For the reaction N₂ + 3H₂ ⇌ 2NH₃, where ∆H is negative, the forward reaction is favored by:
Correct answer: C. Decreasing the temperature.
- A. Adding NH₃ at equilibrium.
- B. Adding a catalyst.
- C. Decreasing the temperature.
- D. Decreasing the concentration of H₂.
Explanation
According to Le Chatelier's principle, for an exothermic reaction (ΔH is negative), decreasing the temperature will shift the equilibrium to the right to produce more heat, thus favoring the forward reaction.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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