Question

question 3 of 32 how would the equilibrium of the reaction below be affected if the temperature increased?
o₂(g) + 2so₂(g) ⇌ 2so₃(g) + 200 kj

a. the concentration of so₃ would increase.
b. the concentrations of o₂, so₂, and so₃ would increase.
c. the concentrations of o₂ and so₂ would increase.
d. the concentrations of o₂, so₂, and so₃ would decrease.

Explanation:

1. First, identify the type of reaction: The given reaction \( \ce{O_{2}(g) + 2SO_{2}(g)

ightleftharpoons 2SO_{3}(g) + 200\ kJ} \) shows that heat (200 kJ) is a product, so this is an exothermic reaction (releases heat).

1. Apply Le Chatelier's Principle: For an exothermic reaction, increasing the temperature is like adding a product. The system will shift to counteract this change, so it will shift in the reverse direction (towards the reactants) to consume the excess heat.
2. Analyze the effect on concentrations: When the equilibrium shifts to the left (reverse direction), the concentrations of the reactants (\( \ce{O_{2}} \) and \( \ce{SO_{2}} \)) will increase, and the concentration of the product (\( \ce{SO_{3}} \)) will decrease.

Answer:

C. The concentrations of \( \ce{O_{2}} \) and \( \ce{SO_{2}} \) would increase.