Temperature of traditional industrial ammonia synthesis

(1) According to the equilibrium constant equal to the power product of the equilibrium product concentration divided by the power product of the reactant concentration, then the denominator of k is the reactant, the molecule is the product, and the power is the previous coefficient. From k, we can know that the reaction is 12N2 +32H2? NH3, so the answer is: 12N2 +32H2? NH3

(2) According to the table, under a certain pressure, the volume fraction of ammonia decreases from 400℃ to 500℃, indicating that the temperature-raising equilibrium moves in the reverse reaction direction, so the equilibrium constant k decreases from 400℃ to 500℃. The name of ammonia synthesis catalyst is iron catalyst, so the answer is: decrease; Iron catalyst;

(3) According to the data analysis in the table, at a certain pressure, the lower the temperature, the greater the volume fraction of ammonia. At a certain temperature, the higher the pressure, the greater the volume fraction of ammonia, so high pressure and low temperature are beneficial to the synthesis of ammonia. However, in industrial production, besides the conversion rate, the reaction rate should be considered, so the conditions selected by the synthetic ammonia industry are 450℃ and 40.5MPa.

Therefore, the answer: from the perspective of chemical reaction rate, the catalyst has the best catalytic effect at 450℃; Considering the chemical reaction rate and equilibrium movement, the volume fraction of ammonia in the equilibrium system is large under the condition of 40.5MPa when energy consumption and material strength allow.

(4) According to the principle of equilibrium movement, in order to improve the conversion rate of the reaction, the equilibrium should move to the positive reaction direction as much as possible;

A. Liquefying and separating ammonia in the mixed system is equivalent to reducing the concentration of the product, moving the balance to the positive reaction direction and improving the conversion rate of the reaction, so A is correct;

B, filling a proper amount of hydrogen into the system, which is equivalent to increasing the concentration of reactants. Although the balance moves to the positive reaction direction, the total amount of hydrogen in the reactant increases a lot, but the conversion rate of hydrogen decreases, so B is wrong;

C, the recovery of hydrogen and nitrogen is equivalent to the re-reaction of unconverted reactants, so the conversion rate of the reaction is improved, so C is correct;

D, charging a proper amount of ammonia into the system is equivalent to increasing the concentration of the product, making the equilibrium move in the reverse reaction direction and reducing the conversion rate of the reaction, so D is wrong;

So choose AC.