adi A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO2, and oxygen, O, shown here. 2SO (g) + O (g) 2503 (g) At low temperatures, the rate of formation of SO3 is lower, but the equilibrium amount (concentration or partial pressure) of SO3 is higher than it would be at higher temperatures. (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?

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. 2SO2(g)+O2(g)2SO3(g) At low temperatures, the rate of formation of SO3 is lower, but the equilibrium amount (concentration or partial pressure) of SO3 is higher than it would be at higher temperatures. (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic