Elemental sulfur reacts with oxygen and water to produce Sulfuric acid in the pr

Question

Elemental sulfur reacts with oxygen and water to produce Sulfuric acid in the presence of a catalyst. What minimum mass of sulfur is needed to prepare 175g of sulfuric acid

Explanation / Answer

From chemical equation, we know that, For every 1 mole of S8 and 12 mole of O2 used, 8 mole H2SO4 and 8 mole of H2O is produced => 1 mole of S8 used = 8 mole of H2SO4 is produced =>8 mole of H2SO4 is produced = 1 mole of S8 used =>1 mole of H2SO4 is produced = 1/8 mole of S8 used ...........APPLYING LINEAR ALGEBRA Moles of H2SO4 = mass of H2SO4 / Molar mass of H2SO4 = 175/ 98 moles Now 1 mole of H2SO4 is produced = 1/8 mole of S8 used => 175/ 98 moles of H2SO4 is produced = 175 / 98*8 moles of S8 are used Moles of H2SO4 = 175/98*8 Mass of H2SO4 = number of moles* molar mass = 175/98*8 * 32*8 g = 57.15 g = 57.2 g

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