move in the direction of the positive reaction, and conversely, move in the direction of the reverse reaction, increase the equilibrium of a + b will move, but when the equilibrium is reached again, the volume fraction of a, b and c of the reaction of a + b = 2c will not change, that is, the equilibrium state will not change, not the equilibrium will not move.

Because the sum of the measurement numbers of A and B is equal to that of the sail circle C, both are 2, so the pressure does not change the equilibrium state, for the reaction with the participation of gas, in the case of other conditions unchanged, increasing the pressure can make the equilibrium move in the direction of volume reduction, on the contrary, move in the direction of volume increase, and this reaction will not change no matter how the difference in the volume of the car rides.

a+b=2c increases the pressure, and the front let the flat bush balance does not move.

a+b=2c increased the reactant a+b, and the balance moved Hui Zhengju.

It must be the wrong answer, I have confidence.

Don't listen to the nonsense from upstairs!

What I really want to ask is, how can a+b=2c increase the pressure and increase the reactant a+b, how can the balance not move.

1. The reaction volume of Lifeng is unchanged before and after, so increasing the pressure has no effect on it.

2. Don't consider pressure and concentration at the same time, you can imagine that AB is charged after the equilibrium is reached outside the system. Hold it all in your hand. Bonus points!

The topic is not complete enough, and it is not rigorous enough, the chemical formula does not have a description of the state of the substance, and the rate of the whole process of the chemical equilibrium reaction is different, the CO generation rate should be added to the word average, and the direction of the reaction start should be explained, otherwise it cannot be done! The following is a correction to the title:

The reaction starts in the positive direction, in a 1L closed container, N2 is 10mol If the equilibrium state is reached in 5 minutes, the average generation rate of CO is how many times the pressure is the original, and the chemical formula is: 3SiO2 (S) + 6C (S) + 2N2 (G) = Si3N4 (S) + 6Co (G).

Solution: The sub-question is about pressure, and the molar mass of the solid can be ignored according to the known conditions of writing:

3sio2（s）+6c（s）+2n2（g）=si3n4（s）+6co（g）

Molar mass 10mol x mol

The rate v starts with the total molar mass of the total gas of the system: 10mol

The average rate of CO * 5min = > total CO reaction is x=9mol

The total amount of N2 reaction is 9mol6(CO coefficient)*2(N2 coefficient)=>3mol

After reaching equilibrium, the total molar mass of the system is: 10mol-3mol (N2 reacted) + 9mol (the amount of CO generated) = 16mol

The anterior-posterior pressure ratio is equal to the molar mass ratio = >16 10 = times.

I don't know if there is a mistake in changing the title!

To put it this way: in a chemical reaction, the chemical reaction is carried out by the effective collision of molecules, and these molecules that can collide in this way are activated molecules. You can understand the kinetic energy of the molecules under the high-speed motion of the molecules.

At a certain temperature, the internal energy (heat energy) of the gas remains unchanged, when the temperature rises, the molecular movement is more intense, the average molecular kinetic energy increases, and the number of hungry molecules exceeds the critical energy score. And because your condition is only the temperature increases, and everything else remains unchanged by default, the total number of molecules is constant.

I hope you understand that. Back to the mold mausoleum.

There is no doubt that the temperature rises, because the temperature is the external embodiment of the energy of the system, and the energy is high, and the intermolecular collision is also violent, and the temperature rises.

And the increase in the energy of the system will increase the number of molecules beyond a certain energy limit, right? Beyond this limit are activated molecules.

As for the total number of molecules, the noisy type is obvious, and it is not said that there is a reaction, so it is natural to keep the spine conserved.

1) Because a and b are on one side of the equation, v(a)=3v(b) is wrong in any case; Because density = mass volume, mass is constant according to the law of conservation, volume is always constant because it is a closed container, volume is constant, so density is always constant, false; Because the consumption A is carried out in the forward direction, and the generation of B is carried out in the reverse direction, and the rate satisfies the coefficient of the equation, it is correct, according to the original definition, the concentration of a substance does not change, and the equilibrium state is proved

2) greater than [the temperature rise is beneficial to the positive reaction, the temperature increases to the direction of the positive reaction, and the positive reaction is an endothermic reaction, so δh=q 0].

3) 2 4 [If the coefficients on both sides of the equation are not equal, then x≠4, then the amount of the original substance of the reactant in the two containers is the same, so 3 3 x+ 3 1 x+ is obtained, and the solution is x=2, and the amount of the substance of a in the two containers A and B is equal; If the coefficients on both sides of the equation are equal, then the ratio of the quantities of the substances to satisfy the original substance is the same, so 6 (,x=4 conforms to the above equation, and the amount of a substance in containers A and B is not equal).

The volume fraction of a in a at equilibrium is 60%.

If the coefficients on both sides of the equation are not equal, then 3a + b ==2c

3x x 2x

6-3x 2-x 2x

2x (6-3x+2-x+2x)= solution x=2 3, and then find the amount of abc at this time, and calculate the mass fraction.

In the same way, when the coefficients on both sides of the equation are equal, i.e., 3a + b ==4c, this method is also used

8:5 [If the pressure is not equal, then it is added according to the original ingredient ratio, then the equation is 3A + B = = = 4C, and the amount of ABC substance in A is6, a total of 8, the amount of matter in B is , a total of 5, because the volume of the two containers is equal, so the ratio of pressure is equal to the ratio of the amount of matter = 8:

5] Hope!! Thank!!

1) Correctly there is 3 mol a consumed and 1 mol b generated; The concentration of C remains the same.

What is wrong is that v(a)=3v(b) does not indicate the direction of the reaction; The density of the mixed gas remains unchanged, and the density of the gas remains unchanged if the reactants are all gases in the constant capacitance device.

2) The higher the temperature, the greater the chemical equilibrium constant of the reaction, indicating that the temperature rise is beneficial to the positive reaction, which is an endothermic reaction, q<0.

3) If the amount of a substance in containers A and B is equal at equilibrium, x=2;If the amount of a substance in containers A and B is not equal at equilibrium, x = 4. The volume fraction of a in A at equilibrium is 30% (at x=2) or 60% (at x=4) If the pressure of the two containers is not equal at equilibrium, the pressure in the two containers: A:

B = 8:5.