Question

In which of the following equilibrium reactions, the equilibrium would shift to the right if pressure is increased?
A.${N_2} + 3{H_2} \rightleftarrows 2N{H_3}$
B.${H_2} + {I_2} \rightleftarrows 2HI$
C.${H_2} + C{l_2} \rightleftarrows 2HCl$
D.${N_2} + {O_2} \rightleftarrows 2NO$

Answer 1

We have to predict the equilibrium of a chemical reaction using Le Chatelier’s principle. Based on this principle, if equilibrium is stressed, the reactions shift to decrease the stress. We can stress equilibrium in several ways.

Complete answer:
We can say that there are a few different stresses to push equilibrium. One path is to add or eliminate a product or a reactant in a chemical reaction at equilibrium. At the point when extra reactant is added, the equilibrium moves to decrease this pressure: it makes more products. At the point when extra product is added, the movement of equilibrium to reactants to lessen the pressure. In the event that reactant or product is taken out, the equilibrium moves to make more reactant or product, separately, to compensate for the loss.
When equilibrium is stressed, the chemical reaction will not be found at equilibrium and reaction shifts to go back towards equilibrium to a path that reduces the stress.
Among the given chemical reactions, the equilibrium would shift to the right if pressure is increased for the reaction (A). We can explain the reason as,
In the reaction ${N_2} + 3{H_2} \rightleftarrows 2N{H_3}$, there is a decrease in the number of moles of the forward reaction and for the reverse reaction, the number of moles increases. When there is an increase in total pressure, the forward reaction would be favored because the forward reactions take place with decrease in the amount of moles based on Le-Chatelier’s principle. So, the position of equilibrium would move towards the product.

Option (A) is correct.

Note:
We have to know that Le Chatelier's principle tends to explain how equilibrium shifts when the states of equilibrium e are altered. The course of shift can be anticipated for changes in temperature, concentrations, or pressure. We have to know that catalysts don't influence the situation of equilibrium; they assist reaction with accomplishing equilibrium quicker.