For (g) + 3(g) 2(g) + heat — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

# Solution: Haber Process Equilibrium I notice the question stem is incomplete, but based on the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{heat}$, this tests **Le Chatelier's Principle** for equilibrium shifts. ## Key Analysis: **This is an exothermic reaction** (heat is a product), so: | Stress Applied | Equilibrium Shifts | Effect on $NH_3$ | |---|---|---| | **↑ Temperature** | Left (opposes heat release) | Decreases | | **↓ Temperature** | Right (favors heat release) | **Increases** ✓ | | **↑ Pressure/↓ Volume** | Right (4 moles → 2 moles) | **Increases** ✓ | | **↑ Concentration of reactants** | Right | **Increases** ✓ | | **Remove product** | Right (shifts to replace it) | **Increases** ✓ | ## Why C is likely correct: Without seeing the options, **C probably states one of:** - **Low temperature favors $NH_3$ production** (industrial conditions: ~400-500°C is a compromise) - **High pressure favors $NH_3$ production** (Haber process uses 150-300 atm) - **Removing $NH_3$ shifts equilibrium right** (condensation is used industrially) All these shift equilibrium **rightward** to increase ammonia yield, which is the principle underlying modern ammonia synthesis.