For a reaction with the equilibrium expression K꜀ = [X]² / (V(a-[X])), what is true for this reaction?
Correct answer: B. Decrease in pressure will favor the forward reaction
- A. Increase in pressure will favor the forward reaction
- B. Decrease in pressure will favor the forward reaction
- C. Decrease in pressure will favor the backward reaction
- D. Increase in volume will favor the backward reaction
Explanation
The volume (V) in the denominator of the K expression indicates that the number of moles of products is greater than the number of moles of reactants. According to Le Chatelier's principle, a decrease in pressure will favor the direction that produces more moles of gas, which is 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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