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For the reversible reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + heat, the equilibrium shifts in forward direction:

1. By increasing the concentration of NH₃(g)
2. By decreasing the pressure
3. By decreasing concentration of N₂(g) and H₂(g)
4. By increasing pressure and decreasing temperature

Correct answer: By increasing pressure and decreasing temperature

Solution

The forward reaction produces fewer gas molecules (4 → 2), so increasing pressure favors it. Decreasing temperature also shifts equilibrium forward as the reaction is exothermic.

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