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Molecular Formula Determination from Empirical Formula & Molar Mass Calculations

This document addresses a series of chemistry questions concerning the determination of molecular formulas from given empirical formulas and molar masses. The focus is on identifying molecular formulas for compounds such as hydrocarbons and carbohydrates based on empirical data. Additionally, it covers diverse questions related to moles, mass, and percent composition of various compounds, including hydrated salts and minerals. Each question is accompanied by its respective answer for clarity and learning purposes.

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Molecular Formula Determination from Empirical Formula & Molar Mass Calculations

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  1. MOLE-O!

  2. M • 12345678 • O • 12345678 • 910111213141516 • L • 12345678 • E • 12345678

  3. M–1 Question • If your empirical formula is CH3 and your molar mass is 45.0 g/mole, what is your molecular formula? • Answer

  4. M-2 Question • If your empirical formula is CH2 and your molar mass is 28.0 g/mole, what is your molecular formula? • Answer

  5. M-3 Question • If your empirical formula is CH2O and your molar mass is 360.0 g/mole, what is your molecular formula? • Answer

  6. M-4 Question • If your empirical formula is CH3 and your molar mass is 60.0 g/mole, what is your molecular formula? • Answer

  7. M-5 Question • If your empirical formula is CH2 and your molar mass is 42.0 g/mole, what is your molecular formula? • Answer

  8. M-6 Question • If your empirical formula is CH2O and your molar mass is 180.0 g/mole, what is your molecular formula? • Answer

  9. M-7 Question • If your empirical formula is CH3 and your molar mass is 30.0 g/mole, what is your molecular formula? • Answer

  10. M-8 Question • If your empirical formula is CH2O and your molar mass is 90.0 g/mole, what is your molecular formula? • Answer

  11. O-1 Question • What is the volume (in L) of 52.0 grams of NH3 at STP? • Answer

  12. O-2 Question • How many formula units are contained in 0.285 grams of potassium hydroxide? • Answer

  13. O-3 Question • You have 8.3 X 108 atoms of zinc. How many moles is this? • Answer

  14. O-4 Question • What is the molar mass of calcium nitrate? • Answer

  15. O-5 Question • What is the molar mass of copper (II) nitrate? • Answer

  16. O-6 Question • You have 264 grams of sodium hydroxide. How many moles is this? • Answer

  17. O-7 Question • You have 1.2 grams of sodium. How many atoms is this? • Answer

  18. O-8 Question • What is the volume (in L) of 4,260 atoms of Neon at STP? • Answer

  19. O-9 Question • What is the volume (in L) of 0.847 grams of carbon dioxide at STP? • Answer

  20. O-10 Question • What is the mass (in grams) of 0.035 moles of chromium (II) chloride? • Answer

  21. O-11 Question • What is the mass (in grams) of 1.74 X 1016 formula units of sodium hydroxide? • Answer

  22. O-12 Question • How many molecules are contained in 26 grams of water? • Answer

  23. O-13 Question • What is the mass of 3 atoms of helium? • Answer

  24. O-14 Question • What is the volume (in L) of 56.27 grams of nitrogen dioxide at STP? • Answer

  25. O-15 Question • What is the mass of 3,720 molecules of O2 gas? • Answer

  26. O-16 Question • What is the mass (in grams) of 263 L of dinitrogenpentoxide at STP? • Answer

  27. L-1 Question • A 1.023 gram sample of hydrated copper (II) sulfate, CuSO4• X H2O, is heated to remove all the water and produce 0.653 grams of the anhydrous salt. What is the value of “X?” Answer

  28. L-2 Question • What is the percent water in copper (II) nitrate trihydrate? • Answer

  29. L-3 Question • What is the percent water in nickel (II) chloride hexahydrate? • Answer

  30. L-4 Question • Hydrated calcium sulfate, CaSO4• X H2O, contains 20.93% water. What is the value of “X?” • Answer

  31. L-5 Question • Borax powder has the formula Na2B4O7• X H2O. When 2.145 grams of the hydrate are heated and the water is removed, 1.130 grams of anhydrous salt remain. What is the value of “X?” Answer

  32. L-6 Question • What is the percent water in magnesium nitrate hexahydrate? • Answer

  33. L-7 Question • What is the percent water in barium chloride dihydrate? • Answer

  34. L-8 Question • If 1.687 grams of epsom salt, MgSO4• X H2O, is heat to remove all water, 0.824 grams of salt remain. What is the value of “X?” • Answer

  35. E-1 Question • What is the percent lead in lead (II) chloride? • Answer

  36. E-2 Question • What is the percent potassium in potassium dichromate? • Answer

  37. E-3 Question • What is the empirical formula of a compound composed of 77.7% iron and 22.3% oxygen? • Answer

  38. E-4 Question • What is the empirical formula of a compound composed of 44.0% iron and 56.0% chlorine? • Answer

  39. E-5 Question • What is the empirical formula of a compound composed of 34.4% iron and 65.6% chlorine? • Answer

  40. E-6 Question • What is the percent sulfur in iron (II) sulfide? • Answer

  41. E-7 Question • What is the percent sodium in sodium sulfate? • Answer

  42. E-8 Question • What is the empirical formula of a compound composed of 69.9% iron and 30.1% oxygen? • Answer

  43. M-1 Answer • C3H9

  44. M-2 Answer • C2H4

  45. M-3 Answer • C12H24O12

  46. M-4 Answer • C4H12

  47. M-5 Answer • C3H6

  48. M-6 Answer • C6H12O6

  49. M-7 Answer • C2H6

  50. M-8 Answer • C3H6O3

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