Le Chatelier's Principle

Question

For the exothermic reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), which change will shift the equilibrium to the right?

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**Le Chatelier's Principle** states that if a system at equilibrium is disturbed, the system will shift its position to counteract the disturbance.
1. **Removing Ammonia ($NH_3$)**: The system tries to produce more to compensate for the loss, shifting the equilibrium to the **right**.
2. **Increasing Temperature**: For an exothermic reaction, heat is a product. Increasing $T$ shifts equilibrium to the **left** (reversing the reaction).
3. **Decreasing Pressure**: Shifts equilibrium towards the side with more moles of gas (left has 4, right has 2). Shifts to the **left**.
4. **Adding Catalyst**: Affects only the rate of reaching equilibrium, not the position.

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Le Chatelier's Principle

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