Problem: A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO 3 is lower than it would be at lower temperatures. 2SO2(g) + O2(g) ⟶ 2SO3(g)(b) Is the reaction endothermic or exothermic?

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A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO 3 is lower than it would be at lower temperatures. 2SO2(g) + O2(g) ⟶ 2SO3(g)

(b) Is the reaction endothermic or exothermic?

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