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Use the reaction, which produces ammonia, to answer the question.
N2(g) + 3H2(g) 2 2NH3(g)
Which change would happen in the system if the concentration of N2 was increased at constant pressure?

O The reverse reaction would increase in order to increase the pressure.

O The reverse reaction would increase to start reducing the concentration of N2.

O The forward reaction would increase to start reducing the concentration of N2.

O The forward reaction would increase in order to increase the pressure.

Respuesta :

sebassandin

This problem shows chemical equation for equilibrium production of ammonia and asks for the correct change when the concentration of nitrogen is increased. Thus, the answer is the forward reaction would increase to start reducing the concentration of N2.

Chemical equilibrium

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:

[tex]N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)[/tex]

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: https://brainly.com/question/26453983

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