• Ibuprofen (C₁₃H₁₈O₂) is the active ingredient in many nonprescription pain relievers. Each tablet contains 200 mg of ibuprofen, and a typical adult dose is two tablets every six hours.
  • Determine the molar mass of ibuprofen (show your work).
  • Calculate the number of moles of ibuprofen in a single tablet (show your work).
  • Calculate the number of moles of ibuprofen that an adult would have taken if she took four doses of ibuprofen in one day (show your work).

  . Sulfur dioxide gas (SO₂) reacts with excess oxygen gas (O₂) and excess liquid water (H₂O) to form liquid sulfuric acid (H₂SO₄). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid.
  · Write a balanced equation for the reaction.
  · Calculate the theoretical yield of sulfuric acid.
  · Calculate the percent yield of the reaction.
  (One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)
  Answer:
  
  
  
  
  
  
  

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