Is there a wrong answer to this question about chemical equilibrium?

A Answer: The equilibrium under the condition should move in reverse, because the input ammonia gas will definitely react to form nitrogen and hydrogen under the conditions, so the equilibrium moves in reverse, but the new equilibrium established under this condition is equivalent to the original equilibrium, and the volume fraction of each component does not change.

The equilibrium under the condition of C answer should also move in reverse, because the volume of the container expands when the gas is filled with constant pressure, but the gas has nothing to do with the reaction, so the concentration of the gas in the reaction decreases due to the increase in volume to make the equilibrium move, which is equivalent to decompression, so the equilibrium should move in the opposite direction.

A must be wrong, C must be right, believe me, absolutely yes

(Helium) is a noble gas that does not react with other substances.

So adding helium, it's just pressurizing.

That's right, the volume can be varied by the premise of constant temperature and pressure.

AC moves in reverse.

Item A: The pressure is constant, the concentration of the product increases, and the equilibrium moves in the opposite direction.

Item C: The partial pressure of each substance is proportional to the amount of each substance, that is, the partial pressure of each substance = the amount of the substance of the substance The amount of the total gas substance * the total pressure. Due to the constant pressure, the partial pressure of HE2, N2, H2, and NH3 becomes smaller, and the balance moves in the direction of increasing pressure, so it moves in the opposite direction.

ac's all wrong.!

A: At constant pressure: when gas is added, the volume must increase, so the system will be in the direction of volume increase (that is, the side with the most gas coefficient) So, !

Already moved to the left! However, the concentration of other substances is less than that of the added one. When ammonia is added, the concentration of the product increases ,!!

So the balance moves in reverse! So! Double Reverse Move!

Definitely move! C: Chong he.!It doesn't affect the original.!But constant pressure...So, increase in volume...An increase in volume means that the concentration of each substance in the system decreases, which decreases. Of course I want to increase it...

Therefore, it moves to the side with more gas coefficients,,, that is, it moves in the opposite direction.!

Hope you understand,!

Absolutely wrong!!

The addition of ammonia at constant pressure equilibrium is definitely reversed.

Take B as an example, and assume that 2mol L of CO and 2mol L of H2O are filled at the beginning

According to the equation, when both CO and H2O have 1mol L left, exactly 1mol L of CO2 and H2 are produced

At this time, it is not necessarily an equilibrium state, because the equilibrium constant k is not necessarily equal to 1, so it is possible that co and h2o continue to react, and when equilibrium, co=h2o≠co2=h2

Note: The basic sign of equilibrium is that the concentration of each substance does not change.

Think about it: because of the conditions, because of the different conditions, the limits of the reversible reaction are not the same, how is it possible to reach chemical equilibrium when the concentration of each substance is the same? If the concentration of each substance is the same under a certain condition and the equilibrium is reached, then after changing the condition and the equilibrium shifts, the concentration of each substance must be different, right?

Because these two are equal volume reactions, the concentration of each gas composition is always the same, regardless of the time of the reaction.

To determine the chemical equilibrium of the reversible reaction of the gas, it does not mean that the concentration of each component is equal to reach equilibrium, but that the concentration of each component does not change anymore The sum of the volume of gas before and after the reaction is equal At any time, as many moles of reactants are generated, as many moles of products are formed, and the amount of substances of the four substances is equal at any time of the reaction, and the concentration is naturally equal, and the volume and unequal volume of the gas before and after the reaction of A In the same way, the concentration of each component of the gas may be equal at some point in the reaction But equilibrium has not yet been reached, and only the concentration of the components does not change, which means that the equilibrium is achieved, and I hope it will be useful to you.

The final substances in the container are: pH3, Hi, P4, H2, I2 and PH4I. The ratio of P:H:I to mass in Ph3, Hi, P4, H2 and I2 should be the same as that of Ph4I, that is, equal to 1:4:1

The amount of iodine I in the product is: 1*8+2*1=10mol, so the amount of PH4I that undergoes decomposition is 10mol, and the amount of H substance decomposed is 40mol. The products containing H are pH3, Hi and H2, where the amount of H substances in Hi and H2 is:

1*8+2*7=22mol, so the amount of pH3 is: (40-22) 3=6mol

Therefore, the amount of each gaseous substance in equilibrium is: PH3 is 6mol, HI is 8mol, H2 is 7mol, and I2 is 1mol

The first sail answers: the equilibrium constant of the high reaction k=[ph3][hi]=6 2*8 2=12

The two equations can be obtained simultaneously, c(s) + h2o(g) +2hbr(g) co(g)+h2(g) +br2(g).

C is the exclusion of solids, so the equation can be reduced to the judgment of the remaining 5 substances, according to the equilibrium code and the original equation, HBR and BR2 are congruent equilibrium in the unified system, so the amount of matter is not used as a criterion for judging the equilibrium concentration, in the first reaction equation, according to the conservation of oxygen atoms, so its equilibrium and its equilibrium concentration cannot be judged by this.

Knowing only two quantities that are unique to one reaction cannot be calculated that another reaction has two quantities that are unique, whereas a gas mixture needs to know all the quantities.

1. Yes. However, it should be more technical, e.g., v(n2)positive : v(nh3)inverse = 1:2

2. Right. Constant temperature and constant pressure, that is, the reaction vessel increases with the increase of gas pressure, that is, the equivalent equilibrium, then all the NH3 in route 2 is converted to the left, which is 2 and 6, and the concentration ratio is 1:2

However, it should also be noted that the starting concentrations of certain substances are stated, such as pathways 1, N2 and H2 starting concentrations of 1mol L and 3mol L respectively. But I didn't say nh3, at this time we think he didn't add it, if he does, then it has to be considered, it may be wrong.