Question

In this reaction,
2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat

Increasing the temperature will...

shift equilibrium right
shift equilibrium left
increase pressure
have no effect
Increasing the temperature in this reaction will shift the equilibrium position to the right.

This is because the reaction is exothermic, meaning heat is released in the forward direction. According to Le Chatelier's Principle, increasing the temperature will cause the system to try and counteract this by shifting the reaction to the side that produces heat. Therefore, the equilibrium will shift to favour the products, 2SO3, and the reaction will proceed in the forward direction.

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