Which of the following is true?

1. when the value of q is large, the equilibrium lies on the product side of the equilibrium reaction.
2. a small value of k means that the equilibrium concentrations of the reactants are small compared to the equilibrium concentration of the products.
3. when the value of k is large, the equilibrium lies on the reactant side of the equilibrium reaction.
4. a large value of k means that the equilibrium concentrations of products are large compared to the equilibrium concentrations of the reactants
5. when the value of k is small, the equilibrium lies on the product side of the equilibrium reaction.

Explanation:

For a general equilibrium

aA +bB ⇔ cC + dD ,

the equilibrium constant is K = [C]^c [D]^d / [A]^a[B]^b.

Our reasoning here should be based on the fact that  Q has the same expression as K, but is used when the system is not at equilibrium, and the system will react to make Q = K to attain it ( Le Chatelier´s principle ).

So with this in mind, lets answer this question.

1. False: Q can large or small but is not the value of the equilibrium constant, it will predict the side towards the equilibrium will shift to attain it.

2. False: Given the expression for the equilibrium constant, we know if K is small the concentrations of the reactants will be large compared to the equilibrium concentrations of the products.

3. False: when the value of K is large, the equilibrium concentrations of the products will be large and it will lie on the product side.

4. True: From our previous reasongs this is the true one.

5. False: If K is small, the equilibrium lies on the reactants side.

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .

it's all four options.