Question

Using the equation 2SO₃(g) ↔ 2SO₂(g) + O₂(g) + 40 kJ, if SO₂ is removed, what way does equilibrium shift?

A) To the left
B) To the right
C) It will not shift
D) It depends on temperature and pressure

Answer 1

The equilibrium will shift to the right when SO2 is removed, according to Le Chatelier's Principle. The equilibrium constant of the exothermic reaction decreases with an increase in temperature, and the reaction releases energy to the surroundings when proceeding to the right.

Step-by-step explanation:

When SO2 is removed from the equilibrium system 2SO3(g) ↔ 2SO2(g) + O2(g) + 40 kJ, the equilibrium will shift to the right. This is because, according to Le Châtelier’s Principle, when a reactant or product is removed from a system at equilibrium, the equilibrium will shift in the direction that tends to replace that substance. In this case, removing SO2 shifts the equilibrium to produce more SO2 and O2 from SO3.

Regarding question (a), as temperature increases, the equilibrium constant for an exothermic reaction typically decreases because the reverse reaction is favored at higher temperatures. Therefore, for an exothermic reaction like the formation of SO3, an increase in temperature would decrease the value of the equilibrium constant.

The reaction is exothermic as indicated by the +40 kJ on the products side of the equation. This heat released signifies that the reaction releases energy to the surroundings when proceeding to the right.