The problem of chemical equilibrium contemptible inorganic chemistry as if it had never been studie

A1 nitrogen reacts with 3 hydrogen to produce 2 ammonia.

So the amount of gaseous matter decreases after this reaction.

However, container A maintains a constant volume, and container B maintains a constant pressure, so the pressure of the gas in A decreases, and the volume of the gas in B decreases (the pressure remains the same).

Because the volume of this reaction decreases after the reaction, the greater the pressure, the more complete the reaction, so the reaction in B is more complete.

d The amount of reaction product is less than that of the reactant, so it is ......

A is certainly not true, and the other three are definitely true.

You see N2 + 3H2 == 2NH3 reactants have 4 stoichioimetric numbers and reaction products have 2 stoichiometric numbers.

In other words, the amount of gaseous substances in the forward reaction decreases, the gas pressure decreases, and the increase of external pressure is conducive to the forward reaction.

Therefore, it is not possible to have the same conversion rate. Container B has constant pressure, so the pressure must be greater than that of container A, and the conversion rate and reaction rate are relatively high for B.

Choosing a to synthesize ammonia is a reaction in which the amount of a substance decreases, so during the reaction, the change in the concentration of reactants in the two containers of A and B is not the same, and the concentration of reactants in container B is constant that is, with the progress of the reaction, the total volume of the gas is reduced (because the reaction is a reaction in which the amount of a substance decreases), and the volume of the gas is constant, and the reaction in container B is equivalent to compressing container A, and the concentration of reactants in container B is larger than that of container A when the reaction is carried out This also results in the reaction of vessel B is faster than that of vessel A, and the ammonia gas produced by vessel A is more correct than that of BCD.

Chemical equilibrium has: chemical reaction equilibrium, ionization equilibrium, precipitation-dissolution equilibrium, hydrolysis equilibrium, I think, you just need to understand.

1 All chemical reactions are incomplete reactions! But there is only a reversible reaction that exists in equilibrium!

2 reverse! Equilibrium only exists in reversible reactions.

3 moves! Dynamic equilibrium.

4th Prize! The whole you reflect at an equal rate.

5 set! The concentration of reactants and products is constant.

6 changes! The chemical equilibrium changes with the change of the external exchange.

Actually, chemical equilibrium is very simple! As long as you understand these six words, you can apply them proficiently. That's it, if there's anything else you can't do, you can ask me. This will be a little better, and I hope my answer will help you 、、、

The feature is 5 words.

Reversed, etc., moving, fixed, changing.

Inverse: The object of chemical equilibrium study is reversible reactions;

etc.: The positive reaction rate is equal to the reverse reaction rate;

Dynamic: The chemical reaction reaches dynamic equilibrium;

Constant: The concentration of each component is kept constant;

Change: When the external equilibrium conditions change, the equilibrium state pit can be destroyed, and the concentration of each component changes accordingly, and the equilibrium is established under the new conditions.

There are 2 ways to directly judge that equilibrium is achieved:

The rate of forward and reverse reactions is equal;

The concentrations of the components do not change.

Thank you for adopting.

It is an exothermic reaction.

Therefore, the temperature is lowered and the equilibrium shifts to the right.

And because m+n>q the number of molecules in the container decreases while the total mass does not change, because the average relative molecular mass is equal to the total mass divided by the number of molecules, the average relative molecular mass of the gas mixture becomes larger.

Choose b a: Dalton's law of partial pressure The pressure of each gas does not change b Do the math yourself. c. Decrease the temperature and the reaction shifts forward because m+n>q the amount of the gas becomes smaller and the average molecular weight is equal to the total mass divided by the total mass Conservation of mass The amount of the substance decreases and the molecular weight becomes larger.

d increases x x and the conversion rate decreases y increases.

==Wrong question. It should be enlarged.

This is an equivalence balance issue. First of all, this reaction is characterized by the gas coefficient before and after the reaction and the constant reaction. Then, whether it is isothermal isobaric or isothermal isochorric, as long as the two feeding ratios are equal, the equivalent equilibrium can be established.

option A, if A2 is 2mol and B2 is 4mol, then the conversion rate of A remains the same. If the addition of A2 is 2mol and B2 is 5mol, the concentration of B2 is increased, the equilibrium is positively shifted, and the A2 conversion rate is increased. That's right.

b option, the equivalent equilibrium will only be established when the input z is zero. Therefore, the quantity of z cannot be expressed (the equation can be listed with the equilibrium constant, but it certainly contains a).Mistake.

Option C, which applies extreme conversion, is equivalent to a feeding ratio of 1:1, which is not equal to the original feeding ratio, so it is not an equivalent equilibrium, and the volume fraction is different. That's right.

d option, the problem should be any value where z is greater than zero, then the extreme value conversion is applied, which is equivalent to the feeding ratio of 1:1, which is not equal to the original feeding ratio, so it is not equivalent equilibrium, wrong.

According to the information given by the question, the sum of the coefficients of the reactants and the sum of the coefficients of the products are equal, in the case of constant temperature and constant capacity, for this problem, as long as the ratio of the quantity of the substance is the same as the original, the constructed equilibrium is equivalent equilibrium, if the constant volume is maintained, when x:y<1:2, z=0, in essence, the amount of the substance of b is increased on the basis of the original horizontal level, then the conversion rate of a must increase when the new equilibrium state is reached, so.

a, c is correct.

The 3 on the denominator of (x+y+z) in answer b is unfounded, although when x:y = 1:2 and z is an arbitrary value, it will constitute an equivalent equilibrium (because the pressure is constant, the ratio of the coefficient of the reactant to the coefficient of the product is the same as the original, forming an equivalent equilibrium), d answer, x:

I don't understand what y0 means, but under constant temperature and pressure, if the volume fraction of b remains unchanged, it can only be that the ratio of the amount of reactants to the product is the same as the original.

Let N2 account for xmol in 4mol of mixed gas, then 28x+2(4-x)=4*, and the solution is x=1, that is, the amount of matter n2:h2 in the original gas is 1:3

n2+3h2<=>2nh3

The volume of the gas changes before and after this reaction, so when the temperature and volume are constant, 1moln molh2 must be added, so.

If x 0, y 0, then z 2mol ;

When the temperature and pressure are constant, as long as n2 and h2 are pressed by 1:3, it is fine, so if x 0 and y 0, then z>0;

In the same way: when the temperature and volume are constant, if x, then y, z;

When the temperature and pressure are constant, if x, then y, z 0;

When the temperature and pressure are constant, the relationship between x, y and z should be satisfied is: x:y=1:3, z 0 or x=y=0, z>0

First, cross to find n2:h2=1:3. in the original questionThey are 1mol and 3mol a: because it is an isothermal and equal volume transformation, the total amount of atoms is the same as the original, z=2mol (the amount in the question is completely transformed);

b: Because the transformation volume becomes larger, the pressure does not change, so the volume increases, so Z>2mol;

As in the first question, z= can be obtained by ensuring that the number of atoms does not change, and the judgment is the same

2x+z=2 and y=3x

Yes, it's handmade.

1. If the conversion rate of reactants increases, the remaining amount will be less during equilibrium, and the volume fraction will decrease

2. You can think of it like this: suppose A and B react, there is AG A at the beginning, which is transformed with the help of BG B, and B is also transformed at the same time, less than BG at the beginning; Later, AG A (i.e., the concentration of A increases), but at this time, the remaining B is less than BG, and A cannot be converted, so the conversion rate is reduced.

3. At the same temperature, take container A as the standard, 1g n2 and 1g h2 in container A, first regard container B as the size of 2 containers A, fill 2g n2 and 2g h2, the concentration and pressure of the two containers are the same at this time, then the equilibrium is equivalent, that is, the rate, concentration, conversion rate and volume fraction are the same; Then the B container is compressed to the size of the A container, the volume is halved, the pressure is doubled, the concentration is doubled, so the rate is accelerated (option A is correct), the balance moves in the positive direction, the main point of Le Chatelier's principle is: moving in the direction of "weakening" the change of external conditions, the concentration of B decreases on the basis of doubling, but weakens, and the increase will not be fully transformed, so it is larger than the original that is, A (option B is correct), and similarly, on the basis of the original conversion rate, it moves forward again, and H2 is transformed again, Then the H2 conversion rate increases (option C is correct), and if the H2 conversion rate increases, the volume score decreases, that is, your question 1 (option D is wrong).

1. False, A+B---C+D, the conversion rate of A increases, and the volume fraction of B may increase;

2. Add more, convert less;

3,b: right; D: False.

a. Correct. If the amount of substances in A and B is not equal in equilibrium, [of course, B is not equal], but the volume fraction of C is equal, it means that the reaction is a reaction with the same number of gas molecules, so x=4.

b. Incorrect. Because the starting ratio of a and b in B is 3:1, that is, the reaction proceeds to the left, and the generated a and b are also 3:

1, so the ratio of the equilibrium concentration of a and b in B must be 3:1, and the ratio of the amount of substances in a and b in containers A and B is equal when equilibrium.

c. Incorrect. c is, then a and b are altogether, they are always 3:1, so a is d, correct.

If the pressure in the two containers is not equal [the total amount of the gas is not equal] at equilibrium, but the volume fraction of c is equal, the same as a, x=4, the pressure in the reaction is always the same, the initial pressure is 8:5, and the difficulty is always 8:5

Note: D is a solid, as long as there is enough of it, the amount of its Zen ruler answer does not affect the balance.

There are questions to know: 1. Increase the temperature, the equilibrium moves in the direction of endothermy, and this reaction shifts to the right; Increase the pressure, the equilibrium moves in the direction of the decrease in the volume of the gas, and shifts to the left during this reaction, so A+B analysis: A, the catalyst only affects the reaction rate, that is, the speed of the reaction rate is changed, and the equilibrium is not changed, so this choice is incorrect;

b, the temperature rises, the equilibrium shifts to the right, and y(q) increases, so this option is correct;

c, the pressure increases, the balance shifts to the left, and y(q) decreases, so this option is incorrect;

d, increase the amount of n, the balance shifts to the right, q will increase, but y(q) will increase or decrease, it is uncertain, so this option is incorrect.

Comparison between Figure 1 and Figure 2: It can be seen that when the pressure increases, m% will increase, indicating that the pressure increases and the balance shifts to the left! (a+b As you can see from the graph, m% decreases as the temperature increases, indicating that the temperature rise equilibrium shifts to the right.) (endothermic reaction).

As z increases, m% decreases.

Let's take a look at the options:

a No, because the catalyst can only affect the reaction rate, not the equilibrium.

b is correct, the temperature rise equilibrium shifts to the right, and q% will increase.

c is not true, because the pressure increases, the balance shifts to the left, and q% decreases.

D is not true, because the denominator of the volume fraction increases when Z increases, and the equilibrium does not change significantly as Z increases when other conditions remain constant, so Q% decreases.

Hope it helps!