Effect of Pressure on Gaseous Equilibrium
In an experiment involving the Haber process, a researcher observes that increasing the system’s pressure causes the equilibrium to shift toward the products. The researcher concludes that for any gaseous reaction at equilibrium, an increase in pressure will always favor the formation of products. Which of the following identifies the flaw in this conclusion?
A
Increasing pressure always favors the reactants, not the products.
B
Pressure changes do not affect reactions involving gases.
C
Increasing pressure decreases the reaction rate, not the equilibrium position.
D
The shift depends on the mole ratio of gases, not just pressure increase.
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