For an equilibrium, which of the following statements is false?
Correct answer: D. There is no correlation between the reaction quotient and Keq in predicting the direction in which the reaction proceeds.
- A. If the reaction quotient of the reaction is greater than Keq the reaction moves in thebackward direction.
- B. If the reaction quotient of the reaction is lesser than Keq the reaction moves in theforward direction.
- C. If the reaction quotient of the reaction is equal to Keq the reaction is at equilibrium.
- D. There is no correlation between the reaction quotient and Keq in predicting the direction in which the reaction proceeds.
Explanation
Option D is false. The reaction quotient (Q) is indeed related to the equilibrium constant (Keq) in predicting the direction in which the reaction proceeds. If Q is greater than Keq, the reaction will shift in the backward direction (toward the left to reach equilibrium), and if Q is less than Keq, the reaction will shift in the forward direction (toward the right to reach equilibrium). When Q is equal to Keq, the reaction is at equilibrium.
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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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