Consider the following endothermic reaction: N2(g) + O2(g) → 2NO(g). What will happen to the equilibrium if the temperature of the system is raised?

Explanation

In an endothermic reaction such as N2(g) + O2(g) → 2NO(g), increasing the temperature provides additional heat that the system can absorb. According to Le Chatelier's principle, the system will adjust by favoring the forward reaction (towards the products) to absorb this extra heat. This results in increased production of NO and a higher equilibrium constant (Kc). Option A is incorrect because a backward shift occurs when temperature is decreased. Option B is incorrect because temperature changes do affect equilibrium. Option D is incorrect because the options cannot all be correct simultaneously.