can someone show how they got the answers for these 3 questions? What is the cor

Question

can someone show how they got the answers for these 3 questions?

What is the correct expression for the equilibrium constant of the following reaction? (NH4)2Se (s) - > 2NH3 (g) + H2Se (g) Answer: [NH3]^2 [H2Se] The equilibrium constant for the following reaction, is 4.34 x 10^-3 @ 300 degree C. At equilibrium, which of the following statements is true? N2 (g) + 3 H2 (g) 2 NH3 (g) Answer: More reactants than products For the exothermic reaction in problem 2, the following energetics are true: N2 (g) + 3 H2 (g) 2 NH3 (g) + heat Which factor (s) might increase the production of large quantities of ammonia? Answer: Raising the pressure, Removing the ammonia, as soon as it is made, and Addition of a catalyst

Explanation / Answer

For the given reaction, aA(g) + bB(g) -----> cC(g) + dD(g),

the equilibrium constant expression is

Keq = [C]c . [D]d / [A]a . [B]b

If any of the product or reactants are labelled as (s), those should be ignored, as pure substances has a value of 1.

So, for the first question, as the reactant is (s), it is ignored.

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As the Keq value is very less, the reaction is more in reactants than in products.

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According to Le chatlier's principle, Changing the concentration of a chemical will shift the equilibrium to the side that would reduce that change in concentration.

So, Removal of ammonia at regualr intervals results in decreased conc of products. So, reactants tends to move to the side of deficiency.

Pressure:

moles of reactnts = 4

Moles of products =2

Increae of pressur pushes the reaction equilibrium in the direction in which there is a decrease in the number of moles. This is accordign to Lechatlier's principle.

So, as products moles are less, it moves towards NH3.

Addition of a catayst :

It increases the rate of reaction.

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