For the reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g), given ΔH° and ΔS° values at 300K and 1200K, the incorrect statement is:
Correct answer: C. At 1200 K, Kₚ > 1
- A. The reaction proceeds in the forward direction at 300 K
- B. At 1200 K, the reaction proceeds in the reverse direction
- C. At 1200 K, Kₚ > 1
- D. At 300 K, the products will be favored more than reactants at equilibrium
Explanation
By calculating the Gibbs Free Energy (ΔG° = ΔH° - TΔS°), the reaction is found to be non-spontaneous in the forward direction at 1200 K (ΔG° > 0). A non-spontaneous forward reaction means the equilibrium constant (Kp) must be less than 1, making statement C incorrect.
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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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