This problem is providing us with the chemical equation depicting the production of ammonia from nitrogen and hydrogen at equilibrium and asks for the correct change when the concentration of nitrogen is increased. At the end, the answer is the forward reaction would increase to start reducing the concentration of N2.
<h3>Chemical equilibrium</h3>In chemistry, chemical reactions not always reach a 100-% conversion when reactants get in contact in order to carry out the chemical reaction. Thus, there is a point wherein the concentrations remain the same and is called equilibrium.
In such a way, for this problem, we have the following chemical reaction at equilibrium:
Now, according to the Le Ch.atelier's principle, an increase in the concentration of any species, shifts the equilibrium away from it, which means that if we increase the concentration of nitrogen, a reactant, the forward reaction will be favored.
Thereby, the correct answer is "the forward reaction would increase to start reducing the concentration of N2".
Learn more about chemical equilibrium: brainly.com/question/26453983