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Given the system at equilibrium: N2O4(g) + 58.1 kJ <----> 2 NO2(g) What will be the result of an increase in temperature at constant pressure?D) The equilibrium will shift to the right, and the concentration of NO2(g) will increaseA) The equilibrium will shift to the left, and the concentration of NO2(g) will decrease. B) The equilibrium will shift to the left, and the concentration of NO2(g) will increase. C) The equilibrium will shift to the right, and the concentration of NO2(g) will decrease.

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STEP-BY-STEP EXPLANATION:

Given information

[tex]N_2O_{4(g)}\text{ + 58.1KJ }\rightleftarrows2NO_{2(g)}[/tex]

From the given reaction, you will see that energy is added to the reactant side. This implies that the reaction is an endothermic reaction.

An endothermic reaction is a type of reaction in which heat is absorbed from the surroundings.

Recall, Le Chatelier's principle states that when external constraints such as (temperature, pressure, and concentration) are imposed in a chemical equilibrium system, the equilibrium shift so as to annul or neutralize the effect of the constraints

When temperature is

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