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For the equilibrium 2 SO2(g) + O2(g) ⇌ 2 SO3(g), with ΔH° = −198 kJ, which set of conditions will shift the equilibrium in favour of product formation according to Le Chatelier’s principle?

1. Raise the temperature and also raise the pressure
2. Decrease the temperature and increase the pressure
3. Any temperature and pressure conditions
4. Decrease both the temperature and the pressure

Correct answer: Decrease the temperature and increase the pressure

Solution

Decreasing the temperature favors the exothermic reaction, which produces more SO3, while increasing the pressure shifts the equilibrium towards the side with fewer moles of gas, thus promoting product formation.

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