Given that the following reaction is exothermic, which of the following sets of changes would cause the following system at equilibrium to shift to increase the number of N₂O₄(g)molecules? 2NO₂(g)⇌ N₂O₄(g)What observation would indicate that the reaction is at equilibrium in a closed container?

Question

Quizplus · Accepted Answer

According to Le Chatelier's principle, when an equilibrium system is subjected to a stress, the system will shift in a way that opposes the stress. In this case, decreasing the volume of the container will increase the pressure, and the system will shift in the direction that has fewer moles of gas to reduce the pressure, which is towards N₂O₄(g). Additionally, decreasing the temperature will also favor the exothermic reaction, which produces more N₂O₄(g) molecules. To determine if the reaction is at equilibrium in a closed container, one can observe any changes in the concentrations or pressure over time. If the concentrations and pressure remain constant over time, then the reaction has reached equilibrium.

Given That the Following Reaction Is Exothermic, Which of the Following