Consider the following reaction at equilibrium at a given temperature: 2NH₃(g)+ heat ⇌ N₂(g)+ 3H₂(g)Which of the following will cause the value of the equilibrium constant for this process to change?

Question

Quizplus · Accepted Answer

According to Le Chatelier's principle, increasing the temperature of an equilibrium system favors the endothermic reaction, which in this case is the forward reaction (since heat is a product in the forward reaction). Therefore, raising the temperature will shift the equilibrium towards the products, leading to an increase in the value of the equilibrium constant. The other choices will not have a significant effect on the equilibrium constant. Adding more reactants (choice A) will shift the equilibrium towards the products temporarily, but the system will eventually reestablish equilibrium. Increasing the pressure (choice B) will only have an effect if the number of moles of gas changes, which is not the case here. Adding a catalyst (choice C) will increase the rate of both the forward and reverse reactions, but will not affect the position of equilibrium or the value of the equilibrium constant. Adding neon to the system (choice E) is essentially adding an inert gas, which will not participate in the reaction and will not affect the equilibrium constant.

Consider the Following Reaction at Equilibrium at a Given Temperature