Problem

Problem

The manufacture of sulfur trioxide can be represented by the equation below: 2SO2(g)+O2(g)⇌2SO3(g)ΔH=−198 kJ mol−12\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{SO}_3(\text{g}) \quad \Delta H = -198 \text{ kJ mol}^{-1} What happens when a catalyst is added to an equilibrium mixture from this reaction?

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