Problem PageQuestion Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial chemical, and world production exceeds per year. The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces of solid sulfur and of oxygen gas at into an evacuated tank. The engineer believes for the reaction at this temperature. Calculate the mass of solid sulfur he expects to be consumed when the reaction reaches equilibrium. Round your answer to significant digits. Note for advanced students: the engineer may be mistaken in his belief about the value of , and the consumption of sulfur you calculate may not be what he actually observes. Clears your work. Undoes your last action. Provides information about entering answers.