Given the equilibrium
Heat + 2FeCl₃ (s) ⇌ 2FeCl₂ (s) + Cl₂ (g)
Which of the following options is correct:
A) to shift the equilibrium to the right, it is necessary to increase the concentration of FeCl₃ (s).
B) to shift the equilibrium to the left, it is necessary to increase the concentration of Cl₂.
C) to shift the equilibrium to the left, it is necessary to remove FeCl₃ (s).
D) to shift the equilibrium to the right, it is necessary to cool the reaction.
E) to shift the equilibrium to the left, it is necessary to increase the concentration of FeCl₂ (s).
IMAT 2025 · Question 41
Q41 - Equilibria in aqueous solution
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The correct answer is B) to shift the equilibrium to the left, it is necessary to increase the concentration of Cl₂.
Two things to keep in mind. Solids don't affect the equilibrium, since they don't appear in Kc (here Kc = [Cl₂]), and heat is on the left, so the forward reaction is endothermic.
Adding Cl₂, the only gas, pushes the equilibrium back to the left. Adding or removing FeCl₃ or FeCl₂ does nothing, and since the reaction is endothermic, cooling would push it left rather than right.
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