Which of the following favors the formation of products in the reaction: CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)?
Correct answer: B. Removing H₂
- A. Adding CO
- B. Removing H₂
- C. Increasing pressure
- D. Adding a catalyst
Explanation
Removing H₂ shifts the equilibrium to the right to produce more H₂, favoring products.
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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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