For the equilibrium reaction 2NO2 ⇌ N2O4 (g) (-61 kJ), increase of temperature would:
Correct answer: B. Favour the Decomposition of N2O4
- A. Favour the Formation of N2O4
- B. Favour the Decomposition of N2O4
- C. No Effect on Equilibrium
- D. Stop the Reaction
Explanation
The reaction is exothermic (ΔH = -61 kJ) in the forward direction (2NO₂ → N₂O₄). Increasing temperature adds heat, which the system counteracts by shifting toward the endothermic reverse reaction. Thus, the equilibrium shifts to decompose N₂O₄ into NO₂.
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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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