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?
Correct answer: C. The equilibrium will shift in the forward direction
- A. The equilibrium will shift in the backward direction
- B. The equilibrium position will remain unchanged
- C. The equilibrium will shift in the forward direction
- D. All of the above
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.
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About Le Chatelier's Principle
Le Chatelier's principle predicts how an equilibrium responds when concentration, pressure or temperature changes. Questions apply it to reversible reactions, identify the direction of shift and distinguish genuine equilibrium changes from the effect of a catalyst, which changes the rate of reaching equilibrium but not its position.
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